Solubility of calcium phosphate (molecular mass,$M$) in water is $W \ g$ per $100 \ mL$ at $25^{\circ} C$. Its solubility product at $25^{\circ} C$ will be approximately.

$A$ 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:

How many grams of $CaC_2O_4$ will dissolve in distilled water to make $1 \, L$ of a saturated solution (in $, g$)? The solubility product $(K_{sp})$ of $CaC_2O_4$ is $2.5 \times 10^{-9} \, mol^2 \, L^{-2}$ and its molar mass is $128 \, g \, mol^{-1}$.

If the ${K_{sp}}$ for $HgSO_4$ is $6.4 \times 10^{-5}$,then the solubility of the salt is:

Calculate the solubility of $A_{2}X_{3}$ in pure water,assuming that neither kind of ion reacts with water. The solubility product of $A_{2}X_{3}$,$K_{sp} = 1.1 \times 10^{-23}$.

The solubility of a sparingly soluble salt $AB_2$ in water is $1.0 \times 10^{-5} \ mol \ L^{-1}$. Its solubility product is .......?