(i) Aqueous HCl is more acidic as compared to the anhydrous HCl. In the presence of water which is dipolar in nature, there is a dipolar interaction between the `H^(+) and Cl^(-)` ions of the acid and the surroundisng `H_(2)O` molecules. As a result, the hydrated ions `H^(+)` (aq) and `Cl^(-)` (aq) get stabilised. This helps in the dissociation of the aid and accounts for the acidic character. Therefore, aqueous HCl is a stronger acid as compared to anhydrous HCl.
(ii) `N_(2)O` is more polar than `CO_(2).` In the molecule of `CO_(2).` the bonds are polar but their polarities cancel out because of its linear and symmetrical nature. On the other hand, `N_(2)O` is unsymmetrical through linear in nature. It is a hybrid of two structures which are both polar. Therefore, the molecular has a dipole moment 0.116 D.
(iii) Ethyl alcohol is more soluble in water. In ethyl alcohol `(C_(2)H_(5)-O-H)`, the O-H bond is highly polar and is involved in intermolecular hydrogen bonding with `H_(2)O` molecules. As a result, alcohol readily dissolves in water. On the contrary, the C-O bond in dimethyl ether `(CH_(3))_(2)` is very little polar and there is hardly any hydrogen bonding with teh `H_(2)O` molecules. Therefore , dimethyl ether is comparactively less soluble in water
