Multiple Choice
What is the molar solubility of barium fluoride (BaF₂) in a 0.12 M Ba(NO₃)₂ solution, given that the solubility product constant (Ksp) for BaF₂ is 2.45 × 10⁻⁵?
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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Calculate the molar solubility of tin(II) hydroxide (Sn(OH)₂) in pure water given that its solubility product constant (Ksp) is 5.45 x 10⁻²⁷.
A
2.27 x 10⁻¹⁴ M
B
1.04 x 10⁻⁹ M
C
3.27 x 10⁻⁷ M
D
5.45 x 10⁻²⁷ M
Verified step by step guidance1
Write the balanced dissolution equation for tin(II) hydroxide: Sn(OH)₂(s) ⇌ Sn²⁺(aq) + 2OH⁻(aq).
Express the solubility product constant (Ksp) in terms of the concentrations of the ions: Ksp = [Sn²⁺][OH⁻]².
Let 's' be the molar solubility of Sn(OH)₂. At equilibrium, [Sn²⁺] = s and [OH⁻] = 2s.
Substitute the expressions for the ion concentrations into the Ksp expression: Ksp = (s)(2s)² = 4s³.
Solve for 's' by setting 4s³ equal to the given Ksp value (5.45 x 10⁻²⁷) and solve for s to find the molar solubility.
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