Of the following 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 A $C l O^{⊝}$
Bronsted base is the substance that can accept $H^{+}$ ion. With the increase in the number of oxygen atoms in the given conjugate bases, the delocalization of the $π$ bond becomes more extended. This results in decrease in electron density. Consequently, proton attraction and basicity also decreases in the order $C l O^{-} > C l O_{2}^{-} > C l O_{3}^{-} > C l O_{4}^{-}$ . Hence, the strongest Bronsted base is $C l O^{-}$ .

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C l O^{-}

C l O_{2}^{-}

C l O_{3}^{-}

C l O_{4}^{-}

C l O^{-}, {C l O_{2}}^{-}, {C l O_{3}}^{-}, {C l O_{4}}^{-}

C l O^{-}, C l O_{2}^{-}, C l O_{3}^{-}

C l O_{4}^{-}

C l - O

C l O^{-}, C l O_{2}^{-}, C l O_{3}^{-}

C l O_{4}^{-}

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