In the following reaction HCO_3^{-} + H_2O ri | vedclass

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(D) According to the Bronsted-Lowry theory,a base is a substance that accepts a proton $(H^{+})$.In the forward reaction: $HCO_3^{-} + H_2O \rightleft

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$CO_3^{2-}$ and $H_2O$

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(D) According to the Bronsted-Lowry theory,a base is a substance that accepts a proton $(H^{+})$.In the forward reaction: $HCO_3^{-} + H_2O \rightleftharpoons CO_3^{2-} + H_3O^{+}$.$HCO_3^{-}$ acts as a Bronsted acid because it donates a proton to form $CO_3^{2-}$.$H_2O$ acts as a Bronsted base because it accepts a proton to form $H_3O^{+}$.In the reverse reaction: $CO_3^{2-} + H_3O^{+} \rightleftharpoons HCO_3^{-} + H_2O$.$CO_3^{2-}$ acts as a Bronsted base because it accepts a proton to form $HCO_3^{-}$.$H_3O^{+}$ acts as a Bronsted acid because it donates a proton to form $H_2O$.Thus,the two Bronsted bases in the reaction are $H_2O$ and $CO_3^{2-}$.

In the following reaction $HCO_3^{-} + H_2O \rightleftharpoons CO_3^{2-} + H_3O^{+}$,which two substances are Bronsted bases?

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