Name: ___________________________________    Date: ______________



1.
The expression for the solubility product of Ba3(AsO4)2 is
A.
[Ba2+]3[AsO43-]2
B.
[3 x Ba2+]3[2 x AsO43-]2
C.
3[Ba2+] × 2[AsO43-]
D.
3[Ba2+]3 + 2[AsO43-]2
E.
[Ba2+]3[AsO43-]2


2.
The expression for the solubility product of Ca3(PO4)2 is
A.
[Ca2+]3 × [PO43-]2
B.
[3 x Ca2+]3 × [2 x PO43-]2
C.
3[Ca2+] × 2[PO43-]
D.
3[Ca2+]3 + 2[PO43-]2
E.
[Ca2+]3 × [PO43-]2


3.
The expression for the solubility product of Fe2(CrO4)3 is
A.
[Fe2+]3 × [CrO43-]2
B.
[2 x Fe2+]3 × [3 x CrO43-]2
C.
3[Fe2+] × 2[CrO43-]
D.
2[Fe2+]3 + 3[CrO43-]2
E.
[Fe3+]2 × [CrO42-]3


4.
The expression for the solubility product of copper(II) hydroxide is
A.
[Cu2+][2 OH-]
B.
[Cu2+] × 2[OH-]2
C.
[Cu2+]2[OH-]
D.
[Cu2+][OH-]2
E.
[Cu2+] × [OH-]2


5.
The expression for the solubility product of calcium fluoride, CaF2 is
A.
[Ca2+][2 × F-]
B.
[Ca2+] × 2[F-]2
C.
[Ca2+]2[F-]
D.
[Ca2+][F-]2
E.
[Ca2+] × [F-]2


6.
The expression for the solubility product of silver oxalate (Ag2C2O4) is
A.
[Ag22+][C2O42-]
B.
[Ag+][C2O42-]2
C.
2[Ag+][C2O42-]
D.
[Ag+]2[C2O42-]
E.
2[Ag+]2[C2O42-]


7.
The solubility of scandium(III) fluoride, ScF3, in pure water is 2.0 × 10-5 moles per liter. Calculate the value of Ksp for scandium(III) fluoride from this data.
A.
1.3 × 10-17
B.
1.4 × 10-18
C.
4.3 × 10-18
D.
1.6 × 10-19
E.
4.8 × 10-19


8.
The solubility of lead(II) fluoride, PbF2, in pure water is 2.1 × 10-3 moles per liter. Calculate the value of Ksp for lead(II) fluoride from this data.
A.
1.3 × 10-7
B.
1.4 × 10-8
C.
3.7 × 10-8
D.
1.6 × 10-9
E.
4.8 × 10-9


9.
The solubility of calcium fluoride, CaF2, in pure water is 2.15 × 10-4 moles per liter. Calculate the value of Ksp for calcium fluoride from this data.
A.
1.85 × 10-7
B.
9.28 × 10-8
C.
1.99 × 10-11
D.
3.98 × 10-11
E.
9.94 × 10-12


10.
The solubility of copper(II) arsenate, Cu3(AsO4)2, in pure water is 3.7 × 10-8 moles per liter. Calculate the value of Ksp for copper(II) arsenate from this data.
A.
6.9 × 10-38
B.
4.2 × 10-37
C.
2.5 × 10-36
D.
3.7 × 10-36
E.
7.5 × 10-36


11.
The solubility of zinc(II) phosphate, Zn3(PO4)2, in pure water is 1.5 × 10-7 moles per liter. Calculate the value of Ksp for zinc(II) phosphate from this data.
A.
2.3 × 10-14
B.
5.1 × 10-28
C.
2.7 × 10-33
D.
8.2 × 10-33
E.
7.6 × 10-35


12.
The solubility of silver oxalate, Ag2C2O4, in pure water is 2.06 × 10-4 moles per liter. Calculate the value of Ksp for silver oxalate from this data.
A.
4.24 × 10-8
B.
8.49 × 10-8
C.
1.75 × 10-11
D.
3.50 × 10-11
E.
8.74 × 10-12


13.
The solubility of silver carbonate, Ag2CO3, in pure water is 1.27 × 10-4 moles per liter. Calculate the value of Ksp for silver carbonate from this data.
A.
1.64 × 10-11
B.
3.28 × 10-11
C.
2.04 × 10-12
D.
4.10 × 10-12
E.
8.19 × 10-12


14.
Which one of the following salts has the highest solubility in water, expressed in moles per liter?
A.
PbF2, Ksp = 3.6 × 10-8
B.
Ag2CrO4, Ksp = 1.2 × 10-12
C.
CaF2, Ksp = 3.9 × 10-11
D.
BaF2, Ksp = 1.7 × 10-6
E.
PbI2, Ksp = 7.9 × 10-9


15.
Which one of the compounds below has the highest solubility in water, expressed in moles per liter?
A.
SrF2, Ksp = 2.8 × 10-9
B.
Sr(IO3)2, Ksp = 3.3 × 10-7
C.
Fe(OH)2, Ksp = 8.0 × 10-16
D.
PbCl2, Ksp = 1.6 × 10-5
E.
PbBr2, Ksp = 3.9 × 10-5


16.
Which one of the compounds below has the highest solubility in water, expressed in moles per liter?
A.
SrF2, Ksp = 2.8 × 10-9
B.
Sr(IO3)2, Ksp = 3.3 × 10-7
C.
MgF2, Ksp = 6.5 × 10-9
D.
PbCl2, Ksp = 1.6 × 10-5
E.
BaF2, Ksp = 1.7 × 10-6


17.
Which one of the compounds below has the lowest solubility in water, expressed in moles per liter?
A.
SrF2, Ksp = 2.8 × 10-9
B.
Sr(IO3)2, Ksp = 3.3 × 10-7
C.
MgF2, Ksp = 6.5 × 10-9
D.
PbCl2, Ksp = 1.6 × 10-5
E.
PbI2, Ksp = 7.9 × 10-9


18.
The solubility of silver sulfate (Ag2SO4), in moles per liter, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?
A.
solubility = 2[Ag+]
B.
solubility = [Ag+]
C.
solubility = [2Ag+]
D.
solubility = 2[SO42-]
E.
solubility = [SO42-]


19.
The solubility of strontium fluoride, SrF2, in moles per liter, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?
A.
solubility = 2[Sr2+]
B.
solubility = [Sr2+]
C.
solubility = [2 Sr2+]
D.
solubility = 2[F-]
E.
solubility = [F-]


20.
The solubility of copper(II) iodate, Cu(IO3)2, in moles per liter, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?
A.
solubility = 2[Cu2+]
B.
solubility = [Cu2+]
C.
solubility = [2 Cu2+]
D.
solubility = 2[IO3-]
E.
solubility = [IO3-]2


21.
The solubility of silver phosphate, Ag3PO4, in moles per liter, can be expressed in terms of the resulting ion concentrations. Which relationship is correct?
A.
solubility = 3[Ag+]
B.
solubility = [Ag+]
C.
solubility = [Ag+]3
D.
solubility = [PO43-]
E.
solubility = [PO43-]3


22.
The solubility product for Ag3PO4 is: Ksp = 2.8 × 10-18. What is the solubility of Ag3PO4 in water, in moles per liter?
A.
1.8 × 10-5 M
B.
2.5 × 10-5 M
C.
1.9 × 10-86 M
D.
3.1 × 10-5 M
E.
4.1 × 10-5 M


23.
The solubility product for BaSO4 is 1.1 × 10-10. Calculate the solubility of BaSO4 in pure water, in moles per liter.
A.
5.5 × 10-11 mol L-1
B.
1.0 × 10-5 mol L-1
C.
2.1 × 10-5 mol L-1
D.
1.1 × 10-10 mol L-1
E.
2.2 × 10-10 mol L-1


24.
The solubility product for PbCl2 is 1.7 × 10-5. What is the solubility of PbCl2 in pure water, in moles per liter?
A.
2.4 × 10-4 mol L-1
B.
6.2 × 10-2 mol L-1
C.
7.7 × 10-3 mol L-1
D.
1.6 × 10-2 mol L-1
E.
6.0 × 10-5 mol L-1


25.
Calculate the concentration of chloride ions in a saturated solution of lead(II) chloride. The Ksp = 1.7 × 10-5.
A.
2.4 × 10-4 M
B.
4.8 × 10-4 M
C.
3.9 × 10-2 M
D.
1.2 × 10-1 M
E.
3.2 × 10-2 M


26.
Calculate the concentration of iodate ions in a saturated solution of lead(II) iodate, Pb(IO3)2. The Ksp = 2.6 × 10-13.
A.
3.2 × 10-5 M
B.
4.0 × 10-5 M
C.
6.4 × 10-5 M
D.
8.0 × 10-5 M
E.
5.1 × 10-7 M


27.
Calculate the concentration of iodate ions in a saturated solution of barium iodate, Ba(IO3)2. The Ksp = 1.5 × 10-9.
A.
1.4 × 10-3 M
B.
2.3 × 10-3 M
C.
7.2 × 10-4 M
D.
3.9 × 10-5 M
E.
7.7 × 10-5 M


28.
The solubility product of barium fluoride (BaF2) is 1.7 × 10-6. Calculate the concentration of fluoride ions in a saturated solution of barium fluoride.
A.
7.6 × 10-3 M
B.
1.5 × 10-2 M
C.
3.4 × 10-5 M
D.
1.7 × 10-6 M
E.
3.4 × 10-6 M


29.
The solubility product for Mg3(PO4)2 is 6.3 × 10-26. What is the solubility of Mg3(PO4)2 in pure water, in grams per liter?
A.
1.7 × 10-23 g L-1
B.
3.4 × 10-7 g L-1
C.
9.4 × 10-4 g L-1
D.
1.2 × 10-3 g L-1
E.
2.4 × 10-3 g L-1


30.
The solubility of lead iodide is 578 mg L-1 at 25 °C. What is the solubility product for PbI2?
A.
7.9 × 10-9
B.
1.6 × 10-6
C.
1.1 × 10-11
D.
2.7 × 10-12
E.
6.3 × 10-6


31.
The solubility of barium carbonate is 14.8 mg L-1 at 30 °C. Calculate the Ksp value for BaCO3.
A.
7.5 × 10-5
B.
1.5 × 10-4
C.
5.6 × 10-9
D.
7.5 × 10-6
E.
1.5 × 10-3


32.
What is the solubility, in moles per liter, of Fe(OH)2 (Ksp = 7.9 × 10-16) in 0.0500 molar NaOH solution?
A.
3.16 × 10-13
B.
3.13 × 10-16
C.
1.58 × 10-14
D.
1.14 × 10-14
E.
3.16 × 10-16


33.
What is the solubility, in moles per liter, of PbSO4 (Ksp = 6.3 × 10-7) in 0.0230 molar MgSO4 solution?
A.
2.14 × 10-5
B.
7.24 × 10-5
C.
2.74 × 10-5
D.
4.72 × 10-5
E.
4.27 × 10-5


34.
What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10) in 0.0300 M CaCl2 solution?
A.
9.0 × 10-3
B.
9.0 × 10-6
C.
6.0 × 10-9
D.
3.0 × 10-9
E.
6.0 × 10-3


35.
What is the solubility, in moles per liter, of BaSO4 (Ksp = 1.1 × 10-10) in 0.0100 M Na2SO4 solution?
A.
1.1 × 10-8
B.
1.1 × 10-6
C.
1.1 × 10-7
D.
1.1 × 10-5
E.
1.1 × 10-4


36.
What is the solubility, in moles per liter, of MgCO3 (Ksp = 3.5 × 10-8) in 0.0200 M Na2CO3 solution?
A.
4.4 × 10-6
B.
8.1 × 10-4
C.
4.4 × 10-3
D.
8.8 × 10-5
E.
1.8 × 10-6


37.
What is the solubility, in moles per liter, of Ag2CO3 (Ksp = 8.1 × 10-12) in 0.0300 M Na2CO3 solution?
A.
2.7 × 10-10
B.
9.0 × 10-9
C.
3.0 × 10-7
D.
4.0 × 10-10
E.
2.7 × 10-9


38.
What is the solubility, in moles per liter, of AgCl (Ksp = 1.8 × 10-10) in 0.0100 molar aqueous potassium chloride solution?
A.
7.5 × 10-5 mol L-1
B.
1.8 × 10-8 mol L-1
C.
1.3 × 10-6 mol L-1
D.
3.6 × 10-8 mol L-1
E.
1.5 × 10-7 mol L-1


39.
The solubility of barium sulfate varies with the composition of the solvent in which it was dissolved. In which solvent mixture would BaSO4 have the lowest solubility?
A.
pure water
B.
0.10 M Na2SO4(aq)
C.
1.0 M (NH4)2SO4(aq)
D.
0.5 M Ba(NO3)2(aq)
E.
1.0 M HCl(aq)


40.
Which solid would be more soluble in a strong acid solution than in pure water?
A.
KCl
B.
MgCl2
C.
NaNO3
D.
LiBr
E.
ZnCO3


41.
Which solid would be more soluble in a strong acid solution than in pure water?
A.
NaCl
B.
MgBr2
C.
LiNO3
D.
CaCO3
E.
AgBr


42.
What is the maximum concentration of Mg2+ ion that can exist in a 0.10 M NaF(aq) solution without causing any precipitate of magnesium fluoride to form? The Ksp of MgF2 is 6.6 × 10-9.
A.
1.3 × 10-7 M
B.
6.6 × 10-9 M
C.
6.6 × 10-8 M
D.
1.6 × 10-7 M
E.
6.6 × 10-7 M


43.
Calculate the minimum concentration of Ag+ ion that must be added to (or built up in) a 0.140 M Na2CrO4 solution in order to initiate a precipitation of silver chromate. The Ksp of Ag2CrO4 is 1.2 × 10-12.
A.
4.8 × 10-9 mol L-1
B.
2.9 × 10-6 mol L-1
C.
2.0 × 10-6 mol L-1
D.
9.5 × 10-7 mol L-1
E.
1.4 × 10-6 mol L-1


44.
The solubility product for Ag3PO4 is 2.8 × 10-18. What is the solubility of silver phosphate in solution which also contains 0.10 moles of silver nitrate per liter?
A.
4.4 × 10-4 mol L-1
B.
4.4 × 10-15 mol L-1
C.
2.8 × 10-15 mol L-1
D.
3.6 × 10-16 mol L-1
E.
2.8 × 10-13 mol L-1


45.
Will a precipitate form when 20.0 mL of 1.8 × 10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 × 10-4 M Na2SO4? The Ksp of (PbSO4) is 6.3 × 10-7.
A.
no, because the ion product < Ksp
B.
no, because the ion product > Ksp
C.
yes, because the ion product < Ksp
D.
yes, because the ion product > Ksp
E.
no, because Ksp is less than the ion product


46.
Will a precipitate of MgF2 form when 300 mL of 1.1 × 10-3 M MgCl2 solution is added to 500 mL of 1.2 × 10-3 M NaF? The Ksp of MgF2 is 6.9 × 10-9.
A.
yes, because the ion product, Q > Ksp
B.
no, because the ion product, Q < Ksp
C.
no, because the ion product, Q = Ksp
D.
yes, because the ion product, Q < Ksp
E.
no, because the ion product, Q > Ksp


47.
In an experiment, it is planned to add 300 mL of 2.0 × 10-5 M AgNO3 to 200 mL of 2.5 × 10-9 M NaI. Will a precipitate form? What is the precipitate? Ksp (AgI) = 8.3 × 10-17.
A.
yes, the ppt is AgNO3(s)
B.
yes, the ppt is NaNO3(s)
C.
yes, the ppt is NaI(s)
D.
yes, the ppt is AgI(s)
E.
no


48.
For PbCl2, Ksp = 1.7 × 10-5. Will a precipitate of PbCl2 form when 200 mL of 3.0 × 10-2 M Pb(NO3)2 solution is added to 300 mL of 5.0 × 10-2 M KCl? Choose one of the following.
A.
yes, the ion product, Q > Ksp
B.
no, the ion product, Q < Ksp
C.
no, the ion product, Q = Ksp
D.
yes, the ion product, Q < Ksp
E.
no, because the ion product, Q > Ksp


49.
Zinc carbonate, a slightly soluble substance, is most soluble in which of the following solvents?
A.
water
B.
0.1 M ZnCl2(aq)
C.
0.1 M NaOH(aq)
D.
0.1 M HCl(aq)
E.
0.2 M Na2CO3(aq)


50.
The pH of a saturated solution of cerium(III) hydroxide in water is 9.20. Calculate a value for the solubility product constant of cerium(III) hydroxide from this data.
A.
2.5 × 10-10
B.
8.4 × 10-11
C.
4.0 × 10-19
D.
2.1 × 10-20
E.
6.3 × 10-20



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