Which of the following sets of concentrations will cause the precipitation of $ZnCl_2$ $(K_{sp} = 1.2 \times 10^{-12} \ M^3)$?

What is the expression for the solubility product of silver chromate $(Ag_2CrO_4)$ if its solubility is expressed as $S \ mol \ L^{-1}$?

$A$ $1.0 \ L$ of aqueous solution contains $1 \times 10^{-8} \ M \ NaBr$,$1 \times 10^{-8} \ M \ NaCl$ and $1 \times 10^{-8} \ M \ NaI$. To this solution,$1 \times 10^{-10} \ M$ aqueous $AgNO_3$ solution is added dropwise. The order of precipitation of $AgX$ $(X = Cl, Br, I)$ is:
$(K_{sp}(AgCl) = 1.8 \times 10^{-10}; K_{sp}(AgBr) = 5 \times 10^{-13}; K_{sp}(AgI) = 8.3 \times 10^{-17})$

If the solubility product $(K_{sp})$ of $Ni(OH)_2$ is $1.9 \times 10^{-15}$,the molar solubility of $Ni(OH)_2$ in $1.0 \ M \ NaOH$ is:

The solubility of $CaF_2$ in a solution of $0.1 \ M \ Ca(NO_3)_2$ is.

If the solubility product of $AgCl$ is $10^{-10}$,what is the solubility of $AgCl$ in $0.001 \ M \ NaCl$?