When $HCl$ is added to a saturated solution of $NaCl$,pure $NaCl$ precipitates because:

Pure $NaCl$ is prepared by passing $HCl$ gas through a saturated solution of common salt in water. The principle used is:

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

Given below are two statements:
Statement $I$: On passing $HCl_{(g)}$ through a saturated solution of $BaCl_2$,at room temperature white turbidity appears.
Statement $II$: When $HCl$ gas is passed through a saturated solution of $NaCl$,sodium chloride is precipitated due to common ion effect.
In the light of the above statements,choose the most appropriate answer from the options given below:

If $S_1, S_2, S_3$ and $S_4$ are the solubilities of $AgCl$ in water,in $0.01 \ M \ CaCl_2$,in $0.01 \ M \ NaCl$ and in $0.05 \ M \ AgNO_3$ respectively at a certain temperature,the correct order of solubilities is

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