The solubility product of $AgI$ at $25\,^oC$ is $1.0 \times {10^{ – 16}}\,mo{l^2}\,{L^{ – 2}}$. The solubility if $AgI$ in ${10^{ – 4}}\,N$ solution of $KI$ at $25\,^oC$ is approximately (in $mol$ ${l^{ – 1}})$

Concentration of $H _2 SO _4$ and $Na _2 SO _4$ in a solution is $1 M$ and $1.8 \times 10^{-2} M$, respectively. Molar solubility of $PbSO _4$ in the same solution is $X \times 10^{- Y } M$ (expressed in scientific notation). The value of $Y$ is. . . .

[Given: Solubility product of $PbSO _4\left(K_{s p}\right)=1.6 \times 10^{-8}$. For $H _2 SO _4, K_{a l}$ is very large and $\left.K_{a 2}=1.2 \times 10^{-2}\right]$

At $298$ $K$ temp. the ${K_{sp}}$ of $Ca{F_2}$ is $1.7 \times {10^{ – 10}}$. One person daily drinks $2.5$ $L$ saturated water by $Ca{F_2}$ . Then how much gram $Ca{F_2}$ present in his body? (Molecular mass of $Ca{F_2}$ is $ 78$ $g$ $mol^{-1}$ )

The solubility of $[Ag^+]$ and $[Cl^-]$ solution is $1.43\times 10^{-3}\,gL^{-1}$ then what is the value of $K_{sp}$ at $25\,^oC$ of $AgCl$ .

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively