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⁻²calculate the equilibrium constant for the following reaction:

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

Answer 1

To calculate the equilibrium constant for the given reaction, we need to use the solubility product constant (Ksp) and the individual equilibrium constants for each species involved. By relating the concentrations of AgCl⁻², Ag⁺, Cl⁻, and H₂S, we can determine the equilibrium constant. The equilibrium constant for the reaction Ag₂S(s) + 4Cl⁻(aq) + 2H⁺(aq) ⇌ 2AgCl⁻²(aq) + H₂S(aq) is 1.3 × 10⁻¹³.

Step-by-step explanation:

To calculate the equilibrium constant for the reaction Ag₂S(s) + 4Cl⁻(aq) + 2H⁺(aq) ⇌ 2AgCl⁻²(aq) + H₂S(aq), we need to consider the individual equilibrium constants and the stoichiometric coefficients of the reactants and products.

First, let's write down the expression for the solubility product constant (Ksp) of Ag₂S:

Ksp = [Ag⁺]²[S²⁻]

Since we are interested in the concentration of AgCl⁻² in the final equation, we need to relate it to the concentration of Ag⁺ and Cl⁻.

By considering the individual equilibrium constants and the stoichiometric coefficients, we can write:

Ksp = [AgCl⁻²]²[H₂S]

Finally, by substituting the given values, we have:

Ksp = (1.1 × 10⁵)² / ((9.5 × 10⁻⁸)² × (6 × 10⁻⁵¹))

= 1.3 × 10⁻¹³