Consider the equilibrium reaction:
$N H_{3} + H_{2} O ⇌ N H_{4}^{+} + O H^{-}$
Which of the following species can act as a Bronsted-Lowry acid?

N H_{3}

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N H_{4}^{+}

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H_{2} O

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Both (b) and (c)

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Solution

The correct option is D Both (b) and (c)
Bronsted Lowry’s Concept :
Bronsted acid - species (molecule or ion) which has a tendency to donate a proton.
Bronsted base - species (molecule or ion) which has a tendency to accept a proton.
In the forward reaction, we can see that, $H_{2} O$ donates a proton $(H^{+})$ to $N H_{3}$ and hence $N H_{4}^{+}$ is formed.
For the backward reaction, $N H_{4}^{+}$ donates a proton to act as Bronsted Lowry acid.
So here, $H_{2} O$ and $N H_{4}^{+}$ both acts as Bronsted -Lowry acids.

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

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

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

N H_{4} O H + H^{+} ⇌ N H_{4}^{+} + H_{2} O

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N H_{3} (a q) + H_{2} O ⇌ N H_{4}^{+} + O H^{-}

H N O_{3} (a q) + H_{2} O (l) \to H_{3} O^{+} (a q) + N O_{3}^{-} (a q)

N H_{3} (g) + H C l (g) \to N H_{4}^{+} (s) + C l^{-} (s)

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