Question

The solubility of Zn(OH)2 is 2.0 x 10^-6 mol/L at a certain temperature. Determine the value of the Ksp at this same temperature.

A) 2.0x10^-6
B.) 4.0x10^-6
C.) 8.0x10^-17
D.) 3.2x10^-17

Answer 1

D) Ksp = 3.2 × 10⁻¹⁷

Step-by-step explanation:

Let's consider the solution of Zn(OH)₂.

Zn(OH)₂(s) ⇄ Zn²⁺(aq) + 2 OH⁻(aq)

We can relate the molar solubility (S) with the solubility product constant (Ksp) using an ICE chart.

Zn(OH)₂(s) ⇄ Zn²⁺(aq) + 2 OH⁻(aq)

I 0 0

C +S +2S

E S 2S

The solubility product constant (Ksp) is:

`Ksp = [Zn^(2+) ]* [OH^(-) ]^(2) =S * (2S)^(2) =4S^(3) =4(2.0 * 10^(-6) )^(3) = 3.2 * 10^(-17)`