The Bronsted acids in the reversible reaction | vedclass

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Question

(C) According to the Bronsted-Lowry theory,an acid is a proton $(H^+)$ donor.In the forward reaction: $HCO_3^- (aq) + OH^- (aq) \rightarrow CO_3^{2-}

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$HCO_3^-$ and $H_2O$

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(C) According to the Bronsted-Lowry theory,an acid is a proton $(H^+)$ donor.In the forward reaction: $HCO_3^- (aq) + OH^- (aq) \rightarrow CO_3^{2-} (aq) + H_2O (l)$,$HCO_3^-$ donates a proton to $OH^-$,so $HCO_3^-$ acts as a Bronsted acid.In the reverse reaction: $CO_3^{2-} (aq) + H_2O (l) \rightarrow HCO_3^- (aq) + OH^- (aq)$,$H_2O$ donates a proton to $CO_3^{2-}$,so $H_2O$ acts as a Bronsted acid.Therefore,the Bronsted acids are $HCO_3^-$ and $H_2O$.

The Bronsted acids in the reversible reaction are $HCO_3^- (aq) + OH^- (aq) \rightleftharpoons CO_3^{2-} (aq) + H_2O (l)$

Similar Questions

The conjugate acid of $NH_2^-$ is

Which of the following species are only Lewis acids but not Bronsted acids from $CO_{2}$,$BCl_{3}$,$NH_{3}$,$CH_{3}NH_{2}$,$NO_{2}^{+}$,and $C_{6}H_{5}NH_{3}^{+}$?

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 :-

Given,$HF + H_2O \rightleftharpoons H_3O^{+} + F^{-}; K_a$
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Which relation is correct?

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