The formula to calculate the molar solubility (S) is:
\[ S = \sqrt{\frac{Ksp}{c₁ \times c₂}} \]
Where:
Ksp, or the solubility product constant, is a measure of the solubility of a compound in water. It is the product of the concentrations of the ions each raised to the power of their coefficients in the balanced equation. Ksp is used to predict whether a precipitate will form when two solutions are mixed, and to calculate the solubility of a compound under various conditions.
For example, if the Ksp is \( 1.0 \times 10^{-10} \), the coefficient of ion 1 (c₁) is 1, and the coefficient of ion 2 (c₂) is 1, the molar solubility (S) can be calculated as follows:
\[ S = \sqrt{\frac{1.0 \times 10^{-10}}{1 \times 1}} = \sqrt{1.0 \times 10^{-10}} = 1.0 \times 10^{-5} \text{ mol/L} \]
So, the molar solubility for these values is \( 1.0 \times 10^{-5} \) mol/L.