Sciencemadness Discussion Board
Not logged in [Login - Register]
Go To Bottom

Printable Version  
 Pages:  1  ..  11    13    15  ..  65
Author: Subject: Pretty Pictures (2)
sparkgap
International Hazard
*****




Posts: 1225
Registered: 16-1-2005
Location: not where you think
Member Is Offline

Mood: equilibrated

[*] posted on 6-6-2014 at 02:19


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..."
View user's profile View All Posts By User
arkoma
Forum Redneck
*****




Posts: 1074
Registered: 3-2-2014
Location: Ar-Kin-Saw
Member Is Offline

Mood: Amazed

[*] posted on 6-6-2014 at 07:05




Pretty sure its Copper(I) Oxide Reference




Self aware bag of organic slime..............

Collector of reagents.
View user's profile View All Posts By User
kristofvagyok
International Hazard
*****




Posts: 659
Registered: 6-4-2012
Location: Europe
Member Is Offline

Mood: No Mood

[*] posted on 6-6-2014 at 07:28


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."
View user's profile Visit user's homepage View All Posts By User
Brain&Force
Hazard to Lanthanides
*****




Posts: 1295
Registered: 13-11-2013
Location: UW-Madison
Member Is Offline


[*] posted on 6-6-2014 at 15:20


Transit of Venus, 2012

<img src="http://i.imgur.com/lMNQGXQ.jpg" title="I wish I had a better camera." width=800>




Raney nickel can't hydrogenate dank memes.
View user's profile View All Posts By User
sasan
Hazard to Self
**




Posts: 92
Registered: 22-2-2014
Location: TEHRAN / IRAN
Member Is Offline

Mood: Radiative

[*] posted on 7-6-2014 at 06:13



how can I post my pix from my pc to here??
I have some flourscent solutions under UV light
View user's profile View All Posts By User
The Volatile Chemist
International Hazard
*****




Posts: 1973
Registered: 22-3-2014
Location: 'Stil' in the lab...
Member Is Offline

Mood: Copious

[*] posted on 7-6-2014 at 09:47


Nice, B&F! What kind of set-up did you use to take it?



View user's profile Visit user's homepage View All Posts By User
Brain&Force
Hazard to Lanthanides
*****




Posts: 1295
Registered: 13-11-2013
Location: UW-Madison
Member Is Offline


[*] posted on 7-6-2014 at 11:58


A cell phone camera through some dude's refractor with a solar filter.



Raney nickel can't hydrogenate dank memes.
View user's profile View All Posts By User
kristofvagyok
International Hazard
*****




Posts: 659
Registered: 6-4-2012
Location: Europe
Member Is Offline

Mood: No Mood

[*] posted on 7-6-2014 at 13:34




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."
View user's profile Visit user's homepage View All Posts By User
Texium (zts16)
Administrator
********




Posts: 3011
Registered: 11-1-2014
Location: San Marcos, TX
Member Is Offline

Mood: Graduated

[*] posted on 9-6-2014 at 13:33


Just a nicely backlit picture some boiling copper sulfate solution, nothing too special, but I think it looks pretty cool.
IMG_1262.jpg - 1.3MB
View user's profile Visit user's homepage View All Posts By User
alexleyenda
National Hazard
****




Posts: 277
Registered: 17-12-2013
Location: Québec, Canada
Member Is Offline

Mood: Busy studying chemistry at the University

[*] posted on 9-6-2014 at 15:15


Quote: Originally posted by zts16  
I think it looks pretty cool.
yuup nice picture, copper sulfate's color always amazed me
View user's profile View All Posts By User
Oscilllator
International Hazard
*****




Posts: 659
Registered: 8-10-2012
Location: The aqueous layer
Member Is Offline

Mood: No Mood

[*] posted on 9-6-2014 at 17:29


Anyone want to hazard a guess what this is?

clue: It isn't an organic compund




View user's profile View All Posts By User
numos
Hazard to Others
***




Posts: 213
Registered: 22-2-2014
Member Is Offline

Mood: No Mood

[*] posted on 9-6-2014 at 17:48


Quote: Originally posted by Oscilllator  
Anyone want to hazard a guess what this is?
clue: It isn't an organic compund


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... :)




"The wisest man is the man who knows he knows nothing"
View user's profile View All Posts By User
Amos
International Hazard
*****




Posts: 1189
Registered: 25-3-2014
Location: Yes
Member Is Offline

Mood: No

[*] posted on 9-6-2014 at 17:48
Fun with Copper!




IMG_0487.JPG - 2.1MB

Copper oxychloride (Dicopper chloride trihydroxide), freshly precipitated from a copper (II) chloride solution.

IMG_0486.JPG - 3.4MB

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.

IMG_0494.JPG - 3.3MB

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.
View user's profile View All Posts By User
Amos
International Hazard
*****




Posts: 1189
Registered: 25-3-2014
Location: Yes
Member Is Offline

Mood: No

[*] posted on 9-6-2014 at 17:50


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]
View user's profile View All Posts By User
numos
Hazard to Others
***




Posts: 213
Registered: 22-2-2014
Member Is Offline

Mood: No Mood

[*] posted on 9-6-2014 at 17:57


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...




"The wisest man is the man who knows he knows nothing"
View user's profile View All Posts By User
Amos
International Hazard
*****




Posts: 1189
Registered: 25-3-2014
Location: Yes
Member Is Offline

Mood: No

[*] posted on 9-6-2014 at 18:06


Quote: Originally posted by numos  


What did you precipitate it from? I collect copper salts, and I have never seen this...


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) :D

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.
View user's profile View All Posts By User
Gooferking Science
Hazard to Self
**




Posts: 97
Registered: 17-7-2013
Location: Somewhere in Kansas, USA...
Member Is Offline

Mood: Halogenated

[*] posted on 9-6-2014 at 19:01


An interesting blob of MEKP prior to detonation

IMG_3980.JPG - 696kB




Check out my YouTube channel! www.youtube.com/user/gooferking
View user's profile Visit user's homepage View All Posts By User
Oscilllator
International Hazard
*****




Posts: 659
Registered: 8-10-2012
Location: The aqueous layer
Member Is Offline

Mood: No Mood

[*] posted on 9-6-2014 at 23:00


Hmmm, people seem to be jumping to the conclusion that this is a copper compound. Understandable, but nonetheless incorrect.
Keep guessing!




View user's profile View All Posts By User
Tsjerk
International Hazard
*****




Posts: 1648
Registered: 20-4-2005
Location: Netherlands
Member Is Offline

Mood: Mood

[*] posted on 10-6-2014 at 03:32


Anhydrous cobalt chloride?
View user's profile View All Posts By User
Amos
International Hazard
*****




Posts: 1189
Registered: 25-3-2014
Location: Yes
Member Is Offline

Mood: No

[*] posted on 10-6-2014 at 05:47


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?
View user's profile View All Posts By User
DraconicAcid
International Hazard
*****




Posts: 3031
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline

Mood: Semi-victorious.

[*] posted on 10-6-2014 at 08:04


Quote: Originally posted by Oscilllator  
Anyone want to hazard a guess what this is?
clue: It isn't an organic compund


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.
View user's profile View All Posts By User
Texium (zts16)
Administrator
********




Posts: 3011
Registered: 11-1-2014
Location: San Marcos, TX
Member Is Offline

Mood: Graduated

[*] posted on 10-6-2014 at 10:16


Quote: Originally posted by No Tears Only Dreams Now  
Can you tell us if it is wet or dry in the picture?

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]
View user's profile Visit user's homepage View All Posts By User
Brain&Force
Hazard to Lanthanides
*****




Posts: 1295
Registered: 13-11-2013
Location: UW-Madison
Member Is Offline


[*] posted on 10-6-2014 at 14:01


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]




Raney nickel can't hydrogenate dank memes.
View user's profile View All Posts By User
The Volatile Chemist
International Hazard
*****




Posts: 1973
Registered: 22-3-2014
Location: 'Stil' in the lab...
Member Is Offline

Mood: Copious

[*] posted on 10-6-2014 at 14:06


Cool image, BUT IT'S SIZE! I just can't get over it's size... :P



View user's profile Visit user's homepage View All Posts By User
Brain&Force
Hazard to Lanthanides
*****




Posts: 1295
Registered: 13-11-2013
Location: UW-Madison
Member Is Offline


[*] posted on 10-6-2014 at 14:33


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.

Quote: Originally posted by DraconicAcid  
Quote: Originally posted by Oscilllator  
Anyone want to hazard a guess what this is?
clue: It isn't an organic compund


It looks the right colour for hexamminenickel(II) chloride.


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]




Raney nickel can't hydrogenate dank memes.
View user's profile View All Posts By User
 Pages:  1  ..  11    13    15  ..  65

  Go To Top