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APO
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Hydrogen Peroxide purification
Well, you can purify it buy fractional crystallation(freezing the water away) which will give 62% concentration, fractional distallation is highly
dangerous with H2O2 so that's out of question. But is there a way of seperating the H2O2 into two layers?
[Edited on 29-12-2012 by APO]
[Edited on 30-12-2012 by APO]
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neptunium
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in short no. they are both missible in one another in all proportion
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APO
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What are the most efficient methods of purification?
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Ephesian
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I have 500 mL of 30% H2O2 fisher scientific if you need some, ill put it up on ebay for you at a reasonable price.
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plante1999
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I think the best way is passing air trough 3% hydrogen peroxide at a temperature of 60-70 degree Celsius. Water evaporate before the hydrogen
peroxide, effectively concentrating the peroxide. I already concentrated it too much at 50%, so I think it could go all the way to 90%. Do not
concentrate it more than 30% for safety!
http://hclo3chem.weebly.com/concentrate-hydrogen-peroxide.ht...
I never asked for this.
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elementcollector1
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I agree with plante, but freezing only gives somewhere around 15-30% before it stops working.
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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APO
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Thanks plante1999! Sounds like a pretty good method, I'll have to try it sometime.
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shannon dove
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Wow, plante, I didn't know concentrating hydrogen peroxide was that simple.
How much is lost along with the water? (How efficient is it?)
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plante1999
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The efficiency is very high, I had made a test with 1 L of 3% H2O2 and got 100ml of about 88.5-90 volume hydrogen peroxide, or about 29-30% more than
95% yield is obtained if one troughly clean the labware and equipment.
I never asked for this.
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kristofvagyok
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Quote: Originally posted by plante1999  | | The efficiency is very high, I had made a test with 1 L of 3% H2O2 and got 100ml of about 88.5-90 volume hydrogen peroxide, or about 29-30% more than
95% yield is obtained if one troughly clean the labware and equipment. |
Khm, 1l of 3% solution contains 30g of pure H2O2, so if you've got 100cm3 at the end and we're saying that you had a 100% yield than your end product
is circa 26% pure.
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plante1999
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If one ml of 3% produce 10 volume of O2 when decomposed, and 6% is 20 volumes, Wouldn't 90 volume be 30%?
I'm sure one ml of the peroxide produced 90 ml of gas. As for the volume of the starting peroxide and finishing volume my glassware are +-10%
(Beaker) since I don't have a large enough measuring cylinder.
I never asked for this.
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shannon dove
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Why was fractional distillation and freezing methods developed if it is that easy to concentrate? Am I missing something here? It's not April fools
day.
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plante1999
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I don't know why air evaporation method is not used, I decided to use it because the low temperature protect peroxide from decomposing, the process is
also easy. But a fish air pump is probably obligatory as fish pump troughly filtrate the air (at least mine do).
I never asked for this.
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kristofvagyok
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Gas volumetric titrations are not the best, they have a high percent failure rate. Titrate it with KMnO4.
You've said that you can go up with this method to 50-90% H2O2 content, you also wrote that you have started from 3% H2O2 and got 100cm3 of +90% H2O2
what is everything but not true.
So what did you get from what? If you have ended up with 30% H2O2, than it's aint special, anyone can buy it and also everyone can make it.
I have a blog where I post my pictures from my work: http://labphoto.tumblr.com/
-Pictures from chemistry, check it out(:
"You can’t become a chemist and expect to live forever." |
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shannon dove
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I have a dream that one day I will go to the nitric acid thread and there will be a just as easy method of of concentrateing nitric acid, then I will
go to the elemental phosphorus thread .......
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plante1999
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| Quote: Originally posted by kristofvagyok | Gas volumetric titrations are not the best, they have a high percent failure rate. Titrate it with KMnO4.
You've said that you can go up with this method to 50-90% H2O2 content, you also wrote that you have started from 3% H2O2 and got 100cm3 of +90% H2O2
what is everything but not true.
So what did you get from what? If you have ended up with 30% H2O2, than it's aint special, anyone can buy it and also everyone can make it.
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I will try to do something for titration, as permanganate is regulated here, and as you may know, not everybody here have the mean and the resource of
a commercial lab as you do.
I NEVER SAID that I got 90% peroxide. I said that I already concentrated too much accidentally to 50% and as such I do think that 90% concentration is
possible. I would greatly want a quote for this affirmation.
I never said that I made 90%, if I did it was by a typo or a misunderstanding..
@shannon dove
If you don't believe in my procedure then you are not obligated to try it. It is not the first time I publish procedure never one saw/used. You can
look in the mercury from cinnabar, as I told a process for neptunium.
Not everyone is obligated to trust a 16 year old guy tough.
[Edited on 30-12-2012 by plante1999]
I never asked for this.
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shannon dove
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I do believe you plante, and I very much appreciate your research.
I would buy you a beer if I could.
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APO
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Would the evaporation method work better in a descicant chamber?
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platedish29
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Guess it works significantly for V > 30% by putting anhydrous silica in it thus easily reaching 70% concentration considering how big silica gel
grows
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Poppy
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How about merging both air evaporation and chemical dessication?
H2O2 + 7 H2O + CaCl2 -> H2O2 + CaCl2.7H2O dessicates
wherein H2O stands for removable water
H2O2 + 3CaCl2 + 2K3PO4 --> H2O2 + 3/2Ca2PO43(ppt) + 6KCl(some ppt)
wherein additional salts were dissolved in the own peroxide but in a different vessel
H2O2 + 2KCl + Fe(ClO3)3--> H2O2 + KClO3(ppt) + FeCl3
H2O2 + FeCl3 + 3NH3 --> H2O2 + Fe(OH)3 + 3NH4Cl Extra dessication occurs by the formation of hydroxides and ammonium ion
H2O2 + 2NH4Cl + PbCO3 --> H2O2 + PbCl2 + CO2 + 2NH3 + H2O
virtually removing ions from the solution
Might that go for 90%?
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ScienceSquirrel
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It is almost inevitable that your dessicants will contain traces of metal ions like copper that will be concentrated in your peroxide.
This is extremely dangerous as highly concentrated hydrogen peroxide is explosively unstable in the presence of dust, some metal ions, finely divided
metals, etc.
Even 35% hdrogen peroxide will cause rapid and painful burns if the cold solution touches the skin.
I use it on a routine scale in litre quantities for cleaning and sterilising brewing equipment and I treat it with respect.
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Poppy
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On account for the need for a centrifuge this route could also be used to prepare the loudest bang after pulling the whole machine into tears!!
Honestly, I don't think there will be any contaminants after the process is done am I wrong?
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elementcollector1
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This is slightly off-topic, but does anyone know what the concentration of hydrogen peroxide is in glow sticks? If it's anywhere higher than 12 or so,
this could be a useful and viable source (esp. from camping stores, Halloween season, etc.).
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APO
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Happy new year!!!
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ScienceSquirrel
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| Quote: Originally posted by Poppy | On account for the need for a centrifuge this route could also be used to prepare the loudest bang after pulling the whole machine into tears!!
Honestly, I don't think there will be any contaminants after the process is done am I wrong? |
You do not want any contaminants at all in hdrogen peroxide as it becomes very concentrated.
Hydrogen peroxide of over 70% concentration should be treated as a strongly corrosive, oxidisng agent and sensitive explosive.
Above this concentration contact with a suitable catalyst will cause instantaneous decomposition into oxygen and steam.
http://en.wikipedia.org/wiki/High-test_peroxide
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