± Solubility of Zinc Hydroxide in Basic Solution The formation constant for the
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Question
± Solubility of Zinc Hydroxide in Basic Solution
The formation constant for the hydroxo complex, Zn(OH)42, is Kf=4.60×1017.
A solubility-product constant, Ksp, corresponds to a reaction with the following general format:
salt(s)cation(aq)+anion(aq)
A formation constant, Kf, corresponds to a reaction with the following general format:
metal ion(aq)+Lewis base(aq)complex ion(aq)
Part A
When Zn(OH)2(s) was added to 1.00 L of a basic solution, 1.01×102 mol of the solid dissolved. What is the concentration of OH in the final solution?
Express your answer with the appropriate units.
Hints
± Solubility of Zinc Hydroxide in Basic Solution
The solubility-product constant for Zn(OH)2 is Ksp=3.00×1016.The formation constant for the hydroxo complex, Zn(OH)42, is Kf=4.60×1017.
A solubility-product constant, Ksp, corresponds to a reaction with the following general format:
salt(s)cation(aq)+anion(aq)
A formation constant, Kf, corresponds to a reaction with the following general format:
metal ion(aq)+Lewis base(aq)complex ion(aq)
Part A
When Zn(OH)2(s) was added to 1.00 L of a basic solution, 1.01×102 mol of the solid dissolved. What is the concentration of OH in the final solution?
Express your answer with the appropriate units.
Hints
[OH] =Explanation / Answer
Solubility product constant
3.00 e-16 = [Zn+2] [OH-]^2
so
[Zn+2] = 3.00 e-16 / [OH-]^2
the formation constant for comlpex ion
4.6 e17 = [Zn(OH)4^2-] / [Zn+2] [OH-]^4
so
[Zn+2] = [Zn(OH)4^2-] / [OH-]^4 (4.6 e17)
Both concentration of Zn+2 must be equal
[Zn+2] = [Zn+2]
then
(3.00 e-16) / [OH-]^2 = [Zn(OH)4^2-] / [OH-]^4 (4.6 e17)
(3.00 e-10) (4.6 e+17) = [Zn(OH)4^2-] [OH-]^2 / [OH-]^4
1380= [Zn(OH)4^2-] / [OH-]^2
[OH-]^2 = [Zn(OH)4^2-] / 1380
[OH-]^2 = [1.01×10^2 ] / 1380
[OH-]^2 = 7.3188 e-6
[OH] = 0.0027
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