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microsoft-com:office:office" /> [MnO4]-(aq) + 8H+(aq) + 5e- Mn2+(aq)+4H2O(l) E= +1.51 V If th ratio of concentreations of [ MnO4 ] - : Mn2+ is 100:1 , determine E at PH values of (a) 0.5 (b) 2.0; and (c) 3.5 (T=298). Over this PH range , how does the ability of permanganate (VII) ( when being reduce to Mn2+) to oxidize aqueous chloride , bromide or iodide ions change?

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