question_answer 1)

Do you expect different products in solution when aluminium (III) chloride and potassium chloride are treated with (i) normal water, (ii) acidified water, (iii) alkaline water.

Answer:

\[AlC{{l}_{3}}\]is a salt of a weak base and a strong acid. It undergoes hydrolysis in normal water. \[AlC{{l}_{3}}+3{{H}_{2}}O\underset{{}}{\leftrightarrows}Al{{(OH)}_{3}}+3HCl\] In acidic water, ionisation of \[AlC{{l}_{3}}\]occurs. \[AlC{{l}_{3}}\xrightarrow[Water]{Acidic}A{{l}^{3+}}(aq)+3C{{l}^{-}}(aq)\] In alkaline water, \[\text{Al}\left( \text{OH} \right)\text{3}\]reacts with \[\text{O}{{\text{H}}^{-}}\]ions to form \[{{[Al{{(OH)}_{4}}]}^{-}}\]or \[AlO_{2}^{-}\] \[Al{{(OH)}_{3}}+O{{H}^{-}}\to \underset{\text{Tetrahydroxoaluminate}}{\mathop{[Al(OH)_{4}^{-}]}}\,\] or \[\underset{\text{Metaaluminate}}{\mathop{\text{AlO}_{\text{2}}^{\text{-}}}}\,+2{{H}_{2}}O\] or \[AlC{{l}_{3}}(s)\xrightarrow[Water]{Alkaline}AlO_{2}^{-}(aq)+2{{H}_{2}}O+3C{{l}^{-}}(aq)\] \[KCl\] is a salt of a strong acid and a strong base. Its hydrolysis does not occur. Only ions are present in each case. \[KCl\to {{K}^{+}}(aq)+C{{l}^{-}}(aq)\]