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Given the solubility product constant (Ksp) of NiS is 3.0 x 10^-15, determine the molar solubility of NiS in 0.052 M K2C2O4.
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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In water, the solubility of Bi(OH)3 is 2.87 × 10⁻⁷ M. Calculate the solubility product constant (Ksp) for Bi(OH)3.
A
Ksp = 5.67 × 10⁻²²
B
Ksp = 8.23 × 10⁻²¹
C
Ksp = 2.36 × 10⁻²⁰
D
Ksp = 1.23 × 10⁻¹⁹
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Start by writing the balanced dissolution equation for Bi(OH)₃ in water: Bi(OH)₃(s) ⇌ Bi³⁺(aq) + 3OH⁻(aq).
Identify the stoichiometry of the dissolution process: 1 mole of Bi(OH)₃ produces 1 mole of Bi³⁺ ions and 3 moles of OH⁻ ions.
Let the solubility of Bi(OH)₃ be represented by 's', which is given as 2.87 × 10⁻⁷ M. Therefore, [Bi³⁺] = s and [OH⁻] = 3s.
Write the expression for the solubility product constant (Ksp): Ksp = [Bi³⁺][OH⁻]³.
Substitute the concentrations into the Ksp expression: Ksp = (s)(3s)³ = s × 27s³ = 27s⁴. Use the given solubility value to calculate Ksp.
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