Multiple Choice
A saturated solution of PbCl2 has [Cl^-] = 2.86×10^-2 M. What is the concentration of Pb^2+? Given that Ksp = 1.17 × 10^-5.
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
2.71×10⁻⁵ mol/L
B
1.31×10⁻³ mol/L
C
3.02×10⁻⁴ mol/L
D
9.14×10⁻⁹ 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).
Define the molar solubility of C2D3 as 's'. This means that at equilibrium, the concentration of C⁺ ions will be 2s and the concentration of D⁻ ions will be 3s.
Write the expression for the solubility product constant (Ksp) based on the dissociation equation: Ksp = [C⁺]²[D⁻]³.
Substitute the expressions for the ion concentrations in terms of 's' into the Ksp expression: Ksp = (2s)²(3s)³.
Set the Ksp expression equal to the given Ksp value (9.14×10⁻⁹) and solve for 's' to find the molar solubility of C2D3.
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