The following is a Bronsted acid but not a Bronsted base:

H_{2} O

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N H_{3}

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N H_{4}^{+}

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H C O_{3}^{-}

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Solution

The correct option is C $N H_{4}^{+}$
Bronsted base are compounds which accept $H^{+}$ ions.
Bronsted acid are compounds which donate $H^{+}$ ions.
$N H_{4}^{+}$ can donate $H^{+}$ but cannot accept $H^{+}$ .

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Similar questions

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

{N H}_{3}

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 C O_{3}^{-} + H_{2} O \to C O_{3}^{2 -} + H_{3} O^{+}

H C O_{3}^{-}

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