If the solubility product of $HgSO_4$ is $6.4 \times 10^{-5}$,then its solubility is:

When solid $Pb(NO_3)_2$ is added to $1 \, L$ of $H_2SO_4$ $(1 \times 10^{-3} \, M)$ to make the concentration of $Pb(NO_3)_2$ equal to $0.002 \, M$,what will happen? $(K_{sp} \text{ of } PbSO_4 = 1.3 \times 10^{-8})$

The solubility of $AgCl$ is $1.435 \times 10^{-5} \ g \ L^{-1}$ at $30^{\circ} C$. Calculate its solubility product $(K_{sp})$. (Molar mass of $AgCl = 143.5 \ g \ mol^{-1}$)

$A$ precipitate of calcium oxalate $(CaC_2O_4)$ will not dissolve in which of the following?

$25.0 \ mL$ of $0.050 \ M \ Ba(NO_3)_2$ is mixed with $25.0 \ mL$ of $0.020 \ M \ NaF$. The $K_{sp}$ of $BaF_2$ is $0.5 \times 10^{-6}$ at $298 \ K$. The ratio of $[Ba^{2+}][F^{-}]^2$ to $K_{sp}$ is $.......$. (Nearest integer)

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.