Use the appropriate values of K_sp and K_f to find the equilibrium constant for the reaction. PbCl₂(s) + 3 OH^-(aq) ⇌ Pb(OH)₃^-(aq) + 2 Cl^-(aq)

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Identify the relevant equilibrium reactions and their constants: (1) The dissolution of PbCl_2: PbCl_2(s) ⇌ Pb^{2+}(aq) + 2 Cl^-(aq) with K_{sp}, and (2) The formation of Pb(OH)_3^-: Pb^{2+}(aq) + 3 OH^-(aq) ⇌ Pb(OH)_3^-(aq) with K_f.

Write the expression for the equilibrium constant K_{sp} for the dissolution of PbCl_2: K_{sp} = [Pb^{2+}][Cl^-]^2.

Write the expression for the formation constant K_f for the complex ion formation: K_f = [Pb(OH)_3^-]/([Pb^{2+}][OH^-]^3).

Combine the two reactions to obtain the overall reaction: PbCl_2(s) + 3 OH^-(aq) ⇌ Pb(OH)_3^-(aq) + 2 Cl^-(aq).

Calculate the equilibrium constant for the overall reaction by multiplying the K_{sp} and K_f: K_{overall} = K_{sp} * K_f.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It quantifies the extent to which a compound can dissolve in water, represented by the concentrations of its ions at equilibrium. For example, for PbCl2, Ksp is calculated from the concentrations of Pb²⁺ and Cl⁻ ions in solution, allowing us to understand its solubility behavior.

Formation Constant (Kf)

The formation constant (Kf) is a measure of the stability of a complex ion in solution, representing the equilibrium between the complex and its constituent ions. It is defined for the reaction where ions combine to form a complex, such as Pb(OH)3⁻ in this case. A higher Kf value indicates a more stable complex, which is crucial for predicting the direction of the reaction and the concentrations of species at equilibrium.

Equilibrium Constant (K)

The equilibrium constant (K) for a reaction is a ratio of the concentrations of products to reactants, each raised to the power of their coefficients in the balanced equation. It provides insight into the position of equilibrium and the extent of the reaction. In this case, the equilibrium constant for the given reaction can be derived from the Ksp and Kf values, allowing us to determine how the reaction favors the formation of products or reactants.

Use the appropriate values of Ksp and Kf to find the equilibrium constant for the reaction. PbCl2(s) + 3 OH-(aq) ⇌ Pb(OH)3-(aq) + 2 Cl-(aq)