Question

2. Which of the following cannot act both as
Bronsted acid and as Bronsted base?
[NEET-2019 (Odisha)]
(1) HSO4
(2) HCO3-
(4) HCI
(3) NH3​

Answer 1

Answer:

HCl cannot act as both bronsted acid and bronsted base because it cannot donate proton

Answer 2

$HCl$ cannot act both as Bronsted acid and as Bronsted base.

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given options:

1. $HSO_4^-+H^+\rightarrow H_2SO_4$

$HSO_4^-$ is gaining a proton, thus it is considered as a base. $HSO_4^-\rightarrow SO_4^{2-}+H^+$

Here, $HSO_4^-$ is loosing a proton, thus it is considered as an acid.

2.  $HCO_3^-+H^+\rightarrow H_2CO_3$

$HCO_3^-$ is gaining a proton, thus it is considered as a base. $HCO_3^-\rightarrow CO_3^{2-}+H^+$

Here, $HCO_3^-$ is loosing a proton, thus it is considered as an acid.

3. $HCl\rightarrow Cl^{-}+H^+$

Here, $HCl$ is loosing a proton, thus it is considered as an acid.

4.  $NH_3+H^+\rightarrow NH_4^+$

$NH_3$ is gaining a proton, thus it is considered as a base. $NH_3\rightarrow NH_2^{-}+H^+$

Here, $NH_3$ is loosing a proton, thus it is considered as an acid.

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