Which of the following is most soluble in water?

The solubility product of a sparingly soluble salt $AX$ is $4.9 \times 10^{-13}$. What is its solubility in $mol \ dm^{-3}$?

If '$s$' and '$S$' are the solubility and solubility product of a sparingly soluble binary electrolyte respectively,then which of the following relations is correct?

In an aqueous solution,$SCN^-$,$Br^-$,$I^-$,and $Cl^-$ are present. Which will get precipitated first when $AgNO_3$ is added to the solution? Given that:
$K_{sp}(AgCl) = 1.2 \times 10^{-10}$,
$K_{sp}(AgI) = 1.7 \times 10^{-16}$,
$K_{sp}(AgSCN) = 7.1 \times 10^{-7}$,
$K_{sp}(AgBr) = 3.5 \times 10^{-13}$

What is the molarity of $F^{-}$ ions in a saturated solution of $BaF_2$? $(K_{sp} = 1.0 \times 10^{-6})$

The moles of $Ag^{+}$ which must be added to decrease the concentration of $Cl^{-}$ from $4 \times 10^{-5} \ M$ to $10^{-5} \ M$ in $100 \ mL$ solution,if $K_{sp}$ for $AgCl$ is $10^{-10} \ M^2$ at $25 \ ^oC$.