For a sparingly soluble salt $A_pB_q$,the relationship of its solubility product $(L_S)$ with its solubility $(S)$ is

If the concentration of lead iodide in its saturated solution at $25 \, ^oC$ is $2 \times 10^{-3} \ mol \ L^{-1}$,then its solubility product is:

The solubility product of $CaCO_3$ is $5 \times 10^{-9}$. Its solubility is equal to .......

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:

For a sparingly soluble strong electrolyte $AgIO_3$ (molar mass = $283 \, g/mol$),the equilibrium in a saturated solution is given by $AgIO_3(s) \rightleftharpoons Ag^+(aq) + IO_3^-(aq)$. If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 \times 10^{-8}$,how many grams of $AgIO_3$ are contained in $100 \, mL$ of its saturated solution?

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 $Ag_2CO_3$.