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 $HCO_3^- (aq) + OH^- (aq) \rightleftharpoons CO_3^{2-} (aq) + H_2O (l)$

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