Conjugate base of $H C O_{3}^{-}$ in the given is:
Reaction : $H C O_{3}^{-} + H_{2} O \to C O_{3}^{2 -} + H_{3} O^{+}$

H_{3} O^{+}

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H_{2} C O_{3}

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C O_{3}^{2 -}

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H_{2} O

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Solution

The correct option is C $C O_{3}^{2 -}$
A Bronsted-Lowry base in an aqueous chemical reaction is one that, in the forward process, accepts a hydrogen ion in solution. We can clearly see that as the reaction proceeds, the carbonate species accepts a proton to form its conjugate acid, $H C O_{3}^{-}$ .
Therefore, In this reaction, the $C O_{3}^{2 -}$ species is acting as the conjugate base of $H C O_{3}^{-}$ .

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Similar questions

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

H C O_{3}^{-}

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

H C O_{3}^{-}

H C O_{3}^{-}

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

(H C O_{3})^{-}

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

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