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Why you can't buy sulfuric acid
Sodium carbonate doesn't decompose at 500C, and you cannot make sodium oxide this way. However, heat ... |
9-7-2012 at 11:25
by: barley81 |
Why you can't buy sulfuric acid
The sulfuric acid drain opener gradually eats through its container. Perhaps this is what happened. ... |
8-7-2012 at 05:18
by: barley81 |
Sulfuric Acid
A mole of copper sulfate pentahydrate weighs ~250g. Each liter of 98% sulfuric acid has 18 moles of ... |
7-7-2012 at 10:23
by: barley81 |
Aluminium amalgam
I don't think mercury can coalesce so easily from a suspension - the black precipitate made by addin ... |
6-7-2012 at 19:03
by: barley81 |
Aluminium amalgam
I think it's best that you dispose of the waste at a recycling center. The tiny amount of mercury in ... |
5-7-2012 at 08:06
by: barley81 |
Odd Result for Haloform Reaction
Are you absolutely sure that it is a solid? The suspension of chloroform produced by the reaction ca ... |
2-7-2012 at 12:02
by: barley81 |
I need more solvents - which ones to get next?
How about glyme and butanone (MEK)? |
1-7-2012 at 14:20
by: barley81 |
Destabilizing Silver Colloid
You could react a known amount of the silver suspension with nitric acid and titrate it against a kn ... |
1-7-2012 at 11:15
by: barley81 |
Pretty Pictures (1)
Simply add ammonia to a solution of a copper (II) salt. You can easily isolate its salts. Look in Br ... |
30-6-2012 at 08:08
by: barley81 |
Reduction of diethyl phenyl malonate with LAH
That's why you can use a large excess of LAH (though it might be somewhat wasteful). I think that th ... |
30-6-2012 at 07:49
by: barley81 |
Selective Amination of Benzoic Acid
You could reduce it to benzyl alcohol with some reducing agent (lithium aluminum hydride for example ... |
25-6-2012 at 16:01
by: barley81 |
Dissolving coconut oil
Maybe your wife could try the hot process instead of the cold process? It requires a lot less curing ... |
25-6-2012 at 05:39
by: barley81 |
Isopropanol for haloform reaction
Yes, first it will be oxidized by NaOCl to acetone, which can then undergo the haloform reaction. Yo ... |
24-6-2012 at 18:19
by: barley81 |
Reaction of NH4OH and MgSO4
Or, use cheap NaOH instead of ammonia. You will get higher yield based on both ammonia and magnesium ... |
24-6-2012 at 06:01
by: barley81 |
Oxalic acid and nitric acid
Plus, oxalic acid can be made by oxidizing sugar with nitric acid in the presence of vanadium pentox ... |
21-6-2012 at 08:16
by: barley81 |
Sulfuric acid from copper sulfate
In a 2M solution of copper sulfate, there are 2 moles of sulfate ions per liter. If only one mole of ... |
20-6-2012 at 17:35
by: barley81 |
Reduction of MEK
Aluminum would react with isopropyl alcohol directly if it weren't for that pesky oxide layer. Anyth ... |
4-6-2012 at 11:21
by: barley81 |
Colour Changes when NaOH added to CUCL2 and water
In an electrified tube filled with chlorine gas at low pressure, there are probably a few Cl<sup& ... |
4-6-2012 at 11:09
by: barley81 |
Reduction of MEK
MPV reduction using aluminum isopropoxide:
http://en.wikipedia.org/wiki/Meerwein%E2%80%93Ponndorf%E ... |
4-6-2012 at 10:59
by: barley81 |
Electrolysis with glassy carbon
2H2O + 2e- -> 2OH- + H2 E0 = -0.83V
Na+ + e- -> Na E0 = -2.71V
To reduce water in a ... |
4-6-2012 at 10:53
by: barley81 |
Making urea formaldehyde resin
Hmm... Methylamine HCl can be made by boiling hexamine and HCl. I don't expect the reaction of sulfu ... |
4-6-2012 at 10:49
by: barley81 |
Identifying Unknown Compounds in a Lab
Add NaOH and you should get rusty brown precipitate indicating iron III.
Since you have identifie ... |
4-6-2012 at 10:45
by: barley81 |
SnI4: A nice covalent compound of tin
Brauer's prep for SnI4 says that no water must be present. Since water is in conc. HNO3 and is produ ... |
3-6-2012 at 19:16
by: barley81 |
SnI4: A nice covalent compound of tin
Nitric acid and hydriodic acid doesn't sound like it'd be too stable. Nitric acid itself can oxidize ... |
3-6-2012 at 16:32
by: barley81 |
Ferric nitrate and sodium thiosulphate
Maybe permanganate titration would be a good way to determine Fe2+ content, but I don't think there ... |
2-6-2012 at 13:33
by: barley81 |
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