The solubility-product constant for Zn(OH)_2 is K_sp = 3.00 times 10^-16. The fo

Question

The solubility-product constant for Zn(OH)_2 is K_sp = 3.00 times 10^-16. The formation constant for the hydroxyl complex, Zn(OH)_4^2, is K_1 = 4.60 times 10^17. A solubility-product constant, K_sp, corresponds to a reaction with the following general format: salt(s) cation(aq) + anion(aq) A formation constant K_f, corresponds to a reaction with the following general format: metal ion(aq) + Lewis base (aq) complex ion (aq) When Zn(OH)_2 (s) was added to 1.00 L of a basic solution. 1.25 times 10^-2 mol of the solid dissolved. What is the concentration of OH^- in the final solution?

Explanation / Answer

Solubility-product Ksp

3.00 x 10^-16 = [Zn+2] [OH-]^2

[Zn+2] = 3.00 x 10^-16 / [OH-]^2

the comlpex ion formation constant Kf
4.6 x 10^17 = [Zn(OH)4^2-] / [Zn+2] [OH-]^4

(4.6 x 10^17) = [Zn(OH)4^2-] [OH-]^2 / (3.00 x 10^-16)[OH-]^4

(3.00 x 10^-16) (4.6 x 10^17) = [Zn(OH)4^2-] / [OH-]^2

138 = [Zn(OH)4^2-] / [OH-]^2

[OH-]^2 = [Zn(OH)4^2-] / 138

[OH-]^2 = [1.25 x 10^2 ] / 138

[OH-]^2 = 9.06 x 10-5

[OH-] = 9.52 x 10-3 M

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