Do you expect different products in solution when aluminium(III) chloride and potassium chloride treated separately with (i) normal water (ii) acidified water, and (iii) alkaline water? Write equations wherever necessary.

Explanation

Potassium chloride (KCI) is the salt of a strong acid and a strong base. In normal water, it simply dissociates into its constituent ions. No hydrolysis takes place in this case.
`KCI(s)overset("Water")toK^(+)(aq)+Cl^(-)(aq)`
The aqueous solution of KCI is neutral. Therefore, in acidified water or alkaline water, no reaction takes place.
Aluminium chloride `(AICl_(3))` is a salt of a weak base and a strong acid. In normal water, it undergoes hydrolysis to form an acidic solution as shown ahead.

In acidified water, `H^(+)` ions react with `Al(OH)_(3)` to form `Al^(3+)` ions and `H_(2)O`, Thus, in acidic water, hydrolysis is checked and `Al^(3+)` and `Cl^(-)` ions exist in solution.
`AlCl_(3)overset("Acidified water")toAl^(3+)+3Cl^(-)`
In alkaline water, `Al(OH)_(3)` reacts to form `AlO_(2)^(-)` ion.
`Al(OH)_(3)+OH^(-)tounderset("Metaaluminate ion")(AlO_(2)^(-))+2H_(2)O`