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Chapter 15 Self Quiz


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
Which of the following equations is the solubility product for magnesium iodate, Mg(IO3)2?
a.
Ksp = [Mg2+][I-]2[O2-]6
b.
Ksp = [Mg2+][I-]2[3O2-]2
c.
Ksp = [Mg2+]ch18b_files/i0020000.jpg
d.
Ksp = [Mg2+]2ch18b_files/i0020001.jpg
e.
Ksp = [Mg2+]ch18b_files/i0020002.jpg2
 

 2. 
The solubility of PbCl2 in water is 4.4 g/L at 25 °C. What is the value of Ksp for PbCl2?
a.
4.0 × 10-6
b.
1.6 × 10-5
c.
2.5 × 10-4
d.
5.0 × 10-4
e.
3.4 × 102
 

 3. 
The Ksp of PbBr2 is 6.6 × 10-6 at 25 °C. What is the concentration of Br- in a saturated solution of PbBr2(aq)?
a.
2.6 × 10-3 M
b.
1.2 × 10-2 M
c.
1.9 × 10-2 M
d.
2.4 × 10-2 M
e.
3.8 × 10-2 M
 

 4. 
The Ksp of AgBr is 5.4 × 10-13 at 25 °C. Calculate the molar solubility of AgBr in 0.015 M NaBr(aq) at 25 °C.
a.
8.1 × 10-15 mol/L
b.
3.6 × 10-11 mol/L
c.
1.1 × 10-8 mol/L
d.
7.3 × 10-7 mol/L
e.
4.9 × 10-5 mol/L
 

 5. 
At 25 °C, only 1.04 mg Cu(NO3)2 will dissolve per liter of a solution that is buffered at pH 6.80. What is the value of Ksp for Cu(OH)2? The molar mass of Cu(NO3)2 is 187.6 g/mol.
a.
2.2 × 10-20
b.
1.4 × 10-19
c.
4.1 × 10-18
d.
3.5 × 10-13
e.
8.8 × 10-13
 

 6. 
What is the molar solubility of Fe(OH)3(s) in a solution that is buffered at pH 2.75 at 25 °C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25 °C.
a.
1.1 × 10-29 mol/L
b.
1.1 × 10-26 mol/L
c.
2.0 × 10-15 mol/L
d.
2.2 × 10-10 mol/L
e.
3.5 × 10-4 mol/L
 

 7. 
At what pH will an aqueous solution of 0.210 M Mn2+ begin to precipitate as Mn(OH)2 at 25 °C? The Ksp for Mn(OH)2 is 1.9 × 10-13 at 25 °C.
a.
3.94
b.
6.02
c.
7.98
d.
9.86
e.
10.06
 

 8. 
An aqueous solution contains 0.010 M Br- and 0.010 M I-. If Ag+ is added until AgBr(s) just begins to precipitate, what are the concentrations of Ag+ and I-? (Ksp of AgBr = 5.4 × 10-13, Ksp of AgI = 8.5 × 10-17)
a.
[Ag+] = 5.4 × 10-11 M, [I-] = 1.0 × 10-2 M
b.
[Ag+] = 8.5 × 10-15 M, [I-] = 1.0 × 10-2 M
c.
[Ag+] = 5.4 × 10-11 M, [I-] = 1.6 × 10-6 M
d.
[Ag+] = 8.5 × 10-15 M, [I-] = 6.4 × 101 M
e.
[Ag+] = 8.5 × 10-15 M, [I-] = 1.6 × 10-6 M
 

 9. 
The following anions can be separated by precipitation as silver salts: Cl-, Br-, I-, CrO42-. If Ag+ is added to a solution containing the four anions, each at a concentration of 0.10 M, in what order will they precipitate?

Compound
K sp
AgCl
1.8 × 10 -10
Ag2CrO4
1.1 × 10-12
AgBr
5.4 × 10 -13
AgI
8.5 × 10 -17
a.
AgCl → Ag2CrO4 → AgBr → AgI
b.
AgI → AgBr → Ag2CrO4 → AgCl
c.
Ag2CrO4 → AgCl → AgBr → AgI
d.
Ag2CrO4 → AgI → AgBr → AgCl
e.
AgI → AgBr → AgCl → Ag2CrO4
 

 10. 
Given the following reactions,

AgCl(s) double sided arrow Ag+(aq) + Cl-(aq) Ksp = 1.8 × 10-10
Ag+(aq) + 2 NH3(aq) double sided arrow Ag(NH3)2+(aq) Kform = 1.6 × 107

determine the equilibrium constant for the reaction below.

AgCl(s) + 2 NH3(aq) double sided arrow Ag(NH3)2+(aq) + Cl-(aq)
a.
1.1 × 10-17
b.
2.9 × 10-3
c.
3.5 × 102
d.
1.6 × 107
e.
8.9 × 1016
 



 
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