Question
The molar solubility of ZnS is 1.6 × 10-10 M in pure water at a certain temperature. Calculate the Ksp for ZnS at this temperature.
Answers
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The solubility product constant, Ksp, is defined as the product of the concentrations of the ions in a saturated solution of a compound. In the case of ZnS, it can be represented as:
ZnS (s) ⇌ Zn²⁺ (aq) + S²⁻ (aq)
The molar solubility of ZnS in pure water is given as 1.6 × 10^-10 M. This means that at equilibrium, the concentration of Zn²⁺ and S²⁻ ions in the solution is 1.6 × 10^-10 M.
Therefore, the Ksp for ZnS can be calculated as follows:
Ksp = [Zn²⁺] × [S²⁻]
Since the molar solubility of ZnS is 1.6 × 10^-10 M, the concentration of Zn²⁺ and S²⁻ ions is also 1.6 × 10^-10 M.
Ksp = (1.6 × 10^-10 M) × (1.6 × 10^-10 M)
Ksp = 2.56 × 10^-20 M²
Therefore, the Ksp for ZnS at this temperature is 2.56 × 10^-20 M².
ZnS (s) ⇌ Zn²⁺ (aq) + S²⁻ (aq)
The molar solubility of ZnS in pure water is given as 1.6 × 10^-10 M. This means that at equilibrium, the concentration of Zn²⁺ and S²⁻ ions in the solution is 1.6 × 10^-10 M.
Therefore, the Ksp for ZnS can be calculated as follows:
Ksp = [Zn²⁺] × [S²⁻]
Since the molar solubility of ZnS is 1.6 × 10^-10 M, the concentration of Zn²⁺ and S²⁻ ions is also 1.6 × 10^-10 M.
Ksp = (1.6 × 10^-10 M) × (1.6 × 10^-10 M)
Ksp = 2.56 × 10^-20 M²
Therefore, the Ksp for ZnS at this temperature is 2.56 × 10^-20 M².