| Pages:
1
2 |
teodor
National Hazard
Posts: 922
Registered: 28-6-2019
Location: Netherlands
Member Is Offline
|
|
Well, Karlos, my experience with this complex was only its usage. For long time it was the only one form of concentrated H2O2 available for my home
experiments. I was able to buy it quite cheap in any household shop (back in SU). I remember it had a quite good shelf life as for 30% H2O2 and I was
able to handle it with my bare hands.
I doubt there is any practical method to remove urea except converting e.g. to BaO2 or some other hydrated metal peroxide. I understand that you don't
want urea always when you want H2O2 in your reaction mixture but it is the price of simplicity and harmless life, I believe you understand me here.
Of course there are some threads here about it from men who had to say more, for example this one: http://www.sciencemadness.org/talk/viewthread.php?tid=23477
And if you like to ask me personally: "urea is dissolved in 30% hydrogen peroxide (molar ratio 2:3) at temperatures below 60 °C. upon cooling this
solution, hydrogen peroxide - urea precipitates in the form of small platelets" (https://doi.org/10.1021/ja01851a007). Don't credit or trust me, it's from wikipedia.
I am also was always interested in the method to remove urea from H2O2 water solution, by the way, it sounds like a good challenge.
As well as purification of H2O2 by recrystallisation of urea complex.
[Edited on 29-7-2021 by teodor]
|
|
|
Mateo_swe
National Hazard
Posts: 548
Registered: 24-8-2019
Location: Within EU
Member Is Offline
|
|
Sodium Perborate could be useful ta have in the future and i dont think its part of any "oxy-action" cleaning compound.
Those usually contain Sodium Percarbonate, at least the ones i have looked at.
So i will try make some Sodium Perborate from the H2O2 before it become useless.
Nice webpage with chemical and physics experiments woelen.
I might try a few of those experiments.
|
|
|
| Pages:
1
2 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
