The $K_{sp}$ of $Ag_2CrO_4$ is $1.1 \times 10^{-12}$ at $298 \ K$. The solubility (in $mol/L$) of $Ag_2CrO_4$ in a $0.1 \ M \ AgNO_3$ solution is

The solubility product of $PbCl_2$ at $298 \ K$ is $3.2 \times 10^{-5}$. What is its solubility in $mol \ dm^{-3}$?

$K_{sp}$ for $Cr(OH)_3$ is $2.7 \times 10^{-31}$. What is its solubility in moles / litre?

Solubility product constant $(K_{sp})$ of salts of types $MX$,$MX_2$ and $M_3X$ at temperature '$T$' are $4.0 \times 10^{-8}$,$3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$,respectively. Solubilities $(\text{mol } dm^{-3})$ of the salts at temperature '$T$' are in the order:

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:

$A$ saturated solution of $Ag_2SO_4$ is $2.5 \times 10^{-2} \ M$. The value of its solubility product is: