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Alternate methods of finding Acid/Alkali concentrations (determining pH!!)
Not really. The key is to use a precipitating reagent. eg. for sulfuric acid, use barium chloride, f ... |
15-5-2004 at 09:02
by: t_Pyro |
NaClO4 production using a Pt clad Ti anode and a Ti cathode.
Er... Don't you think you set your sights a bit too high? 5 Kg of perchlorate a week? You could ... |
30-4-2004 at 18:01
by: t_Pyro |
NaClO4 production using a Pt clad Ti anode and a Ti cathode.
If you're having problems with the voltage drop, it may be possible that the salt solution isn& ... |
28-4-2004 at 18:14
by: t_Pyro |
Metal Solubility and Solvent
They are solutions of the respective copper salts, not of metallic copper.
Metals do form crystal ... |
28-4-2004 at 17:57
by: t_Pyro |
NaClO4 production using a Pt clad Ti anode and a Ti cathode.
I see you've already started using your new-found electrodes to the max! Approximately what is ... |
27-4-2004 at 21:42
by: t_Pyro |
Metal Solubility and Solvent
Alkali metals like lithium are soluble in liquid ammonia. The dilute solutions are blue in colour, t ... |
26-4-2004 at 18:12
by: t_Pyro |
Thermite Igniter?
Not if you're using a titanium wire with your fishing pole... |
22-4-2004 at 19:16
by: t_Pyro |
KMnO4, Sulfur sensitivity
I've heard that explanation lots of times now, and probably it is the right one, but I'm s ... |
22-4-2004 at 19:04
by: t_Pyro |
Precipitation with Alcohol
A compound dissolves by forming weak interactions or "bonds" with the solvent molecules. F ... |
21-4-2004 at 23:29
by: t_Pyro |
NaOH
If you got a ppt of CaCO<sub>3</sub>, then there has to be some NaOH. However, it won� ... |
21-4-2004 at 23:13
by: t_Pyro |
MgSO4 --> H2SO4
The ions with a greater ionic mobility migrate the fastest. Ions are elctronated/de-electronated acc ... |
20-4-2004 at 18:07
by: t_Pyro |
Chloroform
Acetone and conc HCl should undergo acid-catalysed aldol condensation, too, to give mesityl oxide, s ... |
17-4-2004 at 18:41
by: t_Pyro |
Replatinizing and platinizing Ti.
[quote][i]Originally posted by unionised[/i]
Chloroplatinic acid gives PtCl4 2- ions in solution, t ... |
17-4-2004 at 18:37
by: t_Pyro |
Iron Oxide
The "green gunk" would be ferrous chloride. If a substance formed during electrolysis is i ... |
16-4-2004 at 18:58
by: t_Pyro |
Replatinizing and platinizing Ti.
Sorry for playing spoilsport, but...
Hexa chloroplatinic acid has Pt in a positive oxiadtion state, ... |
16-4-2004 at 09:47
by: t_Pyro |
Chlorine
Organikum, I didn't understand what you meant by "metachlorides" in relation to Fried ... |
16-4-2004 at 09:29
by: t_Pyro |
MgSO4 --> H2SO4
Pure Pt and Pt clad Ti ????? I'd KILL for that! Lucky you!  Any chance of
auctioning it of ... |
14-4-2004 at 19:40
by: t_Pyro |
Chlorine
Electrolysis of an aqueous solution of <i>any</i> ionic chloride would result in the for ... |
14-4-2004 at 19:11
by: t_Pyro |
Sciencemadness hax0red!
First off... MD5 hashes aren't secure, not by a looong way. Cain can crack them in less than a ... |
13-4-2004 at 18:21
by: t_Pyro |
Chlorine
Proteios: The reaction you stated most probably is a redox reaction between Fe<sup>2+</sup& ... |
13-4-2004 at 18:03
by: t_Pyro |
What could i do with these chemicals?
fehling's solution: Can be used to detect aldehydes. I assume you've got both the "A& ... |
6-4-2004 at 09:34
by: t_Pyro |
Complex ions of copper
Tetrammine copper compounds have got me confused now. Till now, I always used to regard it as [Cu(NH ... |
2-4-2004 at 20:51
by: t_Pyro |
stains form KMnO4
Thiosulfate would be for the silver stains. Removal as a soluble complex. |
2-4-2004 at 20:41
by: t_Pyro |
stains form KMnO4
[quote]
The stains won't vanish completely by washing
[/quote]
That's odd, if I accid ... |
2-4-2004 at 09:05
by: t_Pyro |
Possible speedbumps ahead
Trouble with chloropicrin? I'm sure nobody would have been making it in large enough quantities ... |
2-4-2004 at 09:00
by: t_Pyro |
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