| Search |
Solubility of SbCl3
oh lord, don't make pentafluoroantimonic acid |
14-8-2004 at 18:19
by: budullewraagh |
KMnO4
if youre looking for something to do, add the KMnO4 to conc H2SO4 slowly. you'll get conc perm ... |
14-8-2004 at 07:52
by: budullewraagh |
Solubility of SbCl3
the other day i was looking through my "lange's handbook of chemistry" and i stumbled ... |
13-8-2004 at 17:50
by: budullewraagh |
Electronegativities/activity of monoatomic and polyatomic ions
can anybody here tell me the electronegativities of monoatomic polyatomic ions? is there an activity ... |
13-8-2004 at 17:49
by: budullewraagh |
Who needs a centrifuge ?
the image doesn't show up. i investigated further by looking through the source script and i f ... |
10-8-2004 at 11:39
by: budullewraagh |
Most corrosive agent?
why the bloody hell would you ever have a want for KCN? |
10-8-2004 at 09:23
by: budullewraagh |
Most corrosive agent?
[quote]Superacids are indeed very acidic by pKa standards but how do they react when exposed to virg ... |
9-8-2004 at 19:50
by: budullewraagh |
Most corrosive agent?
[quote]There is always "magic acid" fluoroantimonic acid, a 50% solution of SbF5 in HF, vi ... |
9-8-2004 at 14:56
by: budullewraagh |
NO2(g) sources
problem is that i wanted to make nitric by bubbling the anhydride into solution |
6-8-2004 at 16:11
by: budullewraagh |
Lithium from Batteries
[quote] CaCl2 or MgSO4 [/quote]
their cations very well may be replaced by the Li |
6-8-2004 at 13:28
by: budullewraagh |
Who needs a centrifuge ?
har har. bush attempting to justify the war again...tsk tsk. |
5-8-2004 at 17:54
by: budullewraagh |
Uranium
can you not be so condescending?
lithium works better in that it releases less energy AND is a be ... |
3-8-2004 at 10:26
by: budullewraagh |
Uranium
lithium works better. |
2-8-2004 at 20:16
by: budullewraagh |
Lithium from Batteries
[quote]No hard feelings, k? [/quote]
no worries at all.
actually, the post above reminded me; NH ... |
2-8-2004 at 14:07
by: budullewraagh |
Lithium from Batteries
mixtures aren't all aqueous solutions.
50mL HCl(l) and motor oil form a mixture but certainly ... |
2-8-2004 at 12:43
by: budullewraagh |
Uranium
hey word is "URANANITE" (ore). please note that i didn't say "uranium ore" ... |
2-8-2004 at 11:16
by: budullewraagh |
Lithium from Batteries
indeed. that's why i didn't say to make an aqueous solution |
2-8-2004 at 11:11
by: budullewraagh |
Uranium
if you have urananite ore, just replace the uranium with a more active element (ex any alkali metal) ... |
2-8-2004 at 08:15
by: budullewraagh |
H2SO3 to H2SO4
eh, soz |
2-8-2004 at 08:05
by: budullewraagh |
H2SO3 to H2SO4
H2O2 is an excellent oxidizing agent. it's also very simple to make it concentrated. just fre ... |
2-8-2004 at 06:37
by: budullewraagh |
Lithium from Batteries
well, i was just saying that if you wanted to have some fun, you could have reacted it with a concen ... |
2-8-2004 at 06:34
by: budullewraagh |
NO2(g) sources
that's a shame. i dont suppose an alkaline solution would work either since there are some cat ... |
1-8-2004 at 20:51
by: budullewraagh |
NO2(g) sources
[quote]
Be forewarned that NO2 is exceedingly toxic[/quote]
of course; it's nitric anhydride: ... |
1-8-2004 at 19:39
by: budullewraagh |
NO2(g) sources
anybody know some reasonably easy to obtain chemicals that would yield NO2(g)? |
1-8-2004 at 18:55
by: budullewraagh |
Lithium from Batteries
ah, so it's the iron sulfide that smells so bad. seriously awful stuff, that. i also got some ... |
1-8-2004 at 18:53
by: budullewraagh |
