The solubility of AgCl in pure water is 0.000012 M. Calculate the value of solubility product constant
The solubility product constant (Ksp) is a measure of the extent to which a sparingly soluble salt dissociates into its ions in a solution and is calculated using the concentrations of the ions involved.
To calculate the value of the solubility product constant (Ksp) for AgCl, we can use the solubility of AgCl in pure water.
Given that the solubility of AgCl in pure water is 0.000012 M, we can assume that AgCl dissociates into Ag⁺ and Cl⁻ ions and their concentrations in the solution are also 0.000012 M.
The chemical equation for the dissociation of AgCl can be written as:
AgCl(s) ⇌ Ag⁺(aq) + Cl⁻(aq)
The solubility product constant (Ksp) is the product of the concentrations of the dissociated ions raised to the power of their stoichiometric coefficients. In this case, both the Ag⁺ and Cl⁻ ions have a stoichiometric coefficient of 1.
Therefore, the Ksp for AgCl can be calculated as:
Ksp = [Ag⁺][Cl⁻]
Given that both [Ag⁺] and [Cl⁻] are 0.000012 M:
Ksp = (0.000012 M) × (0.000012 M) = 1.44 × 10^(-10)
Therefore, the value of the solubility product constant (Ksp) for AgCl is 1.44 × 10^(-10).
...................AgCl ==> Ag^+ + Cl^-
I.................solid...........0...........0
C,,,,,,,,,,,,,,,,solid...........x...........x
E..................solid..........x...........x
Ksp = (Ag^+)(Cl^-) = (1.2E-5)(1.2E-5) = ?