The acid dissociation constant for` Al(H_2 O)_(6)^(3+)` is `1.4 xx 10^(-5)` . It suggests

Options

A. `H_2 O` molecules in the hydrated cation are much stronger proton donors than free solvent water molecules
B. Ionisation `,Al(H_2 O)_(6)^(3+) _((aq)) hArr AL^(3+) _(aq) + H_2O`
C. Ionisation ,
`Al (H_2 O)_(6(aq))^(3+) +H_2 O _((l)) hArr H_3 O^(+) ""_((aq)) +[Al(H_2O)_5(OH)]_((aq))^(2+)`
D. Its pH might be more than 7.

Answer

A, C

Explanation

Ionisation in (b) will not make it acid of `pK_a = 1.4 xx 10^(-5)` as ionsation of water is involved with salt and `K_(a ) gt gt K_(w)`
pH of solution will always be less than 7.