The correct reason(s) for the acidic nature of an aqueous solution of aluminium chloride is that

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$for aluminium ions the, \frac{charge}{surface area}, ratio is large$

$the O - H bonds in {[Al {(H_{2} O)}_{6}]}^{3 +} are weaker as$ compared to the O-H bonds in water.

aluminium chloride is covalent compound and its aqueous solution is acidic.

chloride ions (CI^-) react with water to form hydrochloric acid.

answer is A.

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Detailed Solution

There is a high charge (+3) on aluminium ion (Al³⁺) and the ratio, $\frac{charge}{surface area}$ , is high (.e., charge density is high) so it polarises the H₂O (ligand) and H⁺ ions are
removed. Due to this (i.e., polarisation of Al³⁺ion) there occurs a drift of electron density towards Al³⁺ ion and thus the O — H bond weakens i.e., the O — H bond in ${[Al {(H_{2} O)}_{6}]}^{3 +}$ is weaker than in water.