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Author: Subject: 15% peroxyacetic stoichiometry question.
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[*] posted on 24-7-2005 at 17:02
15% peroxyacetic stoichiometry question.


Bit of a foolish question I think but:

The procedure calls for 15% peracetic
I have 27% h2o2

I need to concentrate the h2o2 then?

Alternatively would the lower percentage peracetic produced with the 27% provide a satisfactory yield if used to oxidize a propenylbenzene?
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[*] posted on 24-7-2005 at 19:37


You have 27% H2O2, but what about your acetic acid stock, glacial, 50%, 3%, we need to know. If you have glacial then no concentration of you peroxide is necessary if you assume the reaction:

H2O2 + CH3COOH ---> H2O + CH3COOOH

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[*] posted on 24-7-2005 at 21:52


I see.

The Acetic acid I would be using is Glacial.
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[*] posted on 24-7-2005 at 22:27


I know nothing of the best way to make the most concentrated peracetic acid from 27% H2O2 and haven't looked it up, but I do remember that I have a related JACS article.

Look here, find page 907, and click "first page", where the author only got 8.6% peracetic with 30% H2O2 in his non-definitive submission.

It is no big deal to concentrate the peroxide to 40-45%, no vacuum required, just a little heat.
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[*] posted on 25-7-2005 at 00:08


Perborate or percarbonate may also be used either insitu or otherwise as a source of essentially anhydrous H2O2.

Some water would be introduced if using a hydrate.
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[*] posted on 26-7-2005 at 06:10


I believe in addition to hydrogen peroxide and glacial acetic acid, conc. sulphuric acid is also needed to catalyse the reaction.
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[*] posted on 26-7-2005 at 14:31


I'm aware of the need for h2so4 and some time at room temp to stabilize but I was just seeking some input on weather one could produce 15% peroxyacetic acid with 27% peroxide

I'm getting the feeling one needs to have more concentrated peroxide. If anyone can clarify that it would be appreciated.

Thanks for the comments.
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