Calculate the solubility of $AgCl(s)$ in $0.1 \ M \ NaCl$ at $25 \ ^oC$. Given ${K_{sp}}(AgCl) = 2.8 \times 10^{-10}$.

When $1.88 \ g$ of $AgBr_{(s)}$ is added to a $10^{-3} \ M$ aqueous solution of $KBr$,the concentration of $Ag^{+}$ is $5 \times 10^{-10} \ M$. If the same amount of $AgBr_{(s)}$ is added to a $10^{-2} \ M$ aqueous solution of $AgNO_3$,the concentration of $Br^{-}$ is

$A$ litre of solution is saturated with $AgCl$. To this solution if $1.0 \times 10^{-4} \ mol$ of solid $NaCl$ is added,what will be the $[Ag^{+}]$ compared to the original concentration,assuming no volume change?

Addition of conc. $HCl$ to saturated $BaCl_2$ solution precipitates $BaCl_2$; because

The commercial salt is purified by passing

Consider the nitration of benzene using mixed conc. $H_2SO_4$ and $HNO_3$. If a large amount of $KHSO_4$ is added to the mixture,the rate of nitration will be