Solubility of an $MX_2$ type electrolyte is $0.5 \times 10^{-4} \ mol/L$,then $K_{sp}$ of electrolyte is

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

The solubility products of some sparingly soluble electrolytes are given below. The increasing order of their molar solubility is:
$(a)$ Formula: $MX$,$K_{sp} = 4.0 \times 10^{-20}$
$(b)$ Formula: $P_2Q$,$K_{sp} = 3.2 \times 10^{-11}$
$(c)$ Formula: $LY_3$,$K_{sp} = 2.7 \times 10^{-31}$

Calculate the solubility in $mol \ dm^{-3}$ of sparingly soluble salt $BA$ if its solubility product is $4.9 \times 10^{-13}$ at the same temperature.

$A$ saturated solution of $Ag_2SO_4$ is $2.5 \times 10^{-2} \ M$. The value of its solubility product is:

The solubility products $(K_{sp})$ of three sparingly soluble salts $M_2X$,$MX$,and $MX_3$ are identical. What will be the order of their solubilities $(s)$?