The solubility product of sparingly soluble salt $AX_{2}$ is $3.2 \times 10^{-11}$. Its solubility (in $mol / L$) is

At $298 \ K$,the solubility of silver chloride in water is $1.434 \times 10^{-3} \ g \ L^{-1}$. The value of $-\log K_{sp}$ for silver chloride is $........$ (Given: molar mass of $Ag = 107.9 \ g \ mol^{-1}$ and $Cl = 35.5 \ g \ mol^{-1}$)

Two insoluble salts $MY$ and $NY_{3}$ have the same $K_{SP} = 6.2 \times 10^{-13}$ at room temperature. Which of the following statements is true regarding $MY$ and $NY_{3}$?

The $K_{sp}$ of $AgCl$ is $1.8 \times 10^{-10}$. The concentration of $Cl^-$ required to initiate the precipitation of $AgCl$ in a solution containing $4 \times 10^{-3} \ M \ Ag^+$ is:

At $25^{\circ} C$,the solubility product of a salt of $MX_{2}$ type is $3.2 \times 10^{-8}$ in water. The solubility (in $mol / L$) of $MX_{2}$ in water at the same temperature will be:

Which one of the following is most soluble?