What is the solubility in moles/liter for copper(I) chloride at 25 oC given a Ksp value of 1 x 10-6

To find the solubility of copper(I) chloride (CuCl) in moles per liter (M) at 25 oC using the given Ksp value, we need to use the principles of equilibrium and stoichiometry.

First, let's write the balanced chemical equation for the dissolution of copper(I) chloride:

CuCl (s) ⇌ Cu+ (aq) + Cl- (aq)

Based on the balanced equation, we can see that for every mole of copper(I) chloride that dissolves, one mole of Cu+ ions and one mole of Cl- ions are produced.

Let's assume the solubility of copper(I) chloride be 'x' M.

The equilibrium expression, Ksp, can be expressed as the product of the concentrations of the dissociated ions raised to their stoichiometric coefficients:

Ksp = [Cu+] * [Cl-]

Substituting the given Ksp value, we have:

1 x 10^-6 = x * x

Simplifying the equation, we get:

1 x 10^-6 = x^2

Taking the square root of both sides, we find:

x = √(1 x 10^-6) ≈ 1 x 10^-3 M

Therefore, the solubility of copper(I) chloride in moles per liter (M) at 25 oC is approximately 1 x 10^-3 M.