The solubility products of three sparingly soluble salts are given below. What is the correct decreasing order of their molar solubility?

$S.No.$	$Formula$	$K_{sp}$
$1$	$PQ$	$4.0 \times 10^{-20}$
$2$	$PQ_2$	$3.2 \times 10^{-14}$
$3$	$PQ_3$	$2.7 \times 10^{-35}$

In which of the following solutions will the solubility of $Ag_2CO_3$ $(K_{sp} = 8 \times 10^{-12})$ be maximum at $30 \, ^\circ C$?

What is the solubility product $(K_{sp})$ of calcium phosphate in pure water? $[S = \text{molar solubility}]$

The $K_{sp}$ of $AgBr$ at $25 \, ^\circ C$ is $4.9 \times 10^{-13}$. If the molar mass of $AgBr$ is $188 \, g/mol$,how much $AgBr$ is required to saturate $20 \, L$ of water?

For a sparingly soluble,strong electrolyte salt,the following equilibrium is established in a saturated solution:
$AgIO_{3(s)} \rightleftharpoons Ag^+_{(aq)} + IO_{3(aq)}^-$
At a certain temperature,the solubility product of $AgIO_3$ is $K_{sp} = 1.0 \times 10^{-8}$. The molar mass of $AgIO_3$ is $283 \ g \ mol^{-1}$. What is the mass of $AgIO_3$ in $100 \ mL$ of its saturated solution?

Solubility of $PbI_2$ is $0.005 \ M$. Then,the solubility product of $PbI_2$ is