1. AP Chemistry Review
Day 5
Chapters 15-20

2. What to expect on test day
Start time: 8:00 am Monday, May 7th
Duration: 3 hr 15 min
90 min multiple choice section first (50% of your score)
60 questions, no calculator allowed.
105 minute free response section last (50% of score)
Graphing calculators allowed.
7 FRQ's: 3 long (7 part questions) and 4 short (3 part questions)
I will provide you with donuts and orange juice/coffee that morning, so please come to my room before taking your test 
I will be here by 7:00 am on Monday if you want to ask me any questions!

3. The reaction quotient Q is usually represented by
[reactants] / [products].
[products] / [reactants].
[reactants]  [products].
d. [reactants] + [products].
Answer: b

4. The reaction quotient Q is usually represented by
[reactants] / [products].
[products] / [reactants].
[reactants]  [products].
d. [reactants] + [products].
Answer: b

5. Which reaction quotient represents the reaction shown
Which reaction quotient represents the reaction shown? Co(s) + 2 H+(aq)  Co2+(aq) + H2(g)
a b.
c d.
Answer: c

6. Which reaction quotient represents the reaction shown
Which reaction quotient represents the reaction shown? Co(s) + 2 H+(aq)  Co2+(aq) + H2(g)
a b.
c d.
Answer: c

7. reactants products catalysts d. water
If the value of the equilibrium constant is large, then at equilibrium mostly _______ will be present.
reactants
products
catalysts
d. water
Answer: b

8. reactants products catalysts d. water
If the value of the equilibrium constant is large, then at equilibrium mostly _______ will be present.
reactants
products
catalysts
d. water
Answer: b

9. increase. decrease. remain unchanged. d. disappear.
CO2 + H2  CO + H2O If all species are gases and H2 is added, the concentration of CO at equilibrium will
increase.
decrease.
remain unchanged.
d. disappear.
Answer: a

10. increase. decrease. remain unchanged. d. disappear.
CO2 + H2  CO + H2O If all species are gases and H2 is added, the concentration of CO at equilibrium will
increase.
decrease.
remain unchanged.
d. disappear.
Answer: a

11. increase decrease not change d. eradicate
CO2 + H2  CO + H2O Increasing the temperature of this endothermic reaction will _______ [CO] at equilibrium.
increase
decrease
not change
d. eradicate
Answer: a

12. increase decrease not change d. eradicate
CO2 + H2  CO + H2O Increasing the temperature of this endothermic reaction will _______ [CO] at equilibrium.
increase
decrease
not change
d. eradicate
Answer: a

13. increase. decrease. remain unchanged. d. vanish.
CO2 + H2  CO + H2O If all species are gases and the container is compressed, the amount of CO will
increase.
decrease.
remain unchanged.
d. vanish.
Answer: c

14. increase. decrease. remain unchanged. d. vanish.
CO2 + H2  CO + H2O If all species are gases and the container is compressed, the amount of CO will
increase.
decrease.
remain unchanged.
d. vanish.
Answer: c

15. increase. decrease. remain unchanged. d. cease to exist.
CO2 + H2  CO + H2O Adding a catalyst to this reaction will cause the [CO] at equilibrium to
increase.
decrease.
remain unchanged.
d. cease to exist.
Answer: c

16. increase. decrease. remain unchanged. d. cease to exist.
CO2 + H2  CO + H2O Adding a catalyst to this reaction will cause the [CO] at equilibrium to
increase.
decrease.
remain unchanged.
d. cease to exist.
Answer: c

17. A Brønsted–Lowry acid is
a proton donor.
a proton acceptor.
an electron-pair donor.
d. an electron-pair acceptor.
Answer: a

18. A Brønsted–Lowry acid is
a proton donor.
a proton acceptor.
an electron-pair donor.
d. an electron-pair acceptor.
Answer: a

19. A Lewis acid is a proton donor. a proton acceptor.
an electron-pair donor.
d. an electron-pair acceptor.
Answer: d

20. A Lewis acid is a proton donor. a proton acceptor.
an electron-pair donor.
d. an electron-pair acceptor.
Answer: d

21. Which of the following is the conjugate base of HPO42−?
d. HPO32−
Answer: c

22. Which of the following is the conjugate base of HPO42−?
d. HPO32−
Answer: c

23. Which of the following is the conjugate acid of SO42−?
HSO4
HSO41−
SO32−
d. H3SO4+
Answer: b

24. Which of the following is the conjugate acid of SO42−?
HSO4
HSO41−
SO32−
d. H3SO4+
Answer: b

25. The stronger the acid, the (X) its conjugate base
The stronger the acid, the (X) its conjugate base. Acids and bases react to form their (Y) conjugates.
X = stronger, Y = stronger
X = stronger, Y = weaker
X = weaker, Y = stronger
d. X = weaker, Y = weaker
Answer: d

26. The stronger the acid, the (X) its conjugate base
The stronger the acid, the (X) its conjugate base. Acids and bases react to form their (Y) conjugates.
X = stronger, Y = stronger
X = stronger, Y = weaker
X = weaker, Y = stronger
d. X = weaker, Y = weaker
Answer: d

27. The value of the ion-product constant for water is
10−7.
10−14.
10+7.
d. impossible to determine without additional information.
Answer: c

28. The value of the ion-product constant for water is
10−7.
10−14.
10+7.
d. impossible to determine without additional information.
Answer: c

29. What is the pH of a 0.0200 M aqueous solution of HBr?
1.00
1.70
2.30 d
Answer: b

30. What is the pH of a 0.0200 M aqueous solution of HBr?
1.00
1.70
2.30 d
Answer: b

31. What is the pH of a 0.0400 M aqueous solution of KOH?
12.60
10.30
4.00
d. 1.40
Answer: a

32. What is the pH of a 0.0400 M aqueous solution of KOH?
12.60
10.30
4.00
d. 1.40
Answer: a

33. What is the pH of a 0.0200 M aqueous solution of HF? The Ka of HF is 6.8  10−4.
1.70
2.43
3.17 d
Answer: b

34. What is the pH of a 0.0200 M aqueous solution of HF? The Ka of HF is 6.8  10−4.
1.70
2.43
3.17 d
Answer: b

35. Which of the following is not a weak base?
NH3
NH2OH F−
OH−
Answer: d

36. Which of the following is not a weak base?
NH3
NH2OH F−
OH−
Answer: d

37. Adding bromide ion to a saturated aqueous solution of _______ decreases its solubility in water.
BaSO4
Li2CO3
PbS
d. AgBr
Answer: d

38. Adding bromide ion to a saturated aqueous solution of _______ decreases its solubility in water.
BaSO4
Li2CO3
PbS
d. AgBr
Answer: d

39. HCl and KCl HNO3 and KNO3 HCl and NH4Cl d. NH3 and NH4Cl
Which of the following mixtures could be used to prepare an effective buffer solution?
HCl and KCl
HNO3 and KNO3
HCl and NH4Cl
d. NH3 and NH4Cl
Answer: d

40. HCl and KCl HNO3 and KNO3 HCl and NH4Cl d. NH3 and NH4Cl
Which of the following mixtures could be used to prepare an effective buffer solution?
HCl and KCl
HNO3 and KNO3
HCl and NH4Cl
d. NH3 and NH4Cl
Answer: d

41. Which solution has the greatest buffer capacity?
1 L of solution containing 0.1 M NH3 and 0.1 M NH4Cl
1 L of solution containing 0.05 M NH3 and 0.05 M NH4Cl
1 L of solution containing 0.1 M NH3 and 0.01 M NH4Cl
d. 1 L of solution containing 0.5 M NH3 and 0.5 M NH4Cl
Answer: d

42. Which solution has the greatest buffer capacity?
1 L of solution containing 0.1 M NH3 and 0.1 M NH4Cl
1 L of solution containing 0.05 M NH3 and 0.05 M NH4Cl
1 L of solution containing 0.1 M NH3 and 0.01 M NH4Cl
d. 1 L of solution containing 0.5 M NH3 and 0.5 M NH4Cl
Answer: d

43. When titrating a weak base with a strong acid, a good indicator to use would be
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
Answer: a

44. When titrating a weak base with a strong acid, a good indicator to use would be
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
Answer: a

45. When titrating a weak acid with a strong base, a good indicator to use would be
a. methyl red (color change at pH = 5).
bromothymol blue (change at pH = 7).
phenolphthalein (change at pH = 9).
d. None of the above
Answer: c

46. When titrating a weak acid with a strong base, a good indicator to use would be
a. methyl red (color change at pH = 5).
bromothymol blue (change at pH = 7).
phenolphthalein (change at pH = 9).
d. None of the above
Answer: c

47. [Ag+][SO42−] [Ag+]2[SO42−] [Ag+] [SO42−]2 d. (2[Ag+])2[SO42−]
Select the correct Ksp expression for the dissolution of silver sulfate, Ag2SO4.
[Ag+][SO42−]
[Ag+]2[SO42−]
[Ag+] [SO42−]2
d. (2[Ag+])2[SO42−]
Answer: b

48. [Ag+][SO42−] [Ag+]2[SO42−] [Ag+] [SO42−]2 d. (2[Ag+])2[SO42−]
Select the correct Ksp expression for the dissolution of silver sulfate, Ag2SO4.
[Ag+][SO42−]
[Ag+]2[SO42−]
[Ag+] [SO42−]2
d. (2[Ag+])2[SO42−]
Answer: b

49. All spontaneous processes are
reversible.
isothermal.
irreversible.
d. exothermic.
Answer: c

50. All spontaneous processes are
reversible.
isothermal.
irreversible.
d. exothermic.
Answer: c

51. Entropy is a measurement of the _______ of a system.
randomness
internal energy
temperature
polarity
Answer: a

52. Entropy is a measurement of the _______ of a system.
randomness
internal energy
temperature
polarity
Answer: a

53. increases decreases remains unchanged d. reaches equilibrium
The Second Law of Thermodynamics says that the entropy of the universe _______ whenever a spontaneous process occurs.
increases
decreases
remains unchanged
d. reaches equilibrium
Answer: a

54. increases decreases remains unchanged d. reaches equilibrium
The Second Law of Thermodynamics says that the entropy of the universe _______ whenever a spontaneous process occurs.
increases
decreases
remains unchanged
d. reaches equilibrium
Answer: a

55. At equilibrium, the value of the free energy change (“delta G”) is
positive.
negative.
fluctuating.
d. zero.
Answer: d

56. At equilibrium, the value of the free energy change (“delta G”) is
positive.
negative.
fluctuating.
d. zero.
Answer: d

57. The oxidation state of nitrogen in the ammonium ion (NH41+) is _______.-5 −1 −3
Answer: d

58. The oxidation state of nitrogen in the ammonium ion (NH41+) is _______.-5 −1
d. −3
Answer: d

59. The oxidation state of manganese in the permanganate ion (MnO41−) is _______.+2 +4
d. +7
Answer: d

60. The oxidation state of manganese in the permanganate ion (MnO41−) is _______.+2 +4
d. +7
Answer: d

61. Zn + Cu2+  Zn2+ + Cu The reducing agent in the reaction above is _______.
d. Cu
Answer: a

62. Zn + Cu2+  Zn2+ + Cu The reducing agent in the reaction above is _______.
d. Cu
Answer: a

63. The purpose of the salt bridge in a voltaic cell is to
provide H+ ions needed to balance charges.
maintain neutrality by allowing the flow of ions.
serve as the site for oxidation to occur.
serve as the site for reduction to occur.
Answer: b

64. The purpose of the salt bridge in a voltaic cell is to
provide H+ ions needed to balance charges.
maintain neutrality by allowing the flow of ions.
serve as the site for oxidation to occur.
serve as the site for reduction to occur.
Answer: b

65. a galvanic a voltaic an electrolytic d. a prison
A cell that uses external energy to produce an oxidation–reduction reaction is called _______ cell.
a galvanic
a voltaic
an electrolytic
d. a prison
Answer: c

66. a galvanic a voltaic an electrolytic d. a prison
A cell that uses external energy to produce an oxidation–reduction reaction is called _______ cell.
a galvanic
a voltaic
an electrolytic
d. a prison
Answer: c

67. Reduction occurs at the
anode, in both galvanic and electrolytic cells.
cathode, in both galvanic and electrolytic cells.
anode in galvanic cells and cathode in electrolytic cells.
cathode in galvanic cells and anode in electrolytic cells.
Answer: b

68. Reduction occurs at the
anode, in both galvanic and electrolytic cells.
cathode, in both galvanic and electrolytic cells.
anode in galvanic cells and cathode in electrolytic cells.
cathode in galvanic cells and anode in electrolytic cells.
Answer: b

69. Corrosion of metals can be prevented by all of the following methods except
a sacrificial anode.
a salt bridge.
formation of an oxide coating.
paint.
Answer: b

70. Corrosion of metals can be prevented by all of the following methods except
a sacrificial anode.
a salt bridge.
formation of an oxide coating.
paint.
Answer: b