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making Cu(OAc)2
[rquote=346495&tid=34109&author=DraconicAcid]
Copper(I) salts that are not insoluble in wat ... |
18-9-2014 at 21:10
by: bbartlog |
making Cu(OAc)2
Where does the copper come in?
So far as your question goes: acetic acid by itself doesn't react ... |
18-9-2014 at 11:32
by: bbartlog |
Haloform with IPA
2ml of glacial acetic acid is not enough to acidify 100ml of 8.25% bleach, and you have too much i ... |
17-9-2014 at 20:30
by: bbartlog |
Washing a halogen contaminated aromatic aldehyde with bisulfite?
I would expect the oxidization of the bisulfite by the halogen to be the primary reaction, and the ... |
17-9-2014 at 12:43
by: bbartlog |
Haloform with IPA
Sodium hypochlorite solution does degrade over time, primarily by way of
3NaOCl -> 2NaCl + NaC ... |
17-9-2014 at 09:57
by: bbartlog |
synthesis of hexamethylethane
I would look at the feasibility of a symmetrical cross-coupling reaction of tert-butyl halides (some ... |
15-9-2014 at 09:39
by: bbartlog |
The Short Questions Thread (4)
[rquote=345283&tid=25055&author=No Tears Only Dreams Now]... cupric oxide is in a pan on the ... |
13-9-2014 at 18:43
by: bbartlog |
The Short Questions Thread (4)
Any possibility that some of your copper is still copper(I)? A bit of red Cu[sub]2[/sub]O might give ... |
13-9-2014 at 17:25
by: bbartlog |
On somewhat larger scale
Did this preparation on a larger scale, since I want to do some experiments using chloroform as a so ... |
13-9-2014 at 16:39
by: bbartlog |
hcl/solvent solution
Generally speaking, if you remove all the water by adding a massive quantity of dessicant, you'll en ... |
12-9-2014 at 21:38
by: bbartlog |
HNO3 from HCl and nitrate salt
Anhydrous AlCl[sub]3[/sub] is soluble in acetone, but you would have some kind of hydroxychloride (t ... |
11-9-2014 at 18:12
by: bbartlog |
Copper Borate?
I expect you are right about it not being metaborate; that should really just be take as a comment o ... |
11-9-2014 at 06:33
by: bbartlog |
distillation problems
You don't say what your oil was, but a lot of organic compounds will start to decompose at such temp ... |
10-9-2014 at 15:51
by: bbartlog |
3-methyl-1-phenylbut-2-en-1-one
A member did this synthesis (or one almost identical; the final step apparently can be done with NaO ... |
10-9-2014 at 08:17
by: bbartlog |
isatoic anhydride synthesis
[quote]520g of 0.42% supermarket sodium hypochlorite bleach[/rquote]
Should be 4.2%, yes?
|
8-9-2014 at 16:31
by: bbartlog |
Copper Borate?
I prepared some copper borate (though it might better be called copper metaborate, since the copper: ... |
8-9-2014 at 12:11
by: bbartlog |
Short question / quick answer - Thread
[rquote=329544&tid=26572&author=hyfalcon]They also sell DampRid which is pure calcium chlori ... |
27-8-2014 at 20:58
by: bbartlog |
The Short Questions Thread (4)
Cuprous oxide, obviously ... should have thought of that one! But the others I was unaware of. Thank ... |
4-8-2014 at 07:03
by: bbartlog |
The Short Questions Thread (4)
Are there any stable cuprous salts where the anion has a charge other than -1? For example, cuprous ... |
3-8-2014 at 21:51
by: bbartlog |
Drivers of colloidal particle size
What fundamental forces or factors make it difficult to make very small particles? Or to put it anot ... |
23-7-2014 at 11:15
by: bbartlog |
Aspirin to...
[rquote=310489&tid=27778&author=Pinkhippo11]...you would save money by making your own...[/r ... |
9-12-2013 at 07:03
by: bbartlog |
Copper Formate
The blue stuff is a hydrate, presumably the tetrahydrate. According to Charles Hurd in 'The pyrolysi ... |
6-12-2013 at 19:18
by: bbartlog |
Suitable reagents for Hydrazine Sulfate Synthesis via Ketazine
If the MSDS is accurate, it should work fine. It's always good to try and match the concentrations u ... |
15-11-2013 at 13:34
by: bbartlog |
Electrolyzing NaOH: finally succeeded !
Cast iron is a better choice than most regular steel alloys. A nickel plated vessel would be even be ... |
15-11-2013 at 13:27
by: bbartlog |
Oxidation of 2-octanol or 2-octanone to hexanoic acid
How would that even work? Assuming you cleave the final carbon and oxidize the remaining chain (via ... |
13-11-2013 at 05:45
by: bbartlog |
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