____
____
____
1. Which of the following is a binary acid?
a. H2SO4
b. CH3COOH
2. Which of the following is not a strong acid?
a. HNO3
b. CH3COOH
3. Which of the following is a strong acid?
a.
____
4.
____
5.
____
6.
____
7.
____
8.
____
9.
____ 10.
____ 11.
c. HBr
d. NaOH
c. H2SO4
d. HCl
c. CH3COOH
b. H2SO4
d. H3PO4
Which of the following is a weak base?
a. NH3
c. NaOH
b. KOH
d. Ba(OH)2
Which of the following is a strong base?
a. KOH
c. NH3
b. H2
d. HCl
Which of the following is a triprotic acid?
a. H2SO4
c. HCl
b. CH3COOH
d. H3PO4
Which of the following is a diprotic acid?
a. H2SO4
c. HCl
b. CH3COOH
d. H3PO4
Whose definition of acids and bases emphasizes the role of protons?
a. Brønsted and Lowry
c. Arrhenius
b. Lewis
d. Bohr
A Brønsted-Lowry acid is a(n)
a. electron-pair acceptor.
c. proton acceptor.
b. electron-pair donor.
d. proton donor.
+
In the equation HCl(g) + H2O(l)  H3O (aq) + Cl–(aq), which species is a Brønsted-Lowry acid?
a. HCl
c. Cl–
b. H2O
d. None of the above
A Brønsted-Lowry base is a(n)
a. producer of OH– ions.
c. electron-pair donor.
b. proton acceptor.
d. electron-pair acceptor.
____ 12. In the reaction represented by the equation
a. Brønsted-Lowry acid.
b. Lewis base.
____ 13. A Lewis acid is
a. an electron-pair acceptor.
b. an electron-pair donor.
____ 14. Whose acid definition is the broadest?
a. Arrhenius
b. Lewis
____ 15. A Lewis base is a(n)
a. producer of OH– ions.
b. proton acceptor.
____ 16. An electron-pair donor is a
a. Arrhenius acid.
b. Brønsted-Lowry acid.
____ 17. In the reaction represented by the equation
a. HF and H2O.
b. F– and H3O+.
, H2O is a(n)
c. Brønsted-Lowry base.
d. Arrhenius.
c. a proton acceptor.
d. a proton donor.
c. Brønsted-Lowry
d. Faraday
c. electron-pair donor.
d. electron-pair acceptor.
c. Brønsted-Lowry base.
d. Lewis base.
, a conjugate acid-base pair is
c. H3O+ and H2O.
d. HF and H3O+.
____ 18. In the reaction represented by the equation
a. F– and H2O.
b. HF and F–.
____ 19. In the reaction represented by the equation
a. HClO3.
b.
.
____ 20. In the reaction represented by the equation
a.
.
b. NH3.
____ 21. In the reaction represented by the equation
CH3COO– is
a. H2O.
b. CH3COOH.
, a conjugate acid-base pair is
c. H3O+ and HF.
d. HF and H2O.
the conjugate acid of NH3 is
c.
.
d. not shown.
, the conjugate base of HClO3 is
c.
.
d. not shown.
, the conjugate acid of
c. H3O+.
d. not shown.
____ 22. In the reaction represented by the equation
H3O+ is
a. H2O.
c. CH3COO–.
b. CH3COOH.
d. not shown.
____ 23. The conjugate of a strong base is a
a. strong acid.
c. strong base.
b. weak acid.
d. weak base.
____ 24. The conjugate of a strong acid is a
a. strong acid.
c. strong base.
b. weak acid.
d. weak base.
____ 25. The conjugate of a weak base is a
a. strong acid.
c. strong base.
b. weak acid.
d. weak base.
____ 26. The conjugate of a weak acid is a
a. strong acid.
c. strong base.
b. weak acid.
d. weak base.
+
–
____ 27. In the equation HI + H2O  H3O + I , HI is a strong acid and I– is a
a. strong acid.
c. weak acid.
b. strong base.
d. weak base.
____ 28. In the equation
a. strong acid.
b. strong base.
, the conjugate base of
, H2O is a weak base and H3O+ is a
c. weak acid.
d. weak base.
____ 29. In the equation
is a weak base and HClO4 is a
a. strong acid.
c. weak acid.
b. strong base.
d. weak base.
____ 30. An amphoteric species is one that reacts as a(n)
a. acid only.
c. acid or base.
b. base only.
d. None of the above
____ 31. A species that can react as either an acid or a base is a(n)
a. Lewis acid.
c. oxyacid.
b. amphoteric substance.
d. salt.
____ 32. Which of the following is amphoteric?
a. H2SO4
c. H+
b.
d.
____ 33. Which of the following is amphoteric?
a. H3PO4
b. H+
c.
d.
____ 34. In the reaction represented by the equation
a. acid.
c. spectator species.
b. base.
d. salt.
____ 35. The substances produced when KOH(aq) neutralizes HCl(aq) are
a. HClO(aq) and KH(aq).
c. H2O(l) and KCl(aq).
b. KH2O+(aq) and Cl–(aq).
d. H3O+(aq) and KCl(aq).
____ 36. Which compound is produced by a neutralization?
a. H2O(l)
c. Ca(OH)2(s)
b. HNO3(aq)
d. H3PO4(aq)
+
____ 37. What is the concentration of H3O ions in pure water?
a. 10–7 M
c. 55.4 M
b. 0.7 M
d. 107 M
____ 38. What is the concentration of OH– ions in pure water?
a. 10–7 M
c. 55.4 M
b. 0.7 M
d. 107 M
____ 39. What is the product of H3O+ ion and OH– ion concentrations in water?
a. 10–28
c. 10–7
–14
b. 10
d. 55.4
____ 40. Which expression represents the concentration of H3O+ ions in solution?
a. 10–14 – [OH–]
c. 10–14  [OH–]
b. 10–14  [OH–]
d. [OH–]  10–14
____ 41. Which expression represents the concentration of OH– ions in solution?
a. 10–14 – [H3O+]
c. 10–14  [H3O+]
–14
+
b. 10  [H3O ]
d. [OH–]  10–14
____ 42. Which expression represents the pH of a solution?
a. log[H3O+]
c. log[OH–]
+
b. –log[H3O ]
d. –log[OH–]
____ 43. If [H3O+] of a solution is greater than [OH–], the solution
a. is always acidic.
c. is always neutral.
b. is always basic.
d. might be acidic, basic, or neutral.
+
–
____ 44. If [H3O ] of a solution is less than [OH ], the solution
a. is always acidic.
c. is always neutral.
b. is always basic.
d. might be acidic, basic, or neutral.
____ 45. What is the pH of a neutral solution at 25ºC?
a. 0
c. 7
b. 1
d. 14
____ 46. The pH scale in general use ranges from
a. 0 to 1.
c. 0 to 7.
b. –1 to 1.
d. 0 to 14.
____ 47. The pH of an acidic solution is
a. less than 0.
c. greater than 7.
b. less than 7.
d. greater than 14.
____ 48. The pH of a basic solution is
a. less than 0.
c. greater than 7.
b. less than 7.
d. greater than 14.
____ 49. A water solution whose pH is 4
a. is always neutral.
c. is always acidic.
b. is always basic.
d. might be neutral, basic, or acidic.
acts as a(n)
____ 50. A water solution whose pH is 10
a. is always neutral.
c. is always acidic.
b. is always basic.
d. might be neutral, basic, or acidic.
____ 51. A water solution whose pH is 7
a. is always neutral.
c. is always acidic.
b. is always basic.
d. might be neutral, basic, or acidic.
–
____ 52. To calculate the pH of a solution whose [OH ] is known, first calculate
a. [H3O+].
c. antilog[H3O+].
–
b. log[OH ].
d. [H2O].
–4
____ 53. What is the pH of a 10 M HCl solution?
a. 4
c. 8
b. 6
d. 10
____ 54. What is the pH of a 10–5 M KOH solution?
a. 3
c. 9
b. 5
d. 11
+
–3
____ 55. If [H3O ] = 1.7  10 M, what is the pH of the solution?
a. 1.81
c. 2.42
b. 2.13
d. 2.77
+
–5
____ 56. If [H3O ] = 8.26  10 M, what is the pH of the solution?
a. 2.161
c. 4.083
b. 3.912
d. 8.024
____ 57. What is the pH of a solution whose hydronium ion concentration is 5.03  10–1 M?
a. 0.2984
c. 1.542
b. 0.5133
d. 5.031
____ 58. What is the pH of a 0.027 M KOH solution?
a. 6.47
c. 12.92
b. 12.43
d. 14.11
____ 59. What is the pH of a 0.001 62 M NaOH solution?
a. 3.841
c. 9.923
b. 5.332
d. 11.210
____ 60. How would you classify KOH in the equation below?
a. a weak acid
c. a weak base
b. a strong acid
d. a strong base
____ 61. How would you classify HCl, in the equation below?
a. a weak acid
c. a weak base
b. a strong acid
d. a strong base
____ 62. How would you classify CH3COOH in the equation below?
a. a weak acid
c. a weak base
b. a strong acid
d. a strong base
____ 63. How would you classify NH3 in the equation below?
a. a weak acid
c. a weak base
b. a strong acid
d. a strong base
+
____ 64. The pH of a solution is 9.0. What is its H3O concentration?
a. 1 10-9 M
c. 1 10-5 M
-7
b. 1 10 M
d. 9 M
____ 65. What is the hydronium ion concentration of a solution whose pH is 4.12?
a. 4.4  10–8 M
c. 6.4  10–5 M
b. 5.1  10–6 M
d. 7.6  10–5 M
____ 66. What is the hydronium ion concentration of a solution whose pH is 7.30?
a. 1.4  10–11 M
c. 5.0  10–8 M
–8
b. 3.8  10 M
d. 7.1  10–6 M
____ 67. The pH of a solution is 10.00. What is its OH– concentration?
a. 1.0  10–10 M
c. 1.0  10–4 M
b. 1.0  10–7 M
d. 10 M
____ 68. What is the OH– concentration of a solution whose pH is 12.40?
a. 2.5  10–2 M
c. 8.9  10–2 M
–-2
b. 4.4  10 M
d. 1.0  10–1 M
____ 69. In an acid-base titration,
a. base is always added to acid.
b. acid is always added to base.
c. base is added to acid or acid is added to base.
d. None of the above
____ 70. An acid-base titration involves a
a. composition reaction.
c. single-displacement reaction.
b. neutralization reaction.
d. decomposition reaction.
____ 71. Which quantity is directly measured in a titration?
a. mass
c. volume
b. concentration
d. density
____ 72. What unknown quantity can be calculated after performing a titration?
a. volume
c. mass
b. concentration
d. density
____ 73. An acid-base titration is carried out by monitoring
a. temperature.
c. pressure.
b. pH.
d. density.
____ 74. In an acid-base titration, equivalent quantities of hydronium ions and hydroxide ions are present
a. at the beginning point.
c. at the end point.
b. at the midpoint.
d. throughout the titration.
____ 75. What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?
a. 0.200 M
c. 0.320 M
b. 0.280 M
d. 0.500 M
____ 76. What is the molarity of an HCl solution if 125 mL is neutralized in a titration by 76.0 mL of 1.22 M KOH?
a. 0.371 M
c. 0.617 M
b. 0.455 M
d. 0.742 M
____ 77. What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of 0.0904 M HNO3?
a. 0.230 M
c. 0.460 M
b. 0.355 M
d. 0.620 M
____ 78. What is the molarity of an H2SO4 solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution whose
concentration is 0.333 M?
a. 0.116 M
c. 0.465 M
b. 0.232 M
d. 0.880 M
____ 79. Calculate the molarity of a Ba(OH)2 solution if 1900 mL is completely titrated by 261 mL of 0.505 M HNO3.
a. 0.0173 M
c. 0.0322 M
b. 0.0254 M
d. 0.0347 M
____ 80. If 72.1 mL of 0.543 M H2SO4 completely titrates 39.0 mL of KOH solution, what is the molarity of the KOH
solution?
a. 0.317 M
c. 1.00 M
b. 0.502 M
d. 2.01 M
____ 81. If 114 mL of 0.008 04 M NaOH completely titrates 118 mL of H3PO4 solution, what is the molarity of the H3PO4
solution?
a. 0.002 59 M
c. 0.007 77 M
b. 0.005 18 M
d. 0.0105 M
____ 82. What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247 M H2SO4?
a. 0.0101 M
c. 0.0402 M
b. 0.0201 M
d. 0.0805 M
____ 83. What is the molarity of an H3PO4 solution if 358 mL is completely titrated by 876 mL of 0.0102 M Ba(OH)2
solution?
a. 0.0111 M
c. 0.0250 M
b. 0.0166 M
d. 0.0333 M
Use the graph below to answer the following questions.
84. What is the approximate volume of the titration standard added to reach the equivalence point, and what is the pH of
the solution at this point?
85. Is the unknown solution an acid or a base, and what is its relative strength (weak or strong)? Is the titration standard
an acid or base, and what is its relative strength?
86. Suggest an appropriate acid-base indicator that could be successfully used to conduct the acid-base titration.
87. What is the pH of a solution that has a hydronium ion concentration of 8.26 10–5 M?
88. What is the pH of a solution with a [OH–] of 3.31 10–7 M?
89. What is the pH of a 0.004 50 M HCl solution?
90. What is the pH of a 0.067 0 M KOH solution?
91. What is the hydronium ion concentration of a solution that has a pH of 4.120?
92. What is the hydroxide ion concentration of a solution that has a pH of 8.570?
93. What is the hydroxide ion concentration of a solution that has a pOH of 8.750?
94. What is the hydronium ion concentration of a solution that has a pOH of 4.120?
95. What is the molarity of an HCl solution if 49.0 mL is completely titrated by 68.4 mL of an NaOH solution whose
concentration is 0.333 M?
96. Calculate the molarity of a Ba(OH)2 solution if 1950 mL is completely titrated by 26.1 mL of 0.505 M HNO3.
97. A 20.0 mL sample of potassium hydroxide (KOH) solution is titrated to the equivalence point with 23.5 mL of
0.350 M hydrobromic acid (HBr) solution. What is the molarity of the potassium hydroxide solution?
98. A 25.0 mL sample of an aqueous solution of calcium hydroxide, Ca(OH)2, is titrated to the equivalence point with
21.2 mL of 0.620 M sulfuric acid, H2SO4, acid solution. What is the molarity of the calcium hydroxide solution?
99. What volume of 4.35 M HCl solution would be required to reach the equivalence point with 0.285 mol Mg(OH)2
dissolved in some de-ionized water?
100. What volume of 4.494 M H2SO4 solution would be required to reach the equivalence point with 7.2280 g LiOH
dissolved in some de-ionized water?
acids-bases
Answer Section
MULTIPLE CHOICE
1.
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35.
36.
37.
38.
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40.
41.
42.
43.
44.
45.
46.
ANS:
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ANS:
C
B
B
A
A
D
A
A
D
A
B
A
A
B
C
D
C
B
C
A
B
A
B
D
A
C
D
A
A
C
B
D
C
B
C
A
A
A
B
C
C
B
A
B
C
D
47.
48.
49.
50.
51.
52.
53.
ANS: B
ANS: C
ANS: C
ANS: B
ANS: A
ANS: A
ANS: A
Solution:
54. ANS: C
Solution:
55. ANS: D
Solution:
56. ANS: C
Solution:
57. ANS: A
Solution:
58. ANS: B
Solution:
59. ANS: D
Solution:
60.
61.
62.
63.
64.
ANS: D
ANS: B
ANS: A
ANS: A
ANS: A
Solution:
65. ANS: D
Solution:
66. ANS: C
Solution:
67. ANS: C
Solution:
68. ANS: A
Solution:
69.
70.
71.
72.
73.
74.
75.
ANS: C
ANS: B
ANS: C
ANS: B
ANS: B
ANS: C
ANS: C
Solution:
76. ANS: D
Solution:
77. ANS: A
Solution:
78. ANS: B
Solution:
79. ANS: D
Solution:
80. ANS: D
Solution:
81. ANS: A
Solution:
82. ANS: C
Solution:
83. ANS: B
Solution:
SHORT ANSWER
84. ANS:
Approximately 23 mL of titration standard is added to reach the equivalence point.
The pH is about 5.0 at this point.
85. ANS:
The graph is an example of a weak base titrated with a strong acid.
86. ANS:
Methyl red, pH range 4.4–6.2, would be a good indicator to choose.
PROBLEM
87. ANS:
4.083
Solution:
88. ANS:
7.520
Solution:
89. ANS:
2.347
Solution:
90. ANS:
12.826
Solution:
91. ANS:
7.59 10–9
Solution
92. ANS:
3.72 10–6 M
Solution:
93. ANS:
1.78 10–9 M
Solution:
94. ANS:
1.32 10–10 M
Solution:
95. ANS:
0.465 M
Solution:
96. ANS:
3.38 10–3 M
Solution:
97. ANS:
0.411 M
Solution:
98. ANS:
0.526 M
Solution:
99. ANS:
131 mL
Solution:
100. ANS:
0.033 58 L or 33.58 mL
Solution: