Ab2 has a molar solubility of 3.72×10−4 m. what is the value of the solubility product constant for ab2?

Solubility product constants are values to describe the saturation of ionic compounds with low solubility. A saturated solution is when there is a dynamic equilibrium between the solute dissolved, the dissociated ions, the undissolved and the compound. It is calculated from the product of the ion concentration in the solution. For the generic salt, AB2, the dissociation would  be as follows:

AB2 = A2+ + 2B-

So, the expression for the solubility product would be:

Ksp = [A2+] [B-]^2
Ksp = [x] [2x]^2 = 4x^3

where x = 3.72×10^−4 M

Ksp = 4( 3.72×10^−4 )^3
Ksp = 2.06x10^-10 M^3

The solubility product constant of AB2 would be Ksp = 2.06x10^-10 M^3.

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