Table of contents

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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Multiple Choice

C2D3 has a solubility product constant (Ksp) of 9.14 × 10⁻⁹. What is the molar solubility of C2D3 in mol/L?

2.14 × 10⁻⁴ mol/L

1.31 × 10⁻³ mol/L

4.57 × 10⁻⁴ mol/L

3.02 × 10⁻³ mol/L

Verified step by step guidance

Identify the dissociation equation for C2D3 in water. Assume it dissociates into its ions: C2D3(s) ⇌ 2C⁺(aq) + 3D⁻(aq).

Express the solubility product constant (Ksp) in terms of the concentrations of the ions at equilibrium: Ksp = [C⁺]²[D⁻]³.

Let 's' be the molar solubility of C2D3. At equilibrium, [C⁺] = 2s and [D⁻] = 3s.

Substitute the expressions for the ion concentrations into the Ksp expression: Ksp = (2s)²(3s)³.

Solve the equation for 's' by substituting the given Ksp value (9.14 × 10⁻⁹) and simplifying the expression to find the molar solubility.

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