Select the set of amphiprotic species.

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Question

(C) Amphiprotic species are those that can act as both a Bronsted-Lowry acid (by donating a proton) and a Bronsted-Lowry base (by accepting a proton).

Vedclass · Accepted Answer

$H_2PO_4^-, H_2PO_3^-, H_2O$

Vedclass · Answer

(C) Amphiprotic species are those that can act as both a Bronsted-Lowry acid (by donating a proton) and a Bronsted-Lowry base (by accepting a proton).$1$. $H_2PO_4^-$: Can accept $H^+$ to form $H_3PO_4$ and donate $H^+$ to form $HPO_4^{2-}$.$2$. $H_2PO_3^-$: Can accept $H^+$ to form $H_3PO_3$ and donate $H^+$ to form $HPO_3^{2-}$.$3$. $H_2O$: Can accept $H^+$ to form $H_3O^+$ and donate $H^+$ to form $OH^-$.Thus,the set $H_2PO_4^-, H_2PO_3^-, H_2O$ consists of amphiprotic species.

$A$. $HI$	$(i)$ $3.2 \times 10^9$
$B$. $HF$	$(ii)$ $3.5 \times 10^{-4}$
$C$. $HCl$	$(iii)$ $1.3 \times 10^6$
$D$. $HBr$	$(iv)$ $1.0 \times 10^9$

Similar Questions

Identify base $2$ for the following equation according to the $BRONSTED-LOWRY$ theory.
$HCl_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O_{(aq)}^{+} + Cl_{(aq)}^{-}$

$A$ $Lewis$ acid is defined as a substance that acts as a:

Write the conjugate base of the following: $HF, CH_{3}NH_{3}^{+}, H_{3}PO_{4}, HPO_{4}^{2-}$

The conjugate base of $HPO_4^{2-}$ is:

Match the given ionisation constant values with the corresponding acids.
$A$. $HI$ $(i)$ $3.2 \times 10^9$
$B$. $HF$ $(ii)$ $3.5 \times 10^{-4}$
$C$. $HCl$ $(iii)$ $1.3 \times 10^6$
$D$. $HBr$ $(iv)$ $1.0 \times 10^9$

The correct match is:

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