For $AgCl$,$K_{sp} = 1.2 \times 10^{-10}$ and for $AgBr$,$K_{sp} = 3.5 \times 10^{-13}$. What is the relationship between their solubilities $(S)$?

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ $(K_{sp} = 1.8 \times 10^{-10})$ will occur only with:

$H_{2}S$ is passed into $1 \ L$ of a solution containing $0.1 \ mole$ of $Zn^{2+}$ and $0.01 \ mole$ of $Cu^{2+}$ until the sulphide ion concentration reaches $8.1 \times 10^{-19} \ M$. Which one of the following statements is true? $[K_{sp}$ of $ZnS$ and $CuS$ are $3 \times 10^{-22}$ and $8 \times 10^{-36}$ respectively.$]$

If the molar solubility (in $mol \cdot L^{-1}$) of a sparingly soluble salt $AB_4$ is $S$ and the corresponding solubility product is $K_{sp}$,then $S$ in terms of $K_{sp}$ is given by the relation:

The solubility of $A_2X_3$ is $y \ mol \ m^{-3}$. Its solubility product is equal to .......

If the solubility products of $AgBrO_3$ and $Ag_2SO_4$ are $5.5 \times 10^{-5}$ and $2 \times 10^{-5}$ respectively,what is the relationship between their solubilities?