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Author: Subject: h202 concentration?
Neil
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[*] posted on 9-4-2008 at 17:06


Quote:
Originally posted by Ozone
Any concentration (1%, even) IV will be instantly broken down by catalase and iron compounds in the blood. This will yield O2 (g) which will (likely) yield clots and death via embolism. Bubbles in the blood stream are bad, mkay!

Greater concentrations should only add to the spectacle, not the final result:o.

WTF?

O3



Google it... 'oxygen revitalises and refreshes you' or some bs like that... people have been there done that...see here...Scary eh?


Edit: as a side note to Canada's moderation of 35% H2O2, buy it from hydro stores with cash.. they don't keep records of their purchasers for some reason ;o)

[Edited on 9-4-2008 by Neil]
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[*] posted on 27-4-2008 at 01:17


Hi everyone,
I had seen in the Handbook that pure H2O2 could be made by extraction of commercial solutions using ethyl ether thjat extracts only pure H2O2, never tried it !
Any suggestions ?
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[*] posted on 26-5-2008 at 06:26


An interesting patent, pitty its jap. It seems its just an acid stabalised H2O2, though it would be interesting to see what concentrations are optained. The reference to it exploding suggests high concentrations.

Concentration of hydrogen peroxide water by heating. Taketa, Kikuo; Watanabe, Satoshi; Sasaki, Shigeru; Naka, Hideo; Okusaki, Junichi. (Sumitomo Chemical Co., Ltd., Japan; Sumika Bunseki Center K. K.). Jpn. Kokai Tokkyo Koho (1998), 5 pp. CODEN: JKXXAF JP 10338508 A 19981222 Heisei. Patent written in Japanese. Application: JP 97-145447 19970603. Priority: . CAN 130:68703 AN 1998:816487 CAPLUS

Patent Family Information

Patent No. Kind Date Application No. Date
JP 10338508 A 19981222 JP 1997-145447 19970603

Priority Application
JP 1997-145447 19970603


Abstract

HCl is added to aq. H2O2, and then the soln. is heated for concn. The HCl addn. prevents explosion of the aq. soln. during the concn.

[Edited on 27-5-2008 by Axt]
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Formatik
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[*] posted on 27-5-2008 at 20:35


Quote:
Originally posted by pbmineral
Hi everyone,
I had seen in the Handbook that pure H2O2 could be made by extraction of commercial solutions using ethyl ether thjat extracts only pure H2O2, never tried it !
Any suggestions ?


I've done some of these with various concentrations but it was a wasn't worth the ether IMO. First you should know that the mixture is detonable, but even more hazardous is the potential of formation of risky organic peroxides and lastly you have to use a very large amount of ether to extract any significant amount
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MagicJigPipe
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[*] posted on 27-5-2008 at 21:31


Quote:

Google it... 'oxygen revitalises and refreshes you' or some bs like that... people have been there done that...see here...Scary eh?


Read up on the details of this story. IMO, it was virtually impossible for her death to have been caused by that little H2O2. 25mL of O2 killed her 4 days later? Bullshit.

I've been thinking about the barium peroxide method for producing H2O2. How is barium peroxide obtained?




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[*] posted on 27-5-2008 at 21:49


Quote:
Originally posted by MagicJigPipe
...
I've been thinking about the barium peroxide method for producing H2O2. How is barium peroxide obtained?


Basically by heating barium oxide in CO2 (and SOx NOx) free air. Usually done under a couple of atmospheres of air pressure at 500 to 600 C. An old process for extracting oxygen from the air started with this, then while keeping the temperature the same pumping off the air and then the released O2; repeat until BaO becomes too unreactive.

The BaO is made by heating a mixture of BaCO3 and carbon, made into a paste with oil or tar, to yellow to white heat. The plain carbonate does not decompose readily until much higher temperatures, the carbon causes a decomposition to carbon monoxide and barium oxide at a lower temperature.

lets see now, here's one old reference, there are plenty of others from this time and earlier.

http://books.google.com/books?id=MAA5AAAAIAAJ&pg=PA640&lpg=P...
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VestriDeus
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[*] posted on 15-11-2009 at 13:18


Has anyone tried this:

http://www.instructables.com/id/Distill-Hydrogen-Peroxide/

It says to add iodine-free table salt to low conc. H2O2, and that the stuff should separate into two layers, salt water and hydrogen peroxide.
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[*] posted on 16-11-2009 at 04:00


I dont want to reject the possibility directly, anyway that guy that wrote the stuff does not really know what he's talking about.
"Distill Hydrogen Peroxide"
Distilling?, what is he distilling?

It could be that NaCl is fully insoluble in hydrogenperoxide, in this case it could be possible to force the H2O2 out by saturating the H2O.

Can anyone support this ?





What a fine day for chemistry this is.
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Formatik
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thumbdown.gif posted on 16-11-2009 at 15:14


Way to contaminate with metallic cations. Sodium chloride is a catalyst for H2O2 decomposition, not as strong as Pt, Ag, Os, MnO2, etc. but in the same order as CuO, Mn(NO3)2, HgO, AgO, FeO, ZnSO4, Na2CO3, CaCl2, BaCl2, etc. Nothing there even hints that a more conc. peroxide results. It looks like a joke.
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[*] posted on 16-11-2009 at 17:59


This more then likely has been suggested already but the idea has been floating in my head for about a week and with all this talk of H2O2 concentration going around how would this work out?

Placing an open bottle of H2O2 into a dessicator bag full of MgSO4 and sealed up in a dark place. It will eliminate the worry of organic dust falling in while still allowing it to evaporate the water from the solution.

I suspect near 100% H2O2 could in theory be formed this way but perhaps some form of equilibrium will setup with water absorbant properties of H2O2 that I do not know about.




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[*] posted on 16-11-2009 at 19:54


I can see your point.
Often i wonder why such hard ways of doing stuff is considered.
Dessicating substances is such an old and plain simple way.
The same thing can be done with HNO3 if the absorbing properties are high enough.

[Edited on 17-11-2009 by User]




What a fine day for chemistry this is.
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Formatik
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[*] posted on 17-11-2009 at 21:58


Quote: Originally posted by Sedit  
This more then likely has been suggested already but the idea has been floating in my head for about a week and with all this talk of H2O2 concentration going around how would this work out?

Placing an open bottle of H2O2 into a dessicator bag full of MgSO4 and sealed up in a dark place. It will eliminate the worry of organic dust falling in while still allowing it to evaporate the water from the solution.


The threat of organics (like cellulosics), is often due to present trace metal catalysts. So, I wouldn't dry H2O2 with metallic salts like MgSO4 because then of airborne particulates that would end up contaminating it. Sterile environment is crucial for high strength peroxide. P2O5 or H2SO4 are good choices. Regular dessication works for higher strength, but takes a long time. Vacuum dessication is said to work even faster. There are other conc. threads that talk about this in detail. I also suggest to see what Mellor has to say about concentration.
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Sedit
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[*] posted on 18-11-2009 at 06:31


Your right Formatik although it can be solved with a little glass wool in the opening though. I hate the idea of drying stuff with H2SO4 for some reason. I will look into Mellor and see what kind of data he gives although its not to important to me since I can get 35% with ease and thats more then enough for most things for me. Very few synthesis call for 100% H2O2 so the rest is just bulk.



Knowledge is useless to useless people...

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