The solubility of $Ca(OH)_{2}$ is $s \ mol \ L^{-1}$. The solubility product $(K_{sp})$ under the same condition is:

The $K_{sp}$ of $AgCl$ at $18\, ^oC$ is $1.8 \times 10^{-10}$. If the concentration of $Ag^{+}$ is $4 \times 10^{-3}\ mol/L$,what is the minimum concentration of $Cl^{-}$ required for $AgCl$ precipitation?

Which of the following pairs of ions would be expected to form a precipitate when their solutions are mixed?

If the solubility product of $Ni(OH)_2$ is $4.0 \times 10^{-15}$,the solubility (in $mol \ L^{-1}$) is

At $25^{\circ} C$,the solubility product of $MCl$ is $1 \times 10^{-10}$. What is its molar solubility in $0.1 \ M \ NaCl$ solution at the same temperature?

$A$ white powder soluble in $NH_4OH$ but insoluble in water is: