14.5 a)

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Belle Calforda3f
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14.5 a)

Postby Belle Calforda3f » Tue Feb 20, 2018 9:15 pm

on part a of 14.5, I do not get why we add OH when balancing the half reaction.

jillian1k
Posts: 54
Joined: Sat Jul 22, 2017 3:00 am

Re: 14.5 a)

Postby jillian1k » Tue Feb 20, 2018 9:17 pm

This is because the problem asks you to balance the half-rxns in basic solution. Therefore, you use H2O and OH-, not H+, to balance the reactions where O and H show up.

McKenna disc 1C
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Re: 14.5 a)

Postby McKenna disc 1C » Wed Feb 21, 2018 4:07 pm

I don't know the problem off the top of my head and I don't have my book on me, but balancing Hydrogen in basic solution is done by adding H2O to one side and OH- on the other. In acidic solution, H+ is added to one side and H2O to the other. So if the reaction in this problem takes place in a basic solution, that explains the presence of OH-.

lindsay lathrop 2C
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Re: 14.5 a)

Postby lindsay lathrop 2C » Sat Feb 24, 2018 4:03 pm

As they said before it is because the reaction is taking place in a basic solution. If that is confusing to add OH- what you can do is go through the problem normally, like add H+, balancing out the Hs and then at the end of the problem you just add one OH- on each side for every H+. Then you combine any H+ and OH- that are on the same side to form H20, and cancel out the extra H2Os.

Jacob Cho 2L
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Re: 14.5 a)

Postby Jacob Cho 2L » Sat Feb 24, 2018 4:51 pm

You add OH when balancing the half reaction because it is in a basic solution. If it were in an acidic solution you would add H+.

Nhan Nguyen 2F
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Re: 14.5 a)

Postby Nhan Nguyen 2F » Sat Feb 24, 2018 4:57 pm

Side note: you can add H3O+ (instead of H+) to acidic solutions that needs an O


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