Question

Consider these two equations:
(i) $HN{O}_3\left(aq\right)+H_{2}O\left(l\right)\to H_3{O}^{+}\left(aq\right)+N{O}_3{}^{-}\left(aq\right)$
(ii) $N{H}_3\left(g\right)+HCl\left(g\right)\to N{H}_4^{+}\left(s\right)+Cl{}^{-}\left(s\right)$
Which of the following statements is/are correct?

• A. $C{l}^{-}$ s a Bronsted-Lowry base
• B. $H^{+}$ is a Bronsted-Lowry base
• C. $C{H}_{3}COOH$ is a Bronsted-Lowry base
• D. None of the above

Answer 1

The correct option is A $C{l}^{-}$ s a Bronsted-Lowry base

An Arrenhius acid releases $H^{+}$ ions while an Arrenhius base is a substance that releases $O{H}^{-}$ ions in an aqueous solution.
$HN{O}_3$ releases $H^{+}$ ions and hence, it acts as an Arrenhius acid.
A Bronsted-Lowry acid is a $H^{+}$ ion donor while a Bronsted-Lowry base is a $H^{+}$ ion acceptor.
$N{H}_3$ acts a Bronsted Lowry base as it accepts a hydrogen ion to form $N{H}_4^{+}$.