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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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-}

Vedclass · Accepted Answer

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

Vedclass · Answer

(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?

Similar Questions

The conjugate acid of $H_2PO_4^-$ is

The dissociation constants of two acids $HA_1$ and $HA_2$ are $3.14 \times 10^{-4}$ and $1.96 \times 10^{-5}$ respectively. The relative strength of the acids will be approximately:

Which of the following acts as an acid in an aqueous solution?

Write the conjugate acids for the following Bronsted bases: $NH_{2}^{-}$,$NH_{3}$ and $HCOO^{-}$

When a solution of $NaOH$ is left exposed to air for a few hours,what happens?

Vedclass Test Series

Exam Paper Generator

Online Exam Module