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Author: Subject: synthesis of H2o2??
thereelstory
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[*] posted on 3-2-2010 at 18:21
synthesis of H2o2??


does anyone have any good suggestions for a synthesis of 1 liter batches of hydrogen peroxide?
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chemoleo
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[*] posted on 3-2-2010 at 18:56


Please search the forum... there must be at least a dozen threads on this...



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thereelstory
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[*] posted on 3-2-2010 at 20:23


ok still learning the tricks of navigation....utfse
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thereelstory
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[*] posted on 3-2-2010 at 20:34


the problem is these h202 posts have lead to dead ends, or at best diluted h202. how increadible would it be for one of these geniuses on here to come out with an illustrated breakdown for conc h202.
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Sedit
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[*] posted on 3-2-2010 at 22:08


That would be great.... I tell ya what, you solve the decomposition problems and we will work on the synthesis when you got that worked out.


Why not just find ways to dehydrate aq H2O2 or risk your life distilling which is gonna enter the synthesis somewhere.





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hissingnoise
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[*] posted on 4-2-2010 at 04:34


IIRC, concentrated H2O2 is dangerous to handle but you can buy 35% H2O2 quite easily.

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[*] posted on 4-2-2010 at 05:39


Concentrated hydrogenperoxide can easily light a piece of paper, saw a nice demonstration once.

You could look into electrolyses preparation books ive seen h2o2 mentioned there a couple of times.
but really dont bother and search for a good supplier.




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DJF90
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[*] posted on 4-2-2010 at 05:51


Wikipedia mentions the method I've seen before...
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[*] posted on 4-2-2010 at 07:10


Food grade 35% hydrogen peroxide is as cheap as chips, about £15 a litre where I live.
As a laboratory reagent it is about as strong as you would want to go under normal circumstances
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hissingnoise
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[*] posted on 4-2-2010 at 07:43


And 'food grade' means no stabilisers so it should be stored in a fridge.


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thereelstory
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[*] posted on 4-2-2010 at 09:18


whats wrong with PURE hydrogen peroxide?
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hissingnoise
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[*] posted on 4-2-2010 at 09:39


It decomposes over time; CH3OH, and other substances, is added as a stabiliser.
Unadulterated, it's slightly thermally unstable!
With higher concentrations than 35% stability falls off quite quickly!



[Edited on 4-2-2010 by hissingnoise]
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DJF90
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[*] posted on 4-2-2010 at 10:16


Quote: Originally posted by hissingnoise  
With higher concentrations than 35% stability falls off quite quickly!


Not true... In fact quite the opposite. 90% Hydrogen peroxide (so long as it is very pure) requires no stabiliser and the rate of decomposition is approx. 1% per year at 30*C, which is much less than for 30-35% solutions

[Edited on 4-2-2010 by DJF90]
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[*] posted on 4-2-2010 at 12:57


Quote: Originally posted by thereelstory  

.. how increadible would it be for one of these geniuses on here to come out with an illustrated breakdown for conc h202.


Or: why don't "one of these geniuses" just stop whatever project they happen to be working on and develop a recipe with photos so I can be spoonfed.




The single most important condition for a successful synthesis is good mixing - Nicodem
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[*] posted on 4-2-2010 at 13:20


Quote: Originally posted by thereelstory  
whats wrong with PURE hydrogen peroxide?



Really concentrated hydrogen peroxide eg 70+% is a lot more dangerous than 35% hydrogen peroxide.
Some materials will catch fire on contact with it and it will decompose explosively to steam and oxygen on contact with catalysts such as finely divided metals.
The 35% hydrogen peroxide is a good compromise as it is concentrated enough to be shipped economically but at the same time it can be handled fairly safely and it is widely used as a sterilising agent in the food industry and elsewhere.
However contact with the skin of the hands causes white burns that rapidly become very painful, you do not want to get it elsewhere!

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hissingnoise
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[*] posted on 4-2-2010 at 15:41


Quote:
Not true... In fact quite the opposite. 90% Hydrogen peroxide (so long as it is very pure) requires no stabiliser and the rate of decomposition is approx. 1% per year at 30*C, which is much less than for 30-35% solutions

That's surprising DJF90, I assumed H2O2 resembled HNO3 in that regard.
I still wouldn't like to have to handle 90% H2O2 because presumably some minor contamination could cause an explosive decomposition.

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[*] posted on 4-2-2010 at 17:01


im a rookie wanna be science freak. spoon fed is a good place to start. i figure there are plenty of intelligent people here who have contributed for the sake of sharing information. for those who modus operandi is quid pro quo, give me a few years and i will gladly reciprocate, after i learn to walk....this is definitely the best science forum i have ever come across.
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watson.fawkes
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[*] posted on 4-2-2010 at 17:15


Quote: Originally posted by thereelstory  
im a rookie wanna be science freak. spoon fed is a good place to start. i figure there are plenty of intelligent people here who have contributed for the sake of sharing information.
If you'd like to be spoon fed, then don't expect to pick your project. There are a number of detailed tutorials out there. Pick one and go.
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[*] posted on 4-2-2010 at 17:34


90+% hydrogen peroxide is highly sensitive and a monopropellant.
Dropping your girlfriend's silver neck chain in to a beaker holding half a litre of 90% hydrogen peroxide could result in an explosion that will kill both of you instantly and probably destroy the building you are standing in.
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[*] posted on 4-2-2010 at 20:03


Hi gents I found this review paper and thought it may be usefull on this thread



Attachment: h2o2-review.pdf (774kB)
This file has been downloaded 5957 times

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DJF90
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[*] posted on 5-2-2010 at 02:40


I never said it would be nice to work with, just that its more stable than 30-35% so long as its sufficiently pure.
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hissingnoise
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[*] posted on 5-2-2010 at 04:42


90% would be interesting though - powering these things. . .
http://www.tecaeromex.com/ingles/peroxidoi.html

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[*] posted on 5-2-2010 at 06:20


Quote: Originally posted by thereelstory  
im a rookie wanna be science freak. spoon fed is a good place to start. i figure there are plenty of intelligent people here who have contributed for the sake of sharing information. for those who modus operandi is quid pro quo, give me a few years and i will gladly reciprocate, after i learn to walk....this is definitely the best science forum i have ever come across.


If you think anyone on here is going to spoon feed you instructions on making high test hydrogen peroxide you are very foolish indeed.
Have a look at the peroxide rocket site, very pure hydrogen peroxide is safe if you have the skills and experience to handle it but a mistake is very serious indeed.
You do not want to 'learn to walk' making it, you might as well learn to drive on the autobahn.
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[*] posted on 5-2-2010 at 06:21


What about this way: (?)

BaO2 + H2SO4 → H2O2 + BaSO4

Should give high concentration, BaO2 could be made from ordinary BaO ... ;
... then the BaSO4 could be recycled ...
==> So the only necessary input-chemical would be H2SO4 ...
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[*] posted on 5-2-2010 at 06:29


Quote: Originally posted by chief  
What about this way: (?)

BaO2 + H2SO4 → H2O2 + BaSO4

Should give high concentration, BaO2 could be made from ordinary BaO ... ;
... then the BaSO4 could be recycled ...
==> So the only necessary input-chemical would be H2SO4 ...


That is a classical way of making hydrogen peroxide but the reaction is carried out with dilute sulphuric acid to produce a weak aqueous solution that is then distilled.
Concentrated acid would produce Piranha solution and you really do not want to go there!
http://en.wikipedia.org/wiki/Piranha_solution


[Edited on 5-2-2010 by ScienceSquirrel]
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