A hypothetical compound mx3 has a molar solubility of 0.00562 m. What is the value of ksp for mx3?

Ksp = 2.6935 * 10^-8 mol^4 dm^-12

Explanation:

In this question, we are asked to calculate the ksp value for a hypothetical compound having molar solubility of 0.00562

Firstly, let us write the dissociation equation for the hypothetical compound.

MX3 ——-> M+ + 3X-

Let’s get the molar solubilities of the component of dissociation

1 mole of MX3 gave 1 mole of M, this means that the molar solubility of M = 0.00562mol/dm^3

1 mole of MX3 yielded 3 moles of the anion X. This means that the molar solubility of X = 0.00562 * 3 = 0.01686 mol/dm^3

Ksp = [M+][ X-]^3

Ksp = 0.00562 * 0.01686^3

Ksp = 2.6935 * 10^-8 mol^4 dm^-12

what is the actual question though?