For a sparingly soluble salt $AB_2$,the equilibrium concentrations of $A^{2+}$ ions and $B^{-}$ ions are $1.2 \times 10^{-4} \ M$ and $0.24 \times 10^{-3} \ M$,respectively. The solubility product of $AB_2$ is :

The $K_{sp}$ for bismuth sulphide $(Bi_{2}S_{3})$ is $1.08 \times 10^{-73}$. The solubility of $Bi_{2}S_{3}$ in $mol \ L^{-1}$ at $298 \ K$ is ......

If the concentration of $Ag^{+}$ ions in the saturated solution of $Ag_2CO_3$ is $1.20 \times 10^{-4} \ mol \ L^{-1}$,then find the solubility product of $Ag_2CO_3$.

The concentration of sulphide ion in $0.1 \ M \ HCl$ solution saturated with hydrogen sulphide is $1.0 \times 10^{-19} \ M$. If $10 \ mL$ of this is added to $5 \ mL$ of $0.04 \ M$ solution of the following: $FeSO_4, MnCl_2, ZnCl_2$ and $CdCl_2$,in which of these solutions will precipitation take place? Given $K_{sp}$ for $FeS = 6.3 \times 10^{-18}, MnS = 2.5 \times 10^{-13}, ZnS = 1.6 \times 10^{-24}, CdS = 8.0 \times 10^{-27}$.

If the solubility products of $AgCl$ and $AgBr$ are $1.0 \times 10^{-10}$ 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:

Which of the following is insoluble in water?