All of the following can act as Bronsted-Lowry acids (proton donors) in aqueous solution except :

H l

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N H_{4}^{+}

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H C O_{3}^{-}

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H_{2} S

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N H_{3}

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Solution

The correct option is E $N H_{3}$
All of the following can act as Bronsted-Lowry acids (proton donors) in aqueous solution except ammonia $N H_{3}$ . Ammonia is Bronsted-Lowry base (proton acceptor) in aqueous solution.
$N H_{3} + H^{+} \to N H_{4}^{+}$

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{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}_{3}, {H S O}_{4}^{-}, H_{2} {S O}_{4}, {H C O}_{3}^{-}, H_{3} O

H^{+} a n d O H^{-} i o n s

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