If the solubility products of $AgCl$ and $AgBr$ are $1.0 \times {10^{ – 8}}\,M$ and $3.5 \times {10^{ – 13}}$ respectively, then the relation between the solubilities (denoted by the symbol$'S'$) of these salts can correctly be represented as

Solubility of $Th_3(PO_4)_4$ $(M_w = m)$ is $w\,g/100\,ml$ at $25\,^oC$ . $K_{SP}$ is

The values of $K_{ sp }$ of two sparingly soluble salts $Ni ( OH )_{2}$ and $AgCN$ are $2.0 \times 10^{-15}$ and $6 \times 0^{-17}$ respectively. Which salt is more soluble? Explain.

Solubility product of a sulphide $MS$  is $3 \times {10^{ – 25}}$ and that of another sulphide $NS $ is $4 \times {10^{ – 40}}$. In ammoniacal solution

If the solubility product of lead iodide $(Pb{l_2})$ is $3.2 \times {10^{ – 8}},$ then its solubility in moles/litre will be