The solubility of $Ca_3(PO_4)_2$ in water is $y \text{ moles/litre}$. Its solubility product is

$A$ precipitate of $CaF_{2}$ $(K_{sp} = 1.7 \times 10^{-10})$ will be obtained when equal volumes of the following are mixed:

The concentration of $KI$ and $KCl$ in a solution containing both is $0.001 \ M$ each. If $20 \ mL$ of this solution is added to $20 \ mL$ of a saturated solution of $AgI$ in water,what will happen?

The solubility product of $AgCl$ is $10^{-10} \, M^2$. The minimum volume (in $m^3$) of water required to dissolve $14.35 \, mg$ of $AgCl$ is approximately

$A$ precipitate of calcium oxalate will not dissolve in

If $0.001435 \ g$ of $AgCl$ is present in $100 \ mL$ of water,calculate the $K_{sp}$.