Let the solubility of an aqueous solution of $Mg(OH)_2$ be $x$,then its $K_{sp}$ is:

The solubility of $AgCl$ in $0.1 \text{ M } NaCl$ is $S \text{ mol/L}$. If the solubility product of $AgCl$ is $1.8 \times 10^{-10}$, then $S$ is approximately:

The solubility products of $Al(OH)_3$ and $Zn(OH)_2$ are $8.5 \times 10^{-23}$ and $1.8 \times 10^{-14}$ at room temperature. If the solution contains $Al^{3+}$ and $Zn^{2+}$ ions,the ion first precipitated by adding $NH_4OH$ is

At $20 \, ^\circ C$,the $Ag^+$ ion concentration in a saturated solution of $Ag_2CrO_4$ is $1.5 \times 10^{-4} \, mol/L$. At $20 \, ^\circ C$,the solubility product of $Ag_2CrO_4$ would be:

The solubility product constants of $Ag_{2}CrO_{4}$ and $AgBr$ are $1.1 \times 10^{-12}$ and $5.0 \times 10^{-13}$ respectively. Calculate the ratio of the molarities of their saturated solutions.

The concentration of $KI$ and $KCl$ in a solution containing both is $0.001 \ M$ each. If $20 \ mL$ of this solution is added to $20 \ mL$ of a saturated solution of $AgI$ in water,what will happen?