PX212CH1516
____
1. Which of the following reactions is not readily explained by the Arrhenius concept of acids and
bases?
A) HCl(g) + NH3(g)  NH4Cl(s)
B) HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
C) HClO4(aq) + H2O(l)  H3O+(aq) + ClO4(aq)
D) HC2H3O2(aq) + H2O(l)
H3O+(aq) + C2H3O2(aq)
+

E) H3O (aq) + OH (aq)  2H2O(l)
____
2. Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?
A) CHCl3
B) HNO3
C) H2SO4
D) H3O
E) HClO4
____
3. What is a conjugate acid–base pair for the following equilibrium?
H2PO4–(aq) + OH–(aq)
H2O(l) + HPO42–(aq)
A)
B)
C)
D)
E)
H2O is an acid and HPO42– is its conjugate base.
HPO42– is an acid and OH– is its conjugate base.
H2O is an acid and OH– is its conjugate base.
HPO42– is an acid and H2PO4– is its conjugate base.
HPO42– is an acid and H2O is its conjugate base.
____
4. Which of the following species cannot act as a Lewis base?
A) H2O2
B) OH–
C) O2–
D) H2O
E) Be2+
____
5. Which of the following is not an example of an acid–base reaction?
A) Al(OH)3(s) + 3H+(aq) Al3+(aq) + 3H2O(l)
B) C2H6(g) C2H4(g) + H2(g)
C) MgO(s) + CO2(g) MgCO3(s)
D) Al(OH)3(s) + OH–(aq) Al(OH)4–(aq)
E) CN–(aq) + H2O(l)
HCN(aq) + OH–(aq)




____
6. Which of the following acids has the weakest conjugate base in aqueous solution?
A) CH3COOH
B) HOCl
C) HF
D) HNO2
E) HClO4
____
7. Given equal concentrations of the following acids, which exhibits the greatest amount of ionization
in water?
A) nitrous acid
B) chlorous acid
C) ascorbic acid
D) hydrobromic acid
E) citric acid
____
8. Which solution has the highest pH?
A) 0.10 M HBr(aq)
B) 0.10 M HI(aq)
C) 0.10 M HF(aq)
D) 0.10 M HCl(aq)
E) 0.10 M HClO4(aq)
____
9. Rank H3PO4, H2PO4–, and HPO42– in order of increasing acid strength.
A) HPO42– < H2PO4– < H3PO4
B) H2PO4– < HPO42– < H3PO4
C) H2PO4– < H3PO4 < HPO42–
D) HPO42– < H3PO4 < H2PO4–
E) H3PO4 < H2PO4– < HPO42–
____
10. What is the equilibrium concentration of amide ion (NH2–) in liquid ammonia at 25°C?
("am" = dissolved in ammonia)
2NH3(l)
A)
B)
C)
D)
E)
____
NH4+(am) + NH2–(am); Kc = 1.8  10–24 at 25°C
2.6  10–12 M
3.6  10–24 M
1.3  10–12 M
1.8  10–24 M
9.0  10–25 M
11. What is the hydronium-ion concentration in a solution formed by combining 750 mL of
0.10 M NaOH with 250 mL of 0.30 M HCl?
NaOH(aq) + HCl(aq)  NaCl(aq) + H2O(l)
A)
B)
C)
D)
E)
____
0.075 M
1.7  10–13 M
1.0  10–7 M
0.30 M
0.10 M
12. At 20°C, the ion-product constant of water, Kw, is 6.88  10 15 . What is the pH of pure water at
20°C?
A) 7.000
B) 6.501
C) 7.181
D) 7.081
E) none of these
____
13. What is the hydronium-ion concentration of a 0.0038 M Ba(OH)2 solution?
A) 7.6  10–3 M
B) 3.8  10–3 M
C) 1.3  10–12 M
D) 2.6  10–12 M
E) 1.0  10–7 M
____
14. What is the pH of a 0.051 M HClO4 solution?
A) 15.29
B) 2.98
C) 12.71
D) 1.29
E) 11.02
____
15. What is the pOH of a 0.044 M HI solution?
A) 3.12
B) 12.64
C) 10.88
D) 15.36
E) 1.36
____
16. The hydronium-ion concentration of a solution is 2.5  10–6 M. What is the pH of the solution?
A) 6.81
B) 3.77
C) 2.00
D) 5.60
E) 10.60
____
17. Which aqueous solution has the lowest pH?
A) 0.30 M HCl
B) 0.30 M NaOH
C) 0.30 M NH3
D) 0.30 M Ba(OH)2
E) 0.30 M H2SO4
____
18. Which solution has the highest pH?
A) 0.1 M Ba(OH)2
B) 0.1 M CH3COOH
C) 0.1 M HCl
D) 0.1 M NH3
E) 0.1 M NaOH
____
19. What is the pH of a 0.0035 M Ba(OH)2 solution?
A) 9.04
B) 11.54
C) 2.46
D) 11.85
E) 2.15
____
20. A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?
A) 15.37
B) 12.63
C) 17.15
D) 7.00
E) 1.37
____
21. What is the pH of a 0.0086 M LiOH solution?
A) 9.24
B) 11.93
C) 2.07
D) 4.76
E) 16.07
____
22. What is the pH of a solution prepared by dissolving 0.365 L of HCl(g), measured at STP, in
enough water such that the total volume of the solution is 6.00 L? (R = 0.0821 L · atm/(K · mol))
A) 2.566
B) 11.434
C) 1.788
D) 7.000
E) 12.212
____
23. What is the pOH of a solution prepared by dissolving 0.465 L of HCl(g), measured at STP, in
enough water such that the total volume of the solution is 4.50 L? (R = 0.0821 L · atm/(K · mol))
A) 12.317
B) 7.000
C) 1.683
D) 11.664
E) 2.336
____
24. The pH of a solution of a strong base is 10.27 at 25°C. What is its hydronium-ion concentration?
A) 2.9  10–3 M
B) 1.9  10–4 M
C) 1.4  10–4 M
D) 5.4  10–11 M
E) 1.4  10–2 M
____
25. What is the hydroxide-ion concentration in a solution formed by combining 200. mL of
0.15 M HCl with 300. mL of 0.090 M NaOH at 25°C?
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)
A)
B)
C)
D)
1.7  10–13 M
0.090 M
1.7  10–12 M
0.054 M
E) 1.0  10–7 M
____
26. For which of the following equilibria does Kc correspond to the acid-ionization constant, Ka, of
HCO3–?
A) HCO3–(aq) + OH–(aq)
CO32–(aq) + H2O(l)
B) H2CO3(aq) + H2O(l)
HCO3–(aq) + H3O+(aq)
C) HCO3–(aq) + H2O(l)
H2CO3(aq) + OH–(aq)
D) HCO3–(aq) + H3O+(aq)
H2CO3(aq) + H2O(l)
–
E) HCO3 (aq) + H2O(l)
CO32–(aq) + H3O+(aq)
____
27. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the
equilibrium-constant expression is
A)
K=
.
B)
K=
.
C)
K=
.
D) K = [H+][NO2–].
E) none of these
____
28. Rank acetic acid (HC2H3O2), hydrocyanic acid (HOCN), and hydrofluoric acid (HF) in order of
increasing strength.
Acid
HC2H3O2
HOCN
HF
A)
B)
C)
D)
E)
____
Ka
1.8  10–5
3.5  10–4
6.8  10–4
HC2H3O2 < HOCN < HF
HOCN < HC2H3O2 < HF
HOCN < HF < HC2H3O2
HF < HOCN < HC2H3O2
HF < HC2H3O2 < HOCN
29. At a temperature of 25°C an initally 0.048 M solution of a weak monoprotic acid is 2.7 % ionized
once equilibrium is established. What is the acid-ionization constant, Ka, for this acid? (assume
Ca/Ka 3 102)
A) 3.5  10 5
B) 1.7  10 6
C) 2.3  10 1
D) 1.5  10 2
E) 1.7  10 7
____
30. A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 4.2  10–4 M.
What is the acid-ionization constant, Ka, for this acid?
A) 2.0  10–2
B) 2.9  10–3
C) 4.2  10–4
D) 1.8  10–6
E) 5.0  10–5
____
31. What is the hydronium-ion concentration of a 0.30 M solution of HCN (Ka = 4.9  10–10) at 25°C?
A) 1.7  10–4 M
B) 3.4  10–6 M
C) 2.2  10–6 M
D) 1.2  10–5 M
E) 4.0  10–5 M
____
32. What is the equilibrium concentration of chloroacetic acid, HC2H2O2Cl, in a solution prepared by
dissolving 0.0221 mol of HC2H2O2Cl in 1.20 L of water? For chloroacetic acid, Ka = 1.4  10–3.
A) 4.43  10–3 M
B) 1.84  10–2 M
C) 5.08  10–3 M
D) 1.40  10–2 M
E) 9.21  10–3 M
____
33. Phosphoric acid, H3PO4, will undergo three successive ionization reactions to varying extents in
water. What is the balanced equilibrium identified as Ka3?
A) H2PO4–(aq) + H2O(l)
H3O+(aq) + HPO42–(aq)
B) HPO42–(aq) + H2O(l)
PO43–(aq) + H3O+(aq)
C) H2PO4–(aq) + H3O+(aq)
H3PO4(aq) + H2O(l)
D) H3PO4(aq) + H2O(l)
H3O+(aq) + H2PO4–(aq)
E) PO43–(aq) + H2O(l)
HPO42–(aq) + OH–(aq)
____
34. For a 0.10 M solution of glutaric acid, HO2C(CH2)3CO2H (Ka1 = 4.6  10–5, Ka2 = 3.9  10–6), rank
the following species in order of increasing equilibrium concentration.
A) H3O+ < –O2C(CH2)3COO– < HO2C(CH2)3COO– < OH– < HO2C(CH2)3CO2H
B) OH– < –O2C(CH2)3COO– < H3O+ < HO2C(CH2)3COO– < HO2C(CH2)3CO2H
C) OH– < –O2C(CH2)3COO– < HO2C(CH2)3COO– < H3O+ < HO2C(CH2)3CO2H
D) H3O+ < HO2C(CH2)3CO2H < HO2C(CH2)3COO– < –O2C(CH2)3COO– < OH–
E) OH– < –O2C(CH2)3COO– < HO2C(CH2)3COO– < HO2C(CH2)3CO2H < H3O+
____
35. What is the hydronium-ion concentration in a 0.030 M solution of carbonic acid, H2CO3? For
carbonic acid, Ka1 = 4.2  10–7 and Ka2 = 4.8  10–11.
A) 3.0  10–2 M
B) 4.2  10–7 M
C) 4.8  10–11 M
D) 1.1  10–4 M
E) 5.6  10–5 M
____
36. What is the concentration of HC2O4– in a 0.390 M oxalic acid, H2C2O4, solution? For oxalic acid,
Ka1 = 5.6  10–2 and Ka2 = 5.1  10–5.
A) 4.4  10–3 M
B) 1.2  10–1 M
C) 1.5  10–1 M
D) 4.5  10–3 M
E) 5.1  10–5 M
____
37. Which of the following reactions is associated with the definition of Kb?
A) CN–(aq) + H+(aq)
HCN(aq)
–
B) F (aq) + H2O(l)
HF(aq) + OH–(aq)
C) Zn(OH2)62+(aq)
[Zn(OH2)5OH]+(aq) + H+(aq)
D) Cr3+(aq) + 6H2O(l)
Cr(OH2)63+(aq)
E) none of these
____
38. What is the hydroxide-ion concentration at equilibrium in a 0.17 M solution of ethylamine
(C2H5NH2, Kb = 4.7  10–4) at 25oC?
A) 8.7  10–3 M
B) 5.4  10–2 M
C) 5.9  10–14 M
D) 1.1  10–12 M
E) 1.7  10–1 M
____
39. Saccharin is a weak organic base with a Kb of 4.80  10–3. A 0.297-g sample of saccharin
dissolved in 25.0 mL of water has a pH of 12.190. What is the molar mass of saccharin?
A) 0.616 g/mol
B) 19.3 g/mol
C) 184 g/mol
D) 181 g/mol
E) 119 g/mol
____
40. Given the following, what will be the approximate equilibrium pH of an aqueous solution of
ammonium acetate, NH4CH3CO2?
NH4+
CH3CO2-
Ka = 5.69 x10-10
Kb = 5.71 x10-10
A) very basic
B) very acidic
C) nearly neutral
____
41. Which of the following salts is most likely to form an aqueous solution having the pH shown in the
figure below?
A)
B)
C)
D)
E)
Na2CO3
RbF
NH4Cl
Zn(NO3)2
KCl
NH4+(aq) + OH–(aq). Kb for NH3 is 1.8  10–5 at
____
42. Consider the reaction NH3(aq) + H2O(l)
25°C. What is Ka for the NH4+ ion at 25°C?
A) 5.6  104
B) 5.6  10–10
C) 1.8  10–5
D) 7.2  10–12
E) 9.2  10–8
____
43. The two acid-ionization constants for sulfurous acid, H2SO3, are 1.3  10–2 and 6.3  10–8 at 25°C.
What is Kb for the HSO3– ion?
A) 6.3  10–8.
B) 6.2  10–22.
C) 7.7  10–13.
D) 1.3  10–2.
E) 8.2  10–10.
____
44. What is the pH of a solution prepared by adding 0.490 g of ammonium iodide to 155 mL of water?
Kb of NH3 is 1.8  10–5.
A) 5.46
B) 3.21
C) 7.00
D) 8.54
E) 10.79
____
45. Which of the following substances, if added to a 0.10 M HC2H3O2 solution, would not increase the
hydronium-ion concentration?
A) Na2CO3(s)
B) NaHSO4(s)
C) H2C2O4(s)
D) HF(l)
E) HCl(g)
____
46. For a solution equimolar in HCN and NaCN, which statement is false?
A) [H+] is equal to Ka.
B) [H+] is larger than it would be if only the HCN were in solution.
C) Addition of NaOH will increase [CN–] and decrease [HCN].
D) Addition of more NaCN will shift the acid-dissociation equilibrium of HCN to the
left.
E) Addition of more HCN will shift the acid-dissociation equilibrium of HCN to the
right.
____
47. Calculate the pH of a solution that is 2.00 M HF, 1.00 M NaOH, and 0.690 M NaF.
(Ka = 6.8  10–4)
A) 3.40
B) 2.94
C) 3.17
D) 2.71
E) none of these
____
48. Which of the following will give a buffer with a pH near 4.76 when the acid and conjugate base
are mixed in equimolar proportions?
Acid
NH4 (from ammonia)
HC2H3O2 (acetic acid)
HF (hydrofluoric acid)
CH3CH2NH3+ (from
ethylamine)
+
A)
B)
C)
D)
E)
Ka
5.69  10-10
1.75  10-5
6.8  10-4
2.12  10-11
acetic acid
hydrofluoric acid
ethylamine
none
ammonia
____
49. Which of the following mixtures will be a buffer when dissolved in a liter of water?
A) 0.4 mol NH3 and 0.4 mol HCl
B) 0.3 mol NaCl and 0.3 mol HCl
C) 0.1 mol Ca(OH)2 and 0.3 mol HI
D) 0.2 mol H3PO4 and 0.1 mol NaOH
E) 0.2 mol HBr and 0.1 mol NaOH
____
50. What is the pH of a solution that is 0.12 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate,
NaC2H3O2, at 25°C? Ka of acetic acid is 1.8  10–5.
A) 4.12
B) 1.53
C) 4.74
D) 2.29
E) 5.36
____
51. What is the hydronium-ion concentration in a solution resulting from mixing 173 mL of 0.100 M
HCN and 73 mL of 0.100 M KOH at 25°C? Ka for HCN = 4.9  10–10 at 25°C.
A) 4.5  10–6 M
B) 7.0  10–6 M
C) 3.4  10–13 M
D) 6.7  10–10 M
E) 1.0  10–13 M
____
52. What molar ratio of acetic acid to sodium acetate is required to create a buffer solution having a
pH of 4.89 at 25°C? Ka for HC2H3O2 is 1.8  10–5.
A) 0.72
B) 1.4
C) 0.56
D) 2.0
E) 2.9
____
53. What is the hydronium-ion concentration of a solution formed by combining 400. mL of 0.21 M
HNO3 with 600. mL of 0.11 M NaOH at 25°C?
A) 0.082 M
B) 6.7  10–13 M
C) 0.21 M
D) 0.018 M
E) 0.11 M
____
54. What is the pH of a solution that is formed at 25°C by combining 300 mL of 0.040 M NaOH with
400 mL of 0.030 M HCl?
A) 2.0
B) 3.0
C) 5.0
D) 7.0
E) 1.0
____
55. What is the pH at the equivalence point of the titration of a strong acid with a strong base?
A) 3.9
B) 4.5
C) 8.2
D) 7.0
E) none of these
____
56. A 75.0-mL sample of 0.0500 M HCN (Ka = 6.2 10–10) is titrated with 0.421 M NaOH. What is
[H+] in the solution after 3.0 mL of 0.421 M NaOH has been added?
A) 8.2  10–6 M
B) 2.0 M
C) 1.2  10–9 M
D) 1.0  10–7 M
E) none of these
____
57. A 25.00-mL sample of propionic acid, HC3H5O2, of unknown concentration was titrated with
0.101 M KOH. The equivalence point was reached when 42.20 mL of base had been added. What
is the concentration of the propionate ion at the equivalence point?
A) 0.101 M
B) 0.147 M
C) 0.0634 M
D) 0.170 M
E) 0.128 M
____
58. Which acid-base combination is depicted by this titration curve?
A)
B)
C)
D)
E)
Titration of a weak acid with a strong base.
Titration of a weak base with a strong acid.
Titration of a strong acid with a strong base.
Titration of a strong base with a strong acid.
Not enough information provided.
____
59. A sample of ammonia (Kb = 1.8  10–5) is titrated with 0.1 M HCl. At the equivalence point, what
is the approximate pH of the solution?
A) 5
B) 1
C) 9
D) 7
E) 11
____
60. In the titration of a weak monoprotic acid with a strong base, the pH at the endpoint will be
A) equal to the pKa of the weak acid.
B) greater than 7.00.
C) equal to 7.00.
D) less than 7.00.
E) less than the pKa of the weak acid.
PX212CH1516
Answer Section
1. ANS: A
PTS: 1
DIF: easy
REF: 15.1
OBJ: Define acid and base according to the Arrhenius concept.
TOP: acids and bases | acid-base concepts
NOT: REVISED
2. ANS: A
PTS: 1
DIF: easy
REF: 15.1
OBJ: Define acid and base according to the Arrhenius concept.
TOP: acids and bases | acid-base concepts
3. ANS: C
PTS: 1
DIF: moderate
REF: 15.2
OBJ: Identify acid and base species. (Example 15.1)
TOP: acids and bases | acid-base concepts
KEY: Brønsted-Lowry concept of acids and bases
MSC: general chemistry
4. ANS: E
PTS: 1
DIF: easy
REF: 15.3
OBJ: Identify Lewis acid and Lewis base species. (Example 15.2)
TOP: acids and bases | acid-base concepts
KEY: Lewis concept of acids and bases
MSC: general chemistry
5. ANS: B
PTS: 1
DIF: moderate
REF: 15.3
OBJ: Identify Lewis acid and Lewis base species. (Example 15.2)
TOP: acids and bases | acid-base concepts
KEY: Lewis concept of acids and bases
MSC: general chemistry
6. ANS: E
PTS: 1
DIF: easy
REF: 15.4
OBJ: Understand the relationship between the strength of an acid and that of its conjugate base.
TOP: acids and bases | acid and base strength
7. ANS: D
PTS: 1
DIF: easy
REF: 15.4
OBJ: Decide whether reactants or products are favored in an acid–base reaction. (Example 15.3)
TOP: acids and bases | acid and base strength
8. ANS: C
PTS: 1
DIF: moderate
REF: 15.6
OBJ: Understand the periodic trends in the strengths of the binary acids HX.
TOP: acids and bases | acid and base strength
KEY: molecular structure and acid strength
MSC: general
chemistry
9. ANS: A
PTS: 1
DIF: easy
REF: 15.5
OBJ: Understand the relative acid strengths of a polyprotic acid and its anions.
TOP: acids and bases | acid and base strength
KEY: molecular structure and acid strength
MSC: general
chemistry
10. ANS: C
PTS: 1
DIF: moderate
REF: 15.6
OBJ: Define the ion-product constant for water.
TOP: acids and bases | self-ionization of water and pH
MSC: general chemistry
11. ANS: C
PTS: 1
DIF: difficult
REF: 15.6
OBJ: Define the ion-product constant for water.
TOP: acids and bases | self-ionization of water and pH
KEY: self-ionization of water
MSC: general chemistry
12. ANS: D
PTS: 1
DIF: moderate
REF: 15.8
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
OBJ: Define the ion-product constant for water.
TOP: acids and bases | self-ionization of water and pH
ANS: C
PTS: 1
DIF: moderate
REF: 15.7
OBJ: Calculate the concentrations of H3O+ and OH– in solutions of a strong acid or base.
(Example 15.4)
TOP: acids and bases | solutions of a strong acid or base
MSC: general chemistry
ANS: D
PTS: 1
DIF: easy
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: B
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: D
PTS: 1
DIF: easy
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: E
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a weak acid or base
ANS: A
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: D
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: B
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: B
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: A
PTS: 1
DIF: difficult
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
ANS: D
PTS: 1
DIF: difficult
REF: 15.8
OBJ: Calculate the pH from the hydronium-ion concentration. (Example 15.5)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
24. ANS: D
PTS: 1
DIF: easy
REF: 15.8
OBJ: Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
25. ANS: C
PTS: 1
DIF: moderate
REF: 15.8
OBJ: Calculate the hydronium-ion concentration from the pH. (Example 15.6)
TOP: acids and bases | solutions of a strong acid or base
KEY: pH of a solution
MSC: general chemistry
26. ANS: E
PTS: 1
DIF: moderate
REF: 16.1
OBJ: Write the chemical equation for a weak acid undergoing acid ionization in aqueous
solution.
TOP: acids and bases | solutions of a weak acid or base
KEY: acid-ionization equilibria
MSC: general chemistry
27. ANS: C
PTS: 1
DIF: moderate
REF: 16.1
OBJ: Define acid-ionization constant and degree of ionization.
TOP: acids and bases | solutions of a weak acid or base
KEY: acid-ionization equilibria
MSC: general chemistry
28. ANS: A
PTS: 1
DIF: easy
REF: 16.1
OBJ: Define acid-ionization constant and degree of ionization.
TOP: acids and bases | acid and base strength
KEY: relative strengths of acids and bases
MSC: general chemistry
29. ANS: A
PTS: 1
DIF: easy
REF: 16.1
OBJ: Define acid-ionization constant and degree of ionization.
TOP: acids and bases | solutions of a weak acid or base
30. ANS: D
PTS: 1
DIF: easy
REF: 16.1
OBJ: Determine Ka from the solution pH. (Example 16.1)
TOP: acids and bases | solutions of a weak acid or base
KEY: acid-ionization equilibria | calculations with Ka
MSC: general chemistry
31. ANS: D
PTS: 1
DIF: easy
REF: 16.1
OBJ: Calculate concentrations of species in a weak acid solution using Ka (approximation
method). (Example 16.2)
TOP: acids and bases | solutions of a weak acid or base
KEY: acid-ionization equilibria | calculations with Ka
MSC: general chemistry
32. ANS: A
PTS: 1
DIF: moderate
REF: 16.1
OBJ: Calculate concentrations of species in a weak acid solution using Ka (quadratic formula).
(Example 16.3)
TOP: acids and bases | solutions of a weak acid or base
KEY: acid-ionization equilibria | calculations with Ka
MSC: general chemistry
33. ANS: B
PTS: 1
DIF: easy
REF: 16.2
OBJ: State the general trend in the ionization constants of a polyprotic acids.
TOP: acids and bases | solutions of a weak acid or base
34. ANS: C
PTS: 1
DIF: moderate
REF: 16.2
OBJ: Calculate concentrations of species in a solution of a diprotic acid. (Example 16.4)
TOP: acids and bases | solutions of a weak acid or base
KEY: acid-ionization equilibria | polyprotic acids
MSC: general chemistry
35. ANS: D
PTS: 1
DIF: moderate
REF: 16.2
OBJ: Calculate concentrations of species in a solution of a diprotic acid. (Example 16.4)
TOP: acids and bases | solutions of a weak acid or base
36.
37.
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16.10)
KEY:
acid-ionization equilibria | polyprotic acids
MSC: general chemistry
B
PTS: 1
DIF: difficult
REF: 16.2
Calculate concentrations of species in a solution of a diprotic acid. (Example 16.4)
acids and bases | solutions of a weak acid or base
acid-ionization equilibria | polyprotic acids
MSC: general chemistry
B
PTS: 1
DIF: easy
REF: 16.3
Define base-ionization constant.
acids and bases | solutions of a weak acid or base
base-ionization equilibria
MSC: general chemistry
A
PTS: 1
DIF: easy
REF: 16.3
Calculate concentrations of species in a weak base solution using Kb. (Example 16.5)
acids and bases | solutions of a weak acid or base
base-ionization equilibria
MSC: general chemistry
D
PTS: 1
DIF: difficult
REF: 16.3
Calculate concentrations of species in a weak base solution using Kb. (Example 16.5)
acids and bases | solutions of a weak acid or base
base-ionization equilibria
MSC: general chemistry
C
PTS: 1
DIF: easy
REF: 16.4
Predict whether a salt solution is acidic, basic, or neutral. (Example 16.6)
acids and bases | solutions of a weak acid or base
E
PTS: 1
DIF: easy
REF: 16.4
Predict whether a salt solution is acidic, basic, or neutral. (Example 16.6)
acids and bases | solutions of a weak acid or base
acid-base properties of salt solutions | prediction of salt solution acid-base properties
general chemistry
B
PTS: 1
DIF: easy
REF: 16.4
Obtain Ka from Kb or Kb from Ka. (Example 16.7)
acids and bases | solutions of a weak acid or base
acid-base properties of salt solutions
MSC: general chemistry
C
PTS: 1
DIF: easy
REF: 16.4
Obtain Ka from Kb or Kb from Ka. (Example 16.7)
acids and bases | solutions of a weak acid or base
acid-base properties of salt solutions
MSC: general chemistry
A
PTS: 1
DIF: moderate
REF: 16.4
Calculating concentrations of species in a salt solution. (Example 16.8)
acids and bases | solutions of a weak acid or base
acid-base properties of salt solutions | pH of a salt solution
general chemistry
A
PTS: 1
DIF: moderate
REF: 16.5
Explain the common-ion effect.
acids and bases | solutions of a weak acid or base with another solute
common-ion effect
MSC: general chemistry
B
PTS: 1
DIF: easy
REF: 16.5
Calculate the common-ion effect on acid ionization (effect of a conjugate base). (Example
TOP:
acids and bases | solutions of a weak acid or base with another solute
common-ion effect
MSC: general chemistry
47. ANS: A
PTS: 1
DIF: difficult
REF: 16.5
OBJ: Calculate the common-ion effect on acid ionization (effect of a conjugate base). (Example
16.10) TOP:
acids and bases | solutions of a weak acid or base with another solute
KEY: common-ion effect
MSC: general chemistry
48. ANS: A
PTS: 1
DIF: moderate
REF: 16.6
OBJ: Define buffer and buffer capacity.
TOP: acids and bases | solutions of a weak acid or base with another solute
49. ANS: D
PTS: 1
DIF: moderate
REF: 16.6
OBJ: Define buffer and buffer capacity.
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: buffer
MSC: general chemistry
50. ANS: E
PTS: 1
DIF: easy
REF: 16.6
OBJ: Calculate the pH of a buffer from given volumes of solution. (Example 16.11)
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: buffer | Henderson-Hasselbalch equation
MSC: general chemistry
51. ANS: D
PTS: 1
DIF: moderate
REF: 16.6
OBJ: Calculate the pH of a buffer when a strong acid or a strong base is added. (Example 16.12)
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: buffer | pH of a buffer
MSC: general chemistry
52. ANS: A
PTS: 1
DIF: moderate
REF: 16.6
OBJ: Learn the Henderson–Hasselbalch equation.
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: buffer | Henderson-Hasselbalch equation
MSC: general chemistry
53. ANS: D
PTS: 1
DIF: easy
REF: 16.7
OBJ: Calculate the pH of a solution of a strong acid and a strong base. (Example 16.13)
TOP: acids and bases | solutions of a strong acid or base
MSC: general chemistry
54. ANS: D
PTS: 1
DIF: easy
REF: 16.7
OBJ: Calculate the pH of a solution of a strong acid and a strong base. (Example 16.13)
TOP: acids and bases | solutions of a strong acid or base
MSC: general chemistry
55. ANS: D
PTS: 1
DIF: easy
REF: 16.7
OBJ: Define equivalence point.
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: acid-base titration curve | titration of a strong acid by a strong base
MSC: general chemistry
56. ANS: C
PTS: 1
DIF: moderate
REF: 16.7
OBJ: Describe the curve for the titration of a weak acid by a strong base.
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: acid-base titration curve | titration of a weak acid by a strong base
MSC: general chemistry
57. ANS: C
PTS: 1
DIF: easy
REF: 16.7
OBJ: Calculate the pH at the equivalence point in the titration of a weak acid by a strong base.
(Example 16.14)
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: acid-base titration curve | titration of a weak acid by a strong base
MSC: general chemistry
58. ANS: A
PTS: 1
DIF: easy
REF: 16.7
OBJ: Describe the curve for the titration of a weak base by a strong acid.
TOP: acids and bases | solutions of a weak acid or base with another solute
59. ANS: A
PTS: 1
DIF: easy
REF: 16.7
OBJ: Calculation of the pH of a solution at several points of a titration of weak base by a strong
acid. (Example 16.15)
TOP: acids and bases | solutions of a weak acid or base with another solute
KEY: acid-base titration curve | titration of a weak base by a strong acid
MSC: general chemistry
60. ANS: B
PTS: 1
DIF: moderate
REF: 16.7
OBJ: Calculation of the pH of a solution at several points of a titration of weak base by a strong
acid. (Example 16.15)
TOP: acids and bases | solutions of a weak acid or base with another solute