Question

Using the value of Ksp=6×10⁻⁵¹ for Ag₂S, Ka₁=9.5×10⁻⁸ and Ka₂=1×10⁻¹⁹ for H₂S, and Kf=1.1×10⁵ for AgCl⁻², calculate theequilibrium constant for the following reaction:

Ag₂S(s)+4Cl⁻(aq)+2H⁺(aq)⇌2AgCl⁻2(aq)+H₂S(aq)

Answer 1

The equilibrium constant, K, can be calculated using the relationship between the individual equilibrium constants, Ksp, Ka₁, Ka₂, and Kf. Given the values of these constants, the equilibrium constant for the given reaction can be calculated using the respective expressions. Plug in the given equilibrium constants and solve for the equilibrium constant, K.

Step-by-step explanation:

The equilibrium constant, K, is the ratio of the product concentrations raised to their stoichiometric coefficients to the reactant concentrations raised to their stoichiometric coefficients, with each concentration term raised to the power of its coefficient in the balanced chemical equation. In this case, the equilibrium constant for the given reaction: Ag₂S(s) + 4Cl⁻(aq) + 2H⁺(aq) ⇌ 2AgCl⁻²(aq) + H₂S(aq), can be calculated using the relationship between the individual equilibrium constants, Ksp, Ka₁, Ka₂, and Kf.

The Ksp expression for AgCl can be written as [Ag+][Cl¯], and the Ka expression for H₂S can be written as [H⁺][HS¯]/[H₂S]. According to the reaction, 2 AgCl⁻²(aq) + H₂S(aq) ⇌ Ag₂S(s) + 4 Cl⁻(aq) + 2 H⁺(aq), we can write the equilibrium constant expression as K = [Ag₂S][Cl⁻]⁴[H⁺]²/[AgCl]²[HS¯][H₂S]². Now, we can substitute the given equilibrium constants into the expression and solve for the equilibrium constant.

Given Ksp = 6×10⁻⁵¹ for Ag₂S, Ka₁ = 9.5×10⁻⁸ for H₂S, Ka₂ = 1×10⁻¹⁹ for H₂S, and Kf = 1.1×10⁵ for AgCl⁻², we can plug these values into the expression and calculate the equilibrium constant, K.