Multiple Choice
Given that the solubility product constant K_{sp} for Cr(OH)_3 is 6.70 imes 10^{-31}, what is the molar solubility of Cr(OH)_3 at pH 11.10?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
Complete the following solubility product constant expression for the dissolution of silver chloride (AgCl) in water: AgCl(s) ⇌ Ag^+(aq) + Cl^-(aq). Which of the following correctly represents the K_{sp} expression for AgCl?
A
K_{sp} = [AgCl]/([Ag^+][Cl^-])
B
K_{sp} = [Ag^+][Cl^-]
C
K_{sp} = [Ag^+]^2[Cl^-]
D
K_{sp} = [Ag^+][Cl^-]/[AgCl]
Verified step by step guidance1
Identify the dissolution reaction: AgCl(s) ⇌ Ag^{+}(aq) + Cl^{-}(aq). Here, solid AgCl dissociates into its ions in aqueous solution.
Recall that the solubility product constant, K_{sp}, is defined using the concentrations of the dissolved ions only, not the solid phase, because the activity of a pure solid is constant and incorporated into the equilibrium constant.
Write the general expression for K_{sp} as the product of the molar concentrations of the ions, each raised to the power of their stoichiometric coefficients: \(K_{sp} = [Ag^{+}]^{1} \times [Cl^{-}]^{1}\).
Since both ions have a coefficient of 1, the expression simplifies to \(K_{sp} = [Ag^{+}][Cl^{-}]\).
Therefore, the correct K_{sp} expression excludes the solid AgCl concentration and does not include any squared terms for the ions in this case.
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