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Vanadium Colloid
Surprisingly enough, the sulfuric acid started dissolving the colloid (with hydrogen bubble evolutio ... |
10-11-2012 at 13:34
by: Mixell |
Vanadium Colloid
Well, not exactly.
At first I rinsed the alloy in nitric acid, which turned it into a powder (which ... |
10-11-2012 at 11:26
by: Mixell |
Vanadium Colloid
I've isolated some vanadium from an aluminium-vanadium alloy (15%-85% by mass).
Now I have a pretty ... |
10-11-2012 at 10:41
by: Mixell |
The short questions thread (3)
Some guy on this forum has created pyrophoric copper from decomposition of copper acetate, so I thin ... |
12-7-2012 at 02:47
by: Mixell |
Test for osmium tetroxide?
OsO4 is highly poisonous, even at low exposure levels, and must be handled with appropriate precauti ... |
11-7-2012 at 06:27
by: Mixell |
Test for osmium tetroxide?
I think that if he has an access to a lab, then testing the OsO4 melting point will not be as lethal ... |
11-7-2012 at 04:19
by: Mixell |
Test for osmium tetroxide?
Check the melting point, it should be around 40C. |
10-7-2012 at 09:54
by: Mixell |
Ebay supplier - legit or not?
Well, it might be soluble in acetone/hexane/chloroform.
I just bought it because it wasn't expensiv ... |
18-6-2012 at 13:55
by: Mixell |
Ebay supplier - legit or not?
What guy from Lithuania? |
15-6-2012 at 13:28
by: Mixell |
Good price on Chems
http://www.cs-chemicals.co.il/heb/index.php
The website is in Hebrew, good luck with that. |
12-6-2012 at 11:48
by: Mixell |
Ebay supplier - legit or not?
Just bought the following chemicals from him:
20g of:
TELLURIUM POWDER - Purity 99.99%
SELENI ... |
11-6-2012 at 12:22
by: Mixell |
Good price on Chems
It's a local company, I highly doubt that they will sell to international clients. |
11-6-2012 at 08:42
by: Mixell |
Good price on Chems
Heh, I bought a liter of 97% sulfuric acid and a liter of 70% nitric acid for about 8$ each.
Everyt ... |
10-6-2012 at 18:18
by: Mixell |
Identifying Unknown Compounds in a Lab
If it did form a precipitate with AgNO3, then you can try to do some titrations (with appropriate in ... |
7-6-2012 at 18:09
by: Mixell |
Identifying Unknown Compounds in a Lab
Add the solid to H2SO4, it should fizz and bubble vigorously, you will not be able to miss it!
If t ... |
7-6-2012 at 15:34
by: Mixell |
Identifying Unknown Compounds in a Lab
C:
Probably Sn II chloride, as the teacher said it has chloride (or iodide) ions in it, and it's a ... |
7-6-2012 at 13:58
by: Mixell |
Identifying Unknown Compounds in a Lab
A:
If A is basic, then it's probably the salt of sodium and a weak acid, but a one that does not fo ... |
6-6-2012 at 08:23
by: Mixell |
Identifying Unknown Compounds in a Lab
C:
A good chance it is Tin II chloride, please check with the procedure I described.
B:
Might b ... |
5-6-2012 at 19:20
by: Mixell |
Identifying Unknown Compounds in a Lab
Remember: always add the chemicals gradually with mixing.
I'll start from C:
Strontium and calci ... |
4-6-2012 at 13:33
by: Mixell |
Identifying Unknown Compounds in a Lab
Fe II solution should be neutral, Fe III should be acidic:
Fe3+ +H2O --> Fe(OH)2+ + H+
Use the ... |
4-6-2012 at 12:55
by: Mixell |
Identifying Unknown Compounds in a Lab
So I think we made a conclusion =)
Next compound? |
4-6-2012 at 11:16
by: Mixell |
Identifying Unknown Compounds in a Lab
Nah, mixing with K2SO4 or H2SO4 will do nothing if its Fe III sulfate.
Just check the pH of the sol ... |
4-6-2012 at 10:14
by: Mixell |
Identifying Unknown Compounds in a Lab
Well here you go, yellow directly on dissolution, yellowish as a solid.
Just check the pH, and may ... |
2-6-2012 at 11:46
by: Mixell |
Identifying Unknown Compounds in a Lab
I think hours is the more accurate time frame.
And I don't think he messed with the solution for ho ... |
2-6-2012 at 05:07
by: Mixell |
Identifying Unknown Compounds in a Lab
Define "fairy rapidly" please, because I've dissolved ferrous sulfate, and it didn't develop any not ... |
2-6-2012 at 01:30
by: Mixell |
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