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Section 3: Using Equilibrium Constants

Using Equilibrium Constants

1.
Which of the solubility product expressions is incorrect?
A)Ksp(Ag2S) = [Ag+]2[S2-]
B)Ksp (Sb2S3) = [Sb2+]3[S3-]2
C)Ksp (CaF2) = [Ca2+][F-]2
D)Ksp(CuS) = [Cu2+][S2-]
2.
The molar solubility for BaCO3 is 9.0 x 10-5M at 25°C. What is the solubility product constant, Ksp, for BaCO3?
A)1.2 x 10-8
B)8.1 x 10-9
C)5.3 x 10-12
D)4.0 x 10-15
3.
The value of the Ksp for SrSO4 is 2.8 x 10-7. What is the molar solubility of SrSO4?
A)7.6 x 10-7M
B)5.8 x 10-13M
C)5.3 x 10-4M
D)5.7 x 10-3M
4.
If NaCl is added to a 0.010M solution of AgNO3 in water at 25°C, what will be [Cl-] when precipitation of AgCl begins? The Ksp for AgCl is 1.8 x 10-10.
A)1.0 x 10-10M
B)1.3 x 10-6M
C)1.8 x 10-8M
D)1.8 x 10-12M
5.
How many grams of MgF2 will dissolve in 150 mL of 0.100M NaF solution? Ksp for MgF2 is 6.4 x 10-9.
A)6.4 x 10-7 g
B)4.1 x 10-6 g
C)1.0 x 10-5 g
D)6.0 x 10-6 g
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