Question

The generic metal hydroxide M(OH)2 has Ksp = 8.25×10−18. (NOTE: In this particular problem, because of...

The generic metal hydroxide M(OH)2 has Ksp = 8.25×10−18. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH− from water can be ignored. However, this may not always be the case.)

Part A: What is the solubility of M(OH)2 in pure water?

Part B: What is the solubility of M(OH)2 in a 0.202 M solution of M(NO3)2?

Homework Answers

Answer #1

Given: Ksp = 8.25 x 10-18

Part A: M(OH)2 M2+ + 2 OH-

Ksp = [M2+] [OH-]2

Ksp = (x) (2x)2

Ksp = 4x3 = 8.25 x 10-18

(x = Solubility)

x = (8.25 x 10-18 / 4)1/3

x = 1.27 x 10-6 M

Part B: In the presence of 0.202 M solution of M(NO3)2

As M(NO3)2 is a strong electrolyte, it will dissociate fully

M(NO3)2 M2+ + 2 NO3-

Now [M2+] = x + 0.202 and OH- will remain same.

Ksp = (x + 0.202) (2x)2 = 8.25 x 10-18

We can neglect x in comparison to 0.202 as we know value of x is very small.

Ksp = 0.202 (4x2) = 0.808x2 = 8.25 x 10-18

x = ( 8.25 x 10-18 / 0.808)1/2

x = 3.19 x 10-9 M

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