One of the following is a Bronsted acid but not a Bronsted base

H_{2} S

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H_{2} O

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H C O_{3}^{⊝}

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N H_{3}

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Solution

The correct option is C $H_{2} S$
According to Bronsted-Lowry concept of acids and bases, an acid is a substance which can give a proton and a base is a substance which accepts a proton.
So $H_{2} S$ is a Bronsted acid.

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

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

{N H}_{3}

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

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