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

If the $[F^{-}] = 2.0 \times 10^{-5} \ M$ in water,how many grams of $CaCl_{2}$ must be added to initiate the precipitation of $CaF_{2}$? Given: $K_{sp}$ for $CaF_{2} = 1.7 \times 10^{-10}$ and the molar mass of $CaCl_{2} = 111 \ g \ mol^{-1}$. Assume the volume of the solution is $1 \ L$.

How many grams of $CaC_2O_4$ (molecular mass $= 128$) on dissolving in one litre distilled water will give a saturated solution (in $g$)? $[K_{sp}(CaC_2O_4) = 2.5 \times 10^{-9} \ mol^2 \ L^{-2}]$

Select the ion exchange reaction,which proceeds in the forward direction in an aqueous medium.

Sodium sulfate is soluble in water,whereas barium sulfate is sparingly soluble. Why?

The solubility of $Sb_2S_3$ in water is $1.0 \times 10^{-5} \ mol/L$ at $298 \ K$. What will be its solubility product?