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Which one of the following orders correctly represents the increasing acid strengths of the given acids?
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Verified Answer
The correct answer is:
$\mathrm{HOCl} < \mathrm{HOClO} < \mathrm{HOClO}_2 < $ $\mathrm{HOClO}_3$
As the oxidation number of the central atom increases, strength of acid also increases.
$\mathrm{HOCl} < \mathrm{HOClO} < \mathrm{HOClO}_2 < \mathrm{HOClO}_3$
Related Theory
The chlorine is more electronegative than bromine. As a result, it will attract electrons more towards itself than bromine. This will result in a donation of $\mathrm{H}+$ more easily in $\mathrm{HOCl}$ than in HOBr. So, the HOCl will be stronger acid than $\mathrm{HOBr}$.
$\mathrm{HOCl} < \mathrm{HOClO} < \mathrm{HOClO}_2 < \mathrm{HOClO}_3$
Related Theory
The chlorine is more electronegative than bromine. As a result, it will attract electrons more towards itself than bromine. This will result in a donation of $\mathrm{H}+$ more easily in $\mathrm{HOCl}$ than in HOBr. So, the HOCl will be stronger acid than $\mathrm{HOBr}$.
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