Author Topic: oxone (Read 125 times)

poisoninthestain · « **on:** July 16, 2009, 09:12:29 PM »

The highest concentrations of oxone I can find are something like 36%. I called the company and requested an MSDS. Turns out there's sodium carbonate, sodium bisulfate(or bisulfite I forget) plus a few other salts in there

I was wondering if 36% as the only active ingredient is enough to perform an oxidation.

I rather opt for 99-100% but I can't find it. Any help would be appreciated.

...reason I ask is because I'd like to go this route as opposed to a traditional halogenation, specifically bromination.

I'm just afraid any PH buffers in my 36% oxone will fuck up the formation of hypobromous acid(which will then brominate the ring).

Thanks in advance.

Sedit · « **Reply #1 on:** July 16, 2009, 09:15:07 PM »

IIRC I have seen higher precentage then that at Wal-Mart in the pool sections.

Vesp · « **Reply #2 on:** July 16, 2009, 10:17:43 PM »

Either way it is pretty expensive, isn't it?

You may be better off making it, if that isn't to hard.

The carbonate and bisulf?te would react once dissolved in solution, and you'd probably have significant bubbling.

Sedit · « **Reply #3 on:** July 16, 2009, 10:36:13 PM »

No not expensive at all I dont think.

Vesp · « **Reply #4 on:** July 16, 2009, 10:45:57 PM »

Oh, well I don't remember the price of it, but for the concentration I remember I wasn't impressed with it and pretty annoyed they'd charge that much for it.

2bfrank · « **Reply #5 on:** July 17, 2009, 01:49:33 AM »

Vesp,

Their are some interesting procedures utilizing plain oxone/acetone/etc for a variety of reactions as well as the precipitation of 2 of the salts leaving the peroxymonosulfate to be very concentrated. This is apparently achieved by dissolving the commercial oxone in D.I. water, at 2 deg Celsius and filtering of most of the precipitated unwanted 2 salts, The attached article goes into this with respect to the baeyer villiger oxidation.
What is of interest is the viability/possibility/??? of preparing a higher concentration of peracid/g on silicon gel - 10mmol/g hence say using, 100g total - hence 1mol. Then with a 2:1 of peracid/silicon gel and ketone respectively in the hope of the stated quantitative yields. Considering oxone is reported to have approx 36% of the peroxymonosulfate, looking into this is something I feel could be worthy. Also making Caro's acid and reacting that with the pottasium salt could also generate the desired peroxymonosulfate. I don't know, and of course these are just hypothetical discussions on amateur chemistry.
I will check my figures again, as perhaps I have got this confused.

2b

2bfrank · « **Reply #6 on:** July 17, 2009, 02:39:43 AM »

I just realised that 10mmol would equate to 1.9 grams of Potasium peroxymonosulfate hence would not be able to load on the 1g of silicon gel. 5 mmol could perhaps, or one increase the amount of gel used, say 150g. I reckon this could somehow be tweaked. DCM, Acidic SiO2gel, Oxone at room temp appears attractive.

Also the MSDS i got from a pool place that deals with dupont direct, showed no other salts other than the potassium as the sulfate, bi, and peroxy etc. Perhaps shop around. Ill hunt down the MSDS and name brand if you like. I also realised that this thread is about another use, so apologies about going of in this particular tangent.

Author Topic: oxone (Read 125 times)

poisoninthestain

oxone

Sedit

Re: oxone

Vesp

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Sedit

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Vesp

Re: oxone

2bfrank

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2bfrank

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