Question

Whic of the following can act as both a bronsted Acid and base ?

• A. $O_2^{+}$​
• B. $HCl$
• C. $N{a}_{2}C{O}_3$
• D. $HSO{4}^{-}$

Answer 1

The correct option is D $HSO{4}^{-}$

A Bronsted-Lowry acid is defined as substance that releases $H^{+}$ ions; a Bronsted-Lowry base is defined as substance that accepts $H^{+}$ ions. In the given option $O_2^{+}$​ neither gives nor accepts $H^{+}$ ion. $HCl$ only gives $H^{+}$ thus is an acid. $N{a}_{2}C{O}_3$​ can accept $H^{+}$ thus is a base. But $HSO{4}^{-}$​ can accept $H^{+}$ to form $H_{2}S{O}_4$ and can release one $H^{+}$ to form $S{O}_4^{2-}$​, therefore it can act as both Bronsted acid and Bronsted base.