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Bismuth oxy compounds
There is a formula for finding the degree of hydrolysis of cations. Information is on this site htt ... |
22-3-2006 at 16:09
by: guy |
Bismuth oxy compounds
Hydrolysis of BiX3 forms BiOX and 2HX. Does it do the samething with Bi(NO3)3? Why does bismuth hy ... |
21-3-2006 at 16:34
by: guy |
Reaction between nitrite and cyanide?
This is what I would do to try and narrow down the choices.
We know that chloride is necessary fo ... |
18-3-2006 at 17:10
by: guy |
Reaction between nitrite and cyanide?
Can any other acid be used, say sulfuric acid? If that works, or doesn't, then you could decide if t ... |
16-3-2006 at 17:54
by: guy |
Magnesium bisulfate?
I think I go it, maybe the HCO3- gets converted to H2CO3 and that forms MgCO3 but that reacts to for ... |
13-3-2006 at 23:22
by: guy |
Magnesium bisulfate?
Stoichiometric amounts of (NH4)2SO4 and MgSO4 are very intamately mixed and heated for about 30 mins ... |
13-3-2006 at 17:12
by: guy |
Copper (II) thiocyanate?
For the solution with NaOH, why would the precipitation of CuOH take so long? After about 30 minute ... |
5-3-2006 at 02:18
by: guy |
Copper (II) thiocyanate?
The acetate one definetley has a different color. It is a forest green (kind of dark-ish), while th ... |
4-3-2006 at 23:58
by: guy |
Copper (II) thiocyanate?
I used the weed killer as is. I don't know how to purify it.
How does the fact that the copper i ... |
4-3-2006 at 23:38
by: guy |
Copper (II) thiocyanate?
Which precipitate? The one in NaOH? That one resembles Cu2O more. The original solution is a real ... |
4-3-2006 at 22:58
by: guy |
Copper (II) thiocyanate?
NaSCN (25% tinted blue, from a weed killer) was added to CuSO4 crystals. Immediatly a dark red (mar ... |
4-3-2006 at 21:50
by: guy |
Azide anion
The charge on each atom of the azide ion is actually -1/3. The electrons are delocalized throughout ... |
2-3-2006 at 15:09
by: guy |
Silicon from Quartz
That might work theoretically, but then theres the problem of Mg reacting with water, and then Si re ... |
1-3-2006 at 22:17
by: guy |
Silicon from Quartz
Just use sodium silicate, since it also has the SiO4 4- structure. It can still be reduced even in ... |
28-2-2006 at 23:03
by: guy |
Silicon from Quartz
Why don't you try it out and see if it works. I would but I don't have any strong acids. Try using ... |
28-2-2006 at 21:18
by: guy |
Cu + HCl + H2O2; Solution color
CuCl2 in HCl can etch copper due to this reaction:
CuCl2 + 2HCl <--> [CuCl4]2- + H+
[CuC ... |
26-2-2006 at 23:16
by: guy |
Cu + HCl + H2O2; Solution color
Anhydrous CuCl2 is brown. Try adding the brown stuff to water and wait and see it turns blue again. |
25-2-2006 at 22:58
by: guy |
Explanation for odd permanganate experiment...
O yeah thats a mistake, it should be oxidized. Also MnO4 2- to MnO4 - can be done by adding H+. It ... |
22-2-2006 at 20:14
by: guy |
Strange copper/iron reaction
Looking at the CuCl2 + CuCl reaction on your site, I think maybe the reaction is [Cu(H2O)4]2(aq)+ + ... |
22-2-2006 at 17:00
by: guy |
Explanation for odd permanganate experiment...
Yes it reduced something in the paper, thats the only explanation |
22-2-2006 at 16:09
by: guy |
Strange copper/iron reaction
[quote]Also, I'd rather stick to the same counterions, i.e. only H2SO4, or only HCl. No mixture of F ... |
21-2-2006 at 22:14
by: guy |
Strange copper/iron reaction
Well I tried to replicate the experiement. I don't have HCl so I used NaCl. Somehow it didnt form ... |
21-2-2006 at 19:38
by: guy |
Strange copper/iron reaction
I have an idea. Reduction potentials are a result of thermodyanamic stability, so if the the produc ... |
21-2-2006 at 18:00
by: guy |
Strange copper/iron reaction
[quote]
(Cu2+) + e- --> Cu+ |+0.16 V
(Fe2+) ---> (Fe3+) + e- | -0.77 V
This reaction ... |
21-2-2006 at 16:33
by: guy |
Gibbs free energy
Yeah, I think there is SOMETHING missing here. Could be electrons, or ionization energy, etc.
Do ... |
20-2-2006 at 23:46
by: guy |
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