Ch. 17 Review
1) Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition
of 5.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M.
A) 0.0850
B) 0.00167
C) 0.0980
D) 0.0817
E) 0.00253
Answer: D Sec. 17.2
2) Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after
addition of 5.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __________ M.
A) 0.107 B) 0.100
C) 0.126
D) 0.00976
E) 0.00193
Answer: A Sec. 17.2
3) The K b of ammonia is 1.77 × 10-5 . The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 50.0 mL of 1.00 M
ammonium nitrate is __________.
A) 4.63
B) 9.25
C) 4.74
D) 9.37
E) 7.00
Answer: B Sec. 17.2
4) Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO2 H) and 0.230 mol of sodium formate (NaCO2 H)
in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10-4 .
A) 2.09
B) 10.46
C) 3.54
D) 2.30
E) 3.95
Answer: C Sec. 17.2
5) Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7 H5O2 H) and 0.150 mol of sodium benzoate
(NaC7H5O2) (NaC7 H5O2 H) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid
is 6.50 × 10-5 .
A) 4.41
B) 2.39
C) 3.97
D) 10.0
E) 4.19
Answer: C Sec. 17.2
6) A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. What is the [H+ ] (molarity) before any base is added?
A) 0.439
B) 1.00 × 10-7
C) 0.723
D) 2.81 × 10-13
E) 0.273
Answer: C Sec. 17.3
7) A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of
KOH is __________ M.
A) 0.440
B) 1.00 × 10-7
C) 0.723
D) 2.81 × 10-13
E) 0.273
Answer: A Sec. 17.3
8) A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of
KOH is __________ M.
A) 0.44
B) 1.0 × 10-7
C) 0.72
D) 2.8 × 10-13
E) 3.6 × 10-2
Answer: E Sec. 17.3
9) The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is __________.
A) 6.29
B) 7.00 C) 8.11
D) 5.78
E) 0.00
Answer: B Sec. 17.3
10) A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base.
The concentration of HCl is __________ M.
A) 11.7
B) 0.00214
C) 0.0856
D) 0.267
E) 0.139
Answer: C Sec. 17.3
11) A 50.0 mL sample of an aqueous H 2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5
mL of the base. The concentration of H 2SO4 is __________ M.
A) 0.234
B) 0.469
C) 0.150
D) 0.300
E) 0.938
Answer: A Sec. 17.3
12) The concentration of iodide ions in a saturated solution of lead (II) iodide is __________ M. The solubility product constant of PbI2 is
1.4  10-8 .
A) 3.8 × 10-4
B) 3.0 × 10-3
C) 1.5 × 10-3
D) 3.5 × 10-9
E) 1.4 × 10-8
Answer: B Sec. 17.4
13) The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2
A) 5.0 × 10-4
B) 4.1 × 10-6
C) 3.1 × 10-7 D) 1.6 × 10-5 E) 1.6 × 10-2
Answer: D Sec. 17.4
14) Determine the Ksp for magnesium hydroxide (Mg(OH)2) where the solubility of Mg(OH)2 is 1.4 × 10-4 M.
A) 2.7 × 10-12
B) 1.1 × 10-11
C) 2.0 × 10-8
D) 3.9 × 10-8
E) 1.4 × 10-4
Answer: B Sec. 17.4
15) Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1
× 10-12.
A) 1.8 × 10-5
B) 1.4 × 10-6 C) 2.8 × 10-6 D) 3.2 × 10-10 E) 8.1 × 10-12
Answer: A Sec. 17.5
16) Which one of the following pairs cannot be mixed together to form a buffer solution?
A) NH3, NH4Cl B) NaC2H3O2, HCl (C2H3O2- = acetate)
C) RbOH, HBr
D) KOH, HF
E) H3PO4, KH2PO4
Answer: C Sec. 17.2
17) The Henderson-Hasselbalch equation is __________.
[base]
[base]
A) [H+ ] = Ka +
B) pH = pKa - log
[acid]
[acid]
[acid]
[acid]
D) pH = pKa + log
E) pH = log
[base]
[base]
C) pH = pKa + log
[base]
[acid]
Answer: C Sec. 17.2
18) Which of the following could be added to a solution of acetic acid to prepare a buffer?
sodium acetate
sodium hydroxide
nitric acid
hydrofluoric acid
A) sodium acetate only
B) sodium acetate or sodium hydroxide
C) nitric acid only
D) hydrofluoric acid or nitric acid
E) sodium hydroxide only
Answer: B
Diff: 2 Page Ref: Sec. 17.2
19) Consider the following graph
20) The molar solubility of __________ is not affected by the pH of the solution.
A) Na3PO4 B) NaF
C) KNO3
D) AlCl3
E) MnS
Answer: C Sec. 17.5
21) In which of the following aqueous solutions would you expect AgCl to have the highest solubility?
A) pure water
B) 0.020 M BaCl2 C) 0.015 NaCl
D) 0.020 AgNO3 E) 0.020 KCl
Answer: A Sec. 17.5
22) In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?
A) pure water
B) 0.20 M NaBr
C) 0.10 M AgNO3 D) 0.15 M KBr
E) 0.10 M LiBr
Answer: B Sec. 17.5
23) In which of the following aqueous solutions would you expect AgBr to have the highest solubility?
A) 0.10 M LiBr
B) 0.10 M AgNO3 C) 0.20 M NaBr
D) 0.15 M KBr
E) pure water
Answer: E Sec. 17.5
24) For which salt should the aqueous solubility be most sensitive to pH?
A) Ca(NO3)2
B) CaF2
C) CaCl2
D) CaBr2 E) CaI2
Answer: B Sec. 17.5