A review on applicability of naturally available adsorbents.pdf

Environ Monit Assess (2011) 183:151–195DOI 10.1007/s10661-011-1914-0 A review on applicability of naturally available adsorbents for the removal of hazardous dyes from aqueous waste Pankaj Sharma · Harleen Kaur · Monika Sharma · Vishal Sahore Received: 29 March 2010 / Accepted: 27 January 2011 / Published online: 10 March 2011 © Springer Science+Business Media B.V. 2011 Abstract The effluent water of many industries, such as textiles, leather, paper, printing, cosmetics, etc., contains large amount of hazardous dyes. There is huge number of treatment processes as well as adsorbent which are available for the processing of this effluent water-containing dye content. The applicability of naturally available low cast and eco-friendly adsorbents, for the removal of hazardous dyes from aqueous waste by adsorption treatment, has been reviewed. In this review paper, we have provided a compiled list of low-cost, easily available, safe to handle, and easy-to-dispose-off adsorbents. These adsorbents P. Sharma (B) · H. Kaur Department of Chemistry, Lovely School of Sciences, Lovely Professional University, Phagwara 144402, Punjab, India e-mail: [email protected] P. Sharma Energy and Environment Fusion Technology Center, Department of Environmental Engineering and Biotechnology, Myongji University, San 38-2, Nam-dong, Cheoin-Gu, Yongin-Si 449-728, Republic of Korea M. Sharma Department of Chemistry, Kurukshetra University, Kurukshetra 136119, India V. Sahore Department of Microelectronics & Photonics, University of Arkansas, Fayetteville, AR 72701, USA have been classified into five different categories on the basis of their state of availability: (1) waste materials from agriculture and industry, (2) fruit waste, (3) plant waste, (4) natural inorganic materials, and (5) bioadsorbents. Some of the treated adsorbents have shown good adsorption capacities for methylene blue, congo red, crystal violet, rhodamine B, basic red, etc., but this adsorption process is highly pH dependent, and the pH of the medium plays an important role in the treatment process. Thus, in this review paper, we have made some efforts to discuss the role of pH in the treatment of wastewater. Keywords Adsorption · Low-cost adsorbents · Dyes · Wastewater treatment · Column studies Introduction With the discovery of the synthetic dyes, the things began to change. Cheaper to produce, brighter, more color-fast, and easy to apply to fabric are some of the characteristic of these new dyes. Scientists have competed to formulate gorgeous new colors, and synthetic dyes had become obsolete for most applications. No doubt, this brightcolored material has changed the world; however, the chemicals used to produce dyes are often toxic, carcinogenic, or even explosive. Among the different pollutants of aquatic ecosystem, dyes are 152 a major group of chemicals (Attia et al. 2008; Namasivayam and Kavita 2002; Goyal et al. 2004; Khattri and Singh 1998). Many industries like textiles, leather, cosmetics, paper, printing, plastics, etc., use many synthetic dyes to color their products. Thus, effluents from these industries contain various kinds of synthetic dye stuffs. For instance dyes used in the textile industries are classified into three classes: (a) Anionic (direct, acid, and reactive dyes), (b) Cationic (all basic dyes), and (c) Non-ionic (dispersed dyes). Basic and reactive dyes are extensively used in the textile industry because of their favorable characteristics of bright color, being easily water soluble, cheaper to produce, and easier to apply to fabric (Karadag et al. 2007; Karcher et al. 2002; Purkait et al. 2005). Presence of color and color-causing compounds has always been undesirable in water for any use. It is, therefore, not at all surprising to note that the color in wastewater has now been considered as a pollutant that needs to be treated before discharge. Thus, color removal is one of the most difficult requirements to be faced by the textile finishing, dye manufacturing, pulp and paper industries, among others. These industries are major water consumers and are, therefore, a source of considerable pollution. In order to implement an appropriate treatment process, it is of utmost importance to minimize pollution, and to do that, it is necessary to know its exact nature. Robinson et al. (2001) made some good efforts to give some collective information related to current available technologies and have suggested an effective, cheaper alternative for dye removal and decolorization applicable on large scale. They have also provided some important data related to the desorption of individual textile dyes and a synthetic dye effluent from dye-adsorbed agricultural residues using solvents (Robinson et al. 2002a, b, c), which is also important in designing the adsorption treatment process. Various physical and chemical techniques, other than adsorption, like coagulation, chemical oxidation, froth floatation, oxidation or ozonation, membrane separation, and solvent extraction processes have been used by a number of researchers for the removal of organics as well as inorganics from the wastewater; however, these processes are effective and economic, only in the Environ Monit Assess (2011) 183:151–195 case where the solute concentrations are relatively high (Panswed and Wongchaisuwan 1986; Malik and Saha 2003; Koch et al. 2002; Ciardelli et al. 2000; Gupta and Suhas 2009). Also, these treatments involve high operational cost and aerobic digestion. For instance, photocatalytic degradation processes have shown considerable success in the removal of organic dyes from wastewater (Li et al. 2008; Pauporte and Rathousky 2007; Jain et al. 2007; Marugan et al. 2007); however, there have certain shortcomings. Coagulation process produces large amount of sludge leading to high disposal costs. Ion-exchange process has no loss of adsorbent on regeneration; however, it cannot accommodate wide range of dyes and is expensive. Membrane separation process is also effective in the removal of dyes; however, due to relatively high investment and membrane fouling problem, its application is restricted as there is a wide range in pH of dyes and even the conventional biological methods are not effective to treat dye bearing wastewaters (Lakshmi et al. 2009). Adsorption has been found to be a superior technique as compared to other methods of waste treatment in terms of cost, simplicity of design and operation, availability, effectiveness, and their insensitivity to toxic substances (Choy et al. 2000; Namasivayam et al. 1996). The more recent methods for the removal of synthetic dyes from water and wastewater were complied and reported in the form of review article by Forgacs et al. (2004). The advantages and disadvantages of the various methods were also discussed and their efficacies were compared. Adsorption is a physiochemical wastewater treatment in which dissolved molecules are attached to the surface of an adsorbent by physical/chemical forces. Depending on the nature of the interactions ionic species and molecular species carrying different functional groups may be held to the surface through electrostatic attraction to sites of opposite charge at the surface or physiosorbed due to action of van der Waals forces or chemisorbed involving strong adsorbate–adsorbent bonding. So, it may lead to attachment of adsorbate molecules at specific functional group on adsorbent surface. It is true that choice of adsorbent plays a very important role (Sarma et al. 2008). This technique is quite popular due to its simplicity as well as Environ Monit Assess (2011) 183:151–195 the availability of a wide range of adsorbents, and it proved to be an effective and attractive process for the removal of non-biodegradable pollutants (including dyes) from wastewater (Han et al. 2006; Aksu 2005). Most commercial systems use activated carbon as adsorbent to remove dyes in water because of its significant adsorption capacity. Although activated carbon is a preferred adsorbent, its widespread use is restricted due to its cost. In order to decrease the cost of treatment, some attempts have been made to find low cost alternative adsorbents. Recently, numerous studies have been conducted to develop cheaper and effective adsorbents from a variety of starting materials such as wheat bran carbon (Weng and Pan 2006), sludge ash (Rozada et al. 2003), mango seed kernel (Kumar and Kumrana 2005; Kumar ˘ and Porkodi 2006), perlite and clay (Acemioglu 2005), sawdust (Shukla et al. 2002; Garg et al. 2004), sugarcane (Ho et al. 2005a), jute fiber (Senthilkumaar et al. 2005), bagasse pith (McKay et al. 1987), and carbons from agricultural wastes. The effectiveness of a combined reduction– biological treatment system for the decolorization of non-biodegradable textile dyeing wastewater was investigated by Ghoreishi and Haghighi (2003). In this treatment system, a bisulfitecatalyzed sodium borohydride reduction is followed by activated sludge technique in order to remove the color at ambient temperature and pressure, and this experimental study consisted of two major parts: reduction treatment and biological oxidation. Joo et al. (2007) reported the decolorization of reactive dyes using inorganic coagulants and synthetic polymer, and they found that the use of inorganic coagulant alone appeared little effective in the removal of reactive dyes from the real wastewater. However, alum/polymer and ferric salt/polymer combinations improved color removal up to 60% and 40%, respectively. In this review, an extensive list of adsorbents obtained from different sources has been compiled, and this review also reports the optimum processing parameters for getting maximum dye removal for effluent water. Main emphasis is on the pH and initial dye concentration in the solution as these two parameter affects the adsorption process more. The other objective to write this review paper is to make some comparisons between 153 the adsorbent capacity of chemically modified, pretreated, and untreated adsorbents. Low cost and easily available adsorbents Keeping all the above points in view, our laboratories are contributing more towards the direction of adsorption by cheap adsorbents. Cost is actually an important parameter for comparing the adsorbent materials. Certain waste products from industrial and agricultural operations, natural materials, and biosorbents represent potentially economical alternative sorbents. Many of them have been tested and proposed for dye removal. Waste materials from agriculture and industries A number of agricultural wastes/by-products and industrial waste products have been proposed by a number of researchers for the dye removal from aqueous wastewater (Namasivayam and Kadirvelu 1994; Pala and Tokat 2002; Crini 2006). These low-cost adsorbents are abundant in nature, inexpensive, require little processing, and are effective for dye removal. The recently reported adsorbents obtained from the industrial waste and agricultural by products with their adsorption capacities (milligrams per gram) are tabulated in Table 1. Activated carbon Activated carbon adsorption is one such method which has great potential for the removal of dyes from aqueous waste. The adsorption capacity of activated carbon depends on various factors, such as surface area, pore size distribution, and surface functional groups on the adsorbent, polarity, solubility, and molecular size of the adsorbate, solution pH and the presence of other ions in solution, and so on. The most widely used activated carbons are microporous and have high surface areas, and as a consequence, show high efficiency for the adsorption of low molecular weight compounds and for larger molecules. Zhi-yuan (2008) carried out an adsorption study of methylene blue on activated carbon fiber (ACF). It has been used in adsorption systems including removal of noxious 154 Environ Monit Assess (2011) 183:151–195 Table 1 Reviewed results representing the adsorption capacity of agriculture and industrial waste materials for the adsorption of dyes and their optimized pH values for maximum adsorption Adsorbent Dye pH Adsorption capacity References Rice husk Activated carbon - RHC Rice husk Activated carbon Activated carbon - RHS Activated carbon - RHZ Rice husk Rice husk Rice husk ash Sugarcane bagasse Sugarcane bagasse Sugarcane bagasse Activated carbon Sugarcane bagasse Sugarcane dust Activated carbon Activated carbon Activated carbon Activated carbon Activated carbon Activated carbon Activated carbon Activated carbon Activated carbon Fly ash SFA Fly ash SFA Fly ash CFA Fly ash CFA Fly ash CFA Fly ash CFA Fly ash CFA Fly ash CFA Cotton waste Fly ash Fly ash Fly ash Fly ash Fly ash Fly ash Fly ash Fly ash Sludge ash Sludge ash Sludge ash Activated carbon (sludge based) Activated carbon (sludge based) Activated carbon (sludge based) Activated carbon (sludge based) Activated carbon (Chemviron GW) Activated carbon (Chemviron GW) Activated carbon (Chemviron GW) Indigo carmine Acid yellow 36 α-picoline Crystal violet Crystal violet Acid blue Congo red Safranine Brilliant green Methylene blue Methylene blue Methyl red Acid orange 10 Basic violet 3 Basic green 4 Acid blue 80 Acid red 114 Acid yellow 117 Reactive blue 2 Reactive yellow 2 Reactive red 4 Methylene blue Crystal violet Rhodamine B Methylene blue Rhodamine B Methylene blue Rhodamine B Egacid orange II Egacid red G Egacid yellow G Midlon black VL Basic blue Acid orange 7 Acid yellow 23 Direct yellow 28 Basic yellow 28 Disperse blue 79 Pyridine Brilliant green Metomega chrome Methylene blue Reactive blue 2 Reactive yellow 2 Basic red 46 Acid brown 283 Direct red 89 Direct black Basic red 46 Acid brown 283 Direct red 89 5.4 3.0 7.0 10.8 10.8 2.0 6.0 7.0 3.0 5.8 7.0 7.0 7.0 7.0 7.0 7.0 7.0 7.0 7.0 7.0 7.0 3.0 3.0 3.0 5.0 5.0 5.0 5.0 5.0 5.0 5.0 5.0 7.0 7.0 7.0 7.0 7.0 7.0 6.0 3.0 7.0 4.0 7.0 7.0 11.0 3.0 3.2 3.0 11.0 3.5 4.0 65.90 mg g−1 86.90 mg g−1 15.46 mg g−1 64.80 mg g−1 61.60 mg g−1 55.40 mg g−1 ≈14.00 mg g−1 178.10 mg g−1 26.20 mg g−1 34.20 mg g−1 99.60 mg g−1 54.60 mg g−1 5.78 mg g−1 3.79 mg g−1 3.99 mg g−1 112.30 mg g−1 103.30 mg g−1 155.80 mg g−1 0.27 mmol g−1 0.24 mmol g−1 0.11 mmol g−1 0.93 mmol g−1 0.43 mmol g−1 0.48 mmol g−1 2.40 × 10−3 mol g−1 0.60 × 10−3 mol g−1 3.60 × 10−3 mol g−1 1.00 × 10−3 mol g−1 4.70 × 10−3 mol g−1 2.20 × 10−3 mol g−1 1.50 × 10−3 mol g−1 3.10 × 10−3 mol g−1 277.00 mg g−1 4.00 μg g−1 23.90 μg g−1 816.00 μg g−1 288.00 μg g−1 0.06 μg g−1 31.06 mg g−1 65.9 mg g−1 742.80 μg g−1 3.5 × 10−6 mol g−1 250.00 mg g−1 333.30 mg g−1 188.00 mg g−1 20.50 mg g−1 49.20 mg g−1 28.90 mg g−1 106.00 mg g−1 22.00 mg g−1 8.40 mg g−1 Lakshmi et al. (2009) Malik (2003) Lataye et al. (2009) Mohanty et al. (2006) Mohanty et al. (2006) Mohamed (2004) Han et al. (2008) Kumar and Sivanesan (2007) Mane et al. (2007a) Filho et al. (2007) Raghuvanshi et al. (2004) Azhar et al. (2005) Tsai et al. (2001) Khattri and Singh (2000) Khattri and Singh (1999) Choy et al. (2000) Choy et al. (2000) Choy et al. (2000) Al-Degs et al. (2008) Al-Degs et al. (2008) Al-Degs et al. (2008) Wang and Zhu (2007) Wang and Zhu (2007) Wang and Zhu (2007) Janoš et al. (2003) Janoš et al. (2003) Janoš et al. (2003) Janoš et al. (2003) Janoš et al. (2003) Janoš et al. (2003) Janoš et al. (2003) Janoš et al. (2003) McKay et al. (1999) Albanis et al. (2000) Albanis et al. (2000) Albanis et al. (2000) Albanis et al. (2000) Albanis et al. (2000) Lataye et al. (2006) Mane et al. (2007b) Gupta and Shukla (1996) Weng and Pan (2006) Aksu (2001) Aksu (2001) Martin et al. (2003) Martin et al. (2003) Martin et al. (2003) Martin et al. (2003) Martin et al. (2003) Martin et al. (2003) Martin et al. (2003) 00 mg g−1 6. (2004a) Okada et al.0 7.3% 83. (2001) Rajeshwarisivaraj et al.0 9. (2008) Noroozi et al.5 8. (1999) Tamai et al.00 mg g−1 98. (2001) Rajeshwarisivaraj et al.04 mg g−1 7. (1999) Tamai et al.8 7. (2002b) Mohan et al. (2002b) Rajeshwarisivaraj et al.8 6.0 7.10 mg g−1 2.90 mg g−1 Martin et al. (2001) Rajeshwarisivaraj et al. (2002a) Juang et al.3 8.8 × 10−4 mol g−1 2. (2001) Rajeshwarisivaraj et al.8 × 10−4 mol g−1 1.00 mg g−1 181.0 Adsorption capacity g−1 References 18.40 mg g−1 4.70 mg 519.7 6. chemical H3 PO4 ) Activated carbon (Cassava peel. (2002b) Mohan et al. (2009) Senthilkumaar et al. (1999) Tamai et al. physical 700◦ C) Activated carbon (Cassava peel.9 7.00 mg g−1 551. (1999) Tamai et al.0 9.0 6. (2003) Magdy and Daifullah (1998) Tan et al.0 9. (2001) Rajeshwarisivaraj et al. (1999) Tamai et al. (1999) Tamai et al.0 × 10−4 mol g−1 8.Environ Monit Assess (2011) 183:151–195 155 Table 1 (continued) Adsorbent Activated carbon (Chemviron GW) Sugar industry mud Activated carbon (oil palm shell) Granular activated carbon Granular activated carbon Silkworm pupa Silkworm pupa Activated carbon W20 Activated carbon W20N Activated carbon (coconut tree flower) Activated carbon (Jute fiber) Activated carbon (rice husk) Metal hydroxide sludge Metal hydroxide sludge Metal hydroxide sludge Activated carbon (newspaper) Powdered activated sludge Charfines Lignite coal Bituminous coal Activated carbon Activated carbon (Cassava peel.0 × 10−4 mol g−1 1.00 mg g−1 243.0 5.0 9.2 8.49 mmol g−1 61. (2002b) Mohan et al.6 8.0 9.1 10.8 6.00 mg g−1 5. chemical H3 PO4 ) Activated carbon (bagasses) Activated carbon (bagasses) Activated carbon (beds) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Activated carbon fiber (pitch) Dye pH Direct black Basic red 22 Methylene blue Basic blue 4 Basic red 18 Basic blue 4 Basic red 18 Bisphenyl A Bisphenyl A Reactive red 3.00 mg g−1 1. (2006) Guo et al.0 6. (2002a) Chern and Wu (2001) Tamai et al. (2008) Noroozi et al.42 mmol g−1 392.0 7.0 9. (2003) Kargi and Ozmıhcı (2004) Mohan et al.2 × 10−3 mol g−1 Senthilkumaar et al. physical 700◦ C) Activated carbon (Cassava peel.0 7.0 7.4 × 10−3 mol g−1 2.9 6. (1999) Tamai et al.0 7. (2001) Rajeshwarisivaraj et al.3 8.0 7. (2001) Rajeshwarisivaraj et al. (1999) Tamai et al. (2001) Rajeshwarisivaraj et al.0 × 10−4 mol g−1 9.2 × 10−4 mol g−1 1.33 mmol g−1 0.0 7.87 mg g−1 51. (2004a) Netpradit et al.0 9.55 mg g−1 390.73 mg g−1 45. (2006) 200. (2001) Rajeshwarisivaraj et al. (2008) Noroozi et al. (1999) .27 mmol g−1 6.1 Reactive red Malachite green Reactive red 2 Reactive red 120 Reactive red 141 Methylene blue Direct yellow 12 Direct brown Direct brown Direct brown Direct brown Rodamine B Direct brown Procion orange Acid violet Malachite green Methylene blue Rodamine B Direct brown Procion orange Acid violet Malachite green Methylene blue Basic red 22 Acid blue 25 Yellow dye Acid blue 9 Acid blue 74 Acid orange 10 Acid orange 51 Direct black 19 Direct yellow 11 Direct yellow 50 Basic brown 1 Basic yellow 6. (2003) Netpradit et al. (2008) Noroozi et al.0 8.0 7.00 mg g−1 548.4% 5. (2009) Liu et al. (2008) Liu et al.3% 100% 100% 608.3 8. chemical H3 PO4 ) Activated carbon (Cassava peel.1 × 10−4 mol g−1 1.90 mg g−1 58.5 7.0 9.00 mg g−1 438. (2004a) Netpradit et al.4 8. (2001) Rajeshwarisivaraj et al.82 mmol g−1 116. (2001) Rajeshwarisivaraj et al. (2001) Juang et al.6 6.1 5.6 8.2 4. physical 700◦ C) Activated carbon (Cassava peel.69 mg g−1 100% 10.0 9.6 7.0 9.0% 100% 100% 100% 100% 100% 86. (2003) Netpradit et al.4 7. (2003b) Otero et al.00 mg g−1 270.50 mg g−1 303.00 mg g−1 2.0 7.0 . (2003b) Otero et al.50 mg g−1 277.0 2.0 5. (1994) Al-Degs et al.0 7.SWC Parthenium hysterophorus .0 8.00 mg g−1 31.60 mg g−1 Namasivayam and Sumithra (2005) Namasivayam and Sumithra (2005) Robinson et al.20 mg g−1 60.4 7. (2003) Nigam et al. (2003) Tseng et al.0 2.4 7.00 mg g−1 556.90 mg g−1 87.0 7. (2003) Tseng et al. (2004) Valix et al. (2003) Gupta et al.70 mg g−1 28.0 8.00 mg g−1 484. (2004) Valix et al.4 7. (2003a) Otero et al.00 mg g−1 1176.90 mg g−1 54.0 7.11 × 10−5 mol g−1 45.60 mg g−1 0.0 h Wheat straw Wheat straw Corn-cob shreds Corn-cob shreds Activated carbon CC-1 Activated carbon CC-3 Activated carbon CC-5 Activated carbon CC-7 Activated carbon CC-10 Activated carbon CC-15 Parthenium hysterophorus .0 7.0 5.0 7. (2000) Nigam et al.00 mg g−1 1119.00 mg g−1 3.0 8.7 44.0 10. (2004b) Woolard et al. (2003b) Tseng et al. (2004) Lata et al. (2003) Tseng et al. (2004) Valix et al.00 mg g−1 1014.00 mg g−1 10.0 7. (2002) Otero et al.5 5. (1997) Gupta et al.5 h Activated carbon (pinewood) AC1.5 h Activated carbon (pinewood) AC2.60 mg g−1 39. (2003) Tseng et al.7 h Activated carbon (pinewood) AC4. (2003a) Gupta et al.0 7.47 mmol kg−1 114. (2003a) Otero et al. (2000) 5. (2004) Valix et al.156 Environ Monit Assess (2011) 183:151–195 Table 1 (continued) Adsorbent Waste Fe(III)/Cr(III) hydroxide Activated carbon (filtrasorb 400) Dye Fe(III)/Cr(III) hydroxide Congo red Ramazol reactive yellow Ramazol reactive black Ramazol reactive red Crystal violet Indigo carmine Crystal violet Indigo carmine Crystal violet Indigo carmine Basic red Basic red Reactive red 141 Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Basic blue 69 Acid blue 264 Methylene blue Basic blue 69 Acid blue 264 Methylene blue Basic blue 69 Acid blue 264 Methylene blue Remazol red Remazol black B Remazol red Remazol black B Acid blue 80 Acid blue 80 Acid blue 80 Acid blue 80 Acid blue 80 Acid blue 80 Methylene blue Methylene blue Basic blue 41 Omega chrome red ME Direct red 12b Fe(III)/Cr(III) hydroxide Methylene blue Corncob Dye mixture Activated carbon (filtrasorb 400) Activated carbon (filtrasorb 400) Sewage sludge ASSg1 Sewage sludge ASSg1 Sewage sludge ASSg2 Sewage sludge ASSg2 Sewage sludge PSSg2 Sewage sludge PSSg2 Waste carbon slurries Blast furnace slag Metal hydroxide sludge Fly ash Sewage sludge – Ud Sewage sludge – Ad Sewage sludge – Up Sewage sludge – Ap Sewage sludge – Ua Sewage sludge – Aa Activated carbon (pinewood) AC1.0 7.40 mg g−1 184.0 8.90 mg g−1 28. (2004) Valix et al.0 8.7 434.0 7. (2003) Tseng et al.0 7. (2003a) Otero et al.70 mg g−1 30. (2000) Nigam et al. (2003b) Otero et al.0 h Activated carbon (pinewood) AC4.00 mg g−1 Al-Degs et al.0 h Activated carbon (pinewood) AC4.7 400. (2003b) Otero et al.80 mg g−1 384.0 7. (2003) Tseng et al.7 h Activated carbon (pinewood) AC2.7 h Activated carbon (pinewood) AC2.00 mg g−1 7. (2003a) Otero et al. (2000) 263.0 7.90 mg g−1 75.0 8. (2002b) 7.60 mg g−1 333.80 mg g−1 10.50 mg g−1 2. (2003a) Otero et al.00 mg g−1 Namasivayam et al.0 8.0 7. (2003) Tseng et al.0 7.00 mg 1111. (2000) Valix et al.2 × 10−5 mol g−1 1.0 10.00 mg g−1 Al-Degs et al. (2003b) Otero et al.00 mg g−1 507.30 mg g−1 59.00 mg g−1 983.00 mg g−1 761.5 h Activated carbon (pinewood) AC1.10 mg g−1 0.0 7.70 mg g−1 88. (2007) Lata et al.70 mg g−1 24. (2007) Liversidge et al.77 mg g−1 Otero et al. (2003) Tseng et al.0 8.0 4.30 mg g−1 598.4 7.0 7.10 mg g−1 0.0 8.0 8.4 7.20 mg g−1 169. (1990) 3.PWC Linseed oil cake Fly ash: coal pH Adsorption capacity g−1 References 3.0 7. (2000) Nigam et al. (2000) 5. (2003) Aygün et al.50 mg g−1 312.60 mg g−1 120.95 mg g−1 Slag Acid blue 29 2.0 4. (2001) Chou et al. (2003) Kadirvelu et al.9 3. (2004) Gulnaz et al.00 mg g−1 128.50 mg g−1 247.30 mg 101.06 mg g−1 9.60 mg g−1 191.00 mg g−1 225.86 mg g−1 Slag Acid red 91 7.1 6.0 g−1 Barley husk Activated carbon Activated carbon Activated carbon Activated sludge Activated sludge White ash Pellet adsorbent White ash Pellet adsorbent Coir pith carbon Coir pith carbon Slag Dye mixture Acid red 114 Polar yellow Polar blue RAWL Basic red 18 Basic blue 9 Congo red Congo red Congo red Congo red Rhodamine B Acid violet Basic blue 9 8.21 mg g−1 16. (2001) Chou et al.1 7. (2003) . (2003) Aygün et al.36 mg g−1 Slag Disperse red 1 2. (2003) Kadirvelu et al.00 mg g−1 222.00 mg g−1 120.20 mg g−1 70. (2002b) Choy et al.1 3.0 2. (2003) Jain et al.0 7.27 mg g−1 10. (2003) Aygün et al.3 3.40 mg g−1 93.Environ Monit Assess (2011) 183:151–195 157 Table 1 (continued) Adsorbent Dye pH Adsorption capacity 7. (2003) Kadirvelu et al.1 5.0 7.82 mg g−1 3.5 11. (2003) Kadirvelu et al. (2003) Kadirvelu et al.00 mg g−1 225.0 4.50 mg g−1 227.7 5.40 mg g−1 171.0 7.0 7. (2003) Kadirvelu et al.0 4. (2008) Karagöz et al.40 mg g−1 211.0 11. (2008) Gong et al.9 3.80 mg g−1 1.50 mg g−1 240.80 mg g−1 100.70 mg g−1 171.33 mg g−1 4. (2004) Chou et al.1 1.2 5.70 mg g−1 256.0 6. (2003) Kadirvelu et al.0 6.00 mg g−1 225. (2003) Kadirvelu et al. (2001a) Ramakrishna and Viraraghavan (1997) Ramakrishna and Viraraghavan (1997) Ramakrishna and Viraraghavan (1997) Ramakrishna and Viraraghavan (1997) Jain et al.0 4. (1999) Choy et al.0 4.60 mg g−1 191. (2003) Kadirvelu et al.00 mg g−1 31. (2001) Namasivayam et al.60 mg g−1 120.11 mg g−1 8. (1999) Choy et al.0 7.0 6.53 mg g−1 References Robinson et al.00 mg g−1 250. (2003) Gong et al. (2003) Kadirvelu et al. (2003) Kadirvelu et al. (2001a) Namasivayam et al. (2008) Karagöz et al. (2003) Kadirvelu et al. (2003) Kadirvelu et al.0 7.50 mg g−1 206.0 7.3 2. (2003) Jain et al.3 4.0 198.90 mg g−1 221.6 3. (2003) Kadirvelu et al.40 mg g−1 233.0 7.00 mg g−1 31.0 7.90 mg g−1 285.0 7.20 mg g−1 Carbonaceous adsorbent Carbonaceous adsorbent Carbonaceous adsorbent Silk cotton carbon Silk cotton carbon Silk cotton carbon Silk cotton carbon Silk cotton carbon Coconut tree sawdust carbon Coconut tree sawdust carbon Coconut tree sawdust carbon Coconut tree sawdust carbon Coconut tree sawdust carbon Maize cob carbon Maize cob carbon Maize cob carbon Maize cob carbon Maize cob carbon Banana pith carbon Banana pith carbon Banana pith carbon Banana pith carbon Banana pith carbon Wheat straw Wheat straw Sunflower oil cake – AC1 Sunflower oil cake – AC2 Sunflower oil cake – AC3 Activated carbon (almond shell) Activated carbon (apricot stone) Activated carbon (hazelnut shell) Activated carbon (walnut shell) Ethyl orange Methylene yellow Acid blue 113 Rhodamine B Congo red Methylene blue Methyl violet Malachite green Rhodamine B Congo red Methylene blue Methyl violet Malachite green Rhodamine B Congo red Methylene blue Methyl violet Malachite green Rhodamine B Congo red Methylene blue Methyl violet Malachite green Methylene blue Citric acid Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue 7. (2001) Chou et al.0 7.2 5.0 7.0 7.0 6. (2003) Kadirvelu et al.0 7.43 mg g−1 15. (2008) Aygün et al. (2003) Kadirvelu et al.5 3.00 mg g−1 206. (2003) Kadirvelu et al. (2008) Karagöz et al.50 mg g−1 239. (1999) Gulnaz et al.0 7.40 mg g−1 93. (2003) Kadirvelu et al.0 4. (2003) Kadirvelu et al.70 mg g−1 2.0 33.2 3.0 7.56 mg g−1 8.40 mg g−1 233. (2003) Kadirvelu et al. (1999) McKay et al.00 mg g−1 914.0 7.0 3.0 7.05 mg g−1 980.0 7.00 mg g−1 120.00 mg g−1 838.00 mg g−1 875.0 7.0 Adsorption capacity g−1 62.0 7.0 7.00 mg g−1 875.00 mg g−1 549.00 mg g−1 1 × 10−2 kg−1 4.60 mg g−1 16.00 mg g−1 914.9 mg g−1 20. (1999) McKay et al.4 7.0 2. (1999) McKay et al. (2003) Kannan and Sundaram (2001) Kannan and Sundaram (2001) Kannan and Sundaram (2001) Kannan and Sundaram (2001) Kannan and Sundaram (2001) Kannan and Sundaram (2001) Raghuvanshi et al. (2005a) Mohamed (2004) Sawada and Ueda (2003) ˘ (2004) Acemioglu Rozada et al.0 7. (2004) Filho et al.00 mg g−1 50.0 7. (2005a) Ho et al.50 mg g−1 472. (1999) McKay et al.56 mg g−1 99.0 7. (1999) McKay et al.00 mg g−1 270.0 7.0 7.30 mg g−1 143.00 mg g−1 312.10 mg g−1 96.0 7.0 7.20 mg g−1 277.20 mg g−1 50.0 7. (1999) McKay et al.0 7.4 mg g−1 13.0 7.08 mg g−1 11.0 7.0 7.0 7.0 7.00 mg g−1 250.4 7.60 mg g−1 203.00 mg g−1 158.0 2.50 mg g−1 765.0 7. (2005a) Ho et al.0 7.0 7. (1999) Namasivayam et al. (1999) McKay et al.00 mg g−1 312.0 7.0 7.4 7.50 mg 48.4 7. (2001b) Mohamed (2004) Zhi-yuan (2008) McKay et al.00 mg g−1 References Netpradit et al.00 mg g−1 828.0 5.00 mg g−1 158. (2004) Raghuvanshi et al.0 7.0 7.30 mg g−1 838. (1999) McKay et al.0 7. (1999) McKay et al. (1999) McKay et al.00 mg g−1 190.00 mg g−1 250.5 8.90 mg g−1 164.63 mg g−1 16.0 7.00 mg g−1 567. (2001b) Namasivayam et al.4 7.5 7.00 mg g−1 99. (1999) McKay et al.0 3.00 mg g−1 190.5 7. (1999) McKay et al.6 mg g−1 50.0 7.0 7. (2003) McKay et al.4 7.30 mg g−1 56. (1999) McKay et al. (1999) McKay et al.00 mg g−1 270. (2003) Netpradit et al.00 mg g−1 1453.158 Environ Monit Assess (2011) 183:151–195 Table 1 (continued) Adsorbent Metal hydroxide sludge Metal hydroxide sludge Metal hydroxide sludge Bark Rice husk Cotton waste Hair Coal Bark Rice husk Cotton waste Hair Coal Core pith Core pith Core pith Activated carbon (rice husk) Activated carbon fibers Rice husk Cotton waste Hair Coal Bark Rice husk Cotton waste Hair Coal Sugarcane dust Sugarcane dust Sugarcane dust Activated carbon (rice husk) Cotton Calcium rich . (1999) McKay et al.90 mg g−1 343.20 mg g−1 1119.0 7. (1999) Ho et al.00 mg g−1 785.5 8.0 7.fly ash Activated carbon (sewage – sludge) Activated carbon (sewage – sludge) Commercial activated carbon Bamboo dust carbon Coconut shell carbon Groundnut shell carbon Rice husk carbon Straw carbon Sugarcane baggase Activated sugarcane baggase Lignin (sugarcane baggase) Activated carbon PKN2 Activated carbon PKN2 Activated carbon PKN2 Activated carbon PKN3 Activated carbon PKN3 Activated carbon PKN3 Activated carbon PKN4 Activated carbon PKN4 Dye Reactive red 2 Reactive red 120 Reactive red 141 Safranine Safranine Safranine Safranine Safranine Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Acid violet Acid brilliant blue Rhodamine B Acid blue Methylene blue Safranine Safranine Safranine Safranine Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Basic violet 10 Basic violet 1 Basic green 4 Acid blue Direct red 28 Congo red Methylene blue Saphranine Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Acid blue 74 Basic brown 1 Methylene blue Acid blue 74 Basic brown 1 Methylene blue Acid blue 74 pH 8.0 7.00 mg g−1 120.0 3. (2003) Rozada et al.00 mg g−1 1. (1999) McKay et al.47 × 105 mol g−1 6. (2003) Netpradit et al.00 mg g−1 561. (2001b) Namasivayam et al.0 4.00 mg g−1 1529. (2007) Tseng (2007) Tseng (2007) Tseng (2007) Tseng (2007) Tseng (2007) Tseng (2007) Tseng (2007) Tseng (2007) . (1999) McKay et al. where reactive dye.39 mmol g−1 0. Li et al.0 7.45 Adsorption capacity g−1 1845.36 mmol g−1 0. (2004) made attempt to evaluate the porous properties and hydrophobicity of activated carbons obtained from several solid wastes. while the rate of displacement was a function of PAC type as well as carbon dose. Moreover.41 mmol g−1 0. Authors reported that the activated carbons with plentiful mesopores prepared from PET and waste tires had quite high adsorption capacity for large molecules. Therefore. The effects of various experimental parameters. (2005) bonization.60 mmol g−1 0.41 mmol g−1 0.0 7.0 7.0 7. (2007) Attia et al. high adsorption capacity. Choy et al. waste PET. thermodynamic parameters Go .0 7.00 mg g−1 412. reproducibility. (2008) Attia et al.19 mmol g−1 0.00 mg g−1 316. The liquid-phase adsorption characteristics of organic compounds from aqueous solution on the activated carbons were determined to confirm the applicability of these carbons. car- pH 7. refuse derived fuel.00 mg 90. waste tires. (2008) Attia et al.26 mmol g−1 0.00 mg g−1 362. and H o were calculated (Wang and Zhu 2007).0 7. (2008) Attia et al.1 2.5 7.9 mg g−1 198.87 × 10−5 mg g−1 222. they are useful for wastewater treatment. on the adsorption rates were investigated.36 mmol g−1 0. and processability. and acid treatment prior to steam activation). well-developed micropores.0 7. were employed as representative adsorbates.34 × 10−5 mg g−1 5. Nakagawa et al.0 7.0 7. The extent of atrazine displacement by NOM was found to be dependent on the type of PAC. Activated carbons having various pore size distributions were obtained by the conventional steam-activation method and via the pretreatment method (i.00 mg g−1 5. especially for removal of bulky adsorbates.39 mmol g−1 0.18 mmol g−1 0.37 mmol g−1 0.0 7.0 7. Equilibrium data was fit well by a Freundlich isotherm equation. (2008) Attia et al.59 mmol g−1 0.0 7.0 3.0 7.0 7. namely.0 7.0 7.e.0 2. (2000) reported the adsorption of .00 mg g−1 306. (2008) Attia et al.. (2007) Jain et al. (2002) reported the displacement of atrazine by the strongly competing fraction of natural organic matter (NOM) in batch and continuousflow powdered activated carbon (PAC) adsorption system.0 7. (2007) Özer and Dursun (2007) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Bouzaida and Rammah (2002) Guo et al. mixture of raw materials with a metal salt. (2008) Jain et al. Black5.0 7.64 mmol g−1 0. such as the initial methylene blue (MB) concentration and the ACF mass. and wastes generated during lactic acid fermentation from garbage.00 mg g−1 309.90 mmol g−1 References Tseng (2007) Ahmad et al.20 mg g−1 0.1 2.0 7.37 mmol g−1 0. So .0 7.0 7. Adsorption measurement shows that the process is very fast.59 mmol g−1 0.Environ Monit Assess (2011) 183:151–195 159 Table 1 (continued) Adsorbent Activated carbon PKN4 Activated carbon (oil palm wood) Activated carbon C1 Activated carbon C2 Activated carbon C3 Activated carbon C4 Activated carbon C5 Activated carbon C6 Activated carbon Rice husk Wheat bran carbon I-GLYTAC-Cotton I-GLYTAC-Cotton I-GLYTAC-Cotton II-GLYTAC-Cotton II-GLYTAC-Cotton II-GLYTAC-Cotton III-GLYTAC-Cotton III-GLYTAC-Cotton III-GLYTAC-Cotton IV-GLYTAC-Cotton IV-GLYTAC-Cotton IV-GLYTAC-Cotton V-GLYTAC-Cotton V-GLYTAC-Cotton V-GLYTAC-Cotton Porous carbon Dye Basic brown 1 Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Rhodamine B Rhodamine B Methylene blue Acid blue 25 Acid yellow 99 Reactive yellow 23 Acid blue 25 Acid yellow 99 Reactive yellow 23 Acid blue 25 Acid yellow 99 Reactive yellow 23 Acid blue 25 Acid yellow 99 Reactive yellow 23 Acid blue 25 Acid yellow 99 Reactive yellow 23 Rhodamine B gases because of its extensive specific surface area. The mesopore contribution to the total pore volume ranged from 52% to 83%.e. The adsorption of CR was better represented by the Langmuir equation. The equilibrium adsorption data were interpreted using Langmuir and Freundlich models. which is the optimum pore size region for TCE adsorption. in general. Also. ACF10.. It also had the highest volume in pores 5–8 Å. groundnut shell. exhibited the least NOM uptake for each fraction. a modified extended Langmuir isotherm with a constant interaction factor. These four models are the extended Langmuir isotherm.It was found that the higher the fraction of mesopores with a size between 10 and 50 nm. Adsorption of congo red (CR) dye on bituminous coal-based mesoporous activated carbon (AC) from aqueous solutions was reported by Grabowska and Gryglewicz (2007). functioning as a molecular sieve during preloading. the kinetics and mechanism of MB adsorption on commercially activated carbon and indigenously prepared activated carbons from bamboo dust. Four models for predicting the multicomponent equilibrium sorption isotherms have been compared in order to determine the best to predict or correlate binary adsorption data. Adsorption of trichloroethylene (TCE) by two ACFs and two granular activated carbons preloaded with hydrophobic and transphilic fractions of NOM was examined by Tanju Karanfil et al. and subsequently the highest TCE adsorption. Adsorption equilibrium and kinetics of Egacid red sorption on PAC were stud- . rice husk. The adsorption capacities of indigenous activated carbons have been compared with that of the commercially activated carbon. they showed higher adsorption efficiency for all NOM fractions. amount of adsorbent used and the initial pH of the solution. was discussed. The intra-particle diffusion into small mesopores was found to be the rate-limiting step in the adsorption process. Therefore.3.8–8. the firstorder Lagergren model. the shorter the time to achieve the equilibrium stage Environ Monit Assess (2011) 183:151–195 for CR adsorption. and straw have been reported by the Kannan and Sundaram (2001). AB80 + AY117. In the same paper. i. The effects of various experimental parameters have been investigated using a batch adsorption technique to obtain information on treating effluents from the dye industry. The extent of dye removal increased with decrease in the initial concentration of the dye and particle size of the adsorbent and also increased with increase in contact time. (2007) contribution deals with study of the combined adsorption-membrane process for organic dye removal. among the four activated carbons. and AY117) and three binary component (AB80 + AR114. as compared to ACF10. Adsorption data were modeled using the Freundlich and Langmuir adsorption isotherms and first-order kinetic equations. negligible. The pseudo-second-order kinetic model describes the adsorption of CR on mesoporous activated carbon very well. dyes adsorption on activated carbon.980 to 0. The adsorption tests were performed under static conditions at solution pH 7. the simplified model based on single-component equilibrium factors. where NOM molecules can be adsorbed. including high volumes in pores larger than 10 Å. The results indicate that such carbons could be employed as the low-cost alternatives to commercially activated carbon in wastewater treatment for the removal of color and dyes. Acid Blue 80 (AB80). and subsequently lower adsorption capacities for TCE. Acid Red 114 (AR114). and AR114 + AY117). (2006) ACF10. AR114. The most microporous activated carbon used in this study had over 90% of its pore volume in pores smaller than 10 Å. and Acid Yellow 117 (AY117) onto activated carbon. coconut shell.991. The kinetics of adsorption was found to be first order with regard to intra-particle diffusion rate. the pseudo-second-order model. The other three sorbents had wider pore size distributions. The effect of solution ionic strength on the uptake of CR by two different mesoporous carbons was also investigated. As a result. and the intraparticle diffusion model. Jirankova et al. they have also reported the adsorption isotherms for the three single components (AB80. The kinetics of adsorption in view of three kinetic models. The monolayer adsorption capacity of ACs was found to increase with increasing both the mesopore volume and the mesopore contribution to their porous texture.160 three acidic dyes. The correlation coefficients ranged from 0. Adsorption of NOM fractions by ACF10 was. and a modified extended Langmuir isotherm incorporating a surface coverage-dependent interaction factor. from aqueous effluent by McKay et al. Several others authors (Al-Degs et al.05%) and high percentage of silica in its mineral ash. Rice husk/rice husk ash Rice husk is insoluble in water. contact time. 2008. t = 8 h.0 g L−1 . (2003) reported that the surface chemistry of a commercially activated carbon has been selectively modified. Batch experiments were carried out to determine the influence of parameters like initial pH. and increase the porosity and surface area. adsorbent dose. The conventional bed depth service time (BDST) model has not been applied to tapered beds before. the acid oxygencontaining surface groups show a positive effect but thermally treated samples still present good performances.44%). such as adsor- . a close relationship between the surface basicity of the adsorbents and dye adsorption is shown. direct. for operating continuous adsorption columns. (2008). The Redlich–Peterson (R– P) isotherm gives the best fit model to describe the sorption process of these organic pollutants. and possesses a granular structure. decrease cellulose crystallinity. The effects of various experimental parameters.34%).24%). (2006). and thermal treatments under a flow of H2 or N2 . NH3 . Tapered bed adsorption columns. The adsorbent obtained by this treatment is light weight with a very external surface area. Equilibrium sorption isotherms were measured to provide the saturation capacity (qe ) of each pollutant by Chemviron Filtrasorb 400 carbon. and m = 10. showing the existence of two parallel adsorption mechanisms involving electrostatic and dispersive interactions. making it a good adsorbent material. has good chemical stability. Nassar and Magdy 1997) have also tested activated carbon for the adsorption of various dyes. high mechanical strength. Pretreatment of rice husk can remove lignin and hemicelluloses.Environ Monit Assess (2011) 183:151–195 ied in batch experiments. The conclusions ob- 161 tained for each dye individually were confirmed in the color removal from a real textile process effluent. lignin (21. and they found that the surface chemistry of the activated carbon plays a key role in dye adsorption performance. The pseudo-secondorder kinetic model represented the adsorption kinetics of IC on to RHA. Lakshmi et al.4. by means of chemical treatments. Langmuir. Temkin. as the linear velocity of fluid is continually changing along the column.34%. For cationic dyes (basic). The basic sample obtained by thermal treatment under H2 flow at 700◦ C is the best material for the adsorption of most of the dyes tested. The positive values of the change in entropy (So ) and heat of adsorption (H o ). H2 O2 . the interaction between the oxygen-free Lewis basic sites and the free electrons of the dye molecule being the main adsorption mechanism. The presented combined adsorption-membrane process has a potential application for organic dye removal. (2009) carried out study of the adsorptive characteristics of Indigo Carmine (IC) dye from aqueous solution onto RHA. it was found that membrane was effective for removal of PAC particles from water suspensions and PAC tendency for irreversible membrane fouling was extremely low. have been used to study the removal of two organic pollutants. using activated carbon. an acid dye and para-chlorophenol. Equilibrium isotherms were analyzed by Freundlich. hemicelluloses (21. using HNO3 . Rice husk consists of cellulose (32. and acid). prepared from low-cost rice husk by two different processes: physical activation and chemical activation. The optimum conditions were found to be: pH = 5. Rice husk can easily be converted into rice husk ash (RHA) at 300◦ C which contains 92% to 95% silica. which is approximately 96. In this study. activated carbons. and mineral ash (15. were used as the adsorbent for the removal of crystal violet. and Redliche Peterson models using a nonlinear regression technique. Adsorption of IC on RHA was favorably influenced by an increase in the temperature of the operation. Wang and Zhu 2007. and the negative value of change in Gibbs free energy (Go ) indicate feasible and spontaneous adsorption of IC on to RHA. Pereira et al. and initial dye concentration on the removal of IC. For anionic dyes (reactive. During the combined hollow fiber membrane microfiltration operated in dead-end mode. Adsorption onto activated carbon is a potent method for the treatment of dye-bearing effluents because it offers various advantages as reported by Mohanty et al. without changing significantly its textural properties. and contact time (Tsai et al. and temperature. with different parameters like dye concentration. (2004). for the removal of MB dye. the influent concentration of CR. The results indicate that RHS and RHZ could be employed as low-cost alternatives to commercially activated carbon in wastewater treatment for the removal of basic dyes. pH. It was found that intra-particle diffusion plays a significant role in the adsorption mechanism. The data were in good agreement Environ Monit Assess (2011) 183:151–195 with BDST model. Formaldehydetreated and sulfuric acid-treated sugarcane baggase were used to adsorb methyl red at varying dye concentration. Adams–Bohart. existing salt. 2005.. The results showed that Thomas model was found suitable for the normal description of breakthrough curve at the experimental condition. (2007) carried out an experiment in which the adsorption kinetics and equilibrium of MB onto reticulated formic lignin from sugar cane baggase was studied. while Adams–Bohart model was only for an initial part of dynamic behavior of the rice husk column. Initially. contact time. The kinetic data were well fitted to the Lagergren. Kumar and Sivanesan 2007. Azhar et al. The adsorption process is . This study investigates the potential use of sugarcane baggase. and bed depth. were studied. the flow rate. (2008) reported a continuous bed study by using rice husk as a biosorbent for the removal of CR from aqueous solution. This study presents findings on identifying the key factor for high desulfurization activity in sorbents prepared from RHA. pH. The maximum uptakes of crystal violet by sulfuric acid activated (RHS) and zinc chloride activated (RHZ) rice husk carbon were found to be 64. The initial pH of 6–10 flavors the adsorption of both PCSB and PCSBC.162 bent dosage and size. contact time. adsorbent dosage. and Yoon– Nelson models were applied to the experimental data in order to predict the breakthrough curves using nonlinear regression and to determine the characteristic parameters of the column useful for process design. such as RHA. in a batch or stirred tank reactors. The isothermal data could be well described by the Langmuir and Freundlich equations. the baggase was investigated in batch experiments with two different forms i. It is proposed that PCSB and PCSBC. respectively. Similar experiment was conducted with commercially available PAC. temperature. It has been reported in one of the papers by Dhalan et al. initial dye concentration. pretreated with formaldehyde (PCSB) and sulfuric acid (PCSBC). initial dye concentration. McKay et al. pseudo-second order. It was concluded that the rice husk column can remove CR from solution (Malik 2003. Han et al. Guo et al. 1999. raw and chemically activated forms. The adsorption efficiency of different adsorbents was in the order PAC>PCSBC>PCSB. Filho et al.575 mg g−1 of adsorbent. 2001). have the potential to be utilized as highperformance sorbents for the flue gas desulfurization process in small-scale industrial boilers. a systematic approach using central composite rotatable design was used to develop a mathematical model that correlates the sorbent preparation variables to the desulfurization activity of the sorbent. An average percent removal difference between the two adsorbents of around 18% was achieved under the different experimental conditions. The effects of important factors. in order to evaluate the performance of PCSB and PCSBC. and the bed depth. Thomas. (2006) that the materials.875 and 61. Mohamed 2004. and intra-particle diffusion models. 2007a). 2008. The data fit well in the Freundlich isotherm. (2005) in one of his papers has reported that adsorbents prepared from sugarcane baggase-an agro industries waste were successfully used to remove the methyl red from an aqueous solution in a batch reactor. The removal is better and more effective with chemically activated baggase in comparison to the raw baggase. Data confirmed that the breakthrough curves were dependent on flow rate. Mane et al. could be employed as a low-cost alternative in wastewater treatment for the dye removal.e. Han et al. while BDST model was used to express the effect of bed depth on breakthrough curves. and adsorbent dose is reported by Raghuvanshi et al. for the removal of methyl red from simulated wastewater. were investigated in batch mode. Adsorbents are very efficient in decolorized diluted solution. Sugarcane dust The adsorption potential of agricultural (sugarcane) by-product. such as the value of pH. The sorption of three basic dyes. High exhaustion of the 163 dye in reverse micellar system was attributed to the very low bath ratio (water–fabric ratio) compared to the conventional aqueous dyeing process. and ionic strength (μ) dependent and obeys the Langmuir model. 99.4% for acid yellow 23. The mean removed amounts of dyes by adsorption on columns of soil mixture with 20% fly ash content and for initial concentration of dye solutions 50 mg L−1 were up to 33. 96. and the three-parameter Redlich–Peterson isotherms. (2009) reported adsorption of pyridine (Py) from aqueous solutions. Freundlich. acid yellow 23. The commercial dyes. basic violet 1.20 mg g−1 ) were observed at pH = 5. the capacity is around 589. 98. a waste material. to be a low-cost sorbent.25% of nitrogen. and direct yellow 28 represent the widely used nitroazo structures. it took from 1 to 10 days to reach equilibrium (Khattri and Singh 1999).2% for direct yellow 28. Bouzaida and Rammah (2002) reported the adsorption of acid dyes on treated cotton in a continuous system. named basic violet 10. Exhaustion of dye was almost perfect and was very superior to that in aqueous system. Conditions for higher adsorption rate and capacity were determined. water absorbency. Cotton waste Cotton is one of the most widely used fibers by the agriculturists.5% for disperse blue 79.0% for acid yellow 7. Fly ash Adsorption and removal of commercial dyes were studied in aqueous suspensions of fly ash mixtures with a sandy clay loam soil of low organic matter content. These interactions between binding sites were detected through Scatchard analysis. (2001).9% for acid yellow 23. 50◦ C. from aqueous solutions onto sugarcane dust was studied by Ho et al. and 88. and dye removal ability. Sawada and Ueda (2003) studied the solubilization and adsorption behavior of direct dye on cotton in Aerosol-OT revere micellar system. using bagasse fly ash (BFA). The maximum removal of Py is determined to be 99% . and 302 mg of adsorbed dye. and basic green 4. The faster adsorption (12 h) and higher adsorption capacity (34. 448.2% for direct yellow 28. The logarithmic form of Freundlich equation gave a high linearity and the K constants are increasing with the increase of fly ash content in adsorbent mixtures and the affinity between the adsorbent surface and adsorbed solute. for acid blue 25. temperature. 44. respectively. Lataye et al. Cotton fabrics could be dyed in deep shade with direct dye from reverse micellar system without adding auxiliaries.8% for acid yellow 7. and Reactive yellow 23 dyes.Environ Monit Assess (2011) 183:151–195 pH. which is a solid waste that is generated from bagasse-fired boilers as an adsorbent. two error analysis methods were used to evaluate the data: the linear coefficient of determination and the Chi-square statistic test for determination of a nonlinear model. and 0. 84. The mean amount of removed dyes by adsorption batch experiments in soil mixture with 20% fly ash content were up to 53. In order to determine the best-fit isotherm for each system. The results revealed the potential of sugarcane dust.8 (acetic acid-sodium acetate aqueous buffer).8% for basic yellow 28.3% for disperse blue 79. Under temperature (50◦ C) control and occasional mechanical stirring.2% for basic yellow 28. on the removal of Py from the aqueous solutions. basic yellow 28. It has become obvious that adsorption of direct dye on cotton in reverse micellar system is similar to that in aqueous system and follows a Freundlich manner. acid yellow 99.1 ionic strength. showing the process to be highly dependent on the concentration of the solution. (2000) at equilibrium conditions for concentrations of dyes between 5 and 60 mg L−1 . Batch and column experiments were carried out by Albanis et al. Moreover. Cotton found naturally and consisting cellulose exhibits excellent physical and chemical properties in terms of stability. It has been concluded that at 20◦ C and for the grafted support at 1. disperse blue 79. 59. Results indicated that the Chisquare test provided a better determination for the three sets of experimental data. Batch adsorption studies have been performed to evaluate the influence of various parameters. and 60. Equilibrium isotherms were analyzed using the Langmuir. The removal of dyes from column experiments decrease with the increase of the solution concentration form 10 to 50 mg L−1 at 20◦ C. acid orange 7. ranged from -4. 5. suggesting that the adsorption could be considered as a physical process. which is simultaneously enhanced by the electrostatic effects. ranged from −6. Results show that the ash could remove the dye effectively from aqueous solution. The adsorptions of crystal violet and basic fuschin follow first-order rate kinetics. In comparison to other low-cost adsorbents. at temperature of 4◦ C.164 at lower concentrations (<50 mg L−1 ) and 95% at higher concentrations (600 mg L−1 ). suggesting that the adsorption was of the typical physical type.3 × 10−6 . The adsorption capacities followed the order CFA > CFA-600 > CFA-NaOH. 2007b.12 mg g−1 . all followed pseudo-secondorder kinetics. using the Langmuir. respectively. Redlich–Peterson. Gupta and Shukla 1996). According to the positive values of H◦ and S◦ . The ARE and EABS error function methods provided the best parameters for the Langmuir isotherms and pseudo-second-order equations.3 × 10−6 . The removal of each dye was found to be inversely proportional to the size of the fly ash particles.63. as expected. respectively. and the capacities for all of them increased upon increasing the temperature (60◦ C > 45◦ C > 30◦ C). and 3. 6.59–103.62 to −7. Go . and CFANaOH for AR1 were 92. The multilayer adsorption energy. using a BFA dosage of 25 kg m−3 at normal temperature. (2002a). The adsorptions of AR1 onto CFA. Both the linear and nonlinear forms of the Langmuir and Freundlich models have fitted the adsorption data. thereby indicating that the process is endothermic in nature. The negative values of free energy indicate the feasibility and spontaneous nature of the process. and adsorbent doses by Mohan et al. The adsorption of each dye was found to increase with increasing temperature. pHs. Values of the first-layer adsorption energy. and 12.0 × 10−6 .66–25. 32. Thermodynamic parameters such as the free energies. the data were better correlated with the nonlinear than the linear form of this equation. Go . 14◦ C.51 to -5. enthalpies. CFA-600. the sorption capacity of the material under investigation is found to be comparable to that of other commercially available adsorbents used for the removal of cationic dyes from wastewater (Mane et al. The adsorption kinetics could be expressed by the modified Freundlich equation and intra-particle diffusion model.5 × 10−6 mol g−1 .09. The adsorption equilibrium analyses are performed. The adsorption rate was fast and about 80% of absorbed MB was removed in 10 min. Studies on Py adsorption equilibrium and kinetics by BFA also have been conducted. respectively. these adsorptions were endothermic processes. Thermodynamic studies revealed that the adsorption of Py on BFA is endothermic in nature and that the isosteric heat of adsorption decreases as the equilibrium uptake of Py on the BFA surface increases. The results indicate that the Freundlich adsorption isotherm fitted the data better than the Langmuir adsorption isotherm. and CFA-NaOH. and the positive heats of enthalpy suggest the endothermic nature of the process. Adsorption studies were carried out for differ ent temperatures. particle sizes. Hsu (2008) carried out experiment in which they found that raw coal fly ash (CFA) that has not been subjected to any pretreatment process have a superior adsorbing ability for the anionic dye Acid red 1 (AR1) than the two modified coal fly ashes (CFA-600 and Environ Monit Assess (2011) 183:151–195 CFA-NaOH). The equilibrium adsorption data was correlated well to the nonlinear multilayer adsorption isotherm. Further. and Temkin isotherm equations.02 kcal mol−1 . The effect of electrical double layer thickness on the adsorption kinetics was discussed. The Langmuir equation is determined to best represent the equilibrium sorption data.65 kcal mol−1 . It was found that both the initial MB concentration and ionic strength could affect the rate of adsorption. and 34◦ C. Freundlich.79–52. The maximum adsorption capacities for MB were 7. the adsorption capacities of CFA. On the basis of the monolayer dye . Sludge ash/bottom ash Weng and Pan (2006) reported that the kinetics and equilibrium adsorption experiments were conducted to evaluate the adsorption characteristics of a cationic dye (MB) onto bio-sludge ash. and entropies of adsorption of the dye-fly ash systems were also evaluated. 24◦ C. CFA-600. in the AR1–CFA adsorption system. The isotherms for the adsorption of AR1 onto the raw and modified coal fly ashes fit the Langmuir isotherm quite well. The equilibrium data was fitted to Langmuir. (2006b). The ion exchange and pseudo-first-order constant rates were 0. Sips. respectively. and India is the second largest consumer and producer of fruits which also leads to the generation of million tones of fruit waste. the specific surface area of this ash sample was estimated as 2.05594 and 0. Tartrazine a highly toxic dye can be adsorbed by bottom ash as demonstrated by Mittal et al. In alkaline pH region. a highly toxic indigoid class of dye from wastewater by bottom ash. pH of the solution. and both the adsorbents have been found to exhibit good efficiency to adsorb indigo carmine. have been observed.9 m2 g−1 which is close to the value (3. Langmuir and Freundlich adsorption isotherms are successfully employed on both the adsorbents. Freundlich. The column studies reveal that about 96% saturation of both the columns is attained during their exhaustion.1–2. was tested as biosorbent for the removal of a cationic dye MB from aqueous solution. and pH on adsorption capacities were studied. and on the basis of these models. indigo carmine has been adsorbed through the column beds of bottom ash and de-oiled soya. dosage of adsorbents. pH. Yellow passion fruit Pavan et al. and Redlich–Peterson isotherm models. sieve size of adsorbents. Adsorption of MB onto this low-cost natural adsorbent was studied by batch adsorption at 25◦ C. Different thermodynamic parameters. The contact time required to obtain the maximum adsorption was 48 h at 25◦ C. the adsorption of MB is favorable. respectively. equilibrium uptake of the dye is observed at different concentrations. Kumar and Porkodi 2006. the data were best fitted to Sips isotherm model. Attempts have been made through batch and bulk removal of the dye.05455 h−1 . (2008a) reported that the use of yellow passion fruit (YPFW). and sieve size of adsorbents. Through the batch technique. particle diffusion process is predominant at higher concentrations. (2006a) carried out an inexpensive adsorption method for the removal of indigo carmine. Taking into account the analysis of the normal distribution of the residuals (difference of qmeasured − qmodel ). Fruit peel and pith is discarded in the juice and soft-drink industries all over the world. have also been evaluated (Aksu and Tezer 2000). The maximum amount of MB is absorbed by YPFW . like Gibb’s free energy. The effects of shaking time. The dye uptake on to both the adsorbents is found to validate Langmuir and Freundlich adsorption isotherms models. and entropy of the ongoing adsorption process. Kinetic investigations reveal that more than 50% adsorption of dye is achieved in about 1 h in both these cases. whereas equilibrium establishment takes about 3 to 4 h. The kinetic data treated to identify 165 rate controlling step of the ongoing adsorption processes indicate that for both the systems. concentration. Under batch technique effect of temperature. Youssef 1993). while about 88% and 84% of the dye material is recovered by eluting dilute NaOH solution through exhausted Bottom Ash. the thermodynamic parameters are evaluated. respectively. The kinetic investigations also reveal for both the adsorbents film diffusion and particle diffusion mechanisms are operative in the lower and higher concentration ranges. we have tried to discuss the cellulose-based waste (fruit waste) for the removal of different types of dyes from water (Table 2). 2008. Four kinetic models were tested.Environ Monit Assess (2011) 183:151–195 adsorption capacity. Such fruit waste can be effectively used for the wastewater treatment (Hameed et al. Mittal et al. while film diffusion takes place at lower concentrations. Fruit waste In this part of the review article. The linear plots obtained in rate constant and mass transfer studies further confirm the applicability of first order rate expression and mass transfer model. enthalpy. a powdered solid waste. and the adsorption follows a first-orderrate kinetics for both the adsorbents. Under the bulk removal. and more than 90% of the dye material has been recovered by eluting dilute NaOH solution through exhausted columns. biosorbent dosage. dosage of adsorbents. being the adsorption kinetics better fitted to pseudo-first-order and ion exchange kinetic models. etc.7 m2 g−1 ) obtained via BET nitrogen gas adsorption measurements. The Batch technique employed for kinetic measurements. 72 mg g−1 21. (2005) Arami et al. (2009) Oei et al.9 5.00 mg g−1 11.00 mg g−1 23. (1996) Sivaraj et al.7 7.0 7.5 – – 2.50 mg g−1 20. (1987) McKay et al.60 mg g−1 14.0 7.70 mg g−1 15.80 mg g−1 20.02 × 10−4 mol g−1 2.30 mg g−1 19. (1996) Namasivayam et al. (2002) Annadurai et al.3 8.3 5.00 mg g−1 20. (2002) Annadurai et al.00 mg g−1 10. (1998) Hameed and Ahmad (2009) Banat et al.90 mg g−1 157.0 8.2 5. (1998) Namasivayam et al. (2002) Annadurai et al.0 5.0 6.0 7. (2007) Pavan et al.9 5. (2007) Namasivayam et al.27 mg g−1 21.22 mg g−1 22.0 3.0 3.0 8.0 8. (2003) Banat et al.8 8. (2008a) Pavan et al.00 mg g−1 44.0 2. (2002) Annadurai et al.0 7. (2009) . (2002) Annadurai et al.0 7.50 mg g−1 8.20 mg g−1 3. (2002c) Royer et al.00 mg g−1 22.30 mg g−1 14. (2002) Annadurai et al.00 mg g−1 75.0 3.40 mg g−1 76.0 8.42 mg g−1 142. (2002) Annadurai et al.0 2.54 × 10−5 mol g−1 1.60 mg g−1 21.00 mg g−1 413.00 mg g−1 2.0 11. (1996) McKay et al.0 8.0 3.30 mg g−1 20. (2009) Akar et al. (2002) Annadurai et al.88 mg g−1 14.8 7. (1996) Chen et al.0 7. (2001) Chen et al.0 7.0 16.05 mg g−1 14.166 Environ Monit Assess (2011) 183:151–195 Table 2 Reviewed results representing the adsorption capacity of fruit waste for the adsorption of dyes and their optimized pH values for maximum adsorption Adsorbent Dye pH Adsorption capacity References Yellow passion fruit Yellow passion fruit Mandarin peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Orange peel Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Banana pith Garlic peel Raw date pits Activated date pits (500◦ C) Activated date pits (900◦ C) Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Bagasse pith Apple pomace Brazilian pine fruit shell .20 mg g−1 12. (1993) Namasivayam et al. (2005) Annadurai et al.0 7. (2002) Annadurai et al.00 mg g−1 1. (1987) McKay et al.0 7.94 mg g−1 17.20 mg g−1 6.60 mg g−1 18. (2001) Annadurai et al. (2002) Annadurai et al. (1987) McKay et al.79 mg g−1 185.3 5.08 × 10−4 mol g−1 Pavan et al.40 mg g−1 1. (2009) Oei et al.2 5. (1999) McKay et al. (2009) Royer et al.90 mg g−1 18. (2002) Annadurai et al. (2001) Chen et al.50 mg g−1 5.0 5.50 mg g−1 18.20 mg g−1 20. (2002) Annadurai et al.50 mg g−1 7.80 mg g−1 20. (2003) Banat et al.0 8. (2003) McKay et al. (1987) Robinson et al.0 6.0 7.86 mg g−1 80.0 8. (2001) McKay et al. (2002) Annadurai et al. (2001) Chen et al.00 mg g−1 152. (2002) Arami et al.5 8.0 7.60 mg g−1 17.0 5.PW Brazilian pine fruit shell .0 7.0 7.92 mg g−1 4. (2002) Annadurai et al.0 8.8 7. (1996) Namasivayam et al.00 mg g−1 158.7 7. (2002) Namasivayam et al.00 mg g−1 77.8 4.29 mg g−1 12.70 mg g−1 22. (1996) McKay et al.C-PW Barley straw Barley straw Olive pomace Methylene blue Methylene blue Methylene blue Rhodamine B Congo red Procion orange Acid violet 17 Direct red 28 Direct red 23 Direct red 80 Basic violet 10 Methyl orange Methylene blue Rhodamine B Congo red Methyl violet Amido black 10B Direct red 28 Basic blue 9 Basic violet 10 Methyl orange Methylene blue Rhodamine B Congo red Methyl violet Amido black 10B Rhodamine B Direct red Acid brilliant blue Methylene blue Methylene blue Methylene blue Methylene blue Acid blue 25 Acid red 114 Basic blue 69 Basic red 22 Acid blue 25 Acid red 114 Basic blue 69 Basic red 22 Basic blue 69 Basic red 22 Acid blue 114 Acid red 25 Reactive dye mixture Methylene blue Methylene blue Acid blue 40 Reactive black 5 Reactive red 198 9. (2002) Annadurai et al. Maximum desorption of 60% was achieved in water medium at pH of 10.70 mg g−1 . he also reported that the total number of experiments for achieving the highest removal of MB from aqueous solutions using yellow passion fruit peel (Passif lora edullis f. respectively. The equilibrium time was found to be 80 min for 10.0 7. (2001) for the removal of an acid dye: acid violet17. five center points. and 323 K). adsorbent dosage. f lavicarpa) and mandarin peel (Citrus reticulata) as biosorbents two independent sets of full 23 factorial designs with two central points (10 experiments) were experimented. 2002). Procion orange. respectively. Using these statistical tools. edullis f. The results indicated that Adsorption capacity g−1 14.42 mg dye per gram of the adsorbent for direct red and acid brilliant blue. 123.3. A maximum removal of 87% was obtained at pH 2.0 biosorbent was 44. In one of his papers.64.0 for an adsorbent dose of 600 mg 50 mL−1 of 10 mg L−1 dye concentration. and time of contact higher than 48 h for PFP and 42.00 mg g−1 285. In order to reduce the total number of experiments for achieving the highest removal of MB from aqueous solutions using yellow passion fruit peel (P. divided into four cube points. and 40 mg L−1 dye concentration. Orange peels have also been investigated as an adsorbent by Sivaraj et al. and Temkin isotherms.20 mg L−1 .45. the best conditions for MB removal from aqueous solution were initially methylene blue (Co ) of 3. and 323 K.Environ Monit Assess (2011) 183:151–195 167 Table 2 (continued) Adsorbent Pith Pith Palm fruit bunch Palm fruit bunch Palm fruit bunch Jack fruit peel Dye Acid blue 25 Basic blue 69 Basic yellow 21 Basic red 22 Basic blue 3 Basic blue 9 pH 5.30 mg 150. 313. adsorbent dosage. a new full 22 factorial design with two central points (six experiments) and a central composite surface analysis (13 experiments. and Rhodamine B dyes. Adsorption isotherms were modeled with the Langmuir. initial concentration (25–200 mg L−1 ). and pH 9 (Annadurai et al.71 mg g−1 References Ho and McKay (2003) Ho and McKay (2003) Nassar and Magdy (1997) Nassar and Magdy (1997) Nassar and Magdy (1997) Hameed (2009) the garlic peel could be an alternative for more costly adsorbents used for dye removal isotherm model.0 for PFP and 11. f lavicarpa) and mandarin peel (C. The adsorption capacity Q0 was 19. pH 9. .88 mg g−1 at initial pH of 6. The maximum monolayer adsorption capacities were found to be 82.00 mg g−1 327.0 for MP. Garlic peel Hameed and Ahmad (2009) reported the potential of garlic peel. (1996) reported the adsorption of Congo red.0 5. pH (4–12). The kinetic data were analyzed using pseudo-first-order and pseudosecond-order models. reticulata) as biosorbents. Namasivayam et al.00 mg g−1 180. Experiments were carried out as function of contact time.92 and 4. The data fitted well with the Freundlich isotherm.0 7. and pH was found to obey Langmuir and Freundlich isotherms.9 h for MP (Hameed 2009). (1998) reported the adsorption of direct red and acid brilliant blue with waste banana pith by varying the agitation time. an agricultural waste to remove MB from aqueous solution. 20. agitation time. and four axial points) were employed for yellow passion fruit peel (PFP) and mandarin peel (MP). Namasivayam et al.86 mg g−1 at 303. and temperature (303. Orange peel and Banana pith Orange peel waste was studied as a very good adsorbent for the adsorption of many dyes. The process was studied at different concentrations of dyes. dye concentration.00 mg g−1 92. and 142.0 7. The adsorption capacity was 5. respectively. 30. Adsorption increases with increase in pH. 313. Freundlich. In order to continue the optimization of the system. two independent sets of full 23 factorial designs with two central points (10 experiments) were experimented.0 7. (2002). AILP load. Plant waste The obvious advantage of above discussed adsorbent for the dyes removal by adsorption treatment is the lower costs involved. (1993). entropy of activation. The adsorp- Environ Monit Assess (2011) 183:151–195 tion was favored by an acidic pH range and was best described by a second-order rate equation. Chemical sorption can occur via the polar functional groups of lignin. (2008).05 mg g−1 . (2005) reported the adsorption capacity of direct red 23 and direct red 80 to be 10. Azadirachta indica (neem) leaf powder (AILP). Corresponding results for the pyrolyzed plant uptakes were 53and 951 mg g−1 .168 respectively. aldehydes. (2008) reported the removal of a basic dye called Rhodamine B from aqueous solution by adsorption onto a biosorbent. and ethers as chemical bonding and ion exchange (Adler and Lundquist 1963). Also the adsorption of Rhodamine-B has been reported by Namasivayam et al. while those for the pyrolyzed plant. this low-cost local plant may also prove useful for the removal of large organic molecules as well as potential inorganic contaminants.3 and 5. This would lead to a better understanding of the mechanisms controlling the adsorption rate. to remove methylene blue and iodine. Tree fern. Thermodynamically. The kinetics of sorption of methylene blue is described by pseudo-secondorder model. which include alcohols. The pseudo-second-order model was the best choice among all the kinetic models to describe the adsorption behavior of RB onto AILP. The approximate amount of dry matter produced per banana plant is about 1. . Effects of initial dye concentration. 1. Ardejani et al. Ofomaja and Ho 2007. has been currently investigated to remove dyes from aqueous solutions (McKay et al. pseudostem. suggesting that the adsorption mechanism might be a chemisorption process. respectively. Tree fern is generally dark brown in color and is a complex material containing lignin and cellulose as major constituents (Newman 1997). and free energy of activation. In comparison. Bestani et al. (2008) identify the effectiveness of a local desert plant characteristic of Southwest Algeria and known as Salsola vermiculata. Arami et al. (2005). an agricultural by-product. Han et al. and fruits. respectively. ketones. there is a need to search for more economical and effective adsorbents. Moreover. Removal was tested in a batch process with concentration of dye solution.” most of the residues are either used as manure or simply thrown away or burnt off to reduce the volume. Plant leaf powder Sarma et al.178 mg g−1 . respectively (Hegde and Srinivas 1991). and Annadurai et al. were 130and 1. phenolic hydroxides. The rate and the transport/kinetic processes of dye adsorption onto the adsorbents are described by applying various kinetic adsorption models. (2007). A maximum removal of 87% of the dye was observed at pH 4. The experimental data were verified by fitting into both Freundlich and Langmuir isotherms. which was pyrolyzed and treated chemically with a 50% zinc chloride solution. Tree fern is naturally and commercially available in all over the world. after cutting off the “fruit bunch. pH. The effect of solution temperature and the determination of the thermodynamic parameters of adsorption of RB on AILP enthalpy of activation. The sorption of methylene blue onto untreated guava leaf powder has been studied by Ponnusami et al. 1981.0 g of leaf. The negative value of the enthalpy change suggested that the rise in the solution temperature did not favor RB adsorption onto AILP (Bhattacharyya and Sharma 2004). the standard Merck-activated carbon capacities were 200 mg g−1 for MB and 950 mg g−1 for iodine. and contact time as the working variables. temperature. This variety of tree fern is generally marketed for horticultural purposes because of its character of adsorbability to retain water and manure for plants. Orange peel is also tested as an adsorbent by Arami et al. on the adsorption rates are important in understanding the adsorption mechanism. Hence. Consequently. the process was found to be exothermic accompanied by a decrease in entropy and increase in Gibbs energy as the temperature of adsorption was increased from 303 to 333 K.72 and 21. Ofomaja 2007. acids. The natural plant adsorption capacities were respectively 23 and 272 mg g−1 for methylene blue and iodine. 2006). chemically treated and activated at 650◦ C.0. the burnoff. respectively. indicating that sorption process to be complex. and an intra-particle diffusion model were tested. and they come to the conclusion that a mayor adsorption capacity of the non-carbonized adsorbent in comparison with carbonized samples is due to the greater amount of surface acidic groups. the mass transfer is the main rate controlling parameter. indicating that the dye uptake is chemisorption. intra-particle diffusion becomes rate controlling. The pseudo-second-order kinetic model was found to better fit the experimental data with high correlation and coefficients at the various fiber dose used. (2007). at high sorbent dose. The activation temperature and time tested were in the ranges 750–900◦ C and 1–4 h. the micropore ratio. for the sorption of MB from aqueous solution and the possible mechanism of sorption has been investigated by Ofomaja (2008b). etching and swelling being the main reactions. The .57 kJ mol−1 . However. and lack of fit have been employed to determine the significance of each coefficient that appeared in the model. The pseudo-second-order rate constant has been correlated as a function of the system variables. The experimental results indicated that the prepared activated carbons were economically promising for adsorption removal of dyes and phenol.Environ Monit Assess (2011) 183:151–195 solution temperature. in contrast to the other commercial adsorbents. a pseudo-second-order. Adsorption isotherms of two commercial dyes and phenol from water on such activated carbons were measured at 30◦ C. Analysis of the kinetic data at different sorbent dose revealed that the pseudo-first-order kinetics fitted to the kinetic data only in the first 5 min of sorption and then deviated from the experimental data. The extent of dye removal and the rate of sorption were analyzed using two kinetic rate models (pseudo-first and pseudosecond-order kinetic models) and two diffusion models (intra-particle and external mass transfer models). namely elemental analysis and temperature programmed desorption. It was shown that the adsorption of both phenols could be fitted to a pseudo-second-order rate law and that of both dyes could be fitted to an intra-particle diffusion model. The kinetics and mechanism of adsorption of two commercial dyes basic red 22 and acid blue 2. the total pore volume. Kinetic parameters were calculated and correlated with the physical properties of the adsorbents. (1999) reported some results of plum kernels on MB. It was found that the change in hydrogen ion concentration and increase in sorption temperature were directly related to the amount of dye sorbed. and activation energy was calculated to be −39. The results revealed a two-stage activation process: Stage 1 activated carbons were obtained at NaOH/char ratios of 0–1. and specific area was from 1478 to 1887 m2 g−1 . It was found that at low sorbent dose. involving valence forces through sharing or exchange of electrons 169 between sorbent and sorbate as covalent forces. Plant f iber The use of Palm kernel fiber. phenol. and application of adsorbents prepared from avocado kernel seeds were discussed by Elizalde-González et al. and 3-chlorophenol from water on activated carbons were studied at 30◦ C by Juang et al. The development. the pore diameter. Wu et al. Stage 2 activated carbons were obtained at NaOH/char ratios of 2–4. characterization. a readily available agricultural waste product. Statistical tools like Student’s t test. surface pyrolysis being the main reaction. F test. and the scanning electron microscope (SEM) observations as well as the chemical properties. Three simplified kinetic models including a pseudo-first-order. and adsorbent dosage have been studied. Model adequacy has been checked by residual distribution. The proposed model explains 95.1% of the total variation in the response. The intra-particle diffusion and mass transfer rate constants were observed to be well correlated with sorbent dose in the first 5 min of sorption. Tseng (2007) reported that activated carbon was prepared from plum kernels by NaOH activation at six different NaOH/char ratios. (2000). ANOVA. The physical properties of stage 2 activated carbons were similar. The dye sorption was confirmed to follow the pseudo-second-order model by investigating the relationship between the amount of dye sorbed and the change in hydrogen ion concentration of the dye solution and also the dependence of dye uptake with solution temperature. were measured. The physical properties including the BET surface area. The max- Environ Monit Assess (2011) 183:151–195 imum adsorption capacity has been calculated to be 35.66 × 10−4 cm2 s−1 . In both cases. temperature. (2008) reported that spruce wood shavings from Picea abies were used for an adsorptive removal of both basic as well as acid dyes from waters. The sorption of acid dye. The treatment of the wood sorbents with alkaline carbonate solution as well as with phosphate solution increased the sorption ability for the basic dye (MB). Various thermodynamic parameters such as enthalpy of sorption H o . Kinetic results suggest the intra-particle diffusion of dyes as rate limiting step. and the equilibrium data were found to be well represented by Langmuir isotherm equation. on the other hand. 45170) from aqueous solutions demonstrated by Panda et al. Analysis of sorption data using Boyd plot confirms that the external mass transfer is the rate limiting step in the sorption process. adsorbent dosage. Equilibrium data were fitted to Freundlich and Langmuir isotherm equation. The pH of the adsorbent . activated carbons prepared by NaOH activation were evaluated in terms of their physical properties. The sorption kinetics was found to follow pseudo-first-order kinetics model. and pH.857 mg g−1 at 303 K. 22120) and RB (C. Tea waste The potentiality of tea waste for the adsorptive removal of MB. and entropy So were estimated. and the activated carbon plum kernel was found to have most application potential. Three kinds of dyes (MB. The MB uptake process was found to be controlled by both surface and pore diffusion with surface diffusion at the earlier stages. and contact time have been varied to study the adsorption phenomenon. from aqueous solution was reported by Uddin et al. (2008).7 and 87. the variations in the surface functional groups and the physical properties. followed by pore diffusion at later stages. and O in the activated carbon. Wood shaving Janoš et al. The maximum sorption capacities estimated from the Langmuir–Freundlich isotherms ranged from 0. chemical properties. Favorable adsorption occurs at around pH 7.170 results of reaction mechanism of NaOH activation revealed that it was apparently because of the loss ratio of elements C.I. and AB74) were used for an isotherm equilibrium adsorption study. solution pH. initial MB concentration. The operating variables studied were the initial solution pH. The nature of the functional groups of adsorbent and their corresponding frequencies are shown by FTIR spectra. whereas temperature has no significant effect on adsorption of both the dyes.060 to 0. Jute stick powder has been found to be a promising material for adsorptive removal of CR (C. adsorption occurs very fast initially and attains equilibrium within 60 min. whereas the treatment with mineral acid decreased the sorption ability for MB to some extent.045 to 0. In this work. and contact time. Kumar and Kumrana (2005) in one of their papers reported the sorption of MB onto mango seed kernel particles. adsorbent mass. The basic dye sorption decreased at low pH values in accordance with a presupposed ionexchange mechanism of the sorption. and Na2 HPO4 . The sorption properties of the sorbents were modified by treating with HCl. Batch kinetics and isotherm studies were carried out under varying experimental conditions of contact time. a cationic dye. H. free energy change Go . The positive value of H o and negative values of Go show that the sorption process is endothermic and spontaneous.513 mmol g−1 for Egacid Orange. (2008). Similar kind of study has also been reported by Ho and McKay (1998a).0.165 mmol g−1 for MB and from 0. Na2 CO3 . The presence of inorganic salts as well as surfactants exhibited only minor effects on the dye sorption. BB1. initial dye concentration. decreased with increasing pH. The adsorption process is in conformity with Freundlich and Langmuir isotherms for RB whereas CR adsorption fits well to Langmuir isotherm only. respectively. The average effective diffusion coefficiency was calculated and found to be 5. The opposite is true for the sorption of the acid dye— Egacid Orange. Physiochemical parameters like dye concentration. The monolayer sorption capacity of mango seed kernel for MB sorption was found to be 142.7 mg g−1 of the biomass for CR and RB. The data fitted well to the Langmuir isotherm equation. temperature.I. and adsorption type. Experimental results showed that pyrolysis and activation conditions leading to various final average temperatures had significant effects on the properties of activated carbons prepared. different adsorbent dose. Sawdust was modified by reacting with cross-linked polyethylenimine (CPEI) to create aminated adsorbent. This material is produced from cutting with a saw. Similar results are also studied by Ferrero (2007). (1997) studied the factors affecting preparation of wood sawdust and used the obtained adsorbents for the removal of anionic dyestuffs. Malik (2003).9 mg g−1 maximum adsorption capacity was found. The most effective of color removal was optimum at pH 7 and the percentage removal increased with the increase in carbon dose while the percentage removal decreased with the increase in initial dye concentration. Ibrahim et al. The sorption was analyzed using pseudo-first-order and pseudo-second-order kinetics models. pyrolysis and physical activation. Methylene blue adsorption was tested and 90. Experiments were conducted 171 at different pH. and Özacar and Sengil (2003). and an activation pilot plant. FTIR characterization indicated that pyrolysis and activation temperatures affected the surface functional groups.Environ Monit Assess (2011) 183:151–195 was estimated by titration method and a value of 4. Oil palm wood Activated carbons were prepared from the biomass of oil palm wood via two stages. and SEM showed that these activated carbons possessed intricate pore network comprising micropores and narrow mesopores. since the CPEI introduced positive sorptive sites in the form of reactive amino groups onto the wood material. Higher adsorption percentages were observed at lower concentrations of methylene blue. Tea waste appears as a very prospective adsorbent for the removal of methylene blue from aqueous solution. and different contact time. N2 adsorption isotherm. The filtrate was collected. The extent of the dye (milligrams per gram) removal increased with increasing initial dye concentration. . for the removal of methylene blue dye from simulated wastewater. The adsorption of methylene blue followed a firstorder rate equation and fit the Lagergren equation well. thus improving the sawdust reactivity and anionic dye uptake.16 mg g−1 . Activated carbon prepared from low-cost palm oil fiber has been utilized as the adsorbent for the removal of basic dye. hence its name. and maximum methylene blue adsorption was dependent on BET surface area.2 was obtained. The latter uses the outlet flue gases from limestone calcination process as activating agents. and its concentration was determined with a UV spectrophotometer. Adsorption equilibrium of tea waste reached within 5 h for MB concentrations of 20–50 mg L−1 . The high micropore fraction. In another case. Optimum pH value for dye adsorption was determined as 7. (2005). (2004) investigates the potential use of Indian Rosewood (Dalbergia sissoo) sawdust. which is several folds higher than the adsorption capacity of a number of recently studied in the literature potential adsorbents.3 ± 0. methylene blue is studied by Darus et al. different initial concentration of dye. The results indicated that palm oil fiber could be employed as low cost alternatives to commercially activated carbon in wastewater treatment for dye removal. The adsorption equilibrium for color reached at 90 min of contact time. pretreated with formaldehyde and sulfuric acid. The adsorption capacities of plant waste were summarized in Table 3. it was studied by Ahmad et al. (2007). Garg et al. Maximum dye was sequestered within 30 min after the beginning for every experiment. The adsorption capacity of MB onto tea waste was found to be as high as 85. The equilibrium data in aqueous solutions were well represented by the Langmuir isotherm model. Modified sawdust was added to acidic dye (pH 3. An adsorption–desorption study was carried out resulting the mechanism of adsorption was reversible and ion exchange. and the sorption kinetics was found to follow a pseudosecond-order kinetics model.0) and shook for 30 min at 25◦ C.0 for both the adsorbents. Sawdust Sawdust is composed of fine particles of wood. The results showed that modification with CPEI increased the adsorptivity of the sawdust. using an environment friendly pyrolysis pilot plant. 02 mg g−1 23.4 7. (2007) Elizalde-González et al.19 mg g−1 183.0 4. (2007) Elizalde-González et al.00 μmol g−1 211.2 25.0 7.10 mg g−1 130.0 7.pitch pine Sawdust carbon Pine sawdust (raw) Pine sawdust (raw) Avocado kernel seeds .20 mg g−1 125.60 mg g−1 Malachite green Malachite green Basic blue 69 Acid blue 25 Methtlene blue Methylene violet Remazol BB Remazol red Remazol black B Methylene blue Red basic 22 Methylene blue Red basic 22 Brilliant green 7. (2008) Bhattacharyya and Sharma (2004) Bestani et al.78 mg g−1 20.AGAP1 Avocado kernel seeds .0 7.0 5.AGAP Avocado kernel seeds .00 mg g−1 59.40 mg g−1 Wood shaving – untreated Wood shaving – HCl treated Wood shaving – Na2 CO3 treated Wood shaving – NaHPO4 treated Wood shaving – untreated Wood shaving – HCl treated Wood shaving – Na2 CO3 treated Wood shaving – NaHPO4 treated Saw dust Methylene blue Methylene blue Methylene blue Methylene blue Egacid orange Egacid orange Egacid orange Egacid orange Methylene blue pH Adsorption capacity References Sarma et al.80 mg g−1 3. (2000) Nigam et al.0 mg g−1 49.0 3.0 27.80 mg g−1 398.AGAP-P-800 Avocado kernel seeds AGAP-P-N-800 Sawdust (Formaldehyde treated) Sawdust (Sulphuric acid treated) Wood Wood Mansonia wood Sawdust Eucalyptus bark Wood chips Wood chips Beech sawdust (CaCl2 treated) Beech sawdust (CaCl2 treated) Beech sawdust (original) Beech sawdust (original) Neem leaf powder Rhodamine B 7. (2008) Garg et al.0 7.70 mg g−1 77.30 mg g−1 Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Congo red Rhodamine B Basic red 13 Acid blue 25 Acid blue 25 Acid blue 25 Acid blue 25 Acid yellow 36 Acid yellow 132 Acid blue 256 Basic blue 41 Basic blue 41 Basic blue 41 Basic blue 41 Basic blue 41 Basic blue 41 6.44 mg g−1 21.0 7.5 7. (2008) Janoš et al.10 mg g−1 2.00 μmol g−1 36.0 7.1 8.0 7.14 mg g−1 33. (2008) Janoš et al. (2008) Ponnusami et al.00 mg g−1 95.0 55.60 mg g−1 43. (2008) Panda et al. (2008) Janoš et al.3 7.00 μmol g−1 33.0 11.98 mg g−1 31.0 5. (2008) Ahmad et al.0 3.70 mg g−1 408.0 7.0 7.00 μmol g−1 39.90 mg g−1 35. (2003) Garg et al.0 5.10 mg g−1 85.0 7.00 μmol g−1 91. (2008) Janoš et al.00 mg g−1 6.0 9.oak Saw dust.0 7.85 mg g−1 26. (2004) .40 mg g−1 67. (2000) Batzias and Sidiras (2004) Batzias and Sidiras (2004) Batzias and Sidiras (2004) Batzias and Sidiras (2004) Bhattacharyya and Sharma (2003) Janoš et al.0 5.7 128.AGAP800 Avocado kernel seeds .0 11. (2008) Janoš et al.0 11. (2008) Ho et al.0 5.0 7.2 7.172 Environ Monit Assess (2011) 183:151–195 Table 3 Reviewed results representing the adsorption capacity of plants waste for the adsorption of dyes and their optimized pH values for maximum adsorption Adsorbent Dye Azadirachta indica (neem) leaf powder Azadirachta indica (neem) leaf powder Activated desert plant Guava leaf powder Tea waste Oil palm wood Oil palm wood Palm kernel fiber Mango seed kernel Jute stick powder Jute stick powder Tree fern Saw dust-Walnut Saw dust.30 mg g−1 86.96 mg g−1 142.0 2. (2007) Garg et al.00 μmol g−1 184.30 mg g−1 13.00 μmol g−1 62. (1999) Nigam et al. (2008) Janoš et al.65 mg g−1 34.0 7.70 mg g−1 87.0 7.98 mg g−1 27.55 mmol g−1 5.90 mg g−1 25. (2008) Uddin et al.0 7.20 mg g−1 0.0 11.0 23.0 10.00 mg g−1 36.0 7.90 mg g−1 9.0 5.0 10.0 7.0 7.16 mg g−1 90.cherry Saw dust. (2007) Elizalde-González et al.00 μmol g−1 111.0 5.5 3.0 7. (2007) Darus et al.30 mg g−1 72. (2008) Janoš et al. (2007) Elizalde-González et al. (2003) Ho and McKay (1998a) Ho and McKay (1998a) Ofomaja (2008a) Ofomaja (2008a) Morais et al. (2005b) Ferrero (2007) Ferrero (2007) Ferrero (2007) Ferrero (2007) Malik (2003) Özacar and Sengil ¸ (2005) Özacar and Sengil ¸ (2005) Elizalde-González et al.AGAP1000 Avocado kernel seeds . (2007) Elizalde-González et al. (2005) Ofomaja (2008b) Kumar and Kumrana (2005) Panda et al.80 mg g−1 280.80 mg g−1 Congo red 6. (2000) investigated the hydrophobic effect on the adsorption of rhodamine 3B dye on laponite particles. It was found that the pseudo-second-order mechanism is predominant and the overall rate of the dye adsorption process appears to be controlled by the more than one step. Sepiolite Sepiolite has been tested as an adsorbent by many researchers (Ozdemir et al. respectively. 2003. Orthman et al. and removal of organic dyes from aqueous solutions. They are classified on the basis of layered structures. microporous. The results showed that the adsorption has been reached the equilibrium in 1 h. the ability to develop internal acidity. hectorite.Environ Monit Assess (2011) 183:151–195 Natural inorganic materials Most recently. Adsorption capacity decreases with increasing pH. Alkan et al. 2004. activated clays by acid treatment or calcinations. and intra-particle diffusion processes thus comparing chemical sorption and diffusion sorption processes. Tahir and Rauf 2006) and needlelike structure (Ozdemir et al. The development perspectives are also proposed. (1998. Clay Clay material possesses a layered structure and is considered to be host material. methylene blue. In order to understand the adsorption mechanism 173 in detail. Clay minerals exhibit a strong affinity for both heteroatomic cationic and anionic dyes (Table 4). kalonite. zeolites are three dimensional. Sepiolite is a natural hydrated magnesium . and molecules based on size. and the high internal surface area along with their ability to absorb molecules/ionic species in to their structure give rise to great variety of applications which makes zeolites special when compared with other inorganic materials (Davis 2002). 2002a. the thermal stability. pH. Furthermore. the regeneration of these low-cost substitutes is not necessary whereas regeneration of activated carbon is essential because of the abundant resources. For zeolite. 2007. 2002b) and Chaudhuri et al. and they also provide highly specific surface area (Zhao and Liu 2008). pseudosecond-order sorption. their unique properties such as the existence of high intra-crystalline surface area. (2006). Arbeloa et al. shape. 2006. Porosity and BET surface area of clay studied were determined. zeta potentials and the conductivities of clay suspensions at various pH (1–11) and cation exchange capacity were measured. Liu and Guo 2006. crystalline solids with well-defined structures that can absorb dyes with a capacity of up to more than 25% of their weight in water. except for the natural pH (5. and montmorillonite in aqueous suspensions with electronic absorption and fluorescence spectroscopies. polarity. and sepiolite (Shichi and Takagi 2000). They separate ions. Gürses et al. On the other hand. Li et al. Clays are natural environment-friendly materials with high specific surface area are now widely used for the adsorption and removal of the organic pollutants. temperature. complex ions. Liu and Zhang (2007) have reviewed the adsorption properties of the raw clays. and sorbent dosage in this study. serpentine. 2004). vermiculite. the ion exchange properties. McKay et al. the clay minerals and zeolites were reported to be unconventional adsorbents for the removal of dyes from aqueous solutions due to their cheap and abundant resources. higher surface areas (Liu and Zhang 2007). mixing rate. It was found that the amount adsorbed of methylene blue increases with decreasing temperature and also with increasing both sorbent dosage and increasing initial dye concentration. 2007) have been increasingly gaining attention because they are cheaper than activated carbons. (2001) and Gürses et al. There are several classes of clays such as smectites. Huang et al. the microporous/mesoporous character of the uniform pore dimensions. Sepiolite. (2006) investigated adsorption kinetics of a cationic dye.6) of clay suspensions. Clay materials with sheet-like structures (Arbeloa et al. and degree of unsaturation. may be a good alternative to these systems. as an adsorbent. Similar results are also investigated by Ho et al. organic-modified clays with small molecules or polymers for the adsorption. (1985) reported the adsorption capacity of fuller’s earth for basic and acid blue to be 220 and 120 mg g−1 . The adsorption kinetics of methylene blue has been studied in terms of pseudo-first-order. onto clay from aqueous solution with respect to the initial dye concentration. 7 6.0 7.0 7.4 × 10−5 mol g−1 156. (1985) Ho et al. (2004) Wang et al.6 5.0 11.59 mg g−1 8. (2004) McKay et al.2 9.0 3.10 mg g−1 120.05 mg g−1 3. (2003) Walker et al.99 mg g−1 15. (2004) Wang et al.0 11. (2001) .0 2.50 mg g−1 8.0 7.7 6. (2004) Ozdemir et al.174 Environ Monit Assess (2011) 183:151–195 Table 4 Reviewed results representing the adsorption capacity of naturally available inorganic minerals for the adsorption of dyes and their optimized pH values for maximum adsorption Adsorbent Dye pH Adsorption capacity References Clay Clay Clay Clay Clay Clay Clay Sepiolite Sepiolite Sepiolite Sepiolite Sepiolite Sepiolite Am-SiO2 Red mud Spent activated clay Zeolite Zeolite Zeolite Zeolite Zeolite Zeolite Perlite Perlite Ca – Montmorillonite Ca . (2004) Ozdemir et al.0 7.49 mg g−1 170.0 4.2 × 10−3 mmol g−1 13. (2005) Woolard et al. (2004) Alkan et al.1 × 10−6 mol g−1 1.0 3. (1995) Ozdemir et al.Montmorillonite Ti – Montmorillonite Glass powder Raw kaolin Pure kaolin Calcined raw kaolin Calcined pure kaolin NaOH treated raw kaolin NaOH treated pure kaolin Calcined alunite Calcined alunite Calcined alunite Fuller’s earth 1 Fuller’s earth 2 Fuller’s earth 3 Fuller’s earth 4 Balkaya lignite Diatomaceous clay Clay Halloysite nanotubes Dolomite Charred dolomite Fly ash Red mud Kaolinite Methylene blue Basic blue 69 Acid blue 25 Acid blue 9 Basic red 18 Basic blue 69 Basic red 22 Reactive red 239 Reactive yellow 176 Reactive black 5 Reactive blue 221 Acid blue 62 Methylene blue Methylene blue Congo red Methylene blue Reactive black 5 Reactive red 239 Reactive yellow 176 Methylene blue Methylene blue Alizarin sulphonate Methylene blue Methyl violet Basic green 5 Basic violet 10 Basic green 5 Basic violet 10 Carminic acid Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Reactive blue 114 Reactive yellow 64 Reactive red 124 Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Brilliant red Brilliant red Methylene blue Methylene blue Safranin . (2001) Ho et al. (1985) McKay et al. (2004) Dogan ˘ and Alkan (2003) Dogan Wang et al.00 mg g−1 110.90 mg g−1 170.55 mg g−1 7.30 mg g−1 414.00 mg g−1 220.00 mg g−1 585.0 7. (2004) Ozdemir et al.11 × 10−4 mol g−1 6.0 4. (2004) Atun and Hisarli (2003) Ghosh and Bhattacharyya (2002) Ghosh and Bhattacharyya (2002) Ghosh and Bhattacharyya (2002) Ghosh and Bhattacharyya (2002) Ghosh and Bhattacharyya (2002) Ghosh and Bhattacharyya (2002) Özacar and Sengil (2003) Özacar and Sengil (2003) Özacar and Sengil (2003) Atun et al.80 mg g−1 157.13 mmol kg−1 9. (2002) Zhao and Liu (2008) Walker et al.80 mg g−1 169.0 9.0 7. (1995) El-Guendi et al. (2002) Namasivayam and Arasi (1997) Weng and Pan (2007) Ozdemir et al.00 mg g−1 4.0 4.86 mmol kg−1 4.2 5.045 mmolg−1 33.41 × 10−4 mol g−1 60.0 5. (2002) ˘ et al.0 7.50 mg g−1 0.0 8.0 8.10 mg g−1 88.0 7.40 mg g−1 108.0 7. (2003) Karaca et al.0 4.0 10.45 μmol m−2 Gürses et al. (2004) Ozdemir et al.0 7.50 mg g−1 111.0 7. (2005) Wang et al. (2005) Harris et al.15 meq g−1 84.50 mg g−1 55.0 4.0 7.0 11.Montmorillonite Ti . (2001) El-Guendi et al.30 mg g−1 1200.34 mg g−1 20.0 5.00 mg g−1 1.2 × 10−4 mmol g−1 0.0 7.70 mg g−1 236.48 × 10−4 mol g−1 6.83 mmol kg−1 7. (2003) Atun et al.0 6.00 mg g−1 488.0 2.0 11.0 11. (2007) Dogan Woolard et al.0 11.0 7.00 mg g−1 4.34 × 10−4 mol g−1 40.0 11.0 4.0 7.0 10.0 7. (2003) Wang et al. (2003) Atun et al. (2005) ˘ et al.32 mg g−1 900. (2004) Shawabkeh and Tutunji (2003) Neumann et al. (2003) Atun et al.9 × 10−4 mol g−1 1.50 mg g−1 961. (2005) Alkan et al.0 10.O 7.2 6.00 × 10−4 mol g−1 6. (2004) Wang et al.00 mg g−1 153. (2004) Wang et al.00 mg g−1 57.87 × 10−4 mol g−1 70.0 7.4 × 10−5 mol g−1 7.0 7.9 × 10−4 mol g−1 32.88 mg g−1 16.0 7. (2002) Woolard et al.8 × 10−6 mol g−1 10. 00 mg g−1 0.00 mg g−1 0. (2001) Harris et al. (2006) Özacar and Sengil (2006) Karim et al.16 mg g−1 0.64 mol g−1 11.80 μmol m−2 1. (2009) Bukallah et al.12 mmol g−1 106. (2001) Harris et al.65 mmol g−1 1.0 7.60 mg g−1 7.0 10.A 3.0 4. (2009) Karadag et al.0 7.50 mg g−1 274.02 μmol m−2 1.6-diamino acridine 9-amino acridine Safranin .85 μmol m−2 0.40 μmol m−2 0.2 9.02 mg g−1 10.5 1.0 6. (2007) Eren (2009) Eren (2009) Demirbas and Nas (2009) Demirbas and Nas (2009) Qiu et al. (2001) Harris et al.9 7.32 mmol g−1 1.6-diamino acridine 9-amino acridine Methylene blue SELLA FAST Brown H Acid blue 29 2 nitrophenol 2 chlorophenol 2 nitrophenol 2 chlorophenol Acid blue 193 Acid blue 193 Basic red 2 Basic blue 9 Basic red 46 Methylene blue Crystal violet Crystal violet Reactive Blue 21 Reactive Blue 21 Amido Black 10B Safranine T Basic red 46 Reactive yellow 176 Reactive yellow 176 Methylene blue Congo red Methylene blue Methylene blue Methylene blue Methylene blue Methylene blue Everzol black B Everzol red 3BS Everzol yellow 3RS H/C Malachite green Basic blue 3 Methylene blue Acid red 57 Methyl violet pH 9.13 μg g−1 11. (2004) Armagan ˘ et al. (2003) Navarro et al.06 mmol g−1 2.0 7. (2003) Espantaleón et al.15 mmol g−1 0.54 mg g−1 13.00 mg g−1 1667.6 Adsorption capacity m−2 8. (2007) Dogan . (2001) Harris et al.0 7.0 1.20 μg g−1 8.O Azure .15 μmol m−2 0. (2004) Armagan ˘ et al. (2001) Harris et al.2 9.34 μmol m−2 0.0 8. (2007) Karadag et al. (2007) Karadag et al. (2008b) Kahr and Madsen (1995) Kahr and Madsen (1995) Kahr and Madsen (1995) Kahr and Madsen (1995) Kahr and Madsen (1995) ˘ et al.0 4.80 μmol 7.62 mg g−1 0. (2009) Özcan et al. (2001) Al-Ghouti et al. (2003) Orthman et al.O Azure .0 7. (2001) Harris et al.70 μmol m−2 0.15 mg g−1 33.0 7.0 7.00 mg g−1 18.2 9.0 7.A 3.90 mg g−1 3. (2007) Alkan et al.2 9. (2009) Navarro et al.2 9.0 10.40 μmol m−2 0.0 7. (2009) Navarro et al.2 9.0 7.Environ Monit Assess (2011) 183:151–195 175 Table 4 (continued) Adsorbent Kaolinite Kaolinite Kaolinite QAL alumina QAL alumina QAL alumina QAL alumina Gibbsite Gibbsite Gibbsite Gibbsite Silica Silica Silica Silica Diatomaceous earth Activated bentonite Anion clay hydrotalcite Bentonite – HDMTA Bentonite – HDMTA Bentonite – BTEA Bentonite – BTEA Bentonite – Na Bentonite – DTMA Bentonite Bentonite Crude clay Sand Raw bentonite Modified bentonite Fly ash Sepiolite Clinoptilolite Clinoptilolite Natural zeolite Modified zeolite – CTAB Modified zeolite – HDTMA Bentonite Anilinepropylsilica xerogel Na-Bentonite Ca-Bentonite Arizona Illite Kaolinite Zeolite Zeolite Zeolite Bentonite Silica Sand Sepiolite Sepiolite Dye Azure .71 mg g−1 66.2 9.67 mg g−1 55.2 9.0 7.2 9.6-diamino acridine 9-amino acridine Safranin .0 7.95 mg g−1 23.0 7.0 7. (2004) Armagan Tahir and Rauf (2006) Ahmed and Ram (1992) Bukallah et al.0 7. (2001) Harris et al.04 mg g−1 67.0 7.00 mg g−1 22. (2001) Harris et al.A 3.75 mmol g−1 0.0 2.A 3.0 7.2 9.6-diamino acridine 9-amino acridine Safranin . (2001) Harris et al. (2001) Harris et al.90 μmol m−2 0.36 mg g−1 34.0 6.2 9.45 μmol m−2 0. (2001) Harris et al.40 μmol m−2 198.2 9.56 mg g−1 5.10 mg g−1 740. (2004) Hu et al.99 μmol g−1 1. (2009) Navarro et al.0 7. (2009) Qiu et al.0 2.5 7.00 mg g−1 54.9 9.72 mg g−1 11.18 μmol m−2 4.64 mol g−1 0.25 mmol g−1 0.2 11. (2001) Harris et al. (2007) Al-Bastaki and Banat (2004) Pavan et al.0 7. (2004) ˘ et al.55 μmol m−2 0.0 7.64 mg g−1 9.2 9. (2001) Harris et al.88 μmol m−2 1.0 7.2 9. (2001) Harris et al.70 mg g−1 7.76 × 10−4 mol g−1 References Harris et al. (2004) Özcan et al.O Azure . 2001).5 is favorable for the adsorption of Acid Blue 193. AB193) removal from aqueous solution in comparison to Na–bentonite. ionic strength. Effects of feed concentration. The sepiolite sample calcinated at 200◦ C has the maximum adsorption capacity. stirring speed. Several studies have been conducted on the sorbent behavior of natural ze˘ et al. (2004) prepared Dodecyltrimethylammonium bromide-modified bentonite (DTMA– bentonite) and tested it as an adsorbent for an acid dye (Acid Blue 193. Also. Quasiequilibrium reached within 3 h. Kinetic study showed that the adsorption of dyes on sepiolite was a gradual process.1 mg g−1 ) at 20◦ C. Zeolites are easily synthesized from industrial wastes such as coal fly ash and paper sludge ash. (2005) using parameters such as calcination temperature. Permeate flux increased linearly with increasing pressure while the permeate concentration remained almost constant (Kahr and Madsen 1995). The adsorption of acid red 57 by natural mesoporous sepiolite has been examined by Alkan et al. 8H2 O Structurally. the specific surface area of sepiolite decreased with increasing calcination temperature.e. Ozcan et al. Hu et al. The results obtained in this study revealed that such a combined process could beneficially be used for the treatment of dye effluents. bentonite dose. and temperature. The isothermal data could be well described by the Freundlich equation.05 g of bentonite at a pH of 9. are efficient adsorbents for positively charged pollutants such as heavy metals. The addition of bentonite significantly increased the rejection coefficient of MB but decreased the permeate flux. feed temperature. Zeolites (Dabrowski 2001) are the only existing crystalline materials with a well-defined pore structure in the microporous range. Bentonite Bentonite is an absorbent aluminum phyllosilicate. generally impure clay consisting mostly of montmorillonite. The suitability Environ Monit Assess (2011) 183:151–195 of such a combined process for the removal of color caused by MB dye was investigated (Al-Bastaki and Banat 2004. Özacar and Sengil 2006. Combining both processes in a one-step treatment process can achieve both goals concurrently. pH. Each structural block is composed of two tetrahedral silica sheets and a central octahedral sheet containing magnesium. However. Sepiolite was used as an adsorbent for the removal of methyl violet and MB from aqueous solutions by ˘ Dogan et al.176 silicate clay mineral. i. (Si12 )(Mg8 )O30 (OH6 )– (OH2 )4. Bentonite can be used to adsorb dyes and UF can be used to purify wastewaters from colloidal matters. and temperature for the removal of these dyes. Zeolites. Adsorption rate increased with the increase in ionic strength. Tahir and Rauf (2006) reported that the maximum adsorption of the dye. ionic strength. The dynamical data fit well with the pseudo-second-order kinetic model. Combining ultrafiltration (UF) and adsorption is an advance technique for the treatment of colored wastes proposed by researchers. Results of this study show that a pH value of 1. The adsorption capacity of DTMA–bentonite (740. (2004) in order to measure the ability of this mineral to remove colored textile dyes from wastewater. >90% has been achieved in aqueous solutions using 0. The rate of adsorption was investigated under various parameters such as contact time. pH. Zeolites Zeolites are microporous. The removal of reactive blue 221 and acid blue 62 anionic dyes onto sepiolite from aqueous solutions has been investigated by Alkan et al. calcination at higher temperature caused a decrease in the amount adsorbed of dye. and operating pressure on the permeate flux and color removal were investigated. Karcher et al. After 200◦ C calcination temperature. The amount adsorbed of reactive blue 221 and acid blue 62 on sepiolite increased with the increased ionic strength and temperature and decreasing pH. (2007). with their permanent negative charges as well as the interconnection of channels and cages that run through their secondary framework structure. aluminosilicate minerals commonly used as commercial adsorbents.5 mg g−1 ) was found to be around 11 times higher than that of Na–bentonite (67. 2006). and temperature. 2004. it is formed by blocks and channels extending in the fiber direction. pH. olites (Armagan . the cuticles of insects. Recent fundamental work has revealed the existence of a wide variety of microorganisms capable of decolorizing an equally wide range of dyes. The aromatic amine is then subjected to further metabolism by algae. These decolorizations were permanent with no color change upon exposure to air: Only one dye. has been carried out by Chatterjee et al. (1996) in his research paper. a number of aerobic and anaerobic cultures able to decolorize dyes in textile effluent samples were isolated after a prolonged enrichment of the culture from textile dye-effluent samples. and the cell walls of fungi. In this review. and Remazol Red (diazo dye) completely within 24– 30 h fermentation process. and yellow 176 onto modified zeolite. One of the cultures decolorized Cibacron Red (reactive dye). The decolorization of some component dyes of the effluent and of a mixture of dyes was achieved under anaerobic conditions. (2007). and they made the following outcomes. Both ionic interaction and physical forces are responsible for binding of congo red with chitosan. Modification of zeolite (clinoptilolite) surface with a quaternary amine. had been made to improve the removal efficiency of reactive azo dyes. was partially reversibly decolorized. The azo reduclase of algae is responsible for degrading azo dyes into aromatic amine by breaking the azo linkage. Chitin and chitosan Chitin is a natural polysaccharide found particularly in the shells of crustaceans such as crab and shrimp. and Remazol Blue within 54 h. Adsorption process has been found to be dependent on temperature with optimum activity at 30◦ C. Remazol Turquoise Blue (a phthalocynaine dye). respectively. Experimental data obtained at different temperatures for the adsorption of each dyestuff by chitin were applied to pseudo-first-order. Physicochemical investigation on adsorption of congo red. Benkli et al. Bioadsorbent The degradation of azo dyes by algae was evaluated by Jinqi and Houtian (1992). The kinetic results follow pseudo-second-order . (1996). It is the second most abundant polysaccharide after cellulose. Potential applications of the cultures obtained in textile dye stuff effluent decolorization and treatment were discussed. (2005) reported the uptake of three types of reactive dyes i. The ability of microorganisms to carry out dye decolorization has been received by Alhassani et al. Red 239. CI Reactive Black 5. In addition.Environ Monit Assess (2011) 183:151–195 Similar conclusions have been found by Ozdemir et al. and Banat et al. It has gained importance in environmental biotechnology due to its very good adsorption capacity towards dyes (Annadurai et al. The reduction rate appears to be related to the molecular structure of the dyes and the species of algae used. hexadecyl trimethyl ammonium bromide. (2007). A simple and practical biological process for the decolorization of colored effluent from a textile company was described by Nigam et al. 1999) and metal ions. they have also examined biological decolorization of dyes used in textile industries and report on progress and limitations. Remazol Navy Blue (diazo dye) and Cibacron Orange (reactive dye) within 48 h. Microbial decolorization and degradation of dyes has been seen as a costeffective method for removing organic pollutants from the environment. pseudo-second-order. Several 177 bacterial cultures capable of total decolorization of some effluent component dyes under anaerobic liquid fermentation conditions were isolated. and pore diffusion rate constants (k p ) at these temperatures were calculated. (2007). an anionic azo dye by chitosan hydrobeads.e. the adsorption isotherms of each dyestuff by chitin were also determined at different temperatures. (2008). The main difference between chitin and chitosan is that the chitin has two hydroxyl groups while chitosan has one amino group and two hydroxyl groups in the repeating hexosamide residue. the rate constants of second-order adsorption (k2 ). Remazol Golden Yellow (azo dye). and it was found that certain algae can degrade a number of azo dyes to some extent. (2004) and Wang et al. indicating that the bacteria were able to break the chromophoric bonds in the dye molecules. and Webere Morris equations. and the rate constants of first-order adsorption (k1 ). The adsorption of reactive yellow 2 (RY2) and reactive black 5 (RB5) by chitin (Sigma C 9213) was investigated by Akkaya et al. and the rate constants were evaluated. and dye concentration was measured after 10 h. Reactive Yellow 2. In this study. 30◦ C. they made the following conclusions: (a) there are many fungal stains capable of decolorization dye wastewater. and wet/dry beads were investigated. 2000. temperature. (2004) also reported about the adsorption of four reactive dyes Reactive Blue 2. and one direct dye direct Red 81. Reactive Yellow 86. The enhancement of abilities for the removal of reactive dyes and immobilization of tyrosinase onto highly swollen chitosan beads was demonstrated compared to the use of common chitosan flakes by Wu et al.4-dihydroxyphenylalanine from tyrosine and ascorbic acid in the heterogeneous catalytic system. as well as the immobilization of acid phosphatase and glucosidase onto swollen chitosan beads was investigated by Juang et al. Fu and Viraraghavan (2001) in their reviewed results said that they have examine various fungi. Activities and lifetimes of the immobilized enzymes were measured to evaluate the potential of practical applications. The pseudo-firstorder. except for the dry beads fitting better with the first-order model.840 g kg−1 at pH 3. Fungi In the recent years. b). summarize the present pretreatment methods for increasing the biosorption capacity of fungal biomass. From these studies. The desorption data shows that the removal percent of dye RR 189 from the crosslinked chitosan beads is 63% in NaOH solutions at pH 10. Wang and Wang 2007). Reactive Red 2. It is becoming a promising alternative to replace or supplement present treatment processes. Langmuir model agrees very well with experimental data.0.911–2. living or dead cells. The adsorption capacities had very large values of 1.802– 1. Finally.4–15. The sorption of reactive dye RR222. they prepared the chitosan from cuttlefish wastes and cross-linked with different dosages of glutaraldehyde and glyoxal. Acid orange 7. and ethylene glycol diglycidyl ether was used and ECH shows a higher adsorption capacity. which are capable of decolorizing dye wastewaters.0 and 2. (2002b). Wu et al. The kinetics of the adsorption with respect to the initial dye con- Environ Monit Assess (2011) 183:151–195 centration. The ionic cross-linking reagent sodium tripolyphosphate was used to obtain more rigid chitosan beads. 2004. It was shown that the adsorption capacity of dyes at 30◦ C using swollen chitosan beads was around five times greater than that using common chitosan flakes. three acidic dyes Acid Orange 12. To stabilize chitosan in acid solutions.498 g kg−1 at pH 3–4. Acid Red 14.0. The adsorption capacity increases largely with decreasing solution pH or with increasing initial dye concentration. inexpensive medium. there has been an intensive research in fungal decolorization of dye wastewater. and its calculated maximum monolayer adsorption capacity has very large value of 1.178 rate equation.4 times those of the commercially activated carbon and chitin. which was reflected by the higher yield of 3. second-order kinetic models. In another paper Chiou et al. report some elution and regeneration methods for fungal biomass. glutaraldehyde. the capacity of tyrosinase immobilization onto swollen beads was about 14 times greater than chitosan flakes. and intraparticle diffusion model were used to describe the kinetic data. chemical cross-linking reagent epichlorohydrin (ECH). pH. In this study. The adsorption of dyes using swollen beads was faster by 10–40% depending on the types of dyes. ionic strength. discuss various mechanisms involved. respectively. at 30◦ C. . The conclusions drawn from this study was that the amounts of sorption of solutes and the immobilization capacities of enzymes onto the swollen chitosan beads were significantly affected by the degrees of cross-linking. The desorbed chitosan beads can be reused to adsorb the dye and to reach the same capacity as that before desorption. Chitosan was prepared from natural cuttlebone wastes. The dynamical data fit well with the secondorder kinetic model.0. 30◦ C.0 to 12. There is a need to develop these fungal strains which can grow in simple. and discuss the effects of various factors on deccolorization.7–27. Chiou and Li (2003) reported batch study for the adsorption of reactive dye (reactive red 189) from aqueous solutions by cross-linked chitosan beads. Chitosan was also tested as an adsorbent (Wong et al. which were 3. Influence of pH on the adsorption process was studied over a range of 3. (2001a. disperse red. and biosorption. chrysosporium and T. The present study reports preliminary findings on the removal of azo dyes from solutions using white rot basidiomycetes. Remazol Black B. The effluent from the dye house was treated using both organisms with different concentration of glucose (1% and 2%). P. decolorization involving dead biomass is easier to operate. Batch cultures of Bjerkandera sp. and basic orange was 98%. The two species of white rot fungi were evaluated for their ability to decolorize Blue CA. They can be effective biosorbents. 50 and 75 mg L−1 . The use of 2. 76%. Remazol Brilliant Blue. versicolor was found to be the most efficient color removing species for the three dyes investigated. T. and Corazol Violet SR by Sathiya moorthi et al. decoloration. Effective decolorization was found to be more by the P.Environ Monit Assess (2011) 183:151–195 and have high production rate and possesses high biosorption capacity. BOS55 and P. Remazol Orange. Phanerochaete chrysosporium. The laccase activity was measured using both solid and aqueous state assays. However. (2007). versicolor rapidly decolorized repeated additions of the different dyes and dye mixtures without any visual sorption of any dye to the pellets. Bjerkandera sp. (b) decolorization by living cells involves more complex mechanisms such as intracellular. versicolor for acid green. f lorida in 2% glucose. BOS55 pellets decolorized only Amaranth. than by dead cells. In static aqueous culture. The choice of buffer had a profound effect on pH stability upon dye addition and. and Trametes versicolor displayed the greatest extent of decoloration. extracellular oxidases. Coriolus versicolor.e. and Remazol Orange. The ability of four different species of white rot fungi i. Termetomyces sp.. and Tropaeolin O in agar plates. Fu and Viraraghavan (2002a) reported some elution and regeneration methods for fungal biomass and summarize the pretreatment methods for fungal biomass. (2007). and Schizophyllum commune to remove azo dyes from aqueous solutions were evaluated in batch culture under laboratory conditions by Nasreen et al. Reactive Blue. The process involving living cells is closely related to the operational conditions. Maximum decolorization was observed in Blue CA and Corazol Violet SR dyes. Maximum removal capacity of C. chrysosporium had a limited ability to decolorize repeated dye additions. Laccase is the ligneolytic enzyme from these fungi. The effective decolorization of Blue CA and Corazol Violet SR dyes by both microorganisms were observed in the fifth day of incubation. and dead cells may possess higher biosorption capacity in certain conditions. Further decolorization activity was verified using various concentrations of dyes 179 such as 25. further research work is required to study the toxicity of the metabolites of dye degradation and the possible fate of the utilized biomass in order to ensure the development of an eco-friendly technology. the influent concentration. Some bacterial and fungal species have been reported that are capable of biodegradation of dyes. In contrast. Trametes hirsute and Pleurotus f lorida displayed the greatest extent of decolorization. Black B133. Wesenberg et al. Kaushik and Malik (2009) in their study conclude that the fungal decolorization has a great potential to be developed further as a decentralized wastewater treatment technology for small textile or dyeing units. the three cultures formed fungal mats which did not decolorize any dye beyond some mycelial sorption. such as nutrition requirements.29dimethylsuccinic acid allowed for excellent pH control and resulted in high decoloration ability. Preliminary studies indicate that C. the biomass grew as mycelial pellets. versicolor pellets were capable of decolorizing most dyes with decoloration by T. Glucose as the carbon source in growth medium is more suitable for the decoloration of dyes in comparison to starch at the same concentration. versicolor being several times more rapid. Pleurotus ostreatus. (2003) summarize the state-of-the-art in the research and prospective use of white-rot fungi and their enzymes . C. and 61%. versicolor has the potential to remove color from aqueous solutions and may be used as an efficient biological agent for the decoloration of dyes in industrial effluents. BOS55. however. and toxicity. respectively. Swamy and Ramsay (1999) reported five species of white rot fungi for their ability to decolorize Amaranth. When agitated at 200 rpm. consequently. The dye absorption ability of the mycelium was studied using appropriate medium containing dyes at the concentration of 75 mg L−1 . Remazol Black B. Bjerkandera sp. Peat is partially fossilized plant matter. The adsorption of acid dyes. The correlation between theoretical and experimental data had only limited success due to competitive and interactive effects between the dyes and the Environ Monit Assess (2011) 183:151–195 dye–surface interactions. based on the assumption of a pseudosecond-order mechanism has been developed to predict the rate constant of sorption. and old bread. usually of a dark brown color. Sun and Yang (2003) reported the adsorption of Basic Magenta and Basic Brilliant Green onto modified peat–resin particle. The batch sorption process. and Toth isotherm equation. It is formed in poorly oxygenated wetlands. onto peat is reported by Allen et al. arrhizus biomass. Basic Blue 69 and Acid Blue 25. O’Mahony et al. where the rate of accumulation of plant matter is greater than that of decomposition. The potential of using peat in wastewater treatment is reviewed by Couillard (1994) with special attention to the following topics: (1) the properties of peat. Basic yellow 21. and temperature. and Basic red 22. Equilibrium sorption isotherms have been measured for the three single-component systems. (2) the pretreatment of peat. and Redlich–Peterson. both in terms of adsorption capacity and cost (Allen et al. initial dye concentration. and at the initial dye concentration of 800 mg L−1 .180 (lignin-modifying enzymes) for the treatment of industrial effluents particularly dye containing effluents.0. High adsorptive capacities for some basic dyes were found. The adsorption of Telon Blue on peat has been investigated by Poots et al. The biomass exhibited maximum dye uptake at pH 2 due to its . The Redlich–Peterson model also yielded the best fit to experimental data for all three dyes using the nonlinear error functions. Equilibrium was achieved after 21 days. The decolorization and detoxification potential of white-rot fungi can be harnessed thanks to emerging knowledge of the physiology of these organisms as well as of the biocatalysis and stability characteristics of their enzymes. (2004). Viraraghavan and Ayyaswami 1987). decaying fruit and vegetables. Modified peat was prepared by mixing thoroughly raw peat with sulfuric acid. onto peat has been studied by Ho and McKay (1998b) in terms of pseudo-second-order and first-order mechanisms for chemical sorption as well as an intra-particle diffusion mechanism process. The sorption of two dyes.2 mg g−1 of reactive black 5 per g using Rhizopus arrhizus biomass. namely Basic blue 3. remazol orange on R. The sorption of three basic dyes. The experimental isotherm data were analyzed using Langmuir. Freundlich. (2002) also reported the biosorption of three reactive dyes cibacron red. and modified peat–resin particle was obtained. A comparison of the equilibrium sorption capacity evaluated has been made from pseudo-second-order rate constant. Peat compares favorably with other adsorbents such as carbon. The adsorption isotherms are described by means of the Freundlich and Langmuir isotherms. namely. remazol blue. the equilibrium constant and initial sorption rate with the effect of agitation. by mixing modified peat with solutions of polyvinyl alcohol and formaldehyde. and zinc ions is reported. and (4) the applications of peat to the removal of impurities from wastewater. (1976). Peat The suitability of peat as a natural adsorbent is supported by a number of studies which have reported the successful treatment of many different types of effluent. Tempkin. This knowledge will need to be transformed into reliable and robust waste treatment processes. The adsorptive capacity of sphagnum moss peat for a range of adsorbates has been studied by Allen (1987). Activation energy of sorption has also been evaluated with the pseudo-second-order rate constants. at the initial pH value of 2. silica and alumina. Rhizopus Rhizopus is a genus of molds that includes cosmopolitan filamentous fungi found in soil. Aksu and Tezer (2000) demonstrated uptake of 588. (3) the principles involved in the removal of wastewater pollutants by peat. Peat has been widely used in the treatment of wastewaters. An extended Langmuir model has been used to predict the isotherm data for the binary systems using the single component data. 1994. basic dyes. animal feces. The fungal biomass exhibited the highest dye uptake capacity at 35◦ C. 0 3. (2004) Chiou et al. (2000) Waranusantigul et al. quilliermendii) Yeast (C.0 4. (2007) Nasreen et al. (2004) Wong et al. (2004) Chiou et al.93 mg g−1 Wong et al. (2000) Wu et al.0 4.28 mg g−1 17. (2004) Chiou et al.23 mg g−1 1106 mg g−1 293 mg g−1 1037 mg g−1 398 mg g−1 1026 mg g−1 494 mg g−1 144. (2001a) Wu et al. (2000) Wu et al.00 mg g−1 5.0 7.0 7. (2007) Fu and Viraraghavan (2002a) Fu and Viraraghavan (2002a) Ho and McKay (1998b) Ho and McKay (1998b) Sun and Yang (2003) Sun and Yang (2003) O’Mahony et al. (2000) Wu et al.) Yeast (C. (2003) Allen et al.0 mg g−1 154.0 2. (2004) Chiou et al.7 mg g−1 152.0 mg g−1 1009.0 3.59 mg g−1 45. (2009) Navarro et al.0 2.0 7.0 mg g−1 1653.00 mg g−1 76.0 7.0 7. (2001a) .0 9. (2002) O’Mahony et al.0 7. (2004) Chiou et al.0 6.0 4.0 4.0 3.0 7.1 mg g−1 922.96 mg g−1 12.3 mg g−1 225.4 mg g−1 97. (2003) Acid green Disperse red Basic orange Disperse red 1 Acid blue 29 Acid blue 25 Basic blue 69 Basic violet 14 Basic green 4 Reactive blue 19 Reactive orange 16 Reactive red 4 Reactive black 5 Remazol blue Remazol blue Remazol blue Remazol blue Remazol blue Direct blue 1 Direct red 128 Direct blue 1 Direct red 128 2 nitrophenol 2 chlorophenol 2 nitrophenol 2 chlorophenol Basic yellow 21 Basic red 22 Reactive red 222 Reactive blue 222 7. versicolor) White rot Fungi ( C. (2000) Wu et al. versicolor) Modified fungal biomass (Aspergillus niger) Peat Peat Peat Peat Biomass (Rhizopus arrhizus) Biomass (Rhizopus arrhizus) Biomass (Rhizopus arrhizus) Biomass (Rhizopus arrhizus) Yeast (Candida sp.0 7.0 7.0 2.0 7.0 3.1 mg g−1 189.0 mg g−1 101.18 mg g−1 71. (2002) Aksu and Tezer (2000) Aksu and Dönmez (2003) Aksu and Dönmez (2003) Aksu and Dönmez (2003) Aksu and Dönmez (2003) Aksu and Dönmez (2003) ˘ and Arıca (2007) Bayramoglu ˘ and Arıca (2007) Bayramoglu ˘ and Arıca (2007) Bayramoglu ˘ and Arıca (2007) Bayramoglu Navarro et al. utilis) Native white rote fungus (Trametes versicolor) Heat-treated white rote fungus (Trametes versicolor) Macrocystis integrifolia Bory Macrocystis integrifolia Bory Lessonia nigrescens Bory Lessonia nigrescens Bory Kudzu (Peuraria lobata ohwi) Kudzu (Peuraria lobata ohwi) Chitosan swollen bead Chitosan swollen bead Acid green 25 Acid orange 10 Acid orange 12 Acid red 18 Acid orange 12 Acid red 14 Acid orange 7 Direct red 81 Reactive blue 2 Reactive red 2 Reactive yellow 2 Reactive yellow 86 Direct red 28 Reactive red 222 Reactive red 222 Reactive red 222 Reactive red 222 Reactive red 222 Reactive red 222 Methylene blue 4.0 4. (2004) Wang and Wang (2007) Wu et al. (2004) Chiou et al.0 mg g−1 182. (2009) Navarro et al.0 4. (2004) Wong et al.0 2.0 4.0 7.0 7.0 6.9 mg g−1 973.0 mg g−1 720.0 3.0 2. tropicalis) Yeast (C.0 3.0 4. (2002) O’Mahony et al.0 2. lipolytica) Yeast (C.0 7.0 7. (2000) Wu et al. (2009) Navarro et al.0 3.0 mg g−1 250. versicolor) White rot Fungi (C.0 mg g−1 Nasreen et al.00 mg g−1 61.0 2. (2004) Wong et al. (2003) Wu et al.33 mg g−1 860.2 mg g−1 1954 mg g−1 1940 mg g−1 1940 mg g−1 2383 mg g−1 2498 mg g−1 2422 mg g−1 2436 mg g−1 1911 mg g−1 81.0 4.0 mg g−1 114.7 mg g−1 167.0 98.37 mg g−1 24.0 3.0 7.0 2. (2009) Allen et al.0 2. (2004) Chiou et al.0 7.0 7. (2007) Nasreen et al.0 3.Environ Monit Assess (2011) 183:151–195 181 Table 5 Reviewed results representing the adsorption capacity of bioadsorbents for the adsorption of dyes and their optimized pH values for maximum adsorption Adsorbent Dye pH Adsorption capacity References Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitin and Chitosan Chitosan bead (crab) Chitosan flake (crab) Chitosan bead (lobster) Chitosan flake (lobster) Chitosan bead (shrimp) Chitosan flake (shrimp) Giant duckweed (Spirodela polyrrhiza) White rot Fungi (C.0 645.3 mg g−1 693.7 mg g−1 195 mg g−1 400 mg g−1 350 mg g−1 90 mg g−1 190 mg g−1 150 mg g−1 500.0 4. (2004) Chiou et al. 5 mg g−1 536.0 7.40 mg g−1 168.0 5. (2004) Chao et al.52 mg g−1 248.0 3.0 6. (1997) Allen et al.3 7.0 mg g−1 44. (2008) Direct red 80 Acid blue 25 Reactive red 222 Reactive yellow 145 Reactive blue 222 Basic blue 3 Basic red 22 Basic yellow 21 Remazol blue Remazol black B Remazol red RB Congo red Acid blue 74 Reactive violet 5 Basic blue 41 Acid blue 25 Basic blue 3 Basic yellow 21 Basic red 22 Malachite Green Remazol black B Remazol red RR Remazol golden yellow Acid blue 25 Basic blue 3 Basic blue 69 Reactive yellow 2 Reactive black 5 Acid blue 25 Basic blue 69 Amarant Remazol black B 2.0 mg g−1 555.6 mg g−1 Punjongharn et al.3 3.0 5.0 2.50 mg g−1 2.0 3.0 7.0 7.0 9. (2001b) Wu et al. (1988b) Allen et al.56 mg g−1 312. (2006) Wu et al.88 mg g−1 14.0 7.0 7.0 7.39 mmol kg−1 99.0 7. (2004) Chiou and Li (2002) Chiou and Li (2002) Punjongharn et al.0 3.0 2.7 mg g−1 Wu et al.5 8. (2004) Chao et al.70 mmol kg−1 101.0 3.76 mmol kg−1 45.00 mg g−1 60.0 7.00 mg g−1 50.33 mg g−1 306.0 3. (2004) Chao et al.0 mg g−1 427.9 5. (2004) Allen et al.72 mg g−1 40.0 35.0 7. (2001a) Wu et al.5 5. (2001b) Wu et al.0 9.0 mg g−1 199.0 2.0 5. (2008) Astrazon red GTLM 6. (2001a) Wu et al. (2001b) Allen et al. (2007) Ho and McKay (2003) Ho and McKay (2003) Swamy and Ramsay (1999) Swamy and Ramsay (1999) .0 7.0 6.90 mg g−1 35.0 mg g−1 41. (2004) Chao et al.0 3.5 5.0 mg g−1 78.0 7.00 mg g−1 2. (2004) Chao et al.0 4.0 mg g−1 88.77 mmol kg−1 66. (2004) Chao et al.736 mmol g−1 185.61 mg g−1 666.00 mg g−1 410.0 mg g−1 32.9 × 10−5 mol g−1 555. (2004) Allen et al. (2001) Vachoud et al. (2007) Akkaya et al.28 mmol kg−1 1936.83 mg g−1 1.0 885.0 113. (2001a) Wu et al.0 0. (2001) Liversidge et al.60 mg g−1 196.8 mg g−1 14.00 mg g−1 Arami et al.0 7. (1988a) Allen et al.124 mmol g−1 1.6 mg g−1 45.10 mg g−1 71.0 2. (1988a) Allen et al.0 9. (1988a) Aksu (2003) Aksu (2003) Aksu (2003) Fu and Viraraghavan (2002b) Vachoud et al.0 9.0 7.0 7. (2004) Mittal (2006) Aksu and Tezer (2005) Aksu and Tezer (2005) Aksu and Tezer (2005) Allen (1987) Allen (1987) Allen (1987) Akkaya et al.0 6.25 mg g−1 84. (2006) Arami et al.0 mg g−1 188. (2008) Astrazon golden yellow 6.00 mg g−1 605.0 mg g−1 1189. (2004) Chao et al.5 mg g−1 48.0 7. (2001a) Chao et al.76 mmol kg−1 67.0 6.09 mmol kg−1 104.5 mg g−1 Punjongharn et al.0 7.182 Environ Monit Assess (2011) 183:151–195 Table 5 (continued) Adsorbent Chitosan swollen bead Chitosan flake Chitosan flake Chitosan flake Chitosan – BA Chitosan – BA Chitosan – DBA Chitosan – DBA Chitosan – PA Chitosan – PA Chitosan – CA Chitosan – CA Cross linked chitosan beads Non-cross-linked chitosan beads Dried seagrape (Caulerpa lentillifera) Dried seagrape (Caulerpa lentillifera) Dried seagrape (Caulerpa lentillifera) Eggshell membrane Eggshell membrane Chitosan Chitosan Chitosan Peat Peat Peat Saccharomyces cerevisiae Saccharomyces cerevisiae Saccharomyces cerevisiae Fungus (Aspergillus niger) Chitin gels Chitin gels Peat Peat Peat Peat Peat Hen feather Dried Chlorella vulgaris (an alga) Dried Chlorella vulgaris (an alga) Dried Chlorella vulgaris (an alga) Peat Peat Peat Chitin Chitin Peat Peat White rot fungi White rot fungi Dye pH Adsorption capacity g−1 References Reactive yellow 145 Reactive red 222 Reactive blue 222 Reactive yellow 145 Crystal violet Bismarck brown Y Crystal violet Bismarck brown Y Crystal violet Bismarck brown Y Crystal violet Bismarck brown Y Reactive red 189 Reactive red 189 Astrazon blue FGRL 7.0 mg g−1 80.0 mg 339.0 7.69 mmol kg−1 107. The pH has two kinds of influences on dye: an effect on the solubility and speciation of dye in the solution.Environ Monit Assess (2011) 183:151–195 183 Table 5 (continued) Adsorbent White rot fungi White rot fungi White rot fungi White rot fungi Peat Chitosan Dye Remazol orange Remazol brilliant blue Reactive blue Tropaeolin O Acid blue 25 Acid red 73 pH 4. Adsorption capacity g−1 60. These pretreatment methods are not cost effective at large scale. or contacting with organic or inorganic chemicals proposed for improving the sorption capacity and the selectivity.7 7. reactor. The . but they have nowhere discussed anything about the role of morphology of the adsorbent. fruit. The comparison of adsorption performance of different adsorbents not only depend on the experimental conditions and analytical methods (column. etc. shape. such as natural materials. fruit waste. Reactive orange 16 dye was adsorbed most effectively to a maximum of approximately 200 mg g−1 . and plant waste. and volume of voids species in the porous materials is directly related to the ability to perform the adsorption application. photodegradation. We also agree with the discussions made by Crini (2006) in the review article that the adsorption process will provide an attractive technology if the low-cost sorbent is ready for use. particle size and shape. physical and chemical processes such as drying. micropore and mesopore volume. The pH value of the solution is an important factor which must be considered during designing adsorption process. Chitin and chitosan exhibits strong affinity for acid/reactive dyes. autoclaving. However. For example.00 mg g−1 20. low-cost adsorbents offer a lot of promising benefits for commercial purposes in the future. Undoubtedly. ozonation. plant waste. crosslinking reactions. surface area. the literature reveals that maximum removal of dyes from aqueous waste can be achieved in the pH range of 5–8.00 mg 40.00 mg g−1 20.0 positively charged nature at acidic pH and the anionic nature of the reactive dyes. The high adsorption of cationic or acidic dyes at higher pH may be due to the surface of adsorbent becomes negative which enhances the positively charged dyes through electrostatic force of attraction and vice versa in case of anionic or basic dyes.6 4. we have made some conclusions as discussed in the following paragraphs: The treatment of industrial effluent that contains the large number of organic dyes by adsorption process.). But the major role of pH was seen in the paper in which inorganic and bioadsorbents are used for the dye waste treatment. As we knew that the distribution of size.2 mg g−1 References Swamy and Ramsay (1999) Swamy and Ramsay (1999) Swamy and Ramsay (1999) Swamy and Ramsay (1999) Poots et al.8 4. and batch techniques) but also depends on the surface morphology of the adsorbent. In case of adsorbents obtained from the industries and agriculture by-products. Conclusions After reviewing the collected data. for the industrial application of biosorption. (2004) etc.0 7. (1976) Wong et al. oxidation. immobilization of biomass is necessary (Aksu 2005). Many researchers have made comparison between the adsorption capacities of the adsorbents. It is well known that surface charge of adsorbent can be modified by changing the pH of the solution and the chemical species in the solution depend on this parameter. waste materials from industrial and agriculture. there are only a few papers where they have studied the morphology of the adsorbent.7 4. even in case of the inorganic material where it plays a major role in the adsorption process.49 μmol g−1 728.00 mg g−1 43. and bioadsorbents are an interesting alternative to the traditionally available aqueous waste processing techniques (chemical coagulation/flocculation. using these easily available low cost adsorbents. and peat is shown to be a particularly effective adsorbent for basic dyes (Table 5). 1). 1976). The common adsorbent. which are of inexpensive material and do not require any expensive additional pretreatment Fig. We have seen that peat shows different adsorption capacities for single dye (Figs. and acid blue (Fig. particularly with the large amount of waste concentrated alkaline solution causing environmental pollution. With advances in fermentation technology chitosan preparation from fungal cell walls could become an alternative route for the production of this biopolymer via an ecofriendly pathway. In view of industrial developments of the various kinds of adsorbents described in the literature. methylene blue (Fig. On analyzing these results. They can be readily cultured in simple nutrients and used as a source of chitosan.184 production of chitosan also involves a chemical deacetylation process. several yeasts and filamentous fungi have been recently reported as containing chitin and chitosan in their cell wall and septa. But its main disadvantages are the high price of treatment and difficult regeneration. 1 Comparison of adsorption capacities of different adsorbents for the removal of cationic dye methylene blue . 2 and 3) (Allen 1987. Ho and McKay 2003. the physical and chemical stability of the materials and the reproducibility of the adsorption properties are of great concern. there is a demand for other adsorbents. 1988a. the bark (McKay et al. 3). we have reached to a conclusion that there is a lack of data concerning the reproducibility of the adsorption isotherms. Thus. Allen et al. commercially available activated carbon has good capacity for the removal of pollutants. 1). it may be due to the differences in the physical and Environ Monit Assess (2011) 183:151–195 chemical characteristic adsorbents obtained from different resources and locations. b. However. Poots et al. Although commercially activated carbon show maximum adsorption potential for methylene blue (Fig. basic blue (Fig. 1999) and activated carbon obtained from plum kernels (Tseng 2007) may prove to be an important alternative for the methylene blue removal from aqueous waste. Commercial production of chitosan by deacetylation of crustacean chitin with strong alkali appears to have limited potential for industrial acceptance because of difficulties in processing. At last. 2). which increases the cost of wastewater treatment. we have tried to make a comparison between the adsorption capacities of adsorbents for three commonly used dyes. Na BB 69 Anion clay hydrotalcite Clay BB 41 Clay Wood BB 41 Clay AGAP-P-N-800 BB 41 Clay Wood Pine sawdust (raw) Saw dust.RHZ Adsorption capacity (mg g-1) Adsorption capacity (mg g-1) Environ Monit Assess (2011) 183:151–195 185 1800 1600 1400 1200 1000 800 600 400 200 0 Fig.7h BB 69 Linseed oil cake AC1. 3 Comparison of adsorption capacities for the adsorption of acid blue (AB) dyes onto the different adsorbents Peat Peat Peat Chitin gels Peat Fungal Bentonite .cherry Bagasse pith Bagasse pith Bagasse pith BB 41 Saw dust-Walnut Pith Bagasse pith Bagasse pith Banana pith Jack fruit peel Slag BB BB 3 BB 69 69 Bagasse pith Activated carbon PKN4 Activated carbon PKN3 Bagasse pith BB 69 Linseed oil cake BB BB 9 BB 9 BB 9 BB 9 BB 69 41 Activated carbon PKN2 Carbonaceous adsorbent Slag Activated carbon CC-15 Activated carbon CC-10 Activated carbon CC-7 AC4.DTMA Peat BB BB 9 BB 3 BB BB 3 BB BB 3 BB 3 BB 69 69 69 41 BB 69 Peat Peat Peat Peat Peat Silica Bentonite Peat BB 69 Bentonite . 2 Comparison of adsorption capacities for the adsorption of basic blue (BB) dyes onto the different adsorbents 1200 1000 800 600 400 200 0 AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB AB 80 25 264 80 80 80 80 80 80 29 113 74 74 74 25 114 25 25 25 25 25 256 25 25 9 29 193 193 29 25 74 25 25 25 .Saw dust.oak Fig.5h BB 69 Activated carbon CC-3 Cotton waste BB Activated carbon CC-1 Activated carbon fiber (pitch) Activated carbon (bagasses) Activated carbon Activated carbon .0h BB 69 Activated carbon CC-5 AC2.pitch pine AGAP1000 AGAP800 BB 41 AGAP-P-800 AGAP AGAP1 BB 41 Saw dust. 73–81. & Ashraf. Ö. et al.. 77. Fuel. B. 1217–1225. T. 2. M. ˘ Alkan.. A. (1963).. Yeni. (2000). Comparison of optimised isotherm models for basic dye adsorption by kudzu. & Ahmad. M. N. D. & Ahmad. Removal of basic dye from waste-water using silica as adsorbent. G. R. 927–935. Sorption of acid red 57 from aqueous solution onto sepiolite. (2009).. (1992). M. Dyes and Pigments. the treatment conditions. Biosorption of reactive dyes on the green alga Chlorella vulgaris. J. Ahmed. Khraisheh. Bioresource Technology. A. Z. Khraisheh. & Dogan. M. J. (2001). Al-Degs. & Tezer. & Banat. A. A comparative study on the biosorption characteristics of some yeasts for Remazol Blue reactive dye.. (2007). & Aziz. References ˘ B. & Johnson. Kaynak. Biosorption of reactive dyes by dried activated sludge: Equilibrium and kinetic modeling. S.. easy availability. Equilibrium and kinetic modeling of biosorption of Remazol Black B by Rhizopus arrhizus in a batch system: Effect of temperature. Adsorption of congo red from aqueAcemioglu. O.. Alhassani. I. the adsorption characteristics of carbon depend on the source of raw material. Allen. Chemosphere. Efficient microbial degradation of toluidine blue by Brevibacillus sp. Effect of carbon surface chemistry on the removal of reactive dyes from textile effluent. M. Dyes and Pigments. Z.. A. Y. Dyes and Pigments. Combining ultrafiltration and adsorption on bentonite in a one-step process for the treatment of colored waters. Demirba¸s. 263–272. Al-Degs. Process Biochemistry. T. Kinetics of the Akkaya. I. 106. 38. M. ˘ Alkan. 388–396. Environmental Pollution. and temperature on adsorption behavior of reactive dyes on activated carbon. 79–84. 135–145. M... Journal of Hazardous Materials. (2007). 1437– 1444. (2005). E. 395–400. (2008). (2007). ˙ & Güzel. 13–26. A.186 step. N. M. S. Environ Monit Assess (2011) 183:151–195 Aksu.. & Walker. 40. P. A. 50. (2000). S. 431–439. Q. (2003). Effect of solution pH. Aksu. and performance of these adsorbents has been remarkably affected upon physical and chemical treatment. Removal of dyes from aqueous solutions by adsorption on mixtures of fly ash and soil in batch and column techniques.. M. But we found that only a few untreated adsorbents show good adsorption potential (Tables 1. M. Aksu. M. M. 2. So now. 66. T. 69. N. & Dogan... (2004). Loh. However. 997–1026. The excellent ability and economic promise of the activated carbon prepared from by-products after physical and chemical treatment have been recently presented and well described by the researches.. (2005). Conservation and Recycling.. S. Y. Gan. S. 1171–1175. M. El-Barghouthi. 7. G. Biochemical Engineering Journal. most of the adsorption studies have been focused on untreated industrial... 73. S. fruit. easy to handle. Journal of Colloid and Interface Science. Allen. R. ˘ Alkan. Adler. & Dogan. Çelikçapa. Z. Adsorption kinetics and thermodynamics of an anionic dye onto sepiolite. M.. N. S. Al-Bastaki. activation time. (2000). ous solution onto calcium-rich fly ash.. 237–244. J. The non-conventional activated carbons exhibited good adsorption properties and characteristics as reported in Table 1. Batch kinetic study of sorption of methylene blue by perlite. A. .. I. The removal of dyes from textile wastewater: A study of the physical characteristics and adsorption mechanisms of diatomaceous earth. 16–23. (1987). & Lundquist. 229– 238. J.. N. Pretreatment of plant wastes can remove soluble organic compounds and increase chelating efficiency and in case of cellulose base adsorbents pretreatment can also remove lignin.. (2003). G.. (2004). 75. H.. 17. (2003). Ahmad. J. Hela. Al-Ghouti. K. Rauf. Z. T.. Journal of Hazardous Materials.. A. (2004). Microporous and Mesoporous Materials.... Preparation and characterization of activated carbon from oil palm wood and its evaluation on Methylene blue adsorption. M. B116. 34. 143–152. Application of biosorption for the removal of organic pollutants: a review. decrease cellulose crystallinity and increase the porosity or surface area. G. 166. El-Sheikh. An attractive agro-industrial by-product in environmental cleanup: Dye biosorption potential of untreated olive pomace. S. Reactive dye bioaccumulation by Saccharomyces cerevisiae. & Dönmez. Water Research. L. & Ram.. Ozkara. Çelikçapa. Matthews. Z. 65. Dyes and Pigments. Resources. Ö. (2003). etc. H. E. A. Allen. and 5). Demirbas. 41. Global Nest: The International Journal. 88. M. 274. S. hemicelluloses. M.. adsorption of reactive dye by chitin. ˘ Acemioglu.. Ö. Aksu. Chemical Engineering Journal. Sakellarides. 251–259. F... Process Biochemistry. 79–86. (2005). Demirba¸s. Process Biochemistry. Removal of reactive blue 221 and acid blue 62 anionic dyes from aqueous solutions by sepiolite. Dyes and Pigments. 3. Z. E. Acta Chemica Scandinavica. 1075–1083. Uzun. 371–379. 103–113. Allen. Sahin. Process Biochemistry. S. Tosun.. 36. 168–177. Aksu. ionic strength. G. Journal of Environmental Management. Albanis. (2007). 77. 101... (2005). Equilibrium adsorption isotherms for peat. Z. & Tezer. Akar. 75.. M. Aksu. 40. & Danis. N. 1347–1361. F.. M. M. S. agricultural. A. plant wastes because of low cost.. Spectrochemical estimation of phenylcoumaran elements in ligini. Dyes and Pigments.. (2005). G. (2007). B114. a carcinogenic textile dye by chitosan hydrobeads: . (2003). K. Prieto. J. 189–195. Martinez. B. (1994). Z. (2002a). S. K. Annadurai. S. (2007). 74. (1988b). ˘ Bayramoglu. Allen.. 33–39. Hafiz. Lin.. Dye adsorption by calcium chloride treated beech sawdust in batch and fixed-bed systems. (2004).. A. G.. Chaudhuri. 58. 487–493. Journal of Hazardous Materials. J... & Sidiras. Can. Shafaei.. & Mahmoodi. & Celik. a low-cost adsorbent. Bestani. Limaee. Bukallah. Aggregation of Rhodamine 3B adsorbed in Wyoming montmorillonite aqueous suspensions.. on Neem leaf powder. 85– 87. H.. Murray. Arbeloa. A. 371–376.. B. Y. 18. F.. Chao. Sheldrick. & Khader. G. B. 39–53. Dyes and Pigments. Arami. 151–155. V. 143. Hisarli. G. Shyu... & Marchant. Desalination.. Journal of Colloid and Interface Science. & Arbeloa. S. 178–185. B. S.. et al. Y.. Adsorption characteristics of the dye. S. D. M. Allen.. Production of granular activated carbon from fruit stones and nutshells and evaluation of their physical. Arami.. Use of cellulose based wastes for adsorption of dyes from aqueous solutions. N. A. S. 65. 263– 274. M. 11. & Porter. L. D. Numerical modeling and laboratory studies on the removal of direct red 23 and direct red 80 dyes from textile effluents using orange peel. 8441–8444. & Krishnan. F. Modification of organo. 39.. American Journal of Applied Sciences. The adsorption of acid dye onto peat from aqueous solution-solid diffusion model. I.. (2008). The hydrophobic effect on the adsorption of Rhodamines in aqueous suspensions of smectite. M... a dye onto glass powder. Banat. L. F.. Attia. 32–39. & Celik. Girgis. F. 322–333. S. K. N. M. Chemosphere. Bhattacharyya. 73. M. K.. Microbial decolorization of textile-dyecontaining effluents: A review. 170. 25– 39. (2003). A. N... M. Dyes and Pigments. N. Bioresource Technology. M. 288. Journal of Hazardous Materials. Mahmoodi. 135–143.. Banat.. 57. Equilibrium studies on the adsorption of reactive azo dyes into zeolite. Microporous and Mesoporous Materials.. M.. R. 193–202. J. Investigation on the adsorption capability of egg shell membrane towards model textile dyes. I. S. K.. & Khader. Atun. L. S. B. J. Aygün.. Bhattacharyya. P. (2003). G. P. H.. McKay. S. 21. S. S.Environ Monit Assess (2011) 183:151–195 Allen. H. & Flynn. 76.zeolite surface for the removal of reactive azo dyes in fixed bed. A. (2004). Dye removal from aqueous solution by using adsorption on treated sugarcane baggase. Conservation and Recycling.. F. F. Arbeloa.. (2007). I. T. M.. 111–119. O. G. S. S. Adsorption of rhodamine 3B dye on saponite colloidal particles in aqueous suspensions. & Fathy.. P. F. N. Adsorption isotherm models for basic dye adsorption by peat in single and binary component systems. Chellapandian. 39. & Muhler.. A. Bouzaida. I.. chemical and adsorption properties. R. 217–227. Removal of methylene blue by carbons derived from peach stones by H3 PO4 activation: Batch and column studies.. Turan.. M. (1996). I.. Adsorption of acid dyes on treated cotton in a continuous system.. 241–249. & Lee. F. 211–222... (2003).. A. F. M. K. Y. B. F. W. Limaee. 95.. & Guha. Batzias.. 126. & Arıca.. J. Nigam. D. & Rammah. D. Peat as an adsorbent for dyestuffs and metals in wastewater. G.. 66. (2004). Mahmoodi. Benderdouche. Arbeloa. 59. Adsorption of reactive dye on chitin. & Hisarli. Water Research. S. Bioresource Technology. M... 99. D. Benkli. G. & Al-Makhadmeh. G. Y. & Duman. 14. Chatterjee.. Chatterjee.. G. Y. T. & Sharma. & Hatim. & Arbeloa. (2006)... Removal of dyes from colored textile wastewater by orange peel adsorbent: Equilibrium and kinetic studies. G. Al-Asheh. Environmental Monitoring and Assessment. L. (2004). & Mi. (2007). Arbeloa. M. J. M. Biosorption of benzidine based textile dyes “Direct Blue 1 and Direct Red 128” using native and heat-treated biomass of Trametes versicolor. Resources. Langmuir. Environmental Pollution. 261. (2003). 91. Yenisoy-Karaka¸s. Process Biochemistry. M. 517–524. M. Rauf. 1499– 1503. Bioresource Technology. Evaluation of the use of raw and activated date pits as potential adsorbents for dye containing waters. Enzymatic grafting of carboxyl groups on to chitosan–to confer on chitosan the property of a cationic dye adsorbent. (2002). Limaee. Journal of Colloid and Interface Science. S. S. R. Turan. & Addou. 246. Arami. Adsorptive removal of congo red. M. S. 2. J. Y. & Arbeloa. Langmuir. G.. (1999). B. Brilliant Green. Multicomponent sorption isotherms of basic dyes onto peat. A. Journal of Colloid and Interface Science... M.. 71. (2005). (2005).reactors. B92. Singh. Brown. Journal of Environmental Management. Belhakem. Methylene blue and iodine adsorption onto an activated desert plant. Adsorption of carminic acid. L. Arbeloa. Ardejani. Azhar. M. 187 Atun. Allen. S. Removal of methylene blue from aqueous solution by adsorption on sand.. D. 52. M.. I. 167–174. 4566–4573. Adsorptive removal of methylene blue from colored effluents on fuller’s earth. 282–289. L.. I.. Azadirachta indica leaf powder as an effective biosorbent for dyes: A case study with aqueous Congo red solutions. A. M. Suhardy. (2002). (2002b). S. Chatterjee. N.. 280. (1988a). Y. V. McKay. L... Liew. A. L. & Sharma. G. Badii. L. Y. ˘ Armagan. Journal of Colloid and Interface Science. (2004). K. (2008). N. 157–162.. Chemical Engineering Journal. Materials Science and Engineering: C. (1998). & Tabrizi. R. A.. A. E. The rhodamine 3B/laponite B system. McKay. Juang. N. Journal of Colloid and Interface Science. B. Journal of Hazardous Materials. 2658–2664.. M. & AlAli. N. 217– 229. 281–287.. K. Benstaali. Martinez. M. Annadurai. Dyes and Pigments. 1999–2008. (2006). Desalination. Fernández. 89.. A. Couillard. F. J. Chemosphere. C.. E. Porter.. (2007).. (2002). Fu. Journal of Chemical & Engineering Data. & Guan. G. The adsorption of congo red and vaccum pump oil by rice hull ash. A. Membrane separation for wastewater reuse in the textile industry. A. (2001). D. & Viraraghavan. A. M. & Nas. Adsorption Science and Technology. & Marucci. 57–71. T. Journal of Analytical and Applied Pyrolysis. R. Peláez-Cid. 75. & Arbeloa. 77–94. Forgacs.. M. G. 93. Venancio. Environmental Science & Technology.. & Haghighi. Applied Clay Science.. 251–262. J. Chen. L... (2000). Eren. 141–148. Nature... Corsi. Langmuir. Gupta. F. 63–70. B. Alkan. 301–308). & Li. 575–584. Y. 109–117. A. Y. 27.. C. & Attyia. & Viraraghavan.. Bioresource Technology. Ferrero. & Özdemir. 50. Bioresource Technology. Adsorption behavior of reactive dye in aqueous solution on chemical cross-linked chitosan beads. Desorption of dye from activated carbon beds: Effects of temperature. R.. Dhalan. 32–41. 69–84. K. E... Chiou. Kumar.. 95. McKay. 24... B109. 6032–6037. R. R. El-Guendi. Chou. (1994).. (2000). 144–152. & Li. Conservation and Recycling. M. H. A. K. M. UKM. Advances in Colloid and Interface Science. 1061–1085. A. W.. an agricultural waste for removal of methylene blue from aqueous solution. Espantaleón. K. S. E. F.. (2008). Use of activated clays in the removal of dyes and surfactants from tannery wastewaters. & Marsal. Cserháti. & Oros.. M. 12. R. 1285–1291. Ni. F. (2007). In Prosiding Seminar Kebangsaan Pengurusan Persekitaran 4–5 July. & Mohamed. Amita. 31.. 1261–1274. K. Hui.. H. 78. A. Ho. K. F. & McKay. (2009). Choy. 82. (2001). I. & McKay. Journal of Hazardous Materials. & Alkan. 121– 124. Use of palm oil fiber. 97. Barriquello. 417. Zhu. Eclética Química. G. (2005).. Bioresource Technology. ˘ Dogan. K. Lee. 217–219.. Ghosh.. L. & Bhattacharyya. A. Demirbas. R. T. T. Environment International. 16. Hashim. Fu. M. Davis. V. Y. Removal of synthetic dyes from wastewaters: A review. Journal of Colloid and Interface Science. Removal of Congo Red from an aqueous solution by fungus Aspergillus niger.. Journal of Hazardous Materials. Chern. Laiman. T. G. (2004). Dabrowski. Gong.. Filho. & Porter. Spectroscopic characterization of the adsorption of Rhodamine 3B in hectorite. and alcohol.. A. M. J. 4159–4165. K. E. (2004). isotherms models applied to the multicomponent sorption of acid dyes from effluent onto activated carbon. M. Key factor in rice husk ash/CaO Sorbent for high flue gas desulfurization activity. Z. Advances in Environmental Research. (2004). Removal of methyl violet from aqueous solution by perlite. E. 105–110. M... R. J. M. Resources. Tsai. (2009). Ismail. (1999). M. A. B93. Y. Chemical catalytic reaction and biological oxidation for treatment of nonbiodegradable textile effluent. Methylene blue adsorption onto modified lignin from sugarcane baggasse. Y.. Bioresource Technology. Conservation and Recycling. 163–169. F. (2001). & Alkan. 243. H. Non-conventional low-cost adsorbents for dye removal: A review.. Journal of Hazardous Materials. E... (2001). M. 953–971. Characterization of adsorbent materials prepared from avocado kernel seeds: Natural. Kamaruddin. 7. 233–248. K. & Li. J. pH. D. T. Bangi (pp. M. Ghoreishi. D. Applied Clay Science. Film-pore diffusion modeling and contact time optimization for the adsorption of dyestuffs on pith.. Langmuir. activated and carbonized forms. K. 40.. S. M. (2006). (2003). Fu. Darus. J. 30. B. A.. Dyes and Pigments. 1335–1363. Water Research. (2002b). Adsorption behavior of cationic dyes on . (2000). Dyes and Pigments. C. M. (2003). 60. Crini. & Wennrich. R. Kinetics and mechanism of removal of methylene blue by adsorption onto perlite. Ordered porous materials for emerging applications. 63. R. Adsorption of anionic dyes in acid solutions using chemically cross-linked chitosan beads. (2007). 162. 35. Elizalde-González. 32. 84. J.. Environ Monit Assess (2011) 183:151–195 ˘ Dogan. 295–300. 267. (2002a). & Nizam. K. Arbeloa. ˘ Dogan. Garg. Chemical Engineering Journal. 189–197. Chen. Equilibrium and kinetic modeling of adsorption of reactive dye on cross-linked chitosan beads. & Lo. 299. P. I. Chiou. & Kumar. V. M. G. Türkyilmaz... M. Ciardelli. 239– 247.. S. H. Garg. (2003). Adsorption of methylene blue on kaolinite. 28. Dye biosorption sites in Aspergillus niger.. Zhanga. Hechenleitner.. Fungal decolorization of dye wastewater: A review. S. (2003). R.. Turkey. 139– 145.. Batch kinetic and equilibrium studies of adsorption of reactive blue 21 by fly ash and sepiolite. M. G. Sorption of acid dyes from effluents using activated carbon. Basic dye (methylene blue) removal from simulated wastewater by adsorption using Indian Rosewood sawdust: A timber industry waste. Choy. 79. C. H.. Activated clay as an adsorbent for cationic dye stuffs. (1995). 8–21. 20.. equilibrium and kinetics. G. (2002). 813–821. M... Yadav. Dyes and Pigments. (2002).. 243–250. Nieto. A. 185–193. The use of peat in wastewater treatment. G. 701–713. G. Colloids and Surfaces A. Dye removal by low cost adsorbent: Hazelnut shells in comparison with wood sawdust. 45. & Gupta. 78. Removal of basic dye by modified Unye bentonite. Adsorption–from theory to practice.. H. (2001). Journal of Hazardous Materials. Bioresource Technology. M. Water Research. Mattusch.. Chiou. Dye removal from aqueous solution by adsorption on treated sawdust. & Wu. P. J. 1095–1105. (2003). & Viraraghavan. 142.. Chaudhuri. H. & Pineda. E. M.. (2004).188 Binding mechanism. Chemical Engineering Journal. M. (2007). L. Resources.. 146–152. Özdemir. C. D. N. R. 135– 224... Adsorption kinetics and mechanism of cationic methyl violet and methylene blue dyes onto sepiolite. Y. Sorption of basic dye from aqueous solution by pomelo (Citrus grandis) peel in a batch system. R. H. Z. C. S. 189 Han. Dogar. 99. S. V. M. Grabowska. V. & McKay. 66. Journal of Hazardous Materials. (2007). C.. 733–738. (2005b). (2008). Y. K. K. B101. Janoš. S. & Lu. 123–128. Guo. Ho. M. T. Water Research. Y. P.. Journal of Hazardous Materials. Gupta. R. 87. D. S. M. Dyes and Pigments. Y. 183–191. & Mittal. Harris. Y.. R. Matyar. G. Sorption kinetics for the dye removal from aqueous solution using activated clay.. & Lu. (1998b).. Guo. Chiang. (2003). D. P.. Removal of the hazardous dye Rhodamine B through photocatalytic and adsorption treatments. using sonicationsurfactant-modified attapulgite clay. A. Ho. Goyal. G. J. & Mohan. Removal of basic (Methylene blue) and acid (Egacid Orange) dyes from water by sorption on chemically . R.. S. Jain. & Johnson. Gupta. H..Plastics Technology and Engineering. Use of rice husk for the adsorption of Congo red from aqueous solution in column mode. 344–350. & Yang. Tropical Agriculture. Huang. & Ahmad. W. G. B. Sorption of dyes from aqueous solutions onto fly ash. A. Han. Carbon Science. 217–228. Acikyildiz. Z. Adsorption studies of a water soluble dye. 38.. Growth yield. W.. Yang. Adsorption of an acid dye onto coal fly ash.. S. S. R. 870–875. & Suhas (2009). S.. Zhao. M. J. B. Hui.. Gürses. F. Coskun. Colloids and Surfaces A. 56.. Process Biochemistry. N... nutrient uptake. Chiang. Hegde. Zou. 219–229. Y. Wang..based porous carbon for adsorption of rhodamine B from aqueous solution. B. 31–42. Use of rice husk. Z. P. H. & Karaca. Sorption of dye from aqueous solution by peat. G. F. Journal of Colloid and Interface Science. C. J. A. (2006).. A. 137.. S. Removal of methylene blue from aqueous solution by chaff in batch mode. Y. Y. B. Q. Gupta. Batch adsorption of methylene blue from aqueous solution by garlic peel.. Sikarwar. Gupta. & Wang. an agricultural waste biomass. H. Journal of Hazardous Materials. 331–334. (2005a). Journal of Environmental Management. Ali. O. S. 2938–2946. 74. & Arikan. Yang. Industrial & Engineering Chemistry Research... W.. K. Wnag. (2004). 36. Selective adsorption of dyes and other organic molecules to kaolinite and oxide surfaces. (1996). Gürses. 1285– 1291. (2009). (2008). Removal of basic dye from aqueous solution using tree fern as a biosorbent. I.. & Gryglewicz. (2008). D. et al... Bioresource Technology.. H. C... A. T. G. Li. An inexpensive adsorption technique for the treatment of carpet effluents by low cost materials. D.. B108. Singh. 220–228. Equilibrium uptake and sorption dynamics for the removal of a basic dye (basic red) using low-cost adsorbents.. (2001).. & Yalcin. (2005). Determination of adsorptive properties of clay/water system: methylene blue sorption. Removal of chrome dye from aqueous solutions by mixed adsorbents: Fly ash and coal. Bioresource Technology.. (1991). (2007). A. (2001). G. Adsorption characteristics of Congo red on coal. B. Z. 36. 34– 40. Wang. Hsu.. Mahmoud.. Adsorption of malachite green on micro. Y. 13. 3040–3045.. S.Environ Monit Assess (2011) 183:151–195 citric acid esterifying wheat straw: kinetic and thermodynamic profile. & Suhas (2003)... Han. Reactive Red MF-3B. Gupta. K. (1990). Y. Buchtová. K. Process Biochemistry. & Shukla. F. Application of low-cost adsorbents for dye removal—A review. C. Hameed. Acikyildiz. Haghseresht. Ho. M. Journal of Hazardous Materials. M. Suhas.. Journal of Hazardous Materials. 131–140. Sorption of dyes and copper ions onto biosorbents. P. Y. V... Janoš. Trans IChemE. Pilarova. Dyes and Pigments. G. Li. 230. M. 24. 310–314. Dogar. 85. L. Ibrahim.. Animation of wood sawdust for removing anionic dyes from aqueous solutions. (2003). Y. 143. & McKay. (1998a). (2008). 45–50. 76B. J.. S. Regression analysis for the sorption isotherms of basic dyes on sugarcane dust. Bhatnagar. M. Dyes and Pigments. J.. V. L. 956–964. F. G.based mesoporous activated carbon. Ho. (2004). 183–188. Sorption of basic dyes from aqueous solution by activated sludge. 15–26. Prasad. (2009). & Rejnek.. J. R. (2007).. Removal of cationic dye from aqueous solution using jackfruit peel as a non-conventional and low-cost adsorbent.. Qiao. 269. X. M. Bayrak.. 4938–4944. P. Y. et al.. Karaca. Adsorption Science and Technology. (2003). B. Ho. E. Jain.. 68. 2473–2488. Y. Y.. 70. 170–179... Kinetic models for the sorption of dye from aqueous solution by wood.. 96. Desalination. Journal of Hazardous Materials. & Abou-Shosha. Adsorption study for the removal of basic red dye using bentonite. Fuel.. Q. C. Ho. K. Hameed. (2003). Journal of Hazardous Materials. Polymer . Yalcin. Hu. & Bansal. A. Wang.. 316. & Srinivas. (2004). 963–971.. (2006).. Z.. S. Wells.. Gulnaz.... Liu. Chemical Engineering Journal. Journal of Environmental Management. Chiu.. Qi. et al. and water uses of banana crops under drip and basic irrigation with N and K fertilization. M. R. & Singh. N.. Separation Science and Technology.. 131. Ding.. The adsorption kinetics of the cationic dye. Bayrak. G. Mathur. (2006).. Equilibrium and dynamic adsorption of methylene blue from aqueous solutions by surface modified activated carbons. H. 550–557. S. & Hsu. 5. D. A. A. 78–84. 119–124. & Ryznarová.. Hameed. 162. Journal of Colloid and Interface Science. 115–124. J. R. J. 180.. Q. Wang. (1997). Colloids and Surfaces A. A. G. Hashem. 90. 37. methylene blue onto clay. Kaya. 265. Y.. A. Wilson. & Ahmad. & Hsueh... 2313–2342. Fu.. V. 164. 257–264. A.. C.. H.Yang. Jin. 40.. 541–548. Y. Utilization of industrial waste products as adsorbents for the removal of dyes. S. Qi.and mesoporous rice husk-based active carbon. 1047–1061. Water Research. 45... Xu. & McKay.. Colour removal from aqueous solutions by adsorption. G. (2008)... V. Tay. Dyes and Pigments. Combined membrane process at wastewater treatment. K.. (2009).. Vennilamani. Activated carbons from waste biomass by sulfuric acid activation and their use on methylene blue adsorption. Kumar. 75. W. Erturk. J. J. G. W. D... Juang. Colour removal from dye wastewater using sugarcane dust as an adsorbent. (2007). Environmental Science & Technology. Displacement effect of NOM on Atrazine adsorption by PACs with different pore size distribution. Chemical Engineering Journal. B. 168. & Pattabhi. L. 710–720. & Ozmıhcı. F. 109–113. Journal of Chemical & Engineering Data. Sorption isotherm for safranine onto rice husk: Comparison of linear and non-linear methods. M. (2006). Basic and reactive dye removal using natural and modification zeolites. (2009). Removal of methylene blue by mango seed kernel powder. Applied Clay Science. J.190 treated wood shavings. C. Karanfil. R. Kannan. M. Dastgheib. Markvartova. S. (2007). Kornm. Chemosphere. Biochemical Engineering Journal. M. D. A. I. & Mall. H.. 45. M. Han. K. Characterization and use of activated carbons prepared from bagasses for liquid-phase adsorption. et al.. H. (2004). Snoeyink. High-efficient degradation of dyes by . K.. J. 35. J. K. Karagöz.. Kaya. V. M. (2006). Use of chemically modified chitosan beads for sorption and enzyme immobilization. M. Lataye. 269–282. H. L. V. Kumar. Wu. & Singh.. M. B. V. S. S. 74. Cakl. Bioresource Technology... Anion exchange resins for the removal of reactive dyes from textile wastewaters. Environ. (2000). B. 273–278. & Porkodi. 267– 271. R. 90. Adsorption Science and Technology... (2003).. 36. & Maluldin. (2004). 87. I. Environmental Pollution. Sun.. A. Khattri.. Teppen. illite and kaolinite by methylene blue adsorption. 299–303.. 304–309. Mechanism of adsorption of dyes and phenols from water using activated carbons prepared from plum kernels. Dyes and Pigments... (2002b). Exploring molecular sieve capabilities of activated carbon fibers to reduce the impact of NOM preloading on trichloroethylene adsorption. Akgul. 58. Radhika. 99... P. & Fu. Hachkar. Journal of Environmental Management. Water. M. Tok. Karadag. Juang.. & Kettrup. (1999). D. T. Kumar. R.. Campos.. (2008).. (2002a). & Singh. S. 35. & Malik. N. K. Insel. Lataye. 1450–1453. D. 1321–1327.. 127–141. 17. Removal of Basic Red 46 dye from aqueous solution by adsorption onto Moroccan clay. 45. & Marias. Energy Conversion and Management. Adsorption of α-picoline onto rice husk ash and granular activated carbon from aqueous solution: Equilibrium and thermodynamic study.. A. (2002). A. U. S. 201. & Bayrak. (2005). D.. Ucar. Degradation of azo dyes by algae. Environment International. Li. & Houtian. Karaca. 2436–2441. 230–234. (2004). (2000). S.. F. Q.. Karim. T. 38.. C. M.. Chen. (2001).... Li. Environ Monit Assess (2011) 183:151–195 Kargi. M. & Jekel. Koch. Karthika. & Erdem. 171–177. H. Huang. S. Kadirvelu. I. 73. 3934–3943. 130–133. & Turan.. Y... Kim.. H. Kavipriya. R. R. Lienert.. D. & Lataye. D. D. 327–336. C. Li. Air. F. Mishra. Dyes and Pigments. S. 1510–1515. Environmental Science & Technology. 147. H. Lakshmi. (2002). A. A. (2002). 191–199. (2001).. 59–64. M. M.. 83–93. Karcher. 1693–1704. X.. & Tseng. Mishra.. Joo. 52... (1992). Indian Journal of Chemical Technology. 129–132. D. Journal of Colloid and Interface Science. (1998).. O. C. Garg. (2007). (2009). F.. 120. 36. Kinetics and mechanism of removal of methylene blue by adsorption on various carbons—A comparative study. R. R. & Singh. Karcher. 6. M. & Jekel.. Advances in Environmental Research. Rice husk ash as an effective adsorbent: Evaluation of adsorptive characteristics for indigo Carmine dye. M. Determination of cation exchange capacity and the surface area of bentonite. A. S. G. M. 227.. K. 25–40. A. M. N. Jinqi. & Yaacoubi. 283–294. (2007). Biosorption performance of powdered activated sludge for removal of different dyestuffs... Kornm. V. (2007). F. S. S. I. Li... Removal of pyridine from aqueous solution by adsorption on baggase fly ash. Screening of commercial sorbents for the removal of reactive dyes. 5. and Soil Pollution. Yediler. Z. V. Juang... Industrial & Engineering Chemistry Research. M. Bioresource Technology. S. Bakasse. Fungal dye decolourization: Recent advances and future potential.. B. 653–658.. K.. 51. Environmental Science & Technology. Wu. A. 9. Mall.. S.. 40. 51.and three-parameter isotherm models for the sorption of methylene blue onto lemon peel. R. He. L.. Bioresource Technology. Shin. M. Choi. S. H. & Sundaram. I.. D.. Lata. Kahr. Water Research.. & Gupta. A.. & Dolecek. 25–40. K.. T. Thermodynamics of nitroaromatic compound adsorption from water by smectite clay. Srivastva. & Sivanesan. Colloids and Surfaces A. H. Wu. A. & Madsen. Kaushik. Ozonation of hydrolyzed azo dye reactive yellow 84 (CI).. F. S. & Boyd. 6214–6222. R. M. (2009). Removal of a basic dye from aqueous solution by adsorption using Parthenium hysterophorus: An agricultural waste. (2006). Gürses. 139–149. Jirankova.. Separation and Purification Technology.. 27. Enzyme and Microbial Technology. K.. Dyes and Pigments. & Tseng. 100. 437–444. & Tseng. A. Khattri. K. Khattri. & Mall. E. 72.. 633–635. 4717–4724. Effect of some pre-treatments on the adsorption of methylene blue by Balkaya lignite. & Kumrana. 5433–5442. 46. Utilization of various agricultural wastes for activated carbon preparation and application for the removal of dyes and metal ions from aqueous solutions. 138. M. Colour removal from synthetic dye wastewater using a bioadsorbent. Choi. P.. Journal of Hazardous Materials. Decolorization of reactive dyes using inorganic coagulants and synthetic polymer. (1995).. Relation between some two. Mounir. Journal of Hazardous Materials. J. Johnston. T. S. Dyes and Pigments. . B133. (2006). Equilibrium studies during the removal of dyestuffs from aqueous solutions using baggase pith. X. Journal of Hazardous Materials. (1999). J.. Trans IChemE. Naidu. 567–578. & Daifullah. 219–226. (1994).. Separation and Purif ication Technology. & Saha. Removal of Congo red from water by adsorption onto activated carbon . L. R. Bioresource Technology. Removal of basic blue 41 dye from aqueous solution by linseed cake. 136.. A. 323–339.. (2002a). Journal of Hazardous Materials. A. P. Adsorption isotherms. D. Industrial & Engineering Chemistry Research. K. McKay.. Removal of Congo red from wastewater by adsorption onto waste red mud. 1513–1520. C. Use of activated carbons prepared from sawdust and rice. Ma. M. Martin. 84. Singh. 14943– 14947. Munoz-Lopez.. (1999). Industrial & Engineering Chemistry Research. M. (2006). (2002). Vasconcelos.. Mohanty. Mane. tatrazine from aqueous solutions using waste materials: . (2006a). Mohan. H. M. Mittal. Coirpith. G. G. S. G. Reactive dyes removal from wastewaters by adsorption on eucalyptus bark: Variables that define the process.. 137. Mukai. Mane. for the treatment of dyeing wastewater. 45. D.. & Arasi.. 32. (2004). Fuller earth and fired clay as adsorbents for dyestuffs— Equilibrium and rate studies. L. E. Water. J. M. M. & Prasad. G. 189–204. a lowcost adsorbent. (2009). Rao. Photocatalytic decolorization and mineralization of dyes with nanocrystalline TiO2 /SiO2 materials. N. Journal of Hazardous Materials. van Grieken. Mittal.. 46. (1998). A. F. Mohamed. J. R. R.. G. E. Y.. from wastewater by using hen feathers. 390–400. Batch and bulk removal of hazardous dye. Otterburn. Adsorption of bisphenol A from aqueous solution onto activated carbons with different modification treatments. G.. 164. El-Geundi. Liversidge.. & Otterburn. & Beça. Adsorption of dyes from aqueous solutions or suspensions with clay nanoadsorbents. Artola. International Journal of Environmental Technology and Management. & Agr.. McKay.. Adsorption kinetics of removal of a toxic dye. 21. C. Mittal. A.. V. T. 34.. K. K. F. & Zhang.. and Soil Pollution. The Journal of Physical Chemistry C. Journal of Colloid and Interface Science. & Kadirvelu. Tamon. G.. (1996). Malik. Activated carbons developed from surplus sewage sludge for the removal of dyes from dilute aqueous solutions. M. M. P. Industrial & Engineering Chemistry Research. Li. J. (2007). H. C. C. Nakagawa. Polyacrylamide grafted attapulgite (PAM-ATP) via surface-initiated atom transfer radical polymerization (SI-ATRP) for removal of Hg(II) ion and dyes. Liu. McKay. Process Biochemistry.. Acid dye removal: comparison of surfactant-modified mesoporous FSM-16 with activated carbon derived from rice husk.. J. Dyes and Pigments. & Tanthapanichakoon. B90. M. Lloyd. M. (2002b). The removal of organic pollutant from industrial effluents via tapered bed adsorption column. Namasivayam. P. T. Journal of Hazardous Materials. Water Research. M. C. Adsorption of a basic dye from aqueous solutions onto sugarindustry-mud in two modes of operations. M. V. 1791–1798. M. Air. 73.. D.. McKay. K. 241– 250. Porter. A. Namasivayam. S. 28–34. E. and Soil Pollution. S. McConvey. P. kinetics and column operations for the removal of hazardous dye. S. M.. Morais.... L.. (1985). 307–322. W.. Liu. Journal of Environmental Management. V. P. S.. (2006b). 269–278. P. J. (1981). F. Marugan.. J. Separation and Purif ication Technology. Chemical Engineering Journal. C. Chemosphere. V. Journal of Colloid and Interface Science. (2007). & Forster.. P. M. 74. as adsorbents.. Dyes and Pigments. Wase. & Srivastava. & Fan.. Removal of dyes from wastewater using flyash. 3688–3695. Water Research. 423–438. G.. 80. Pore diffusion during the adsorption of dyes onto bagasse pith. 56.. & Rigola. (2003). B... (2003). & Karthikeyan. (2003). S... an agricultural waste byproduct. Freitas. Use of baggase fly ash as an adsorbent for the removal of brilliant green dye from aqueous solution. K. Mall. Magdy. Colloids and Surfaces A. Namasivayam. Mohan. L. S. Meikap. J.. I. N.. J. (2007a). S. Removal of crystal violet from wastewater by activated carbons prepared from rice husk. 591–602. 33. 1275–1280. The removal of dye colors from aqueous solutions by adsorption on low-cost materials. C.husk for adsorption of acid dyes: a case study of acid yellow 36.Bottom ash and de-oiled soya. & Kavita. (2006). 20–33.. Balaguer. 9. 401–417. Q. 18. 498–503. G. C. A. 48. A. 38. J. 239–249. C.. O. M. & Srivastava. (1997).. indigo carmine from wastewater through adsorption. 38. D. (2004). Ariyadejwanich. Mittal. 31. Water. 272. 79–81. J. 7605–7610. D. (1987). (2007b)..Environ Monit Assess (2011) 183:151–195 ZnCdS solid solutions under visible irradiation. D. D. J. Malik. F. & Nassar. & Kumar. S. J. & Aguado. L. M. Geundi. A. Adsorptive removal of direct azo dye from aqueous phase onto coal based sorbents: A kinetic and mechanistic study... & Biswas. Transport processes in the sorption of 191 colored ions by wood particles... 32–39. K. 473–477.. 196– 202. I. Liu. 282–283. J. Water Research. Allen. 5165–5171. Air. Sze. Oxidation of direct dyes with hydrogen peroxide using ferrous ion as catalyst. 24. G. 58. & Guo. 979–988. Malachite Green. 94. M. J. & Nassar. M. Kinetic and equilibrium isotherm studies for the adsorptive removal of brilliant green dye from aqueous solution by rice husk ash. McKay. Adsorption of phenol and reactive dye from aqueous solution on activated carbons derived from solid wastes. Mall. A. (1997). 231–239. V. K. 46. Namba. K. Journal of Hazardous Materials. C.. R. McKay. & Kurup. S. Gonçalves.. (2008). Mittal. G.. G. Singh. 114. Waste Management. J. I. 277–288. & Kurup. & Qin. Removal of direct red and acid brilliant blue by adsorption on to banana pith. & Towprayoon. M. 126. & Arami. & Ranganathan. Crystalline forms of cellulose in the silver tree fern Cyathea dealbata. A. E. 57. J. K. M. T. Jeyakumar. Cellulose. . 211–224. (2008b). (2003b). (2008). Waste banana pith as adsorbent for the removal of Rhodamine-B from aqueous solutions. García. Singh. C. 255–261. 13. M. G. Removal of different basic dyes from aqueous solutions by adsorption on palm-fruit bunch particles. Thiravetyan.. 15. 31... 72. & Yamuna. N.. & Morán. Kanchana. O’Mahony.. Cuizano. Waste Management.. M. 269– 279.. (2001a)... Z. Netpradit. 85–95. Process Biochemistry. Effect of pH on cadmium biosorption by coconut copra meal. Selvi. Ofomaja. 49–52. (1993). D. Gayatri. Elimination of organic water pollutants using adsorbents obtained from sewage sludge. & Towprayoon. 14.. R. (2005). (2002). Nigam. Thiravetyan. Comparative study of the removal of phenolic compounds by biological and non-biological adsorbents. Journal of Hazardous Materials. Navarro. (2004b). C... Rani. Lazo. (2003a). & Yamuna. Y. Chemical Engineering Journal. S. Gessner. D. 477–483. Oei. Begum. Ofomaja. P. Orthman. K. Evaluation of metal hydroxide sludge for reactive dye adsorption in a fixed-bed column system. H. Nasreen. 53–59. & Tobin. & Sumithra. R. B... C. 31. Namasivayam. Adsorption of reactive Özacar. dyes on calcined alunite from aqueous solutions. (2003).. M. Otero. Dyes and Pigments. Namasivayam. A. Namasivayam. 791–795. and electrolytes. Sorption dynamics and isotherm studies of methylene blue uptake on to palm kernel fibre. Separation and Purif ication Technology.. 77–79.. 4. Bioresource Technology. Banat. Journal of Environmental Management. I. A. P. Wang. P.. A. P. C. K. N.. & Yamuna. & Sartori. C. H. C. 71–78. Y. E. Nigam. A. M. 54.. Removal of dyes from aqueous solutions by cellulosic waste orange peel. Journal of Colloid and Interface Science. & Morán. Q. & Marchant. Adsorption of three azo reactive dyes by metal hydroxide sludge: Effect of temperature.. N. M. Calvo. Decolorization of textile dyes and their effluents using white red fungi. Vanathi. Removal of direct red 12B and methylene blue from water by adsorption onto Fe (III)/Cr (III) hydroxide. Muniasamy. 55–65. Zhu. (2001b). G. A. & Towprayoon. R. 262. Biochemical Engineering Journal. Adsorption of metal Özacar.. & Kumutha. ¸ I. S.... C. Uptake of dyes by a promising locally available agricultural solid waste: Coir pith. (2003). R. Namasivayam.. 21. F. C. I. 8–18. Chemical Engineering Journal. Sun-Kou.. Sorptive removal of methylene blue from aqueous solution using palm kernel fibre: Effect of fibre dose. S. S. Journal of Hazardous Materials. & Kusar. T. 784–791. Bajwa. (1997). 381– 387. Environ Monit Assess (2011) 183:151–195 Newman. (2003). Dyes and Pigments. 40. 89–95. (2002). H. Water Research.. R. A. Mycopath. & Marchant. F. 254–259. 74.. 143. P. 164. Noroozi. Bahrami. Journal of Colloid and Interface Science.. 763– 772. ˙ A. & Llanos.. Ofomaja. Surfactant modified barley straw for removal of acid and reactive dyes from aqueous solution. 66. & Suba. R. G. 194–199. R. & Magdy. A.. Ibrahim. 435–442. Bioresource Technology.. 96.. (1997). an agricultural solid waste. 100. Bioresource Technology. S. 643–648. A. 35–43. E.. A.. Journal of Hazardous Materials. Water Research. (2009). R. Rozada.. C.. E. S. E. (2003). Bioresource Technology. Physical removal of textile dyes from e.. & Ho. Prabha.uents and solid-state fermentation of dyeadsorbed agricultural residues.. Ofomaja. (2008a). S. Dyes and Pigments. 356–362. L.. F. & Ang... (2007). Reactive dye biosorption by Rhizopus arrhizus biomass. T. Use of anion clay hydrotalcite to remove coloured organics from aqueous solutions. Microbial process for the decolorization of textile effluent containing azo.. Kinetic study and sorption mechanism of methylene blue and methyl violet onto mansonia (Mansonia altissima) wood sawdust. Netpradit. M. M.. Chemical Engineering Journal. Y. Namasivayam. M. H. 38.. Neumann. B139. Singh. T. L.. A. Banat. Nassar.... C.. 57. E. & Yasumori. 456– 463. D. Namasivayam. N. & Sengil. 1439–1446. Kameshima. A. (1994). Okada. Namasivayam. B... H. R. J. S. (2000). Guibal. Schmitt. Enzyme and Microbial Technology. Waste Management. F. 47–58. Yamamoto. 31. Adsorption of binary mixtures of cationic dyes. (1996). S. García. Influence of the layer charge and clay particle size on the interactions between the cationic dye methylene blue and clays in an aqueous suspension.. S. A. 5. B. 37–43. 270. Application of ‘waste’ metal hydroxide sludge for adsorption of azo reactive dyes. Bioresource Technology. Kinetic and equilibrium modelling of the methylene blue removal from solution by adsorbent materials produced from sewage sludges. pH. T. R. M. 207–215.. B98. Netpradit. 64. R. (2005).. Otero. Rozada... M.. Biochemical Engineering Journal.. an industrial solid waste. (1996). C. Waste Management.192 prepared from coir pith. Kumar. Thiravetyan. ‘Waste’ coir pith—A potential biomass for the treatment of dyeing wastewaters.. 219–226. S. Journal of Colloid and Interface Science. Armour. K. I. M. D.. 76. Dye removal from wastewater by adsorption on ‘waste’ Fe(III)/Cr(III) hydroxide. ˙ A. Biomass & Bioenergy. (2007). F. 4292–4295. Calvo. T. R. M. & Lu. I. M. P.. (2004a). & Sengil. complex dyes from aqueous solutions by pine sawdust. 223–226. Adsorption properties of activated carbon from waste newspaper prepared by chemical and physical activation. G. 255. 59–68. I.. Radhika. (2009). A. (2007). diazo and reactive dyes. J. (1998). Sorial.. 21. Y. 37. Comparison of the adsorption characteristics of azo-reactive dyes on mesoporous minerals. G. (2006). S. Journal of Hazardous Materials. J. R. 233–235. C.. (2007). M. Krithika. 47. L.. K. 111.. 140. 164. S. (2003). J.. J. an agricultural waste. Kinetics study of methylene blue dye bioadsorption on baggase. & Nigam. F. L.. P. The removal of acid dye from effluent using natural adsorbents-I peat. Sathiya Moorthi... 10. Özer. Lima. B. T. G.. Pauporte... Panswed.. S. 146. 139–144. C. 419–427. Robinson. T. Chandran. K. 262–269. Applied Ecology and Environmental Research. Y. 7639–7644. Journal of Hazardous Materials. McMullan. Das. J. Dyes and Pigments. T. Ponnusami.. Purkait. 2824–2830. M. Removal of Congo red from aqueous solution by anilinepropylsilica xerogel. Mazzoczto. P. S. (2001). F. 62. M. (1997). K. (2008). 35–43. Journal of Colloid and Interface Science. (1986). A. Water Research. 41. & Tokat.. 80. P. 96. N. Effects of process variables on kinetics of methylene blue onto untreated guava powder: Statistical analysis. Bioresource Technology. R. P. A. Wu. N. A. B.. & Celik.. 811–821.. & Özcan. (2001). Biosorption of commercial dyes on Azadiracta indica leaf powder: A case study with a basic dye Rhodamine B. P. Dyes and Pigments. E. F. F. S. Raghuvanshi. L. & Alkan. K. P. (2008b). Soares. S.. M. Gushikem. Removal of dyes from an artificial textile dye effluent by two agricultural waste residues. Waste Management. Methylene blue biosorption from aqueous solutions by yellow passion fruit waste. M. Xu.. A. 84. McKay.. P. & Subburam. 18. Carbon from cassava peel. Chandran. Chandran. Martin-Villacorta. 49–60. Robinson. Sivakumar. 243.. Robinson. S. Use of slag for dye removal.. Turan. Rozada. Dias. F. V.. Pala. V.. R. Murugesan. 372–379.. 76. Bioresource Technology. A. 609– 613. Water Research. Lima. M.. Periyar selvam. Ozdemir. & Lima. P. Qiu. 36.. (2002b). A. (2007). 36. R. Bioresource Technology. F. 20. T. Applications of Brazilian pine-fruit shell in natural and carbonized forms as adsorbents to removal of methylene blue from aqueous solutions—Kinetic and equilibrium study. & Kaushik. & Pavasant. (2002a). Studies on the adsorption of dyes into clinoptilolite. 483–488. (2003).. & Bhattacharyya. sorber design for methylene blue removal to minimize contact time. (2004). 72. C. E. Water Research.. & Nigam. as an adsorbent in the removal of dyes and metal ions from aqueous solution. Carbon.. J. Pavan. C. & Sengil. & Srivastva. Chemical Engineering Journal.. (2008). 247–255. 280. S. A. Singh. L. Color removal from cotton textile industry wastewater in an activated sludge system with various additives. Qian.. 1061–1066.. & Rathousky. Adsorption of Acid Blue 193 from aqueous solutions onto Na-bentonite and DTMA. M. G.. & Mazzocata. & Guha. & Dursun. & Wang. (2007). Royer.. Statistical design of experiments as a tool for optimizing the batch conditions to methylene blue biosorption on yellow passion fruit and mandarin peels.. 164. Meevasana. A. Studies on desorption of individual textile dyes and a synthetic dye effluent from dye-adsorbed agricultural residues using solvents.. A. S. (2004). Ramakrishna. F. 76. Simon. E.. (2002). J. B. A. & Nigam. G. Y. 44–54. Dye adsorption by sewage sludge-based activated carbons in batch and fixedbed systems. K. Madhuram. C.. S. 193 Punjongharn. K. 760–768. T. V.Environ Monit Assess (2011) 183:151–195 ˙ A. Dyes and Pigments.. Lima. 28. 286–292. G. Marchant. M. Dogan. Garcia. M. 80. P. A two stage batch adÖzacar. N. & De. 135–142. Rajeshwarisivaraj. & Nigam. P. Journal of Environmental Sciences. J. Calvo. R.bentonite.. P.. & Kalaichelvan. 374– 379. Bioresource Technology. C. Adsorption of dyes on activated carbons: Influence of surface chemical groups. B. S. Panda. Poots. A. A.. 17. Journal of Environmental Management. V. (2002c). Órfão. Water Science and Technology. (2008)... The Journal of Physical Chemistry C. P. Pereira. P. Calvete. 150. Adsorption of cationic dyes from aqueous solutions by sepiolite. 87. & Benvenutti. 77... A. 5433–5440. & Healy. (2004). Sasikalaveni. L. Dias.. B. V. Journal of Hazardous Materials. Adsorption of eosin dye on activated carbon and its surfactant based desorption. Microporous and Mesoporous Materials. 1213– 1222. Armagan. C.. Sarma. C. Desalination.. Özcan.. P.. 703–712. Cardoso. 64–69. 2. J. Pavan. Journal of Hazardous Materials. E. P.. Removal of methylene blue from aqueous solution by dehydrated wheat bran carbon. A. Pavan. (2009). Decolorization of textile dyes and their effluents using white . T. G.. Mechanism of dye wastewater color removal by magnesium carbonate-hydrated basic. J. Journal of Environmental Management. J. 29–33. (2006)... (2008a).. C. S. F. (2009). E.. 256– 266.. M. S. T. G. Jute stick powder as a potential biomass for the removal of Congo red and rhodamine B from their aqueous solution. Vaghetti. I. Senthilkumar. J.. B. (2007). ˘ Ozdemir. P. Electrodeposited mesoporous ZnO thin films as efficient photocatalyst for the degradation of dye pollutants. Sarma. (2008).. (1976). Remediation of dyes in textile effluent: A critical review on current treatment technologies with a proposed alternative... T... & Wongchaisuwan. Environment International. Industrial & Engineering Chemistry Research. corncob and barley husk.. E. Erdem. C. Influence of particle size and salinity on adsorption of basic dyes by agricultural waste: Dried Seagrape (Caulerpa lentillifera). J. I. 221– 230. & Viraraghavan. K.. Dias. J. O.. et al. 2920– 2925. S. Das. 299– 301.. (2005). M. & Figueiredo.. & Otero. Removal of dyes from a synthetic textile dye effluent by biosorption on apple pomace and wheat straw.. Robinson.. 78–82. (2004).. Dyes and Pigments. (2006). Clay minerals as photochemical reaction fields. Porkodi. & Zhu. 1. & Juang. C. Zhang. Hsu. 274. C.. Pokethitiyook.equilibrium isotherm analyses.. H. & Subburaam. S. Hanna. Adsorption of a cationic dye (methylene blue) onto spent activated clay. P. 147. 37. Adsorptive removal of methylene blue by tea waste. & Allen. & McKay... Journal of Colloid and Interface Science. P. N. M. V. 22. & Erasmus. (2001). S. B.194 rot fungi. & Shukla. & Hameed. Varadarajan. A. H. Waranusantigul. H. H. P. 39. M. Photocatalytic degradation of C. G. Shukla. Wang.. Kyriakides. 979–985. W.. Adsorption of acid dyes on chitosan. Water Research. C. Tseng. Waste Management.. M. 28. & McKay. Basic Violet 10 using TiO2 catalysts supported by Y zeolite: An investigation of the effects of operational parameters.. 97. W. C.. (2003). Water Research. R. K. Zydowicz. Journal of Hazardous Materials. K. Lee. 41. M. & Ramsay. Removal of a cationic dye from aqueous solutions by adsorption onto bentonite clay. Boyjoo. N. (2001). M. S. The adsorption of basic dyes from aqueous solution on modified peat. Liquid-phase adsorption of dyes and phenols using pinewood-based activated carbons. T. 225.. Margrave. Sawada. 424– 429. 51–58. Y. C. Carbon. Removal of dyes from aqueous solution using fly ash and red mud. Z.I. Tamai. Lee. Sun. 487–495. Vachoud. Dyes and Pigments. Y. (2000). Weng. & Hsieh. (2007). & Rukanuzzaman.. 355–362. Preparation of activated carbon using low temperature carbonisation and physical activation of high ash raw bagasse for acid dye adsorption. 111–120.. 1020–1027. Applied Clay Science.. 1618–1625. L. Senthilkumaar. Kalaamani. Adsorption of dissolved reactive red dye from aqueous phase onto activated carbon prepared from agricultural waste.. L. Water Research. S. The role of sawdust in the removal of unwanted materials from water. H. Evaluation of the use of modified coal ash as a potential . (2007). Kinetics of basic dye (methylene blue) biosorption by giantduckweed (Spirodela polyrrhiza). Wang. Bioresource Technology. L.. J. F. Sorption and desorption studies on chitin gels. J. M. Z. Adsorption of basic dye using activated carbon prepared from oil palm shell: Batch and fixed bed studies. B95.. (2001). Juang. H. 273. Experimental study and modeling of basic dye sorption by diatomaceous clay. Choueib.. Desalination. Environ Monit Assess (2011) 183:151–195 Uddin. V. Cheung. L. F. C. Wang. & Kadirvelu. Strong. S. L. Lyu. (2004). 24. R. & Yang. Adsorption characteristics of methylene blue from aqueous solution by sludge ash. 56. F. S... Dyes and Pigments. Tseng. Lin. 45. F.. & Pan. Journal of Colloid and Interface Science. Journal of Hazardous Materials. R.. L. C. 58. Y. K. & Tutunji. Sasaki. & Pan. Adsorption of methylene blue onto jute fiber carbon: Kinetics and equilibrium studies. African Journal of Biotechnology.resin particle. C. Effects of acidic treatment of activated carbons on dye adsorption. 144. Colloids and Surfaces A.. T. (2002). S. G.. K. Lee. M. A. Mahmud. Environmental Pollution. 37. (2004). (2008). & Takagi. Wesenberg. R. Sun... Wang. 76. J. Biotechnology Advances. C. Varadarajan. M.. I. Woolard. Y. R. The evaluation of white rot fungi in the decoloration of textile dyes. 63. Journal of Hazardous Materials. J. (2003). J. (2008). R. D. L. (1987). Swamy. Y.. 493–501.. 284. Chien. S. Adsorption characteristics of Congo red onto the chitosan/ montmorillonite nanocomposite. 93–101.. Kruatrachue. 164. 75. (2005). Shawabkeh. 6. 129– 138. 39. Chemosphere. W. 21. Islam. (2007). P. Chemosphere. (2008). 695– 704. Y. E. Adsorption of acid dye onto activated carbons prepared from agricultural waste bagasse by ZnCl2 activation. T. A. Chemosphere. H. Physical and chemical properties and adsorption type of activated carbon prepared from plum kernels by NaOH activation. C. Journal of Hazardous Materials. Wong... A. Adsorption behavior of direct dye on cotton in non-aqueous media. Process Biochemistry. S.. (2002). 14. Cheung... (2007).. D. & Wang. & Ayyaswami. (2006).. 161–187. A. F. S. J.... 113– 130. A. Szeto.. 154–162. Chang. M. Dye adsorption on mesoporous activated carbon fiber obtained from pitch containing yttrium complex. M. Tan. C.. (1999). 1535–1544. Valix. A. C. & Huang. 105–110. A.. N... Wang. Tahir. J.. (2005). 53–60. Senthilkumaar. Orange peel as an adsorbent in the removal of acid violet 17 (acid dye) from aqueous solutions. P. Use of peat in water pollution control: A review.. W. H. K.. 983–989. (2006). Dubey. Weng. & Domard.. S. Ahmad. 306–314.. Adsorption of basic dyes onto montmorillonite. 37. Walker. M. Viraraghavan. & Rauf. Tsai. Canadian Journal of Civil Engineering. T. C. I. A. Journal of Photochemistry and Photobiology C: Photochemistry Reviews. 385–392... International Journal of Biological Macromolecules. 817–824. 1842–1848. A. 125. L. (1999).. R. T. Journal of Hazardous Materials. 24. 2081– 2089. & Yasuda. (2003)... Y. Enzyme and Microbial Technology.. 37–40. & Ueda.. & Zhu. G.. Carbon. 147. Q. Sivaraj. T. Kinetics of a reactive dye adsorption onto dolomitic sorbents. 80–86. & Upatham. S. (2003). M. 230–233. Shichi. & Subbhuraam. White-rot fungi and their enzymes for the treatment of industrial dye effluents. S. 137–152. Yoshida. P. Namasivayam... & Juang... 130–137. (2003)... F... Wu. & Agathos. 13–28. A.. (2003). (2003). S. R. Hansen. C. Porkodi. and bead. Zhao. Enhanced abilities of highly swollen chitosan beads for color removal and tyrosinase immobilization. M. 0437– 0440. R. Tseng. Zhi-yuan. B. 419– 424. (1999). 287–302. F. R.Environ Monit Assess (2011) 183:151–195 sorbent for organic waste streams.. Kinetic modeling of liquid-phase adsorption of reactive dyes and metal ions on chitosan. B81. Journal of Hazardous Materials. M. Tseng. R. Wu. Tseng. 30– 33. Water Research. & Juang. F. (2000). Wu. (2008). 69. 73. 35. & Juang. 1159–1164. & Liu. R. . Pore structure and adsorption performance of the activated carbons prepared from plum kernels. 82. R. 63–75. (2001a). F. (2008). Youssef. Adsorption behavior of methylene blue on halloysite nanotubes. Y.. Kinetics and Mechanism of the adsorption of methylene blue onto ACFs. R. Applied Geochemistry.. Adsorption of acid dyes by cellulose derivatives.. Tseng.types of chitosans prepared from fishery wastes. (1993). & Juang. Microporous and Mesoporous Materials.. Journal of China University of Mining and Technology. (2001b).. 17. Wu. Journal of Hazardous Materials. 195 Wu. F. & Juang. 112. Journal of Hazardous Materials.. Comparative adsorption of metal and dye on flake. P. American Dyestuf f Reporter. R.. 167–177. 18.. 613–618. R. Further reproduction prohibited without permission.Reproduced with permission of the copyright owner. .