Why is potassium permanganate(VII) such a strong oxidising agent, why does its behaviour depend on pH of the solution it is present in?

Asked Jan 14 '17 at 19:12

Active Jan 14 '17 at 19:30

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Why is potassium permanganate such a strong oxidizing agent? Let is say we have a $\ce{KMnO4}$ aqueous solution which is acidified by adding sulfuric acid. What is going on in the solution which makes it so oxidizing that immediately if we add an organic or inorganic molecule it gets immediately oxidized?

Also why under different pH potassium permanganate behaves differently i.e. Mn reduces from +7 to +2 in acidic conditions whereas it goes to +4 in neutral conditions?

edited Jan 14 '17 at 19:30

aventurin

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asked Jan 14 '17 at 19:12

Matt

Related: http://chemistry.stackexchange.com/questions/9001 – Klaus-Dieter Warzecha Jan 15 '17 at 09:03
The answer in the question only explains the results and chemical equations not the reason behind it . – Matt Jan 15 '17 at 14:41
So I guess there is no explanation for this another exception – Matt Feb 05 '17 at 15:07

Why is potassium permanganate(VII) such a strong oxidising agent, why does its behaviour depend on pH of the solution it is present in?

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