Answer: The equilibrium constant, K, for the given reaction can be calculated using the acid dissociation constants and the solubility product constant.
The balanced chemical equation for the reaction is:
ZnS(s) + 2H⁺(aq) → Zn²⁺(aq) + H₂S(aq)
The equilibrium constant expression for this reaction is:
K = [Zn²⁺][H₂S] / [H⁺]²
Given information:
- The successive acid dissociation constants for H₂S are Ka1 = 9.50 × 10⁻⁸ and Ka2 = 1.00 × 10⁻¹⁹
- The solubility product constant of zinc sulfide (ZnS) equals Ksp = 1.60 × 10⁻²⁴
To find the equilibrium constant, we need to consider the ionization of H₂S and the solubility of ZnS. However, the given information does not directly provide the concentration of Zn²⁺, so it's not possible to calculate the equilibrium constant without additional information about the concentrations of the reactants and products at equilibrium.
Explanation: Okay, let's go through the step-by-step explanation:
1. The balanced chemical equation for the given reaction is:
ZnS(s) + 2H⁺(aq) ⇌ Zn²⁺(aq) + H₂S(aq)
2. The equilibrium constant (K) for this reaction is defined as:
K = [Zn²⁺][H₂S] / [H⁺]²
3. To find the value of K, we need to relate the concentrations of the reactants and products at equilibrium.
4. The given information provides the successive acid dissociation constants (Ka1 and Ka2) for H₂S:
Ka1 = 9.50 × 10⁻⁸
Ka2 = 1.00 × 10⁻¹⁹
5. These acid dissociation constants can be used to determine the equilibrium concentrations of H₂S, HS⁻, and S²⁻ in the solution.
6. However, the given information does not provide the initial concentration of ZnS or the initial concentration of H⁺. Without this information, it is not possible to calculate the equilibrium concentrations of Zn²⁺ and H₂S.
7. The only additional information provided is the solubility product constant (Ksp) of ZnS, which is 1.60 × 10⁻²⁴.
8. The Ksp value alone is not sufficient to determine the equilibrium concentrations of the reactants and products, as we still need to know the initial concentrations or the amount of ZnS dissolved.
In summary, while the given information provides the necessary acid dissociation constants and the solubility product constant, the lack of initial concentrations or other parameters prevents us from calculating the equilibrium constant (K) for the given reaction. Additional information would be required to determine the value of K.
