Multiple Choice
A solution is 0.040 M in Pb²⁺. What minimum concentration of Cl⁻ is required to begin to precipitate PbCl₂? For PbCl₂, Ksp = 1.17×10⁻⁵.
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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C2D3 has a solubility product constant (Ksp) of 9.14 × 10⁻⁹. What is the molar solubility of C2D3 in mol/L?
A
2.14 × 10⁻⁴ mol/L
B
1.31 × 10⁻³ mol/L
C
4.57 × 10⁻⁴ mol/L
D
3.02 × 10⁻³ mol/L
Verified step by step guidance1
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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