$A$ 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?

We have taken a saturated solution of $AgBr$. The $K_{sp}$ of $AgBr$ is $12 \times 10^{-14}$. If $10^{-7} \ mol$ of $AgNO_3$ are added to $1 \ L$ of this solution,find the conductivity (specific conductance) of this solution in terms of $10^{-7} \ S \ m^{-1}$ units.
Given: $\lambda^{\circ}_{(Ag^{+})} = 6 \times 10^{-3} \ S \ m^2 \ mol^{-1}$,$\lambda^{\circ}_{(Br^{-})} = 8 \times 10^{-3} \ S \ m^2 \ mol^{-1}$,$\lambda^{\circ}_{(NO_3^-)} = 7 \times 10^{-3} \ S \ m^2 \ mol^{-1}$.

On addition of ammonium chloride to a solution of ammonium hydroxide,what happens to the concentration of $OH^{-}$ ions?

Assertion : $Sb(III)$ is not precipitated as sulphide when $H_2S$ is passed through its alkaline solution.
Reason : The concentration of $S^{2-}$ ion in alkaline medium is inadequate for precipitation.

Sodium chloride is purified by passing hydrogen chloride gas in an impure solution of sodium chloride. It is based on

What concentration of $Ac^{-}$ ions will reduce $H_3O^{+}$ ion concentration to $2 \times 10^{-4} \ M$ in a $0.40 \ M$ solution of $HAc$ (in $M$)? Given $K_a (HAc) = 1.8 \times 10^{-5}$.