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?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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Solubility of Sn(OH)2 was found to be 1.11 x 10-9 M; calculate Ksp of this compound.
A
5.47 × 10−27
B
4.44 × 10−9
C
1.23 × 10−18
D
1.37 × 10−27
Verified step by step guidance1
Understand the dissolution process of Sn(OH)2 in water. The compound dissociates into Sn²⁺ and OH⁻ ions. The balanced chemical equation for this process is: Sn(OH)₂(s) ⇌ Sn²⁺(aq) + 2OH⁻(aq).
Identify the expression for the solubility product constant (Ksp) for Sn(OH)₂. The Ksp expression is derived from the equilibrium concentrations of the ions: Ksp = [Sn²⁺][OH⁻]².
Recognize that the solubility of Sn(OH)₂ is given as 1.11 x 10⁻⁹ M, which represents the concentration of Sn²⁺ ions at equilibrium. Therefore, [Sn²⁺] = 1.11 x 10⁻⁹ M.
Determine the concentration of OH⁻ ions. Since each formula unit of Sn(OH)₂ produces two OH⁻ ions, the concentration of OH⁻ ions is twice the solubility of Sn(OH)₂: [OH⁻] = 2 x 1.11 x 10⁻⁹ M.
Substitute the concentrations into the Ksp expression: Ksp = (1.11 x 10⁻⁹) * (2 x 1.11 x 10⁻⁹)². Calculate the Ksp value using these concentrations.
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