Question

Use the Ksp values to calculate the molar solubility of each of the following compounds in...

Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.

Part A MX (Ksp = 9.20×10−11) Express your answer in moles per liter.

Part B Ag2CrO4 (Ksp = 1.12×10−12)

Part C Ca(OH)2 (Ksp = 4.68×10−6) Express your answer in moles per liter.

Homework Answers

Answer #1

A)

The salt dissolves as:

MX <----> M+ + X-

   s s

Ksp = [M+][X-]

9.2*10^-11=(s)*(s)

9.2*10^-11= 1(s)^2

s = 9.592*10^-6 M

Answer: 9.59*10^-6 moles/L

B)

The salt dissolves as:

Ag2CrO4 <----> 2 Ag+ + CrO42-

   2s s

Ksp = [Ag+]^2[CrO42-]

1.12*10^-12=(2s)^2*(s)

1.12*10^-12= 4(s)^3

s = 6.542*10^-5 M

Answer: 6.54*10^-5 moles/L

C)

The salt dissolves as:

Ca(OH)2 <----> Ca2+ + 2 OH-

   s 2s

Ksp = [Ca2+][OH-]^2

4.68*10^-6=(s)*(2s)^2

4.68*10^-6= 4(s)^3

s = 1.054*10^-2 M

Answer: 1.05*10^-2 moles/L

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