Multiple Choice
Given that the solubility product constant (Ksp) of C2D3 is 9.14 × 10^{-9}, what is the molar solubility of C2D3 in mol/L?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
For the salt AgCl, which dissociates as AgCl(s) ⇌ Ag^+(aq) + Cl^-(aq), how can the solubility product constant (K_{sp}) be expressed in terms of the molar solubility (s)?
A
K_{sp} = s^2
B
K_{sp} = s^3
C
K_{sp} = s
D
K_{sp} = 2s
Verified step by step guidance1
Identify the dissociation equation for AgCl: \(\mathrm{AgCl(s) \rightleftharpoons Ag^{+}(aq) + Cl^{-}(aq)}\).
Define the molar solubility \(s\) as the concentration of \(\mathrm{Ag^{+}}\) ions in solution at equilibrium, which is also equal to the concentration of \(\mathrm{Cl^{-}}\) ions because they dissociate in a 1:1 ratio.
Write the expression for the solubility product constant \(K_{sp}\) in terms of the ion concentrations: \(K_{sp} = [\mathrm{Ag^{+}}][\mathrm{Cl^{-}}]\).
Substitute the molar solubility \(s\) into the expression, since \([\mathrm{Ag^{+}}] = s\) and \([\mathrm{Cl^{-}}] = s\), so \(K_{sp} = s \times s\).
Simplify the expression to get \(K_{sp} = s^{2}\), which relates the solubility product constant to the molar solubility.
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