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May31-06, 11:50 AM
I've been working on some redox reactions for the oxidation of manganese.
Write the complete formulae for the redox reactions below:
i.) Manganese reacts with nitric acid (V) to form Mn2+ ions.
ii.) The Mn2+ ions reacts with potassium iodate, KIO4 to form MnO4- (VII)
Oxidation: 3Mn (s) --> 3Mn2+ (aq) + 6e- (aq)
Reduction: 6HN03 (aq) + 6e- (aq) --> 6N03- (aq) + 6H+ (aq)
Overall reaction: 3Mn + 6HN03 -> 6NO3- + 3Mn2+ + 6H+
Is this correct? If so, does the single protons regenerate the acid and/or become attached to substances like water?
Oxidation: Mn2+ + X -> MnO4- + ?H+
Reduction: IO4- + ?H+ -> I? + 4H2O
Overall reaction: Mn2+ + IO4- -> MnO4- + I2-
I'm having trouble with this part of the question. I does not have -II as one of its common oxidation number.
Any help or hints would be greatly appreciated
May31-06, 06:16 PM
metal + acid --> salt + (?)
You do not get protons. Look at the reduction reaction you've written. The charge is not balanced. Fix that one mistake using above hint and you're good.
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