What will be the conjugate bases for the foll | vedclass

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(A) The conjugate base of a Bronsted acid is formed by removing one proton $(H^{+})$ from the acid molecule.For $HF$: $HF - H^{+} \rightarrow F^{-}$.F

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$F^{-}, HSO_{4}^{-}, CO_{3}^{2-}$

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(A) The conjugate base of a Bronsted acid is formed by removing one proton $(H^{+})$ from the acid molecule.For $HF$: $HF - H^{+} \rightarrow F^{-}$.For $H_{2}SO_{4}$: $H_{2}SO_{4} - H^{+} \rightarrow HSO_{4}^{-}$.For $HCO_{3}^{-}$: $HCO_{3}^{-} - H^{+} \rightarrow CO_{3}^{2-}$.Therefore,the corresponding conjugate bases are $F^{-}$,$HSO_{4}^{-}$,and $CO_{3}^{2-}$ respectively.

What will be the conjugate bases for the following Bronsted acids: $HF$,$H_{2}SO_{4}$ and $HCO_{3}^{-}$?

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