Which one of the following species acts as bo | vedclass

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(C) species that acts as both a Bronsted acid and a base is called an amphoteric species. It must be able to donate a proton $(H^+)$ and accept a prot

Vedclass · Accepted Answer

$HPO_4^{2-}$

Vedclass · Answer

(C) species that acts as both a Bronsted acid and a base is called an amphoteric species. It must be able to donate a proton $(H^+)$ and accept a proton $(H^+)$.$HPO_4^{2-}$ can accept a proton to form $H_2PO_4^-$ (acting as a base) and donate a proton to form $PO_4^{3-}$ (acting as an acid).$HPO_4^{2-} + H_2O \rightleftharpoons H_2PO_4^- + OH^-$$HPO_4^{2-} + H_2O \rightleftharpoons PO_4^{3-} + H_3O^+$$H_2PO_2^-$ is the conjugate base of $H_3PO_2$ (a monobasic acid) and cannot donate any more protons.$HPO_3^{2-}$ is the conjugate base of $H_2PO_3^-$ (derived from the dibasic acid $H_3PO_3$) and cannot donate any more protons.

Which one of the following species acts as both Bronsted acid and base?

Similar Questions

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

What is the conjugate acid of $HPO_4^{2-}$?

Which of the following can act both as a Bronsted acid and a Bronsted base?

Identify the acids in the following reaction: $HCl_{(aq)} + H_2O_{(aq)} \rightleftharpoons H_3O^{+}_{(aq)} + Cl^{-}_{(aq)}$. Which of these acids is stronger?

The compound that is not a Lewis acid is

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