Solubility product of a salt $AB$ is $1 \times 10^{-8}$ in a solution in which the concentration of $A^{+}$ ions is $10^{-3} \ M$. The salt will precipitate when the concentration of $B^{-}$ ions is kept

The solubility of $PbI_2$ at $25 \, ^\circ C$ is $0.7 \, g \, L^{-1}$. What is the solubility product $(K_{sp})$ of $PbI_2$ at this temperature? (Molar mass of $PbI_2 = 461.2 \, g \, mol^{-1}$)

The solubility of $AgCl$ at $20 \, ^oC$ is $1.435 \times 10^{-3} \, g/L$. The solubility product $(K_{sp})$ of $AgCl$ is:

$A$ solution is $0.1 \ M$ in $Cl^{-}$ and $0.001 \ M$ in $CrO_{4}^{2-}$. Solid $AgNO_{3}$ is gradually added to it. Assuming that the addition does not change in volume and $K_{sp}(AgCl) = 1.7 \times 10^{-10} \ M^{2}$ and $K_{sp}(Ag_{2}CrO_{4}) = 1.9 \times 10^{-12} \ M^{3}$. Select the correct statement from the following:

Why is only $As^{3+}$ precipitated as $As_2S_3$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$,while $Zn^{2+}$ is not precipitated as $ZnS$?

On the addition of a solution containing $CrO_4^{2-}$ ions to a solution containing $Ba^{2+}$,$Sr^{2+}$,and $Ca^{2+}$ ions,the precipitate obtained first will be of