Thermal - 24-7-2005 at 17:02
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?
BromicAcid - 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
Goes to completion.
Thermal - 24-7-2005 at 21:52
I see.
The Acetic acid I would be using is Glacial.
S.C. Wack - 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.
bio2 - 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.
praseodym - 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.
Thermal - 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.