From the following reactions identify each of an Arrhenius acid or base, Bronsted-Lowry acid or base, or Lewis acid or base.
(A) $N a O H$ , in $N a O H \to {N a}^{+} + {O H}^{-}$
(B) $H C l$ , in $H C l \to H^{+} + {C l}^{-}$
(C) $N H_{3}$ , in $N H_{3} + H^{+} \to N H_{4}^{+}$
(D) $N H_{4}^{+}$ , in $N H_{4}^{+} \to N H_{3} + H^{+}$
(E) ${(C H_{3})}_{3} N :$ , in ${(C H_{3})}_{3} N : + B F_{3} \to {(C H_{3})}_{3} N : B F_{3}$

Open in App

Solution

(A) $N a O H$ is Arrhenius Base as it release $O H^{-}$ ion.
(B) $H C l$ is Arrhenius Acid as it release $H^{+}$ ion.
(c) $N H_{3}$ is Bronsted and Lewis Base as it accepts $H^{+}$ ion and donates electron pair of N.
(d) $N H_{4}^{+}$ is Bronsted Acid as it releases $H^{+}$ ion.
(e) $(C H_{3})_{3} N$ is Lewis base as it donates electron pair of N.

Suggest Corrections

Similar questions

P H_{3} + \oplus N H_{4} ⟶ \oplus P H_{4} + N H_{3}

N H_{3} + P {\oplus H}_{4} ⟶ N {\oplus H}_{4} + P H_{3}

(C H_{3})_{3} P + \oplus N H_{4} ⟶ (C H_{3})_{3} \oplus P H + N H_{3}

(C H_{3})_{3} N + P H_{4}^{\oplus} ⟶ (C H_{3})_{3} \oplus N H + P H_{3}

H_{2} O + N H_{3} \to N H_{4}^{+} + O H^{-}

{NH}_{3} (aq) + H_{2} O (l) \to {NH}_{4}_{4}^{+} (aq) + {OH}^{-} (aq)

N H_{3} + N H_{3} ⇌ N H_{4}^{+} + N H_{2}^{-}

N H_{3} + H_{2} O \to N H_{4}^{+} + O H^{-} i s :

Join BYJU'S Learning Program