August 28, 2009 [PROBLEM SET FROM R.CHANG TEST BANK] Chapter 16 Acid-Base Equilibria and Solubility Equilibria Student: ___________________________________________________________________________ NOTE: A table of ionization constants and Ka's is required to work some of the problems in this chapter. 1. In which one of the following solutions will acetic acid have the greatest percent ionization? A. B. C. D. 2. 0.1 M CH3COOH 0.1 M CH3COOH dissolved in 1.0 M HCl 0.1 M CH3COOH plus 0.1 M CH3COONa 0.1 M CH3COOH plus 0.2 M CH3COONa Which one of the following is a buffer solution? A. B. C. D. E. 0.40 M HCN and 0.10 KCN 0.20 M CH3COOH 1.0 M HNO3 and 1.0 M NaNO3 0.10 M KCN 0.50 M HCl and 0.10 NaCl 3. Which one of the following combinations cannot function as a buffer solution? A. B. C. D. E. HCN and KCN NH3 and (NH4)2SO4 HNO3 and NaNO3 HF and NaF HNO2 and NaNO2 4. Which of the following is the most acidic solution? A. B. C. D. E. 0.10 M CH3COOH and 0.10 M CH3COONa 0.10 M CH3COOH 0.10 M HNO2 0.10 M HNO2 and 0.10 M NaNO2 0.10 M CH3COONa www.kau.edu.sa/aasiri2 1 August 28, 2009 [PROBLEM SET FROM R. CHANG TEST BANK] 5. Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium benzoate (C6H5COONa). [Ka = 6.5 × 10-5 for benzoic acid] A. B. C. D. E. 6. 3.97 4.83 4.19 3.40 4.41 A solution is prepared by mixing 500. mL of 0.10 M NaOCl and 500. mL of 0.20 M HOCl. What is the pH of this solution? [Ka(HOCl) = 3.2 × 10-8] A. B. C. D. E. 4.10 7.00 7.19 7.49 7.80 7. Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 × 10-4] A. B. C. D. E. 0.97 3.10 4.40 3.70 4.30 8. Calculate the pH of a solution that is 0.410 M in HOCl and 0.050 M in NaOCl. [Ka(HOCl) = 3.2 × 10-8] A. B. C. D. E. 0.39 3.94 6.58 7.49 8.40 9. Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 × 10-4] A. B. C. D. E. 0 3.0 3.7 4.4 5.0 www.kau.edu.sa/aasiri2 2 2 × 10-8) NaNO2/HNO2 (Ka = 4.0 . B.+ OCl.3? A. E.5 pH 6. C. What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution? A.pH 9.→ HOCl HOCl → H+ + OClH+ + HOCl → H2OCl+ HCl + HOCl → H2O + Cl2 12.NaOCl buffer effective? A.00 ± 0. D.→ HOCl + O2Na+ + HOCl → NaCl + OHH+ + HOCl → H2 + OClNaOH + HOCl → H2O + NaCl 13.18 0. B.0 14.sodium acetate buffer solution with a pH of 4.August 28. 0. CH3COONa/CH3COOH (Ka = 1. C. D. Over what range of pH is a HOCl .edu.pH 9. B.+ HOCl → H2O + OClOH.pH 8. E.02. which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9. B. E.0 .5 . Assuming equal concentrations of conjugate base and acid. C. C.84 1. pH 2.5 pH 1. D.sa/aasiri2 3 . OH. H+ + H2O → H3O+ H+ + OCl.2-9. D.10 11. D.pH 14.pH 4.6 × 10-10) NaOCl/HOCl (Ka = 3. What molar ratio of CH3COOH to CH3COONa should be used? A.5 . Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer? A.kau.19 5. 2009 [PROBLEM SET FROM R.8 × 10-5) NH3/NH4Cl (Ka = 5. Consider a buffer solution prepared from HOCl and NaOCl. C.5 × 10-4) NaCl/HCl www. E.50 0. You are asked to go into the lab and prepare an acetic acid .0 pH 7.5 pH 6. E.5 . B. CHANG TEST BANK] 10. D.84 5.07 18.20% 2. C. D. You have 500.56 4.0 × 10-4.0 mL of a buffer solution containing 0. B. Assuming equal concentrations of conjugate base and acid.0% 20% 19.5 × 10-4) NaCl/HCl 16. E.8 × 10-5] A.30 M sodium acetate (CH3COONa). B. 4.50 M HCNO and 0.00 M NaOH solution? [Ka = 1. CHANG TEST BANK] 15.30 M acetic acid (CH3COOH) and 0. You have 500. C. B. E.92 5. E.0 mL of 1.2 × 10-8) NaNO2/HNO2 (Ka = 4.6-4.2 M HCl 0. Calculate the percent ionization of cyanic acid. which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.edu. D.41 4.kau.20 M acetic acid (CH3COOH) and 0.6 × 10-10) NaOCl/HOCl (Ka = 3. D. 2009 [PROBLEM SET FROM R.1 M CH3COOH dissolved in 0.10 M NaCNO. What will the pH of this solution be after the addition of 20. C. In which one of the following solutions will acetic acid have the greatest percent ionization? A.2 M CH3COONa www.August 28.10% 0. CH3COO2Na/CH3COOH (Ka = 1. Ka = 2. 4.74 4.0 mL of 1.0 mL of a buffer solution containing 0.1 M CH3COONa 0. C.1 M CH3COOH plus 0. C.1 M CH3COOH plus 0. 0. B.1 M CH3COOH 0.8 × 10-5) NH3/NH4Cl (Ka = 5. E.07 17.1 M CH3COOH dissolved in 0. B. E.1 M HCl 0. A. D.20 M sodium acetate (CH3COONa).8 × 10-5] A.56 4.71 4.8? A. What will the pH of this solution be after the addition of 20. 0. in a buffer solution that is 0.02% 0.65 4.00 M NaOH solution? [Ka = 1.sa/aasiri2 4 . For which type of titration will the pH be basic at the equivalence point? A.10 M HNO2 (nitrous acid. B.+ PO43-. www.+ HPO42-. the indicator used. C.edu.August 28. E.17 3. C. B. Ka = 4. B.10 M KOH solution. a buffer with a pH = 9 can best be made by using A. B. all of the these none of these 23. pure NaH2PO4-. the self-ionization of H2O. strong base. a strong acid and a strong base. hydrolysis of the salt formed. B.kau. Strong acid vs. a strong acid and a weak base. a weak acid and a weak base (where Ka equals Kb). C. Weak acid vs. D. D. Strong acid vs. 2. the initial concentration of the standard solution. H2PO4. D. strong base. CHANG TEST BANK] 20.sa/aasiri2 5 .5 × 10-4) is titrated with a 0. H2PO4.00 24. C.35 2. weak base. The pH at the equivalence point of a titration may differ from 7. After 25.00 mL of 0.0 due to A. the pH in the titration flask will be A. On the basis of the information below. 22. E. E. the initial pH of the unknown.00 mL of the KOH solution is added. 21.41 1. A titration of an acid and base to the equivalence point results in a noticeably acidic solution.48 7. D.+ PO43-. HPO42. 50. C. 2009 [PROBLEM SET FROM R. a weak acid and a strong base. D. It is likely this titration involves A. C.0 27.0 29.0 mL of 0.10 M HCN (Ka = 4. What color would a methyl red solution have at pH = 7. D.10 M HCN (Ka = 4.0 mL of 0. C. B.15 8.0 11.3 × 10-6. D.0 6. B.0 12.87 4.0 6.00 11.kau. CHANG TEST BANK] 25. Calculate the pH of the solution resulting from the addition of 10. What is the pH at the equivalence point in the titration of 100 mL of 0. Methyl red is a common acid-base indicator. A.0 7. E. E.edu.8 × 105 ). Calculate the pH at the equivalence point for the titration of 0. 2009 [PROBLEM SET FROM R. 2. B. 1. D. E.10 M NaOH? A.12 7. B. D. C. 5.0 13. B. It has a Ka equal to 6.0 28. D.9 × 10-10) solution. E. C. green red blue yellow violet www. A. 3.91 13.9 × 10-10) with 0.20 M HCl with 0. Its un-ionized form is red and its anionic form is yellow.10 M NaOH? A.20 M NH3 (Kb = 1.10 M HCl with 0. C. What is the pH at the equivalence point in the titration of 100 mL of 0.12 26. E.8? A.10 M NaOH to 50.0 8.85 9.0 7.sa/aasiri2 6 .98 5.71 5.August 28. 4 × 10-4).4g 2.16 M 2.10. No. What mass of ammonium nitrate must be added to 350.3g 0.edu. D. C. 0. B.00? (Kb(NH3) = 1. 2009 [PROBLEM SET FROM R. because Q < Ksp.0 mL of a hydrofluoric acid solution of unknown concentration is titrated with 0.050 M 0. mL of a 0. (Ka(HF) = 7. What mass of sodium fluoride must be added to 250.072 M 0. For PbCl2 (Ksp = 2.100 M NaOH. 0.49 g 1.200 M NaOH. E.sa/aasiri2 7 .50? (Ka(HF) = 7.23 M 34. C.100 M HF solution to give a buffer solution having a pH of 3. D. www. mL of a 0.3g 32.1 × 10-4) A. 7.0 × 10-2 M Pb(NO3)2 is added to 400 mL of 9.4M 0.39 M 0. because Q = Ksp.0 mL of the base solution has been added. E.10 L of 3. the pH in the titration flask is 5.150 M solution of ammonia to give a buffer having a pH of 9.0 ml of an acetic acid of unknown concentration is titrated with 0. because Q > Ksp. B. E. E. No.022 M 0. C. C. Yes.5g 3. Yes.August 28. B.00. the pH in the titration flask is 3. D. B.0 mL of the base solution has been added. D.015 M 33.11 M 0. will a precipitate of PbCl2 form when 0.1 × 10-4) A. CHANG TEST BANK] 30. What was the concentration of the original acetic acid solution? (Ka(CH3COOH) = 1. 0.75 g 31. because Q < Ksp. 25.8 × 10-5) A.kau. 40. After 20.0 × 10-2 M NaCl? A. What was the concentration of the original hydrofluoric acid solution. B.6 g 2.27 M 0.4g 5.8 × 10-5) A.4g 11g 3. C. D. After 20. C. 2009 [PROBLEM SET FROM R. Calculate the Ksp value for this compound.6 × 10-9 7.2 × 10-8 2.0 × 10-16 1. E. E.8 × 10-4 mol/L.2 × 10-6 1.28 × 10-2 mol/L. What is the solubility product for lead(II) iodide? A.28 × 10-2 4.5 × 10-3 www. E.9 × 10-6 1.edu.4 × 10-6 1.8 × 10-14 37. E.0 × 10-3 38.sa/aasiri2 8 . 7.kau.5 × 10-4 5. C.4 × 10-6 3. D.0011 g/100 mL at 20oC. E.5 × 10-5 1. C.064 g/100 mL at 20oC. CHANG TEST BANK] 35. D. B.1 × 10-11 2. The molar solubility of manganese(II) carbonate is 4. D.8 × 10-11 2. B.4 × 10-3 36. B. The molar solubility of magnesium carbonate is 1. A. What is Ksp for this compound? A.August 28. The solubility of lead(II) iodide is 0.3 × 10-7 3. B. 4. What is Ksp for this compound? A. C.6 × 10-4 2. D. The molar solubility of tin(II) iodide is 1.1 × 10-8 3.2 × 10-6 M.2 × 10-6 8.7 × 10-12 1.5 × 10-6 1. 1. D. 1.1 × 10-6 39. The solubility of strontium carbonate is 0. B. 8.6 × 10-4 1. What is Ksp for this compound? A.8 × 10-4 3. C. 2 × 10-1 M 1.3 × 10-26.6 × 10-3 M 1. 1. 1. A. D.sa/aasiri2 9 .1 × 10-5 mol/L 2. A. The Ksp for silver(I) phosphate is 1.2 × 10-3 M 1.0 × 10-5 mol/L.kau. 5.5 × 10-7 M 2. Calculate the molar solubility of barium sulfate.6 × 10-6 M 42.6 × 10-11.2 × 10-3 M 6.0 × 10-15 41. C.5 × 10-11 mol/L 1. B. CHANG TEST BANK] 40. 2009 [PROBLEM SET FROM R.4 × 10-14 2.2 × 10-10 mol/L 43. The solubility product for calcium phosphate is Ksp = 1. A. E. D.1 × 10-10. The solubility product for chromium(III) fluoride is Ksp = 6.1 × 10-5 mol/L 1. Calculate the molar solubility of silver(I) phosphate. Calculate Ksp for lead(II) iodate.6 × 10-5 M 2. What is the molar solubility of calcium phosphate? A. E.8 × 10-1 M 44.8 × 10-18.3 × 10-26 M 1. B.0 × 10-5 4. D. C.6 × 10-13 4.7 × 10-5 M 7. B.6 × 10-11 M 2. C. The solubility product for barium sulfate is 1.1 × 10-10 mol/L 2.August 28.6 × 10-6 M 4.6 × 10-6 M www. The molar solubility of lead(II) iodate in water is 4. E.1 × 10-5 M 3.6 × 10-6 M 6. 1. 1.6 × 10-9 6. What is the molar solubility of chromium(III) fluoride? A. C. C. B. D.edu. B. D. E. E. B.August 28. 2.9 × 10-2 M 1. CHANG TEST BANK] 45.0 × 10-5 mol/L 46. C. A.8 × 10-18. D.sa/aasiri2 10 . B. C. D.5 × 10-2 M 2.4 × 10-4. E. Determine the silver ion concentration in a saturated solution of silver(I) phosphate. C. E. 2009 [PROBLEM SET FROM R. D.1 × 10-5 M 3. E.4 × 10-4 mol/L 6. C. Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (Ksp = 1. E.0 × 10-5 M 2. Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp = 8.4 × 10-4) solution.8 × 10-5 M 48.7 × 10-5 M 1.2 × 10-2 mol/L 7.0 × 10-4 M 8. A.1 × 10-12). 2. D. D. E. C. B.2 × 10-1 M 7. 1.1 × 10-13 M 4.4 × 10-2 M 3. The Ksp value for lead(II) chloride is 2.4 × 10-4 M 4.9 × 10-2 mol/L 6. What is the molar solubility of lead(II) chloride? A.3 × 10-4 M 2.5 × 10-4 M 1. B.7 × 10-3 mol/L 3.6 × 10-5 M 2.0 × 10-2 M 1. 5.8 × 10-2 M www. The Ksp for silver(I) phosphate is 1. B.kau. 1. A.edu.8 × 10-4 M 3. Calculate the concentration of chloride ions in a saturated lead(II) chloride (Ksp = 2.4 × 10-5 M none of these 49.4 × 10-5).1 × 10-4 M 47. A. 10 M NaF in order to initiate a precipitate of magnesium fluoride. 2009 [PROBLEM SET FROM R.032 M 7. E. B.edu.4 × 107 M 6. C.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.2 × 10-3 M Pb(NO3)2 are added to 50. (For CrF3. Ksp = 6.9 × 10-8 M 1. D.9 × 10-9 M 6. Yes. 52.August 28. 7. Yes. Ksp = 6. B. B.7 × 10-7 M 6. the precipitate is NaNO3. the precipitate is Na2S. Yes.7 × 10-6 M 3. Will a precipitate form (yes or no) when 50.kau. the precipitate is PbS. D. E.9 × 10-9. Lowering the pH of the solution Adding a solution of Pb(NO3)2 Adding a solution of KI None of these—the Ksp of a compound is constant at constant temperature. the precipitate is Pb(NO3)2.4 × 10-6 M 51. (For MgF2. Which of the following would decrease the Ksp for PbI2? A. identify the precipitate. C.4 × 10-5 M 1.0 × 10-4 M Na2S? If so. E.0 mL of 2.023 M 0.7 × 10-6) solution. A. C. D. No.5 × 10-2 M 3. www.9 × 10-7 M 53. Yes.6 × 10-3 M 1. C.) A. D. B. D.7 × 10-8 M 2.sa/aasiri2 11 . A. Calculate the minimum concentration of Mg2+ that must be added to 0. a precipitate will not form. 0.) A. Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.0 mL of 1.9 × 10-10 M 54. CHANG TEST BANK] 50. Calculate the minimum concentration of Cr3+ that must be added to 0. 1.6 × 10-11.9 × 10-9 M 6. E. B. C. Will a precipitate (ppt) form when 300. Yes. Q > Ksp No. No. A. Yes. E.9 × 10-9) A. Yes. the ppt is NaNO3(s). Will a precipitate (ppt) form when 20. Yes. Yes. Q > Ksp No.9 × 10-3 M MgCl2 are added to 300. C. www. B. mL of 2. Will a precipitate of magnesium fluoride form when 300. and identify the precipitate if there is one.0 mL of 1. Yes. Q = Ksp Yes. Yes. 59. D. Yes. the ppt is NaNO3. Yes. Will a precipitate (ppt) form when 300. D.August 28. the ppt is AgI(s). the ppt is NaBr(s).9 × 10-9) A.edu. the ppt is Ba(NO3 )2.0 mL of 8. Q < Ksp 56. the ppt is AgNO3(s). C. No. Yes.4 × 10-4 M Na2CO3? A. E. B. Q = Ksp Yes. mL of 1. Q < Ksp No.sa/aasiri2 12 . mL of 5. 58. 2009 [PROBLEM SET FROM R. a precipitate will not form.2 × 10-3 M NaF? (Ksp (MgF2) = 6. Yes. a precipitate will not form.4 × 10-2 M NaF? (Ksp (MgF2) = 6. a precipitate will not form.0 × 10-5 M AgNO3 are added to 200. D. No. Yes. C. the ppt is NaI(s). Will a precipitate of magnesium fluoride form when 200. mL of 1. the ppt is AgNO3(s). B. B. D. B. C.kau. Q < Ksp 57. the ppt is BaCO3. the ppt is AgBr(s).0 × 10-5 M AgNO3 are added to 200. mL of 2. mL of 1. the ppt is NaNO3(s).5 × 10-9 M NaI? Answer yes or no.5 × 10-7 M NaBr? Answer yes or no. A.1 × 10-3 M MgCl2 are added to 500. Yes. Yes. mL of 1. and identify the precipitate if there is one.1 × 10-3 M Ba(NO3)2 are added to 80. C. mL of 2. E. CHANG TEST BANK] 55. Q < Ksp No. the ppt is Na2CO3. D. 105 M. C. B.150 M KI. D.33 M Na2CrO4 are added to 250 mL of 0. 1.sa/aasiri2 13 .27 × 10-8 M www.1 × 10-12) What is the concentration of the silver ion remaining in solution? A.00 mL of 12.August 28.0 M HCl.39 × 10-8. Yes. Yes.3 × 10-4 M.00 L of a 0.3% 12% 1. C.14 2.7 × 10-9] A. D. [Ag+] = 0. B.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1. D.4 × 10-10 1.54 × 10-7 M 6.] A. 3. [Ag+] = 2. D. To 1. E.060 M.3 × 10-5 63. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [Given: Kb(C5H5N) = 1.52% 0. C. Yes.00 L of a 0. What is the percentage ionization of the benzoic acid in the resulting solution? [Given: Ka(C6H5COOH) = 6.5 × 10-5] A. B. 3.edu.00 mL of 14. No.065% 62.3% 0. 61. [Ag+] = 1.100 M aqueous solution of the week base pyridine (C5H5N) is added 1. B. Which response has both answers correct? Will a precipitate form when 250 mL of 0.0 M NaOH.04 × 10-4 M 1. mL of 0. Find the concentration of Pb2+ ions in a solution made by adding 5.060 M. [Ag+] = 0.kau. To 1. 2009 [PROBLEM SET FROM R.12 M AgNO3? (Ksp(Ag2CrO4) = 1.1 × 10-5 0. C. Ksp = 1. CHANG TEST BANK] 60.00 g of lead(II) iodide to 500.18 × 10-7 M 1.52 × 10-4 M 9.9 × 10-6 M. E. E.2 × 10-7 4. [Ag+] = 0. E. [For PbI2. No. 29 × 10-4 M 6. D.0500 M sodium hydroxide should be added to 250. 2009 [PROBLEM SET FROM R. mL 340 mL 500. The solubility product constant for sodium carbonate at this temperature is A.200 M potassium hydroxide should be added to 300.] A.5 g of dissolved sodium carbonate per 100. B.32 × 10-10 M 2. C. 3. B.7 × 10-4] A. C. 79. CHANG TEST BANK] 64.125 M NaF. C. 316.16 × 10-10 M 2. 540 mL 420 mL 80.30. mL of 0. C. 3. 67.100 M HCOOH to obtain a solution with a pH of 4.90. D.edu.kau. E.2.2 × 10-3. The solubility product constant for sodium carbonate at this temperature is A. D.0790. [For CaF2. 32 mL 210mL 160mL 65mL 13mL www. 0. B. D.53 × 10-9 M 4.316.August 28. 36. 1.95 × 10-11.50? [Ka(HCOOH) = 1. Ksp = 3. E. 1. 0.8. C. A saturated sodium carbonate solution at 0°C contains 7. Find the concentration of calcium ions in a solution made by adding 3. E.34 × 10-5] A. mL of solution. mL 68. 0. E. 66. B.15 × 10-4 M 65. mL of 0. mL of solution.150 M propanoic acid (C2H5COOH) to obtain a solution with a pH of 5.25? [Ka(C2H5COOH) = 1. A saturated sodium carbonate solution at 100°C contains 45. What volume of 0. mL of 0.0 × 10-4.0.1 g of dissolved sodium carbonate per 100. B.50 g of calcium fluoride to 750. What volume of 0. D.sa/aasiri2 14 . E. 0. Ka1 = 4.August 28.75 M CH3COONa. Ka = 1.7 × 10-4) 72. What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid. CHANG TEST BANK] 69.4 × 10-8). 71.8 × 10-5) 70.2 × 10-7. www. Ka= 1. Calculate the pH of a solution that is 0. 73.edu. Ka1 = 4.77. Ka2 = 2. Ka2 = 2.kau. Write an equation showing the net reaction that occurs when a strong acid is added to a CO32-/HCO3buffer solution (for carbonic acid. Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3buffer solution (for carbonic acid.15 M CH3COOH and 0.sa/aasiri2 15 . Describe how to make a sodium formate (HCOONa)/formic acid (HCOOH) buffer that has a pH of 4. What is the effective pH range for a sodium acetate/acetic acid buffer? (For CH3COOH.2 × 10-7.4 × 10-8). 74. 2009 [PROBLEM SET FROM R. Calculate the percent ionization of formic acid in a solution that is 0.sa/aasiri2 16 . Calculate the percent ionization of formic acid in a solution that is 0.7 × 10-4) 77. Calculate the percent ionization of formic acid in a 0. if any. Write a net ionic equation for the reaction that occurs when a small amount of hydrochloric acid is added to a buffer solution containing NH4Cl and NH3 . (Ka = 1.August 28.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.010 M HCOOH and 0.010 M HCOOH solution.5 × 10-5) 79.20? (Ka(C6H5COOH) = 6. Explain the difference. www. 2009 [PROBLEM SET FROM R.kau. What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5. (Ka = 1.7 × 10-4) 78.edu.010 M HCOOH and 0. CHANG TEST BANK] 75.050 M HCOONa. Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH4Cl and NH3. (Ka = 1.7 × 10-4) 76. 80. 22 M NaOH. mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO) buffer having a pH of 4.kau. Calculate the pH at the equivalence point for the titration of 0. Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.80. (For CH3COOH.sa/aasiri2 17 . Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO2/HNO2 buffer. CHANG TEST BANK] 81. (Ka(HCNO) = 2.6 × 10-7.August 28. 2009 [PROBLEM SET FROM R. (Ka = 4.9 × 10-10 for HCN.0 × 10-4) www.8 × 10-5) 84. 83.22 M HCN with 0.) 85.25 M CH3COOH with 0.8? 86.edu. 82. Its un-ionized form is yellow and its conjugate base is blue.25 M NaOH. What color would a solution have at pH = 5. Calculate the pH at the equivalence point for the titration of 0. It has a Ka equal to 1. Describe how to prepare 500. Bromothymol blue is a common acid-base indicator. Ka= 1. edu. (Ksp (PbI2) = 1.050 M AgNO3. Ksp (AgI) = 8. mL of 0.0050 M Ag+. Ksp (AgI) = 8.3 × 10-17) What percent of Ag+ remains in solution at this point? 90.4 × 10-8. Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0. What is the maximum concentration of Ca2+ possible in a 0.sa/aasiri2 18 . 5.0 mL of 12 M NH3 is added to 500.0050 M Pb2+ and 0. 2009 [PROBLEM SET FROM R. (Ksp (PbI2) = 1. The Ksp of CaF2 is 4 × 10-11. Solid sodium iodide is slowly added to a solution that is 0.10 M NaF solution? 91. (Ksp (PbI2) = 1.4 × 10-8.3 × 10-17) Calculate the Ag+ concentration when PbI2 just begins to precipitate. Solid sodium iodide is slowly added to a solution that is 0. CHANG TEST BANK] 87.0050 M Ag+.3 × 10-17) What compound will precipitate first? 88. What concentration of silver ion will exist after equilibrium is established? (Kf for Ag(NH3)2+ = 1.4 × 10-8.August 28.kau. Ksp (AgI) = 8.5 × 107) www.0050 M Pb2+ and 0. 89.0050 M Ag+. Ksp( 0 K NH 5 (AgCl) = 1.050 mol NaCl( and 0. for Ag(CN)2 .kau. so th are bette solvents t hey er than water for insolubl f le substance such as Ca(OH)2.0 M NH3? (Kf for Ag(N 3)2 = 1. Will a pre 7 -10 + mL of 3. Kb for NH3 i 1.8 × 10-5. Kf = 1. × 10-2 M.) 4.001 M in Fe3+? (For Fe(O 3.6 × 10 . -10 21 r (For AgCl. Ksp = 1. 0 (s) 50 NO d 92.10 M C 3COONa.0 .) 95.8 × 10-36. 2009 [PR . Calculate the equilibr rium consta Kc for th following overall rea ant he g action.05 mol AgN 3(s) are dissolved in 500. × 10 ) .0 × 10 ) AgCl(s) + 2CN-(aq) Ag(CN)2-(aq) + Cl-(aq) A ) www w. Ide es entify two re eactions tha added tog at. Then dete ermine Kc fo the overa reaction.0 is Ca(O 2(s) + 2N 4+ (aq) OH) NH Ca2+(a + 2NH3( aq) (aq) + 2H2O 96. Will Fe(O 3 precipi OH) itate from a buffer solu ution that is 0.6 93. give the overall reaction be e l elow. if the H nd CH solution is also made to be 0.sa a/aasiri2 19 .60 M CH3COOH an 0. CHA M ANG TEST BANK] ecipitate of A AgCl form when 0.5 × 10 . The conce entration of Mg2+ in seawater is 5. roxide concentration is needed to r remove 2+ -11 90% of th Mg by p he precipitation (For Mg n? g(OH)2. or all 5 (Ksp for C Ca(OH)2 is 4 × 10-8.edu.August 28.) s e 1 OH) ) 94.2 × 10 . ROBLEM SET FROM R. Ksp = 1. gether. Ksp = 6. Ammoniu chloride solutions a slightly a um are acidic. What hydr f . The solub bility of Ba(NO3)2 is 13 g/L at 0oC. the he www w. mL samp of ple the water and titrates this sample with a .050 M NaOH solution. what is the molar of rity acid in the rainwater? e ? 100. How m 30.kau.4 milliters of 0. mL s acid prese is sulfuro acid.edu.0122 M NaOH.August 28.3 × 10 . 2009 [PR . Estimate t pH of th lake. mL of the NaOH solution. for A AgI( + 2NH3(a (s) aq) Ag(NH3)2+(a + I-(aq) A aq) 98. 97.sa a/aasiri2 2 20 . Kf = 1. A sample of rainwate collected near a lead smelter is a er d analyzed fo acid conte Experim or ent. Assuming that the he r zed 4 t 100. N e H Neutralizatio of the lak water req on ke quires f 40. He o e d the he obtains a 200.5 many moles of dissolved salt are pr resent in 4. CHA M ANG TEST BANK] rium consta Kc for th net reacti shown b ant he ion below. Ksp = 8.5 × 10 . A wildlife biologist is interested in testing t pH of th water in a lake.) (For AgI. ments show that a w sample of th rainwater is neutraliz by 22. w ent ous which resulte from the reaction of SO2 with w ed f water. Calculate the equilibr -17 7 + Ag(NH3)2 .0 L of a 0 o saturated solution of Ba(NO3)2 a 0 C? at 99. ROBLEM SET FROM R. Ag+.sa/aasiri2 21 . basic. A wildlife biologist is interested in testing the pH of the water in a lake. A wildlife biologist is interested in testing the pH of the water in a lake. What is the copper(I) ion concentration in this system at equilibrium? www. Which compound will precipitate first? 104. The formation constant of the complex ion Cu(CN)32. mL sample of the water and titrates this sample with a .August 28.010 M each in Cu+.9 × 10-7.kau. mL sample of the water and titrates this sample with a . 2009 [PROBLEM SET FROM R. m. 103.0 × 10-4 M CuNO3 is added to 50.3 km wide.edu. He obtains a 200. and 2. mL of the NaOH solution. 1.8 × 10-10. The Ksp's for CuCl. and AuCl are 1.0 × 10-13. AgCl. A 50. NaCl is added slowly to a solution that is 0. Neutralization of the lake water requires 40. estimate how many moles of acid are present in the lake water. He obtains a 200.050 M NaOH solution. or neutral? 102.0 M NaCN. and has a depth of 10. Neutralization of the lake water requires 40. CHANG TEST BANK] 101. mL of the NaOH solution? If the size of the lake can be described as 1. respectively.0 × 109.0 mL sample of 2. and Au+.050 M NaOH solution.0 mL of 4.1 km long by 2. Is the lake acidic.is 1. The percent ionization of a weak acid HA is greater in a solution containing the salt NaA than it is in a solution of the weak acid only.150 M solution of ammonia at 25°C. mL of 0.8 × 10-5. How many moles of NaF must be dissolved in 1. 109. CHANG TEST BANK] 105. 107.8 × 10-5. Determine the pH of a solution prepared by adding 0. The solubility product constant for magnesium hydroxide is 1. True False www.150 M solution of ammonia at 25°C. 108.kau.0 × 10-6 M? (Ksp of PbF2 at 25 °C = 4. 2009 [PROBLEM SET FROM R.8 × 10-5.sa/aasiri2 22 . If 0. the base ionization constant for NH3 is 1. the base ionization constant for NH3 is 1.150 M ammonia. Determine the percentage ionization of a 0.0 × 10-8) 106. the base ionization constant for NH3 is 1. At 25°C. mL of 0.0500 mol of solid ammonium chloride to 100. At 25°C.edu. Determine the hydroxide ion concentration in a 0.August 28.150 M ammonia.0800 mole of solid magnesium chloride is dissolved in a solution prepared by adding 0.] 110. the base ionization constant for NH3 is 1.0500 mol of solid ammonium chloride to 100.5 × 10-11. At 25°C.8 × 10-5. will a precipitate of magnesium hydroxide form? [Assume the volume of the solution is unchanged. At 25°C.00 liter of a saturated solution of PbF2 at 25°C to reduce the [Pb2+] to 1. All indicators are weak acids that are one color in acidic solution and another color in basic solution.20 M CH3COOH and 0.kau.August 28.sa/aasiri2 23 . CHANG TEST BANK] 111. 2009 [PROBLEM SET FROM R. True False 112. The pH of a solution that is 0.edu. A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution. True False www.20 M CH3COOH solution. True False 113. True False 114. For any conjugate acid-base pair.20 M CH3COONa should be higher than the pH of a 0. it is true that Kb = KaKw. C 5. 2009 [PROBLEM SET FROM R.C 23.sa/aasiri2 Page 1 . CHANG TEST BANK] Chapter 16 Acid-Base Equilibria and Solubility Equilibria Key 1.C 4.C 9.A 25.D www.C 19.kau.C 26.edu.D 11.A 3.August 28.E 17.B 10.C 14.E 8.A 20.C 27.B 12.B 15.A 16.C 7.B 18.E 22.C 21.A 6.B 24.A 13.A 2. B 51. 2009 [PROBLEM SET FROM R.B 42.B 58.B 47.A 39.A 55.A 34.C 49.C 40.E 53.A 32.D www.August 28.A 44.D 38.D 37.C 41.B 43.kau.D 46.B 29.D 31. CHANG TEST BANK] 28.C 33.C 45.D 30.B 35.E 50.edu.A 57.A 36.sa/aasiri2 Page 2 .E 48.B 56.D 52.C 59.C 54. + H2O 75. the addition of formate suppresses the ionization of formic acid by shifting the ionization equilibrium towards the un-ionized acid.77 72.5.and HCO3.→ CO32.0 mol HCOONa to 1. 77.13% 76.6 mol NaCNO to 1.August 28.D 62.A 61.5.7-5.11.+ HNO2 → NO2.Dissolve amounts of the two compounds equal to a molar ratio of 12.+ NH4+ → NH3 + H2O 81.0 mol HCOOH.92 84.8.B 65.0 mol HCNO in enough water to yield 500.Yellow 86.3.7 70.A 66. mL of solution.+ H+ → H2CO3 74.sa/aasiri2 Page 3 .0 × 10-14 M 89.4%.4 × 10-9 M www.1.H+ + NO2.C 69.kau.Prepare a solution having a molar ratio of 10.44 71.+ H2O 83.A 63.E 67.B 68.C 64.edu.3.18 85.+ H+ → HCO3.3.H+ + NH3 → NH4+ 80. 2009 [PROBLEM SET FROM R.34% 78.10.3 79.AgI 88.OH.+ OH.HCO3. 87. 73. CHANG TEST BANK] 60.0.OH.→ HNO2 82.CO32.0 × 10-9 % 90. 1% 108.1.2 101.T TRUE FALSE 112.T Ca2+(aq) + 2OH-(aq) 2NH3(aq) + 2H2O H www.2 × 108 mol 2.8 8. C Ca(OH)2(s) 2NH4+(aq) + 2OH-(a aq) Kc = 120 96.kau.August 28.1 × 10-3 M 107.1 × 10-14 M 1.0 moles 99.37 × 10-3 M 2 100.2 × 10-9 98.edu.2.5 103. 1.73 1.a acidic 102. 1. 2009 [PR .A AuCl 104.4.20 1.F TRUE 114. ROBLEM SET FROM R.8.3 105.sa/aasiri2 Page 4 .Yes 93.0 mol 0. CHA M ANG TEST BANK] 91.Y Yes FALSE 110.4 × 10-6 M 92.Yes 94.1 109.F 111.6 106.9 × 10-5 M 95.F FALSE 113.6 × 1011 97.
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