This sulphate reacts differently with iodine and bromine in the reaction given below 2S₂O₃^-2+I₂→S₄O₆^-2+2I^-1

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Bromine is weaker oxidant than iodine

Thisulphate undergoes oxidation by bromine and reduction by iodine in these reaction

Bromine undergoes oxidation and iodine undegoes reduction in these reactions

Bromine is stronger oxidant than iodine

answer is A.

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Detailed Solution

$2 \overset{+ 2}{S_{2}} \overset{- 2}{O_{2}^{2 -}} (aq) + I_{2}^{0} (s) \to \overset{2 .5}{S_{4}} O_{6}^{2 -} (aq) + 2 I^{-} (aq)$
$\overset{+ 2}{S_{2}} \overset{- 2}{O_{3}^{2 -}} (aq) + 2 \overset{0}{B} r_{2} (l) + 5 H_{2} O (l) \to 2 \overset{+ 6}{S} \overset{2 -}{O_{4}^{2 -}} (aq) + 4 {Br}^{-} (aq) + 10 H^{+} (aq)$
Bromine being stronger oxidising agent than $I_{2}$ , Br₂ oxidises S of $S_{2} O_{3}^{2 -}$ to ${SO}_{4}^{2 -}$ whereas $I_{2}$ oxidises it only into $S_{4} O_{6}^{2 -}$ ion.