Of the given anions, the strongest Bronsted base is:

C l O^{⊝}

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C l O_{2}^{⊝}

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C l O_{3}^{⊝}

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C l O_{4}^{⊝}

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Solution

The correct option is C $C l O^{⊝}$
The Bronsted base is the substance that can accept $H^{+}$ .
$O x i d a t i o n s t a t e o f t h e c e n t r a l a t o m ↑, A c i d i t y ↑$

Thus the order of acidic strength of the conjugate acid would be:
$H C l O < H C l O_{2} < H C l O_{3} < H C l O_{4}$
Weaker the conjugate acid stronger the conjugate base.
In the given conjugate bases the order of base strength is :

$C l O^{-} > C l O_{2}^{-} > C l O_{3}^{-} > C l O_{4}^{-}$
Hence, the correct option is A.

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