Table of contents

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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Multiple Choice

Given the molar solubility of Pd(SCN)₂ in pure water is 2.22×10⁻⁸ M, what is the solubility product constant (Ksp) for Pd(SCN)₂?

1.23×10⁻¹⁵

4.39×10⁻²³

5.00×10⁻²⁴

9.84×10⁻¹⁶

Verified step by step guidance

Identify the dissociation equation for Pd(SCN)₂ in water: Pd(SCN)₂(s) ⇌ Pd²⁺(aq) + 2 SCN⁻(aq).

Recognize that the molar solubility of Pd(SCN)₂ is given as 2.22×10⁻⁸ M, which means [Pd²⁺] = 2.22×10⁻⁸ M at equilibrium.

Since each formula unit of Pd(SCN)₂ produces one Pd²⁺ ion and two SCN⁻ ions, the concentration of SCN⁻ ions at equilibrium will be 2 × 2.22×10⁻⁸ M.

Write the expression for the solubility product constant (Ksp): Ksp = [Pd²⁺][SCN⁻]².

Substitute the equilibrium concentrations into the Ksp expression: Ksp = (2.22×10⁻⁸) × (2 × 2.22×10⁻⁸)² and simplify to find the Ksp value.

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