According to Bronsted-Lowry concept, the relative strengths of the bases $C H_{3} C O O^{-}$ , $O H^{-}$ and $C l^{-}$ are in the order:

O H^{-} > C H_{3} C O O^{-} > C l^{-}

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C l^{-} > O H^{-} > C H_{3} C O O^{-}

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C H_{3} C O O^{-} > O H^{-} > C l^{-}

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O H^{-} > C l^{-} > C H_{3} C O O^{-}

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Solution

The correct option is A $O H^{-} > C H_{3} C O O^{-} > C l^{-}$
$O H^{-}, C H_{3} C O O^{-}, C l^{-}$ are the conjugate bases of $H_{2} O, C H_{3} C O O H, H C l$ respectively.
We know,
$H C l > C H_{3} C O O H > H_{2} O acid strength$
$∴ C l^{-} < C H_{3} C O O^{-} < O H^{-} basic strength$
Stronger the acid, weaker will be its conjugate base.

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