Consider the half-reaction:
[Mn04]–(aq) + 8H+(aq) + 5e– ⇌ Mn2+(aq) + 4H2O(1)
E°=+1.51V
If the ratio of concentrations of [Mn04]– : Mn2+ is 100:1, determine E at pH values of
(a) 0.5;
(b) 2.0; and
(c) 3.5 (T = 298 K). Over this pH range, how does the ability of permanganate(VII) (when being reduced to Mn2_r) to oxidize aqueous chloride, bromide or iodide ions change?
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