When ${H C O_{3}}^{-}$ acts as a Bronsted base, which of the following is formed?

C O_{2}

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C O_{3}

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{C O_{3}}^{2 -}

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H_{2} C O_{3}

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Solution

The correct option is B $H_{2} C O_{3}$
A Bronsted base is a species that accepts a proton. When $H C O_{3}^{-}$ acts as a Bronsted base, it accepts a proton to form $H_{2} C O_{3}$ .

$H_{2} C O_{3}$ when dissociates forms $H^{+}$ ion and $H C O_{3}^{-}$ ion. This $H C O_{3}^{-}$ is the Bronsted base.

Hence, $H_{2} C O_{3}$ is formed.

$H C O_{3}^{-} + H^{+} ⟶ H_{2} C O_{3}$ .

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Similar questions

H C O_{3}^{-}

H C O_{3}^{-}

C O_{3}^{2 -}

H_{2} C O_{3}

When $C O_{2}$ is passed through water which of the following species will be present in water?

C O_{2}

C O_{2}

C O_{2}

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