In the reaction HC_2O_4^{-} + PO_4^{3-} right | vedclass

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(C) According to the Brønsted-Lowry theory,a base is a proton $(H^+)$ acceptor.In the given reaction: $HC_2O_4^{-} + PO_4^{3-} \rightarrow HPO_4^{2-}

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$PO_4^{3-}$ and $C_2O_4^{2-}$

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(C) According to the Brønsted-Lowry theory,a base is a proton $(H^+)$ acceptor.In the given reaction: $HC_2O_4^{-} + PO_4^{3-} \rightarrow HPO_4^{2-} + C_2O_4^{2-}$$1$. $HC_2O_4^{-}$ acts as an acid because it donates a proton to become $C_2O_4^{2-}$.$2$. $PO_4^{3-}$ acts as a base because it accepts a proton to become $HPO_4^{2-}$.$3$. In the reverse reaction,$HPO_4^{2-}$ acts as an acid (donates $H^+$) and $C_2O_4^{2-}$ acts as a base (accepts $H^+$).Therefore,the two Brønsted bases are $PO_4^{3-}$ and $C_2O_4^{2-}$.

In the reaction $HC_2O_4^{-} + PO_4^{3-} \rightarrow HPO_4^{2-} + C_2O_4^{2-}$,which are the two Brønsted bases?

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