# CH302 Exam 4 Practice Problems (buffers, titrations, Ksp)

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1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) 1 Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO 2 H K a = H 2 CO 3 K 1 = HNO 2 K a = K 2 = HOCl K a = (COOH) 2 K 1 = HF K a = K 2 = HCN K a = CH 3 COOH K a = H 2 SO 4 K 1 = very large C 6 H 5 NH 2 K b = K 2 = NH 3 K b = HOBr K a = Refer to Equilibrium Constants. What is the [H 3 O + ] of a solution that is M in HOCl and M in NaOCl? a M d M b M e M c M 2. Refer to Equilibrium Constants. A solution is made by combining 500 ml of 0.10 M HF with 300 ml of 0.15 M NaF. What is the ph of the solution? a d b e c Refer to Equilibrium Constants. A solution that is 0.20 M in NH 3 is also 0.30 M in NH 4 Cl. What is the [OH - ] in this solution? a M d M b M e M c M 4. Refer to Equilibrium Constants. What is the ph of a solution that is M in aqueous ammonia and M in NH 4 Cl? a d b e c Refer to Equilibrium Constants. Which one of the following combinations is not a buffer solution? a. NH 3 - (NH 4 ) 2 SO 4 d. NH 3 - NH 4 Br b. HBr - KBr e. CH 3 COOH - NaCH 3 COO c. HCN - NaCN 6. Refer to Equilibrium Constants. Which response contains all the statements true of buffer solutions, and no false statements? I. A buffer solution could consist of equal concentrations of ammonia and ammonium bromide. II. A buffer solution could consist of equal concentrations of perchloric acid, HClO 4, and sodium perchlorate. III. IV. A buffer solution will change only slightly in ph upon addition of acid or base. In a buffer solution containing benzoic acid, C 6 H 5 COOH, and sodium benzoate, NaC 6 H 5 COO, the species that reacts with added [OH - ] is the benzoate ion.

2 2 a. II, III, and IV d. I and III b. I and IV e. another combination c. II and III 7. Refer to Equilibrium Constants. A solution is initially M in HOCl and M in NaOCl. What is the ph if mol of solid NaOH is added to 1.00 L of this solution? Assume no volume change. a d b e c Refer to Equilibrium Constants. What is the ph of a solution that is 0.15 M in HOCl and 0.25 M NaOCl after mol HCl per liter has been bubbled into the solution? a d b e c Refer to Equilibrium Constants. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 M in CH 3 COOH and 0.10 M in NaCH 3 COO, how will the ph of the solution change? a. The ph increases from 4.74 to d. The ph decreases from 4.74 to b. The ph decreases from 7.00 to e. The ph increases from 4.74 to c. The ph does not change. 10. Refer to Equilibrium Constants. What is the [H 3 O + ] of a solution resulting from the mixture of 10.0 ml of M KF with 20.0 ml of M hydrofluoric acid, HF? a M d M b M e M c M 11. Refer to Equilibrium Constants. It is desired to buffer a solution at ph = What molar ratio of CH 3 COOH to NaCH 3 COO should be used? a. 1.2/1 d. 2.8/1 b. 0.8/1 e. 6.2/1 c. 0.12/1 12. Refer to Equilibrium Constants. One of the following buffer solutions has poh = Which one? Hint: Solve the general problem rather than 5 specific problems. a M NH 3 and 0.10 M NH 4 Cl d M NH 3 and 0.20 M NH 4 Cl b M NH 3 and 0.20 M NH 4 Cl e M NH 3 and M NH 4 Cl c M NH 3 and 0.10 M NH 4 Cl 13. Refer to Equilibrium Constants. If 0.10 mole of HCl is bubbled into 1.0 liter of 0.25 M NH 3 solution, what will be the ph of the resulting solution? a d b e c Refer to Equilibrium Constants. The nonionized form of an acid indicator is yellow, and its anion is blue. The K a of this indicator is What will be the approximate ph range over which this indicator changes color? a. 3-5 d b. 4-6 e c Refer to Equilibrium Constants. The equivalence point of the titration of an unknown base with HCl is at ph = What would be the K a for the best choice of an indicator for this titration? a d b e c. 10-8

3 3 16. Refer to Equilibrium Constants. What is the ph at the point in a titration at which ml of M KOH has been added to ml of M HBr? a d b e c Refer to Equilibrium Constants. Which titration curve could describe the titration of a solution of HCl by addition of a solution of KOH? a. b. c. d. e. 18. Refer to Equilibrium Constants. Which indicator could be used to titrate aqueous NH 3 with HCl solution? Acid Range Color ph Range Basic Range Color a. pink yellow b. blue yellow c. yellow purple d. colorless red e. none of these indicators 19. Refer to Equilibrium Constants. Calculate the ph of a solution prepared by adding 60.0 ml of M NaOH to 100. ml of M CH 3 COOH solution. a d b e c. 5.00

4 20. Refer to Equilibrium Constants. Calculate the ph of a solution resulting from the addition of 50.0 ml of 0.30 M HNO 3 to 50.0 ml of 0.30 M NH 3. a d b e c Refer to Equilibrium Constants. Which of the following titrations could the following curve describe? 4 a. NaOH added to HF d. KOH added to HClO 4 b. HCl added to aqueous NH 3 e. HNO 3 added to NaOH c. CH 3 COOH added to aqueous NH Refer to Equilibrium Constants. A 50.0 ml solution of a 0.10 M weak monoprotic acid was mixed with 20.0 ml of 0.10 M KOH, and the resulting solution was diluted to 100. ml. The ph of the solution was found to be What is the ionization constant for the acid? a d b e c Refer to Equilibrium Constants. Consider the titration of 30.0 ml of M nitrous acid, HNO 2, by adding M aqueous ammonia to it. Which statement is true? The solution is buffered. a. before the equivalence point only d. before and at the equivalence point b. at the equivalence point only e. before and after the equivalence point c. after the equivalence point only 24. Refer to Equilibrium Constants. Consider the titrations of the pairs of aqueous acids and bases listed at the left. Which pair is incorrectly described (at the right) in terms of the acidic, basic, or neutral character of the solutions at the equivalence point? Acid-Base Pair Character at Equivalence Point a. HClO + NaOH acidic b. HNO 3 + Ca(OH) 2 neutral c. CH 3 COOH + KOH basic d. HCl + NH 3 acidic e. CH 3 COOH + NH 3 neutral 25. Which of the following solubility product expressions is incorrect? a. = [Ag + ] 2 [S 2- ] b. = [Ca 2+ ][F - ] 2 c. = [Sb 2+ ] 3 [S 3- ] 2 d. = [Cu 2+ ][S 2- ] e. = [Ag + ] 3 [PO 4 3- ]

5 5 26. How is the K sp of Ca 3 (PO 4 ) 2 related to s, the molar solubility of Ca 3 (PO 4 ) 2? a. K sp = 4s 5 d. K sp = 54s 4 b. K sp = 27s 3 e. K sp = 108s 5 c. K sp = 18s Calculate the solubility product constant for aluminum hydroxide. Its molar solubility is mole per liter at 25 C. a d b e c The solubility of Fe(OH) 2 is g in 2.00 liters at 18 C. What is its K sp at 18 C? a d b e c The solubility of cobalt(iii) hydroxide is 54 pg/100. ml of water at 25 C. Calculate the K sp for cobalt(iii) hydroxide at 25 C. a d b e c The K sp for magnesium arsenate is at 25 C. What is the molar solubility of Mg 3 (AsO 4 ) 2 at 25 C? a M d M b M e M c M 31. Calculate the concentration of OH - ions in a saturated Mn(OH) 2 solution. The solubility product for Mn(OH) 2 is a M d M b M e M c M 32. Calculate the ph in a saturated Mn(OH) 2 solution. The solubility product for Mn(OH) 2 is a. 9.0 d. 9.5 b. 9.2 e. 9.7 c Calculate the concentration of F - ions in saturated CaF 2 solution at 25 C. K sp = a M d M b M e M c M 34. What mass of Zn(OH) 2 is contained in 1.0 liter of saturated solution? K sp = a g d g b g e g c g 35. The solubility product constant for MgF 2 is How many grams of MgF 2 will dissolve in 150 ml of H 2 O at 25 C? a g d g b g e g c g

6 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Answer Section 6 MULTIPLE CHOICE 1. ANS: E TOP: The Common Ion Effect and Buffer Solutions 2. ANS: B TOP: The Common Ion Effect and Buffer Solutions 3. ANS: B TOP: The Common Ion Effect and Buffer Solutions 4. ANS: D TOP: The Common Ion Effect and Buffer Solutions 5. ANS: B TOP: Buffering Action 6. ANS: D TOP: Buffering Action 7. ANS: D TOP: Buffering Action 8. ANS: A TOP: Buffering Action 9. ANS: A TOP: Buffering Action 10. ANS: E TOP: Preparation of Buffer Solutions 11. ANS: D TOP: Preparation of Buffer Solutions 12. ANS: B TOP: Preparation of Buffer Solutions 13. ANS: E TOP: Preparation of Buffer Solutions 14. ANS: C TOP: Acid-Base Indicators 15. ANS: D TOP: Acid-Base Indicators 16. ANS: B TOP: Strong Acid/Strong Base Titration Curves 17. ANS: B TOP: Strong Acid/Strong Base Titration Curves 18. ANS: B TOP: Weak Acid/Strong Base and Weak Base/Strong Acid Titration Cu 19. ANS: B TOP: Weak Acid/Strong Base and Weak Base/Strong Acid Titration Cu 20. ANS: D TOP: Weak Acid/Strong Base and Weak Base/Strong Acid Titration Cu 21. ANS: B TOP: Weak Acid/Strong Base and Weak Base/Strong Acid Titration Cu 22. ANS: D TOP: Weak Acid/Strong Base and Weak Base/Strong Acid Titration Cu 23. ANS: E TOP: Weak Acid/Weak Base Titration Curves 24. ANS: A TOP: Weak Acid/Weak Base Titration Curves 25. ANS: C TOP: Solubility Product Constants 26. ANS: E TOP: Determination of Solubility Product Constants 27. ANS: E TOP: Determination of Solubility Product Constants 28. ANS: D TOP: Determination of Solubility Product Constants 29. ANS: C TOP: Determination of Solubility Product Constants 30. ANS: C TOP: Uses of Solubility Product Constants 31. ANS: E TOP: Uses of Solubility Product Constants 32. ANS: E TOP: Uses of Solubility Product Constants 33. ANS: B TOP: Uses of Solubility Product Constants 34. ANS: B TOP: Uses of Solubility Product Constants 35. ANS: A TOP: Uses of Solubility Product Constants

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