Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.K_sp (CuCl)= 1.0 × 10^-6. A)1.0 × 10^-12 M B)5.0 × 10^-7 M C)2.0 × 10^-5 M D)1.0 × 10^-3 M E)0.050 M

Question

Quizplus · Accepted Answer

The solubility product constant (Ksp) for CuCl is 1.0 × 10^-6. The equilibrium reaction for the dissolution of CuCl is:

CuCl ⇌ Cu+ + Cl-

If we let the molar solubility of CuCl be represented by x, then the equilibrium concentrations of Cu+ and Cl- are both equal to x. The concentration of K+ and Cl- from KCl do not affect the dissolution of CuCl, since they are in a different ionic equation.

The Ksp expression for CuCl is:

Ksp = [Cu+][Cl-] = x^2

Substituting the given value of Ksp, we get:

1.0 × 10^-6 = x^2

Taking the square root of both sides gives:

x = 2.0 × 10^-5 M

Therefore, the molar solubility of CuCl in the presence of 0.050 M KCl is 2.0 × 10^-5 M.

Determine the Molar Solubility of CuCl in a Solution Containing