${\mathrm{AlCl}}_3$is a salt of weak base and strong acid, it undergoes cationic hydrolysis

${\mathrm{Al}}^{+3}+3{\mathrm{H}}_2\mathrm{O}\to \mathrm{Al}(\mathrm{OH}{)}_3+3{\mathrm{H}}^{+}$

H⁺ ions are released in to the solution.Hence, the aqueous  solution of ${\mathrm{AlCl}}_3$ turns acidic in nature.

Aqueous solution of ${\mathrm{CH}}_3\mathrm{COONa}$ undergoes anionic hydrolysis as it is a salt of weak acid and strong base and the solution will basic in nature due to the release of OH^- ions.

${\mathrm{CH}}_3{\mathrm{COO}}^{-}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{CH}}_3\mathrm{COOH}+{\mathrm{OH}}^{-}$

Al₂O₃ is amphoteric in nature as it reacts with both acids and bases.

Aqueous solution of KCl  is highly conductive in nature as KCl is an ionic compound.

Hence, the correct match is 

	List-I		List-II
(A)	$\mathrm{Aq}.$ Solution of ${\mathrm{AlCl}}_3$		Acidic
(B)	$\mathrm{Aq}.$ solution of ${\mathrm{CH}}_3\mathrm{COONa}$		Basic
(C)	$\mathrm{Aq}.$ solution of $\mathrm{KCl}$		Highly conductive
(D)	${\mathrm{Al}}_2{\mathrm{O}}_3$		Amphoteric