Page 1
1.
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
2.
In which of the following aqueous solutions would you expect PbCl2 to
have the lowest solubility?
a. 0.020 M KCl
b. 0.020 M BaCl2
c. 0.015 M PbNO3
d. pure water
e. 0.015 M NaCl
3.
Calculate the fluoride ion concentration (in M) in a 1.0-L aqueous
solution containing 0.40 mol of HF and 0.10 mol of HCl. (Ka for HF = 6.8
x 10-4)
a. 1.0
b. 0.40
c. 0.016
d. 2.7 x 10-3
e. 1.4 x 10-3
4.
Calculate the percent ionization of HF in a 1.0-L aqueous solution
containing 0.30 mol of HF and 0.10 mol of HCl. (Ka for HF = 6.8 x 10-4)
a. 33
b. 4.1
c. 11
d. 0.68
e. 2.7
5.
The pH of a solution containing 0.818 M acetic acid (Ka = 1.76 x 10-5)
and 0.172 M sodium acetate is __________.
a. 4.077
b. 5.432
c. 8.568
d. 8.370
e. 9.922
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6.
Which one of the following pairs cannot be mixed together to form a
buffer solution?
a. NH3, NH4Cl
b. NaC2H3O2, HCl
c. RbOH, HBr
d. KOH, HF
e. H3PO4, KH2PO4
7.
A solution containing which one of the following pairs of substances
will be a buffer solution?
a. NaI, HI
b. KBr, HBr
c. RbCl, HCl
d. CsF, HF
e. none of these
8.
The Kb of ammonia is 1.8 x 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. 9.26
c. 4.74
d. 9.37
e. 7.00
9.
Calculate the pH of a solution prepared by dissolving 0.37 mol of formic
acid (HCO2H) and 0.23 mol of sodium formate (NaCO2H) in 1.00 L of
solution. Ka = 1.8 x 10-4 for formic acid.
a. 2.09
b. 10.46
c. 3.54
d. 2.30
e. 3.95
10. Determine the pH of a solution prepared by dissolving 0.75 mol of NH3
and 0.25 mol of NH4Cl in a liter of solution. Kb = 1.8 x 10-4 for NH3.
a. 4.27
b. 8.78
c. 10.73
d. 5.22
e. 9.78
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11. The pH of a solution prepared by dissolving 0.35 mol of solid CH3NH3Cl
(methylamine hydrochloride) in 1.00 L of 1.1 M CH3NH2 (methylamine) is
__________. The Kb for methylamine is 4.4 x 10-4.
a.
b.
c.
d.
e.
1.66
2.86
10.15
11.14
10.64
12. Consider a solution prepared by dissolving 0.35 mol of solid CH3NH3Cl
(methylamine hydrochloride) in 1.00 L of 1.1 M CH3NH2 (methylamine).
The Kb for methylamine is 4.4 x 10-4. If 10 mL of 0.01 M HCl is added to
this buffer solution, the pH of the solution will _________ slightly
because the HCl reacts with the _________ present in the solution.
a.
increase, OHb.
increase, CH3NH2
c.
decrease, CH3NH2
d.
+
decrease, CH3NH3
e.
This is a buffer solution so that the pH does not change.
13. Which of the following could be added to a solution of sodium acetate to
prepare a buffer?
acetic acid
hydrochloric acid
ammonium acetate
a. acetic acid only
b. acetic acid or hydrochloric acid
c. hydrochloric acid only
d. ammonium acetate only
e. sodium chloride or ammonium acetate
sodium chloride
14. Which of the following could be added to a solution of acetic acid to
prepare a buffer?
sodium acetate
sodium hydroxide
nitric 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
hydrofluoric acid
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15. Consider the titration of 25.0 mL of 0.723 M HClO4 with 0.273 M KOH.
The H3O+ concentration before any KOH is added is __________ M.
a. 0.439
b. 1.00 x 10-7
c. 0.723
d. 2.81 x 10-13
e. 0.273
16. Consider the titration of 25.00 mL of 0.723 M HClO4 with 0.273 M KOH.
The H3O+ concentration after addition of 10.0 mL of KOH is _________ M.
a. 0.438
b. 1.00 x 10-7
c. 0.723
d. 2.81 x 10-13
e. 0.273
17. Consider the titration of 25.0 mL of 0.723 M HClO4 with 0.273 M KOH.
The H3O+ concentration after addition of 66.2 mL of KOH is __________ M.
a. 0.439
b. 1.00 x 10-7
c. 0.723
d. 2.81 x 10-13
e. 0.273
18. Consider the titration of 25.0 mL of 0.723 M HClO4 with 0.273 M KOH.
The H3O+ concentration after addition of 80.0 mL of KOH is __________ M.
a. 0.439
b. 1.00 x 10-7
c. 0.723
d. 2.79 x 10-13
e. 3.58 x 10-2
19. A _______ yields a titration curve with an initial pH of 1.00, an
equivalence point at pH 7.0, and a relatively long, nearly vertical
middle section.
a. strong acid titrated by strong base
b. strong base titrated by strong acid
c. weak acid titrated by strong base
d. weak base titrated by strong acid
e. weak base titrated by weak acid
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20. An initial pH of 4.00, an equivalence point at pH 9.35, and a moderately
short, nearly vertical middle section correspond to a titration curve
for __________.
a. strong acid titrated by strong base
b. strong base titrated by strong acid
c. weak acid titrated by strong base
d. weak base titrated by strong acid
e. weak base titrated by weak acid
21. An initial pH of 13.00, an equivalence point at pH 7.0, and a relatively
long, nearly vertical middle section correspond to a titration curve for
__________.
a. strong acid titrated by strong base
b. strong base titrated by strong acid
c. weak acid titrated by strong acid
d. weak base titrated by strong acid
e. weak base titrated by weak acid
22. 50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. How many mL of
the base are required to reach the equivalence point? (Ka for HF is 6.8
x 10-4)
a. 101
b. 50.5
c. 52.7
d. 24.2
e. 48.8
23. 50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. What is the pH
when 25.00 mL of base have been added? (Ka for HF is 6.8 x 10-4)
a. 5.118
b. 3.146
c. 6.168
d. 3.547
e. 3.189
24. 50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH.
at the equivalence point? (Ka for HF is 6.8 x 10-4)
a. 13.064
b. 7.000
c. 7.969
d. 12.771
e. 1.229
What is the pH
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25. 50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. What is the pH
after 50.50 mL of base have been added? (Ka for HF is 6.8 x 10-4)
a. 7.000
b. 11.300
c. 12.778
d. 8.119
e. 4.631
26. The solubility of which one of the following will not be affected by the
pH of the solution?
a. Na3PO4
b. NaF
c. KNO3
d. AlCl3
e. MnS
27. The concentration (in M) of bromide ions in a saturated solution of
mercury(II) bromide, Ksp = 8.0 x 10-20, is _____ M.
a. 1.4 x 10-10
b. 2.0 x 10-20
c. 5.4 x 10-7
d. 2.7 x 10-7
e. 8.0 x 10-20
28. What is the molar solubility of PbS?
a. 4.0 x 10-28
b. 2.8 x 10-14
c. 6.4 x 10-55
d. 8.0 x 10-19
e. 8.0 x 10-28
29. The Ksp for Ag2S is 1.0 x 10-51.
a. 1.0 x 10-17
b. 7.9 x 10-18
c. 6.3 x 10-18
d. 8.3 x 10-53
e. 1.0 x 10-51
Ksp(PbS) = 8.0 x 10-28
What is the molar solubility of Ag2S?
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30. The solubility of Mn(OH)2 is 2.2 x 10-5 mol/L.
Mn(OH)2?
a. 1.1 x 10-14
b. 4.3 x 10-14
c. 2.1 x 10-14
d. 4.8 x 10-10
e. 2.2 x 10-5
What is the Ksp of
31. What is the maximum concentration (in M) of chloride ions in a solution
that contains 0.100 M Pb2+. The Ksp for lead(II) chloride is 1.0 x 104.
a. 0.058
b. 0.029
c. 0.0.0010
d. 0.032
e. 1.0 x 10-4
32. Calculate the solubility (in M) of aluminum hydroxide, Ksp = 1.9 x 1033, in 0.0182 M KOH solution.
a. 3.2 x 10-28
b. 2.9 x 10-9
c. 1.2 x 10-11
d. 3.1 x 10-12
e. 1.9 x 10-33
33. What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl?
(Ksp PbCl2 = 1.6 x 10-5)
a.
b.
c.
d.
e.
2.0
1.1
1.8
7.1
1.6
x
x
x
x
x
10-3
10-4
10-4
10-4
10-5
34. The Ksp for Zn(OH)2 is 5.0 x 10-17. Determine the molar solubility of
Zn(OH)2 in a buffer solution with a pH of 11.50.
a. 5.0 x 106
b. 1.2 x 10-12
c. 1.6 x 10-14
d. 5.0 x 10-12
e. 5.0 x 10-17
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35. In which one of the following solutions is silver chloride the most
soluble?
a. 0.181 M HCl
b. 0.0176 M NH3
c. 0.744 M LiNO3
d. pure water
e. 0.181 M NaCl
36. For which salt should the aqueous solubility be most sensitive to pH?
a. Ca(NO3)2
b. CaF2
c. CaCl2
d. CaBr2
e. CaI2
37. In
a.
b.
c.
d.
e.
which
H2O
0.5 M
0.2 M
1.0 M
0.8 M
aqueous system is PbI2 least soluble?
HI
HI
HNO3
KI
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