| Search |
| [Next Page] |
unconventional sodium
http://avogadro.chem.iastate.edu/MSDS/NaOAc-3H2O.htm
Looks like anhydrous acetate is insoluble in e ... |
29-9-2003 at 04:55
by: Theoretic |
PbO or PbO2
Correct me if I'm wrong...
Cathode:
Pb + 2H2O => Pb(OH)2 + 2H+
Anode:
2H+ + 2e- => ... |
29-9-2003 at 04:31
by: Theoretic |
cheapest way to 96% hno3
The original question was: can NH4NO3 work? Yes it CAN!
At high temperatures the reaction of NH3/NH ... |
12-9-2003 at 07:10
by: Theoretic |
Cyanogen nitrite/nitrate
Thanks, that's quite useful (although I thought of NO2Cl too, I didn't know it could be ma ... |
12-9-2003 at 04:22
by: Theoretic |
Perperation of calcium
Apparently NOT. If this reaction is used as a purification reaction, then it must be quite easy and ... |
10-9-2003 at 04:50
by: Theoretic |
Cyanogen nitrite/nitrate
I'm thinking about compounds-cyanogen nitrite and nitrate. I think they could be made by:
ClC ... |
10-9-2003 at 04:44
by: Theoretic |
Perperation of calcium
Industrially, the Ca metal obtained by electrolysis is purified from salt impurities by passing (mol ... |
8-9-2003 at 06:24
by: Theoretic |
High-t (useful) ion exchange
You don't need especially pure Al2O3. I think anything with a content of Al2O3 will do (as long ... |
8-9-2003 at 04:50
by: Theoretic |
unconventional sodium
The McGraw-Hill "Handbook of inorganic industrial chemicals" says Na reacts with NaOH betw ... |
12-8-2003 at 06:05
by: Theoretic |
electrolytic manufacturing of HNO3 from Ca(NO3)2
Well, Ca(OH)2 will still act as an insoluble base - compare with CaCO3.
It would still create a HIG ... |
11-8-2003 at 08:09
by: Theoretic |
PbO or PbO2
Yeah, Na2 is theoretically possible, but with zero thermodynamical stability. Just nothing to hold i ... |
11-8-2003 at 07:58
by: Theoretic |
Processing chlorate cell electrolyte
Well... if anyone wants to try NaClO3 for a change? More oxygen per gram and a "golden flame&qu ... |
8-8-2003 at 05:58
by: Theoretic |
NH4NO3->nitric acid + ammonia
Actually, ammonium amalgam decomposes readily at ordinary temperatures. It COULD be that you still g ... |
8-8-2003 at 05:49
by: Theoretic |
Yes, comments, comments...
Yes! It won't work! 
Apart from clogging the electrode and stopping the current from flow ... |
7-8-2003 at 06:00
by: Theoretic |
NH4NO3->nitric acid + ammonia
Er, chemoleo, there's actually a 40C gap between AN's melting temperature (170C)
and its ... |
4-8-2003 at 06:56
by: Theoretic |
Potassium ferrate
Mistake! Not 2.7, but 2.07!
Well, 2.07 according to some, 2.08 according to another, and 2.75 accor ... |
1-8-2003 at 07:09
by: Theoretic |
Decomposing Urea
Hmmm, urea into ammonia...
Ca(OH)2+CO(NH2)2=>CaCO3+NH3
(melt) |
1-8-2003 at 07:02
by: Theoretic |
Potassium ferrate
It's red/purple.
Could Na2FeO4 be made by electrolysing a NaOH solution with a steel or iron c ... |
31-7-2003 at 09:35
by: Theoretic |
High-t (useful) ion exchange
Yes, that's one reactant solid and one liquid (Edit: or gas). A link? No, I coined the term mys ... |
31-7-2003 at 08:37
by: Theoretic |
Nitric acid
OOPS... the problem is where we least expect it (more so if you need anhydrous HNO3).
4NO2+2H2O+O2= ... |
31-7-2003 at 08:35
by: Theoretic |
Cyanate to cyanide - fresh thread
Somewhere in the deep core of the old cyanide thread there's a few posts about
cyanate, with u ... |
31-7-2003 at 06:47
by: Theoretic |
Sodium!
Oh well,  .
But what about tribasic sodium phosphate? It's m.p. is 73-77C, and it's not ... |
31-7-2003 at 06:33
by: Theoretic |
O3?
Well, electrolysis of HClO4 at high current density yields 30% O3, and I guess it's much more f ... |
28-7-2003 at 06:12
by: Theoretic |
Anhydrous ammonia preparation
How about THIS?
CO(NH2)2+Ca(OH)2=>CaCO3+2NH3
 |
24-7-2003 at 09:50
by: Theoretic |
Nitric acid
So it WOULD work after all... |
24-7-2003 at 09:46
by: Theoretic |
| [Next Page] |
