The solubility product $(K_{sp})$ for sodium chloride is $36 \text{ mol}^2/\text{L}^2$. The solubility of sodium chloride is:

The $K_{sp}$ expression for $Ca_3(PO_4)_2$ is:

The solubility of a sparingly soluble salt $AX_2$ is $1 \times 10^{-4} \ mol \ dm^{-3}$ at $298 \ K$. Calculate its solubility product $(K_{sp})$?

Assign $A, B, C, D$ from the given type of reaction: $PbCl_2(s) + \text{Hot water} \longrightarrow Pb^{2+}(aq) + 2Cl^{-}(aq)$

The concentration of $500 \ mL$ $NaOH$ solution is $0.02 \ M$. How many grams of $FeSO_4$ must be added to this solution to initiate the precipitation of $Fe(OH)_2$? The $K_{sp}$ of $Fe(OH)_2$ is $1.5 \times 10^{-15}$. The molecular mass of $FeSO_4$ is $152 \ g \ mol^{-1}$.

Sodium sulfate is soluble in water,whereas barium sulfate is sparingly soluble. Why?