Question

Which of the following is Bronsted-Lowry base (proton acceptor) in aqueous solution?

• A. $HI$
• B. $N{H}_4^{+}$
• C. $HC{O}_3^{-}$
• D. $H_{2}S$
• E. $N{H}_3$

Answer 1

Answer: (E)

$N{H}_3$

Bronsted-Lowry acids in aqueous solution can donate a proton $H^{+}$.
HI, $N{H}_4^{+}$ , $HC{O}_3^{-}$ and $H_{2}S$ are proton donors. Hence, they are Bronsted-Lowry acids in aqueous solution.
$HI\rightleftharpoons H^{+}+I^{-}N{H}_4^{+}\rightleftharpoons N{H}_3+H^{+}HC{O}_3^{-}\rightleftharpoons C{O}_3^{2-}+H^{+}{H}_{2}S\rightleftharpoons H{S}^{-}+H^{+}$
Bronsted-Lowry bases in aqueous solution can accept a proton $H^{+}$.
$N{H}_3$ can accept a proton. Hence, it is Bronsted-Lowry base in aqueous solution.
$N{H}_3+H^{+}\rightleftharpoons N{H}_4^{+}$