An ionic compound is dissolved simultaneously in heavy water and simple water. Its solubility is

The solubility product of $AgCl$ is $1 \times 10^{-6}$ at $298 \, K$. Its solubility in $mol \, L^{-1}$ would be:

Evaporation of $1 \ L$ of a saturated solution of $CaCO_3$ leaves a residue of $7.0 \ g$. What is the solubility product $(K_{sp})$ for $CaCO_3$?

The solubility of $PbF_2$ (formula weight $= 245$) is $0.46 \ g/L$. What is the solubility product?

Calculate the molar solubility of $Ni(OH)_2$ in $0.10 \ M \ NaOH$. The solubility product of $Ni(OH)_2$ is $2 \times 10^{-15}$.

At $25\,^{\circ}C$,the solubility product of $Mg(OH)_2$ is $1.0 \times 10^{-11}$. At which $pH$ will $Mg^{2+}$ ions start precipitating in the form of $Mg(OH)_2$ from a solution of $0.001\, M\, Mg^{2+}$ ions?