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sparkgap
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Quite nice! I hadn't realized that Mercurochrome's fluorescing color is different from its usual red. The green is quite different from that of plain
Jane fluorescein, I suppose.
If it's not much trouble, do you have similar pictures using other triphenylmethane/phthalein pigments?
sparky (~_~)
"What's UTFSE? I keep hearing about it, but I can't be arsed to search for the answer..."
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arkoma
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Pretty sure its Copper(I) Oxide Reference
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kristofvagyok
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Quote: Originally posted by sparkgap  |
If it's not much trouble, do you have similar pictures using other triphenylmethane/phthalein pigments?
sparky (~_~) |
Not really, we have circa 20kg phenolphthalein, but I never photographed it, maybe once(:
But here is a nice one:
I tried a trifluoromethyation with sodium trifluoroacetate in dimethylformamide on trinitrobenzene.
While heating the reaction mixture, the trifluoroacetate decomposed to give carbon dioxide, difluorocarbene and sodium fluoride. Since the sodium
fluoride is an enough strong base in DMF to remove a proton from the trinitrobenzene, this red/orange thing formed what indicates the trinitrophenyl
anion.
I have a blog where I post my pictures from my work: http://labphoto.tumblr.com/
-Pictures from chemistry, check it out(:
"You can’t become a chemist and expect to live forever." |
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Brain&Force
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Transit of Venus, 2012
<img src="http://i.imgur.com/lMNQGXQ.jpg" title="I wish I had a better camera." width=800>
At the end of the day, simulating atoms doesn't beat working with the real things...
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sasan
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how can I post my pix from my pc to here??
I have some flourscent solutions under UV light
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The Volatile Chemist
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Nice, B&F! What kind of set-up did you use to take it?
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Brain&Force
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A cell phone camera through some dude's refractor with a solar filter.
At the end of the day, simulating atoms doesn't beat working with the real things...
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kristofvagyok
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One of the most simple tests to show an organic compound present in a reaction mixture is irradiating the sample with UV light. If you know, that the
product of the reaction should fluorescence blue, while the starting materials do not emit any light after irradiating the sample with UV, could help
a lot while doing a reaction.
In this case a side product formed from the reaction above 130 °C, while the desired product formed at 100 °C. The starting material and the product
did not emit any light under UV, while the side product did. So after taking the picture, I was sure, that the reaction is ready.
For more pics, visit: http://labphoto.tumblr.com/
I have a blog where I post my pictures from my work: http://labphoto.tumblr.com/
-Pictures from chemistry, check it out(:
"You can’t become a chemist and expect to live forever." |
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Texium
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Just a nicely backlit picture some boiling copper sulfate solution, nothing too special, but I think it looks pretty cool.
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alexleyenda
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yuup nice picture, copper sulfate's color always amazed me
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Oscilllator
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Anyone want to hazard a guess what this is?
clue: It isn't an organic compund
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numos
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Just a wild guess, is it a copper sulfate, sodium dichloroisocyanurate complex? Otherwise no clue.
Although it's too light for that, I would like to make some,whatever it is, that color is... unseen.
U2U the name please? If you don't want to give it away here... 
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Amos
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Fun with Copper!
Copper oxychloride (Dicopper chloride trihydroxide), freshly precipitated from a copper (II) chloride solution.
A vial in which I was conducting Fehlig's test for reducing sugars. The top layer is partially hydrolyzed starch, the middle is Fehlig's solution, and
the bottom shows some hydrated copper (I) oxide precipitating, indicating glucose in the starch.
I don't find this as pretty as I do just neat, but these are some US nickels freshly plated in copper from a hot copper (II) acetate solution.
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Amos
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Oscillator, I recently precipitated an unknown copper(surprising, right?) compound that looked just like that by accident, waxy texture and
everything. I am very interested in finding out what it is. Upon long exposure to air at ambient temperature that same sample turned blue-green, and
returns to the violet color with heating.
[Edited on 6-10-2014 by No Tears Only Dreams Now]
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numos
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| Quote: Originally posted by No Tears Only Dreams Now | | Oscillator, I recently precipitated an unknown copper(surprising, right?) compound that looked just like that by accident, waxy texture and
everything. I am very interested in finding out what it is.[Edited on 6-10-2014 by No Tears Only Dreams Now] |
What did you precipitate it from? I collect copper salts, and I have never seen this...
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Amos
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I was going for precipitating cuprous oxide for my collection by reducing copper sulfate by the method in the second half of this video: http://www.youtube.com/watch?v=IIHZ_zFu9lA
Long story short, it requires citric acid; I was impatient and tried to use kool-aid powder (cheap american drink mix) 
It requires heating to complete the reaction; however, this curious precipitate formed almost immediately. And what is even more strange is that I can
light it with a lighter, and it will weakly smolder for a bit.
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Gooferking Science
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An interesting blob of MEKP prior to detonation
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Oscilllator
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Hmmm, people seem to be jumping to the conclusion that this is a copper compound. Understandable, but nonetheless incorrect.
Keep guessing!
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Tsjerk
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Anhydrous cobalt chloride?
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Amos
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| Quote: Originally posted by Oscilllator | Hmmm, people seem to be jumping to the conclusion that this is a copper compound. Understandable, but nonetheless incorrect.
Keep guessing! |
I think rather we are hoping it is, so that we can add it to our collections(which, apparently, I'm not the only person obsessed with copper
compounds). Can you tell us if it is wet or dry in the picture?
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DraconicAcid
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It looks the right colour for hexamminenickel(II) chloride.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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Texium
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Indeed, that would be quite helpful.
I don't really have any idea what it really is, but I would guess wet cobalt carbonate.
Edit: Or possibly cobalt phosphate.
[Edited on 6-10-2014 by zts16]
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Brain&Force
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Iodine spill! Did this for a bunch of curious biology students.
<a href="http://imgur.com/DU8fKVG"><img src="http://i.imgur.com/DU8fKVG.jpg" title="Mmm...swimming pool." width=800 /></a>
[Edited on 10.6.2014 by Brain&Force]
At the end of the day, simulating atoms doesn't beat working with the real things...
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The Volatile Chemist
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Cool image, BUT IT'S SIZE! I just can't get over it's size... 
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Brain&Force
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I had to keep turning the fume hood on and off in order to flush the fumes. I was attempting to get rid of some residual iodine coating on the vial.
I thought [Ni(NH3)6]Cl2 is pink. I tried making some today, but I never got past the blue tetraammine complex.
http://www.theodoregray.com/periodictable/Samples/NiCl2/inde...
[Edited on 10.6.2014 by Brain&Force]
At the end of the day, simulating atoms doesn't beat working with the real things...
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