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Oxidation Reduction (redox) Balancing

by krackers
Tags: balancing, oxidation, redox, reduction
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krackers
#1
Jul5-13, 05:07 PM
P: 57
When balancing oxidation reduction reactions involving acids or bases, what (in the case of acids) allows you to add H+ ions to one side of the reaction and H2O to the other, or in the case of bases, OH- and H2O to balance out hydrogen/oxgen? Normally you are not allowed to just add random compounds to either side of the equation.

I suspect this has something to do with the ability of H+ to grab oxygen atoms to form H2O, as similarly with 2OH- to supply Oxygen atoms and give H2O, as demonstrated by these two reactions:
[itex]2H^{+}\; +\; O^{2-}\; -->\; H_{2}O[/itex]

[itex] 2OH^{-}\; -->\; H_{2}O\; +\; O^{2-} [/itex]

However, is this the real reason? And instead of using H+ ions for the acids, wouldn't it be more appropriate to use the hydronium ion, H3O+?


In case the question is not clear, here is an example reaction.

[itex]MnO_{4}^{-}\; +\; I^{-}\; -->\; I_{2}\; +\; Mn^{2+}[/itex]

One of the half reactions would be:

[itex]5e^{-}\; +\; MnO_{4}^{-}\; +\; 8H^{+}\; ->\; Mn^{2+}\; +\; 4H_{2}O[/itex]

However, in this half reaction what allows you to add H+ to one side and H2O to the other?
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Borek
#2
Jul6-13, 02:15 AM
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P: 23,395
These reactions usually take place in water, and typically in either low or high pH - so you can safely assume there is plenty of H2O and H+/OH- around. As there is plenty of them, they can be between reactants and products and you won't even notice changes in their concentrations.


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