Mg(OH)2 is a sparingly soluble compound, in this case, a base, with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams.
Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in pure H2O?
Let "S" be the molar solubility of Mg(OH)2 in water
As it is a sparingly soluble, there exists an equilibrium between soluble substance and insoluble substance.
The equilibrium is shown as
Mg(OH)2 ⇌ Mg+2 + 2 OH-
S S 2S
[Mg(OH)]e = S
[Mg2+] = S
[OH-] = 2S
KSP is given by
KSP = [Mg2+][OH-]2
= S. (2S)2
KSP = 4S3
S3 = Ksp/4
S = (Ksp/4)1/3
Given that Ksp = 5.61×10-11
S = (5.61×10-11/4)1/3
S = (1.45×10-11/4)1/3
S = (0.145*10-12)1/3
= 0.525*10-4
= 5.25*10-3 M
Molar solubility of Magnesium hydroxide = 5.25*10-3 M
Mg(OH)2 is a sparingly soluble compound, in this case, a base, with a solubility product, Ksp,...
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