Multiple Choice
The solubility of Ni₃(PO₄)₂ in water at a particular temperature is 8.0 × 10⁻⁶ M. What is the solubility product constant (Ksp) for Ni₃(PO₄)₂?
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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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?
A
1.23×10⁻¹⁵
B
4.39×10⁻²³
C
5.00×10⁻²⁴
D
9.84×10⁻¹⁶
Verified step by step guidance1
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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