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(A) According to the Bronsted-Lowry theory,an acid is a proton $(H^+)$ donor and a base is a proton $(H^+)$ acceptor.In the reaction $ClO_4^{-} + HCO_

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$HCO_3^{-}$ and $HClO_4$

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(A) According to the Bronsted-Lowry theory,an acid is a proton $(H^+)$ donor and a base is a proton $(H^+)$ acceptor.In the reaction $ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$:$1$. $HCO_3^{-}$ donates a proton to $ClO_4^{-}$ to form $CO_3^{2-}$,so $HCO_3^{-}$ acts as an acid.$2$. $HClO_4$ is the conjugate acid formed from the base $ClO_4^{-}$. In the reverse reaction,$HClO_4$ acts as a proton donor,so it is an acid.Therefore,$HCO_3^{-}$ and $HClO_4$ are the acids in the given reaction.

According to the Bronsted-Lowry theory,the acids in the following reaction are:
$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$

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According to the Bronsted-Lowry theory,the acids in the following reaction are:$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$