The following equilibrium exists in aqueous solution: $CH_3COOH \rightleftharpoons CH_3COO^{-} + H^{+}$. If dilute $HCl$ is added,without change in temperature,the:

The following equilibrium exists in an aqueous solution of hydrogen sulphide: $H_2S \rightleftharpoons H^{+} + HS^{-}$. If dilute $HCl$ is added to an aqueous solution of $H_2S$ without any change in temperature,what happens?

$H_2S$ gas,when passed through a solution containing $HCl$,precipitates the cations of group $II$ of qualitative analysis but not those belonging to the fourth group. This is because:

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: $\lambda^{\circ}_{(Ag^{+})} = 6 \times 10^{-3} \ S \ m^2 \ mol^{-1}$,$\lambda^{\circ}_{(Br^{-})} = 8 \times 10^{-3} \ S \ m^2 \ mol^{-1}$,$\lambda^{\circ}_{(NO_3^-)} = 7 \times 10^{-3} \ S \ m^2 \ mol^{-1}$.

When $H_2S$ is passed through a solution containing $HCl$ for qualitative analysis,it does not precipitate group $IV$ cations. Why is this?

Aqueous ammonia is used instead of an aqueous solution of $NaOH$ to precipitate $Al^{+3}$ ions as $Al(OH)_3$ because: