The ammonium ion $(NH_4^+)$ acts as:

$CH_3COOH_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O^{+}_{(aq)} + CH_3COO^{-}_{(aq)}$. Between $H_2O$ and $CH_3COO^{-}$,which one is the weaker base?

Ionisation of which of the following will be maximum in water?

The dissociation constants of two acids $HY$ and $HZ$ are $2.88 \times 10^{-4}$ and $1.8 \times 10^{-5}$ respectively. The relative strength of the acids will be :-

Which of the following compounds can act as both a $Br\o nsted$ acid and a $Br\o nsted$ base?

Accepting the definition that an acid is a proton donor,the acid in the following reaction $NH_3 + H_2O \to NH_4^+ + OH^-$ is