According to the reaction $PbCl_2 \rightleftharpoons Pb^{2+} + 2Cl^-$,the solubility product constant $(K_{sp})$ of $PbCl_2$ is

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

The precipitate of $CaF_2$ $(K_{sp} = 1.7 \times 10^{-10})$ is obtained when equal volumes of the following are mixed:

The solubility product of $AgCl$ at $25 \, ^\circ C$ is $5 \times 10^{-13}$. Its solubility is = .......

At $T(K)$,the solubility product of $AgBr$ is $4 \times 10^{-13}$. What is its solubility in $0.1 \ M$ $KBr$ solution?

If the concentration of $OH^{-}$ ions in the reaction $Fe(OH)_{3(s)} \rightleftharpoons Fe^{3+}_{(aq)} + 3OH^{-}_{(aq)}$ is decreased by $1/4$ times,then the equilibrium concentration of $Fe^{3+}$ will increase by $......$ times.