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Account for the acidic nature of HClO_4 In terms of Bronsted-Lowry Theory, Identify its conjugate base. |
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Answer» Solution :`HClO_4 leftrightarrow H^(+) +ClO_4^(-)` According to LOWRY -Bronsted concept, a strong acid has weak conjugate base and a weak acid has a strong conjugate base. Let us consider the stabilities of the conjugate bases `ClO_4^(-),ClO_3^(-),ClO_2^(-) and ClO^(-)` formed from these acid `HClO_4,HClO_3,HClO_2,HOCl` respectively. these anions are stabilized to GREATEST extent, it has lesseer attraction for proton and therefore,will behave as weak base. Consequently the corresponding acid will be strongest because weak conjugate base has strong acid and strong conjugate base has weak acid. The charge stabilization increases in the order, `CIO^(-) LT ClO_2^(-) lt ClO_3^(-) lt ClO_4^(-)` This means `ClO_4^(-)` will have maximum stability and therefore will have minimum attraction for `H^+` . Thus `ClO_4^(-)` will be weakest base and its conjugate acid `HClO_4` is the strongest acid. `ClO_4^(-)` is the conjugate base of the acid `HClO_4`. |
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