In the absence of the formation of complex ions by the addition of a common ion,the solubility of a given salt is

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

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

Statement $A$: Addition of $NH_4OH$ in the presence of excess $NH_4Cl$ to an aqueous solution of $BaCl_2$ results in the precipitation of $Ba(OH)_2$.
Reason $R$: $Ba(OH)_2$ is insoluble in water.

Solubility of $AgCl$ in conc. $HCl$ is ...... than in water.

When $H_2S$ gas is passed through a solution containing $HCl$ during qualitative analysis,cations of the second group are precipitated,but cations of the fourth group are not precipitated because: