The solubility of $Ag_2C_2O_4$ is $2 \times 10^{-4} \ mol \ L^{-1}$ at $298 \ K$. What is its solubility product?

Given that the solubility product constants $(K_{sp})$ follow the order $K_{sp}(Mg(OH)_2) > K_{sp}(Zn(OH)_2) > K_{sp}(Fe(OH)_3)$,what is the order of precipitation of these hydroxides?

The solubility of $AgCN$ increases on adding $KCN$ due to the formation of .......

Consider two Group $IV$ metal ions $X^{2+}$ and $Y^{2+}$. $A$ solution containing $0.01 \ M$ $X^{2+}$ and $0.01 \ M$ $Y^{2+}$ is saturated with $H_2S$. The pH at which the metal sulphide $YS$ will form as a precipitate is . . . . . . (Nearest integer). (Given: $K_{sp}(XS)=1 \times 10^{-22}$ at $25^{\circ} C$, $K_{sp}(YS)=4 \times 10^{-16}$ at $25^{\circ} C$, $[H_2S]=0.1 \ M$ in solution, $K_{a1} \times K_{a2}(H_2S)=1.0 \times 10^{-21}$, $\log 2=0.30, \log 3=0.48, \log 5=0.70$)

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

If $K_{sp}$ of $CaF_2$ at $25\,^{\circ}C$ is $1.7 \times 10^{-10}$,the combination amongst the following which gives a precipitate of $CaF_2$ is