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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

Respuesta :

dsdrajlin

Answer:

D) Ksp = 3.2 × 10⁻¹⁷

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:

[tex]Ksp = [Zn^{2+} ]\times [OH^{-} ]^{2} =S \times (2S)^{2} =4S^{3} =4(2.0 \times 10^{-6} )^{3} = 3.2 \times 10^{-17}[/tex]

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