Sometimes a species in a given oxidation state undergoes self-oxidation reduction reaction (disproportionation) in aqueous medium...

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Sometimes a species in a given oxidation state undergoes self-oxidation reduction reaction (disproportionation) in aqueous medium to give products of lower and higher oxidation states. For example, when Br₂ is added in an alkaline solution ([OH-] = 1 mol dm³), it disproportionates to give bromide and hypobromide ions. Rationalize the above results from the standard potentials given below: (1) Br₂+e → Br (ii) BrO + H₂O + €¯ → (iii) 2BrO + 2H₂O + 4e (iv) BrO3 + 2H₂O + 4e Br₂ + 20H → 2Br + 40H™ BrO + 40H™ The above data may be presented in a condensed form as 0.54 V 1.07 V BrO3 Bro. 0.45 V Eº = 1.07 V E° = 0.45 V E° = 0.71 V E° = 0.54 V + B₁₂(1) 0.71 V What would be the overall reaction of Br₂ in an alkaline solution? Br Sometimes a species in a given oxidation state undergoes self-oxidation reduction reaction (disproportionation) in aqueous medium to give products of lower and higher oxidation states. For example, when Br₂ is added in an alkaline solution ([OH-] = 1 mol dm³), it disproportionates to give bromide and hypobromide ions. Rationalize the above results from the standard potentials given below: (1) Br₂+e → Br (ii) BrO + H₂O + €¯ → (iii) 2BrO + 2H₂O + 4e (iv) BrO3 + 2H₂O + 4e Br₂ + 20H → 2Br + 40H™ BrO + 40H™ The above data may be presented in a condensed form as 0.54 V 1.07 V BrO3 Bro. 0.45 V Eº = 1.07 V E° = 0.45 V E° = 0.71 V E° = 0.54 V + B₁₂(1) 0.71 V What would be the overall reaction of Br₂ in an alkaline solution? Br

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