The two salts AgX and AgY have very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?
A.
Nothing.
B.
HY is stronger than HX.
C.
HX is stronger than HY.
D.
The acids have equal strengths.
2.
Solubility Products (Ksp)
BaSO4
1.5 ´ 10–9
CoS
5.0 ´ 10–22
PbSO4
1.3 ´ 10–8
AgBr
5.0 ´ 10–13
Which of the following compounds is the most soluble (in moles/liter)?
A.
BaSO4
B.
CoS
C.
PbSO4
D.
AgBr
E.
BaCO3
3.
How many moles of Fe(OH)2 [Ksp = 1.8 ´ 10–15] will dissolve in one liter of water buffered at pH = 12.00?
A.
1.8 ´ 10–11
B.
1.8 ´ 10–9
C.
8.0 ´ 10–6
D.
5.0 ´ 10–12
E.
4.0 ´ 10–8
4.
You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which salt is more soluble in acidic solution?
A.
AgX
B.
AgY
C.
They are equally soluble in acidic solution.
D.
Cannot be determined by the information given.
5.
You have a solution consisting of 0.10 M Cl– and 0.10 M CrO42–. You add 0.10 M silver nitrate dropwise to this solution. Given that the Ksp for Ag2CrO4 is 9.0 ´ 10–12, and that for AgCl is 1.6 ´ 10–10, which of the following will precipitate first?
A.
silver chloride
B.
silver chromate
C.
silver nitrate
D.
cannot be determined by the information given
E.
none of these
6.
The solubility of CaSO4 in pure water at 0°C is 1 gram per liter. The value of the solubility product is
A.
1 ´ 10–3
B.
7 ´ 10–2
C.
1 ´ 10–4
D.
5 ´ 10–5
7.
The molar solubility of PbI2 is 1.5 × 10–3 M. Calculate the value of Ksp for PbI2.
A.
1.5 × 10–3
B.
2.3 × 10–6
C.
1.4 × 10–8
D.
3.4 × 10–9
E.
none of these
8.
Calculate the concentration of chromate ion, CrO42–, in a saturated solution of CaCrO4. (Ksp = 7.1 ´ 10–4)
A.
0.027 M
B.
5.0 ´ 10–7 M
C.
7.1 ´ 10–4 M
D.
3.5 ´ 10–4 M
E.
3.5 ´ 10–2 M
9.
The molar solubility of BaCO3 (Ksp = 1.6 ´ 10–9) in 0.10 M BaCl2 solution is:
A.
1.6 ´ 10–10
B.
4.0 ´ 10–5
C.
7.4 ´ 10–4
D.
0.10
E.
none of these
10.
The Ksp of AgI is 1.5 ´ 10–16. Calculate the solubility in mol/L of AgI in a 0.30 M NaI solution.
A.
1.7 ´ 10–8
B.
0.30
C.
2.6 ´ 10–17
D.
8.5 ´ 1017
E.
5.0 ´ 10–16
11.
The molar solubility of AgCl (Ksp = 1.6 ´ 10–10) in 0.0020 M sodium chloride at 25°C is:
A.
0.0020
B.
1.3 ´ 10–5
C.
8.0 ´ 10–8
D.
1.7 ´ 10–10
E.
none of these
12.
Silver chromate, Ag2CrO4, has a Ksp of 9.0 ´ 10–12. Calculate the solubility in mol/L of silver chromate.
A.
1.3 ´ 10–4 M
B.
7.8 ´ 10–5 M
C.
9.5 ´ 10–7 M
D.
1.9 ´ 10–12 M
E.
9.8 ´ 10–5 M
13.
The Ksp of PbSO4(s) is 1.3 ´ 10–8. Calculate the solubility (in mol/L) of PbSO4(s) in a 0.0010 M solution of Na2SO4.
A.
1.3 ´ 10–11 M
B.
4.5 ´ 10–6 M
C.
1.3 ´ 10–5 M
D.
1.3 ´ 10–8 M
E.
1.4 ´ 10–4 M
14.
The Ksp for PbF2 is 4.0 ´ 10–8. If a 0.050 M NaF solution is saturated with PbF2, what is the [Pb2+] in solution?
A.
3.8 ´ 10–3 M
B.
3.6 ´ 10–4 M
C.
5.4 ´ 10–7 M
D.
1.6 ´ 10–5 M
E.
2.7 ´ 10–8 M
15.
The solubility of Mg(OH)2 (Ksp = 8.9 ´ 10–12) in 1.0 L of a solution buffered (with large capacity) at pH 10.0 is:
A.
8.9 ´ 109 moles
B.
8.9 ´ 10–4 moles
C.
8.9 ´ 10–1 moles
D.
8.9 ´ 10–7 moles
E.
none of these
16.
Given the following Ksp values
Ksp
Ksp
PbCrO4
2.0 ´ 10–16
Pb(OH)2
1.2 ´ 10–15
Zn(OH)2
4.5 ´ 10–17
MnS
2.3 ´ 10–13
which statement about solubility in mol/L in water is correct?
A.
PbCrO4, Zn(OH)2, and Pb(OH)2 have equal solubilities in water.
B.
PbCrO4 has the lowest solubility in water.
C.
The solubility of MnS in water will not be pH dependent.
D.
MnS has the highest molar solubility in water.
E.
A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution.
17.
The Ksp of Al(OH)3 is 2 ´ 10–32. At what pH will a 0.2 M Al3+ solution begin to show precipitation of Al(OH)3?
A.
3.7
B.
1.0
C.
5.6
D.
10.3
E.
8.4
18.
3.5 ´ 102 mL of 3.2 M Pb(NO3)2 and 2.0 ´ 102 mL of 0.020 M NaCl are added together. Ksp for the lead chloride is 1.6 ´ 10–5.
Will precipitation occur?
A.
Yes
B.
No
C.
Maybe, it depends on the temperature.
D.
Maybe, it depends on the limiting reagent concentration.
E.
None of these.
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