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kjpmi
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[*] posted on 24-1-2015 at 17:17


Quote: Originally posted by Firmware21  

These beauties crystallized out from a "homemade" FeCl3 etchant solution. Since I didn't want to use H2O2 to oxidize it (I like my solutions concentrated), FeCl2 was still present, even after 7 month of "oxidation".







Those crystals look so cool. I love that green color.
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[*] posted on 25-1-2015 at 11:10


Well, they already started to convert to FeCl3. Now they look a bit darker.
Too bad I can't keep them like this forever :(
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[*] posted on 30-1-2015 at 10:04


Quote: Originally posted by Firmware21  
Well, they already started to convert to FeCl3. Now they look a bit darker.
Too bad I can't keep them like this forever :(


I guess you could keep them in a container flushed with nitrogen or carbon dioxide to prevent aerial oxidation. That would keep the nice green colour




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[*] posted on 2-2-2015 at 18:34




Bismuthate, the iodine crystal was created by melting the iodine under sulfuric acid. The bismuth nitrate and potassium thiocyanate formed this odd yellow solution with a white precipitate when mixed;





[Edited on 2-3-2015 by Pinkhippo11]




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[*] posted on 2-2-2015 at 18:37


Wow! That is stunning!
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[*] posted on 2-2-2015 at 18:39


What are those crystals?



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[*] posted on 2-2-2015 at 18:41


Potassium permanganate! Cooled over eight hours.



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[*] posted on 2-2-2015 at 20:26


Calcium acetate: I made some attempts to prepare Aluminium acetate for making water proof cloth. When I was doing so, I had left some calcium acetate solution in a beaker (prepared by mixing calcium hydroxide and concentrated acetic acid) for later use. But, I completely forgot about it. After a couple of weeks, wow! calcium acetate crystallized out beautifully and you can see that in the pic :)


Ammonium tetraborate: I've crystallized this compound for my video posted a couple of days back in youtube:)

Calcium acetate1.jpg - 383kB IMG_0926.JPG - 2.5MB
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[*] posted on 2-2-2015 at 20:48


Thats amazing, and not only for the beauty, it looks like you have the cleanest lab around to grow that accidentally without dust contamination or whatnot.
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quantumcorespacealchemyst
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[*] posted on 2-2-2015 at 22:54


Quote: Originally posted by Brain&Force  
Man, I really wish I could get a GoPro - I want to shoot videos, and that would be convenient!

Do the below compounds contain vanadium?

[Edited on 12.1.2015 by Brain&Force]


I am thinking Google glass may be perfect for filming reactions while keeping the operator uninhibited.

And

Realgar: Paloma Mine, Castrovirreyna Province, Huancavelica Department, Peru

Size: 3.4 x 3.3 x 2.8 cm (miniature)

Weight: 55grams

Realgar on galena/with galena and orpiment coating

p9n.jpg - 252kB rnhw.jpg - 236kB tkoe.jpg - 223kB jm8r.jpg - 215kB xaoi.jpg - 210kB 2bmj.jpg - 247kB v36i.jpg - 271kB

http://stores.ebay.com/jlminerals/

[Edited on 3-2-2015 by quantumcorespacealchemyst]
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[*] posted on 2-2-2015 at 23:26


[rquote]
The bismuth nitrate and potassium thiocyanate formed this odd yellow solution with a white precipitate when mixed;
[/rquote]

How does it turn red? Is it mixed longer and/or heated?

Also, Pinkhippo11, how did you cool the KMnO4 over 8 hours? Was it in a kiln type of environment?

Also, has anyone read/seen about the salts made from BiI3 and halide salts? Bismuth(III) iodide forms iodobismuth(III) anions when heated with halide donors:[10]
2 NaI + BiI3 → Na2[BiI5]
http://en.wikipedia.org/wiki/Bismuth(III)_iodide
(10. ^ Norman, Nicholas C. (1998), Chemistry of Arsenic, Antimony and Bismuth, Springer, pp. 168–70, ISBN 0-7514-0389-X, retrieved 2008-06-19)
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[*] posted on 3-2-2015 at 14:33


Put it in a tub of boiling water, let it sit, covered, and wrapped in towels. That's what I'd do....



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[*] posted on 4-2-2015 at 13:49


Dissolved some natural Arsenic ore in Aqua Regia.

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[*] posted on 4-2-2015 at 15:46


Great pic! What form of ore, and from where?



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[*] posted on 4-2-2015 at 16:13


That is awesome
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[*] posted on 4-2-2015 at 17:11


I found this after drinking the coffee that was in my window at least a few days. It was freezing and thawing and was partly thawed when I took it out to drink. I think I did the best I could to get the crystals pictures and it still doesn't look the way I see it. The camera only is 1 MP.

picture466.jpg - 163kB picture478.jpg - 197kB picture499.jpg - 158kB picture503.jpg - 187kB picture507.jpg - 237kB

also there are these
it looks different in front of the computer compared to a light bulb. it is not a pure compound but has insoluble brown powder in it
More here> http://www.sciencemadness.org/talk/viewthread.php?tid=61446#...

[Edited on 5-2-2015 by quantumcorespacealchemyst]

picture407.jpg - 194kB picture419.jpg - 183kB picture411.jpg - 172kB

[Edited on 5-2-2015 by quantumcorespacealchemyst]

[Edited on 5-2-2015 by quantumcorespacealchemyst]
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[*] posted on 4-2-2015 at 17:46


Liquid Chlorine

011.JPG - 2.4MB
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[*] posted on 5-2-2015 at 03:11


@The Volatile Chemist :

Not really sure. A friend sent it with some other chemicals. I didn't really know what to do with it so I thought since
I only have Sodium Arsenite and Sodium Biarsenate at home some more Arsenic Compounds would be good for the
collection. Actually tried to make Arsenic Acid from it but it somehow didn't turn out that well.

I though of dissolving it in Aqua Regia to gain like a crude form of Arsenic acid, than neutralizing it and hopefully precipitating it with Barium ( I think Barium Arsenate should be quite insoluble ). Filtering that of and mixing it again
with Sulfuric Acid to get insoluble Bariumsulfate and a clear Phase of Arsenic Acid. But while the reaction above white crystals fell out. I washed them but I'm not really sure what they are.

I've read that if you prepare Arsenic acid from the Oxide you will get crystalls of the Acid Hydrate so since the products for the Metal + acid and the oxide + acid are pretty much the same the crystalls could indeed be Arsenic Acid. But I can't find much in literature.

I've made a second attempt now with just Nitric Acid and we'll see whether there are crystalls, too or not.


The Ore is pretty clean, some dark grey stones with shining parts in it. At some points there are like yellow impurities but I've sorted them out. It should be somewhere from Germany (but I can ask for that).


EDIT:

Some Arsenic in conc. Nitric acid at room temperature and on the right close to it's boiling point. On the right is a indicator paper. That happens if you hold a dry indicator paper into Nitrous Gases. It get's pink and then white. Saw that at the university where I found dozens of pink strips after people worked with Aqua Regia. So I tested that out some time ago and found that they get that weird color when treated with Nitrous Gases. I guess the dye is destroyed in the reaction thus forming a color that is usually not found on the universal indicator.

Reaction.jpg - 77kB

[Edited on 5-2-2015 by fluorescence]
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[*] posted on 6-2-2015 at 09:13


Nice job! I like the fume pictures.
The liquid chloride is impressive.




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[*] posted on 6-2-2015 at 12:22


Yea.

what do you think about putting a calculated amount of liquid chlorine in a super cold bomb flask?

(accounting for PTFE expansion/contraction, wiggling/turning/loosening on warming) I saw a corning glass article on the practice of acclimating PTFE joints to/from cold.

[Edited on 6-2-2015 by quantumcorespacealchemyst]

[Edited on 6-2-2015 by quantumcorespacealchemyst]

I guess not much would be containable due to gas pressure; nonetheless, it seems like a good, highly controllable source of Cl2 gas.

[Edited on 7-2-2015 by quantumcorespacealchemyst]
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[*] posted on 7-2-2015 at 17:35
Silver Tree


I'm not sure if pictures of this have been posted before but here's some I took of my Silver Tree.
The first one is when the crystals are still big enough to reflect light and in the second one the crystals are smaller and absorb light more, giving it a grey colour. Reminds me of a big storm cloud or something!

Silver Tree 1.jpg - 210kB Silver Tree 2.jpg - 274kB

[Edited on 8-2-2015 by TheAustralianScientist]




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[*] posted on 9-2-2015 at 04:43


That's really cool
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[*] posted on 9-2-2015 at 08:34


Nice TheAustralianScientist, looks to me like the ash and dust in a nuclear mushroom cloud! When I do the silver tree I use a less concentrated solution of silver nitrate (about 0.1 molar) and it makes larger crystals which reflect more light.
How'd you condense the chlorine Hawkguy? I've used dry ice in acetone with some success for that in the past. Don't use styrofoam Hehe.


[Edited on 9-2-2015 by Molecular Manipulations]




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[*] posted on 10-2-2015 at 18:00


Quote: Originally posted by Molecular Manipulations  
Nice TheAustralianScientist, looks to me like the ash and dust in a nuclear mushroom cloud! When I do the silver tree I use a less concentrated solution of silver nitrate (about 0.1 molar) and it makes larger crystals which reflect more light.
How'd you condense the chlorine Hawkguy? I've used dry ice in acetone with some success for that in the past. Don't use styrofoam Hehe.


[Edited on 9-2-2015 by Molecular Manipulations]


Thanks! I thought it looked really nice. I used 1.6g of Silver(I) Nitrate in 50mL of distilled water which equals a 0.19M solution. I might try it again with a more dilute solution. I got a really good recovery of silver crystals, 0.995g, which I was really pleased with.




"The chemists are a strange class of mortals, impelled by an almost insane impulse to seek their pleasures amid smoke and vapor, soot and flame, poisons and poverty; yet among all these evils I seem to live so sweetly that may I die if I were to change places with the Persian king" - Johann Joachim Becher, 1635 to 1682.
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[*] posted on 10-2-2015 at 19:41


Quote: Originally posted by quantumcorespacealchemyst  
Yea.

what do you think about putting a calculated amount of liquid chlorine in a super cold bomb flask?

(accounting for PTFE expansion/contraction, wiggling/turning/loosening on warming) I saw a corning glass article on the practice of acclimating PTFE joints to/from cold.

[Edited on 6-2-2015 by quantumcorespacealchemyst]

[Edited on 6-2-2015 by quantumcorespacealchemyst]

I guess not much would be containable due to gas pressure; nonetheless, it seems like a good, highly controllable source of Cl2 gas.

[Edited on 7-2-2015 by quantumcorespacealchemyst]



I don't wanna store the stuff though, because of escapes, and Chlorinated Organics are often carcinogenic, apparently...
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