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

The solubility of lithium sodium hexafluoroaluminate $Li_3Na_3(AlF_6)_2$ is $s \ mol \ L^{-1}$. Its solubility product constant $(K_{sp})$ will be:

The solubility of $AgBr_{(s)}$,having solubility product $5 \times 10^{-10}$ in $0.2 \ M$ $NaBr$ solution,equals

The solubility of $A_2 X_3$ is '$y$' $M$. Its solubility product is:

On adding $0.1 \ M$ solution each of $[Ag^+]$,$[Ba^{2+}]$,and $[Ca^{2+}]$ to a $Na_2SO_4$ solution,which species precipitates first? Given: $K_{sp}(BaSO_4) = 10^{-11}$,$K_{sp}(CaSO_4) = 10^{-6}$,$K_{sp}(Ag_2SO_4) = 10^{-5}$.

The $K_{sp}$ value of $AgCl$ at $25^{\circ}C$ is $1.8 \times 10^{-10}$. If $10^{-5} \ mol$ of $Ag^{+}$ is added to the solution,the new $K_{sp}$ value will be: