The solubility of salt $AX_2$ is $6 \times 10^{-12} \text{ mol dm}^{-3}$. What is the solubility product $(K_{sp})$ of the salt?

Calculate the molar solubility of $Ni(OH)_{2}$ in $0.10 \, M$ $NaOH$. The solubility product constant $(K_{sp})$ of $Ni(OH)_{2}$ is $2.0 \times 10^{-15}$.

The solubility product of $Ag_2CO_3$ and $FeCO_3$ in water at $25 \, ^\circ C$ are $4 \times 10^{-12}$ and $2.5 \times 10^{-11}$ respectively. If $S_1$ and $S_2$ are their solubilities in water respectively when dissolved separately,then $S_1/S_2$ is

The molar solubility $(mol \ L^{-1})$ of a sparingly soluble salt $MX_4$ is $s$. The corresponding solubility product is $K_{sp}$. $s$ is given in terms of $K_{sp}$ by the relation:

If $pH$ of a saturated solution of $Ba(OH)_2$ is $12$,the value of its $K_{sp}$ is

Explain the difference between ionic product and solubility product. Explain the condition for the precipitation of a sparingly soluble salt.