Bronsted Neutralization reaction

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ckilkeary 2G
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Bronsted Neutralization reaction

Postby ckilkeary 2G » Sat Mar 14, 2020 11:02 am

If given the reaction (and told its a Bronsted neutralization reaction): H+ (aq) + OH- (aq) ----> H2O (l)
and told to write the half reactions in the anode and cathode the textbook gives the answers:
anode: 4OH- (aq) -----> O2 (g) + H2O (l) + 4e-
cathode: O2 (g) + 4H+ (aq) + 4e- ----> 2 H2O (l)

How do we know to use O2 when we are writing those half reactions?

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Re: Bronsted Neutralization reaction

Postby Chem_Mod » Sat Mar 14, 2020 1:33 pm

Look at the species involved in the given overall reaction and pick two equations that when combined will give you that reaction.

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Re: Bronsted Neutralization reaction

Postby Jared_Yuge » Sat Mar 14, 2020 1:40 pm

write out the skeletal reaction like H+ ---> H20. and OH- ---> H2O and then follow the regular instructions for balancing a redox reaction.

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