1. © 2015 Pearson Education, Inc. Clicker Questions Chapter 17 Barbara Mowery York College

2. © 2015 Pearson Education, Inc. Adding bromide ion to a saturated aqueous solution of _______ decreases its solubility in water. a.BaSO 4 b.Li 2 CO 3 c.PbS d.AgBr

3. © 2015 Pearson Education, Inc. Adding bromide ion to a saturated aqueous solution of _______ decreases its solubility in water. a.BaSO 4 b.Li 2 CO 3 c.PbS d.AgBr

4. © 2015 Pearson Education, Inc. Which of the following mixtures could be used to prepare an effective buffer solution? a.HCl and KCl b.HNO 3 and KNO 3 c.HCl and NH 4 Cl d.NH 3 and NH 4 Cl

5. © 2015 Pearson Education, Inc. Which of the following mixtures could be used to prepare an effective buffer solution? a.HCl and KCl b.HNO 3 and KNO 3 c.HCl and NH 4 Cl d.NH 3 and NH 4 Cl

6. © 2015 Pearson Education, Inc. Which solution has the greatest buffer capacity? a.1 L of solution containing 0.1 M NH 3 and 0.1 M NH 4 Cl b.1 L of solution containing 0.05 M NH 3 and 0.05 M NH 4 Cl c.1 L of solution containing 0.1 M NH 3 and 0.01 M NH 4 Cl d.1 L of solution containing 0.5 M NH 3 and 0.5 M NH 4 Cl

7. © 2015 Pearson Education, Inc. Which solution has the greatest buffer capacity? a.1 L of solution containing 0.1 M NH 3 and 0.1 M NH 4 Cl b.1 L of solution containing 0.05 M NH 3 and 0.05 M NH 4 Cl c.1 L of solution containing 0.1 M NH 3 and 0.01 M NH 4 Cl d.1 L of solution containing 0.5 M NH 3 and 0.5 M NH 4 Cl

8. © 2015 Pearson Education, Inc. Select the best acid or base to pair with its conjugate salt to prepare a buffer with pH ≈ 8.5. a.acetic acid, K a = 1.8 x 10 −5 b.ammonia, K b = 1.8 x 10 −5 c.hydroxylamine, K b = 1.1 x 10 −8 d.citric acid, K a = 7.4 x 10 −4

9. © 2015 Pearson Education, Inc. Select the best acid or base to pair with its conjugate salt to prepare a buffer with pH ≈ 8.5. a.acetic acid, K a = 1.8 x 10 −5 b.ammonia, K b = 1.8 x 10 −5 c.hydroxylamine, K b = 1.1 x 10 −8 d.citric acid, K a = 7.4 x 10 −4

10. © 2015 Pearson Education, Inc. For HCN, K a = 4.9  10 −10. What is the pH of a buffer solution in which [HCN] = 0.100 M = [KCN]? a.4.7 b.7.0 c.9.3 d.14.0

11. © 2015 Pearson Education, Inc. For HCN, K a = 4.9  10 −10. What is the pH of a buffer solution in which [HCN] = 0.100 M = [KCN]? a.4.7 b.7.0 c.9.3 d.14.0

12. © 2015 Pearson Education, Inc. For HCN, K a = 4.9  10 −10. [HCN] = 0.100 M, [KCN] = 0.200 M, pH of buffer solution = _____. a.7.0 b.9.0 c.9.3 d.9.6

13. © 2015 Pearson Education, Inc. For HCN, K a = 4.9  10 −10. [HCN] = 0.100 M, [KCN] = 0.200 M, pH of buffer solution = _____. a.7.0 b.9.0 c.9.3 d.9.6

14. © 2015 Pearson Education, Inc. For HCN, K a = 4.9  10 −10. [HCN] = 1.00 M, [KCN] = 0.100 M, pH of buffer solution = _____. a.7.0 b.8.3 c.9.0 d.9.3

15. © 2015 Pearson Education, Inc. For HCN, K a = 4.9  10 −10. [HCN] = 1.00 M, [KCN] = 0.100 M, pH of buffer solution = _____. a.7.0 b.8.3 c.9.0 d.9.3

16. © 2015 Pearson Education, Inc. Select the correct representation of the Henderson-Hasselbach equation? a.K a = [H + ][A − ] b.K w = [H + ][OH − ] = 10 −14 c.pH = pK a + d.pK a = pH +

17. © 2015 Pearson Education, Inc. Select the correct representation of the Henderson-Hasselbach equation? a.K a = [H + ][A − ] b.K w = [H + ][OH − ] = 10 −14 c.pH = pK a + d.pK a = pH +

18. © 2015 Pearson Education, Inc. When titrating a weak base with a strong acid, a good indicator to use would be a.methyl red (color change at pH = 5). b.bromothymol blue (change at pH = 7). c.phenolphthalein (change at pH = 9). d.None of the above

19. © 2015 Pearson Education, Inc. When titrating a weak base with a strong acid, a good indicator to use would be a.methyl red (color change at pH = 5). b.bromothymol blue (change at pH = 7). c.phenolphthalein (change at pH = 9). d.None of the above

20. © 2015 Pearson Education, Inc. When titrating a weak acid with a strong base, a good indicator to use would be a.methyl red (color change at pH = 5). b. bromothymol blue (change at pH = 7). c. phenolphthalein (change at pH = 9). d.None of the above

21. © 2015 Pearson Education, Inc. When titrating a weak acid with a strong base, a good indicator to use would be a.methyl red (color change at pH = 5). b. bromothymol blue (change at pH = 7). c. phenolphthalein (change at pH = 9). d.None of the above

22. © 2015 Pearson Education, Inc. For BaCO 3, K sp = 5.0  10 −9. What is [Ba 2+ ] in a saturated aqueous solution of BaCO 3 ? a.7.1  10 −5 M b.1.0  10 −8 M c.2.5  10 −9 M d.5.0  10 −9 M

23. © 2015 Pearson Education, Inc. For BaCO 3, K sp = 5.0  10 −9. What is [Ba 2+ ] in a saturated aqueous solution of BaCO 3 ? a.7.1  10 −5 M b.1.0  10 −8 M c.2.5  10 −9 M d.5.0  10 −9 M

24. © 2015 Pearson Education, Inc. For BaF 2, K sp = 1.7  10 −6. What is [Ba 2+ ] in a saturated aqueous solution of BaF 2 ? a.1.7  10 −6 M b.3.4  10 −6 M c.7.6  10 −3 M d.1.5  10 −2 M

25. © 2015 Pearson Education, Inc. For BaF 2, K sp = 1.7  10 −6. What is [Ba 2+ ] in a saturated aqueous solution of BaF 2 ? a.1.7  10 −6 M b.3.4  10 −6 M c.7.6  10 −3 M d.1.5  10 −2 M

26. © 2015 Pearson Education, Inc. Select the correct K sp expression for the dissolution of silver sulfate, Ag 2 SO 4. a. [Ag + ][SO 4 2− ] b. [Ag + ] 2 [SO 4 2− ] c. [Ag + ] [SO 4 2− ] 2 d. (2[Ag + ]) 2 [SO 4 2− ]

27. © 2015 Pearson Education, Inc. Select the correct K sp expression for the dissolution of silver sulfate, Ag 2 SO 4. a. [Ag + ][SO 4 2− ] b. [Ag + ] 2 [SO 4 2− ] c. [Ag + ] [SO 4 2− ] 2 d. (2[Ag + ]) 2 [SO 4 2− ]

28. © 2015 Pearson Education, Inc. For BaF 2, K sp = 1.7  10 −6. What is [F 1− ] in a saturated aqueous solution of BaF 2 ? a.1.7  10 −6 M b.5.7  10 −5 M c.7.6  10 −3 M d.1.5  10 −2 M

29. © 2015 Pearson Education, Inc. For BaF 2, K sp = 1.7  10 −6. What is [F 1− ] in a saturated aqueous solution of BaF 2 ? a.1.7  10 −6 M b.5.7  10 −5 M c.7.6  10 −3 M d.1.5  10 −2 M

30. © 2015 Pearson Education, Inc. For BaF 2, K sp = 1.7  10 −6. If KF is added to a saturated solution so that [F 1− ] = 0.10 M, what is [Ba 2+ ]? a.1.7  10 −6 M b.1.7  10 −5 M c.1.7  10 −4 M d.1.7  10 −3 M

31. © 2015 Pearson Education, Inc. For BaF 2, K sp = 1.7  10 −6. If KF is added to a saturated solution so that [F 1− ] = 0.10 M, what is [Ba 2+ ]? a.1.7  10 −6 M b.1.7  10 −5 M c.1.7  10 −4 M d.1.7  10 −3 M

32. © 2015 Pearson Education, Inc. Silver bromide is insoluble in water, but dissolves in aqueous ammonia, due to the formation of _______. a.Ag(NH 3 ) 2 1+ b.Ag(NH 3 ) 2+ c.NH 3 Br 1− d.NH 4 Br

33. © 2015 Pearson Education, Inc. Silver bromide is insoluble in water, but dissolves in aqueous ammonia, due to the formation of _______. a.Ag(NH 3 ) 2 1+ b.Ag(NH 3 ) 2+ c.NH 3 Br 1− d.NH 4 Br

34. © 2015 Pearson Education, Inc. Which ion will precipitate first when sulfide ion is added to a solution containing all of the ions below? a.Hg 2+ b.Pb 2+ c.Zn 2+ d.Cd 2+

35. © 2015 Pearson Education, Inc. Which ion will precipitate first when sulfide ion is added to a solution containing all of the ions below? a.Hg 2+ b.Pb 2+ c.Zn 2+ d.Cd 2+

36. © 2015 Pearson Education, Inc. Which ion will precipitate when HCl is added to a solution containing all of the ions below? a.Zn 2+ b.Pb 2+ c.Al 3+ d.Ba 2+

37. © 2015 Pearson Education, Inc. Which ion will precipitate when HCl is added to a solution containing all of the ions below? a.Zn 2+ b.Pb 2+ c.Al 3+ d.Ba 2+

38. © 2015 Pearson Education, Inc. Which ion will precipitate when phosphate ion is added to a solution containing all of the ions below? a.K 1+ b.Ba 2+ c.Na 1+ d.NH 4 1+

39. © 2015 Pearson Education, Inc. Which ion will precipitate when phosphate ion is added to a solution containing all of the ions below? a.K 1+ b.Ba 2+ c.Na 1+ d.NH 4 1+

40. © 2015 Pearson Education, Inc. Which ion will form a precipitate upon addition of chloride ion, hydrogen sulfide, ammonium sulfide, or ammonium hydrogen phosphate? a.Ba 1+ b.Na 2+ c.K 1+ d.NH 4 1+

41. © 2015 Pearson Education, Inc. Which ion will form a precipitate upon addition of chloride ion, hydrogen sulfide, ammonium sulfide, or ammonium hydrogen phosphate? a.Ba 1+ b.Na 2+ c.K 1+ d.NH 4 1+