The solubility of $AgCl$ in its solution is $1.25 \times 10^{-5} \ mol \ dm^{-3}$. What is the solubility product of $AgCl$?

The $K_{SP}$ of $AgI$ is $1.5 \times 10^{-16}$. On mixing equal volumes of the following solutions,precipitation will occur only with:

The solubility products of some sparingly soluble electrolytes are given below. The increasing order of their molar solubility is:
$(a)$ Formula: $MX$,$K_{sp} = 4.0 \times 10^{-20}$
$(b)$ Formula: $P_2Q$,$K_{sp} = 3.2 \times 10^{-11}$
$(c)$ Formula: $LY_3$,$K_{sp} = 2.7 \times 10^{-31}$

The solubility of $AgCN$ in a buffer solution of $pH = 3$ is $x$. The value of $x$ is [Assume : No cyano complex is formed; $K_{sp}(AgCN) = 2.2 \times 10^{-16}$ and $K_{a}(HCN) = 6.2 \times 10^{-10}$]

The solubility of $BaSO_4$ in pure water (in $g \, L^{-1}$) is closest to
[Given: $K_{sp}$ for $BaSO_4$ is $1.0 \times 10^{-10}$ at $25^{\circ} C$. Molecular weight of $BaSO_4$ is $233 \, g \, mol^{-1}$]

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