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Author: Subject: Pretty Pictures (2)
The Volatile Chemist
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[*] posted on 19-11-2015 at 10:28


Quote: Originally posted by Pinkhippo11  
Copper phosphate finally dried out:

How'd you make it? Or do you own phosphoric acid...?




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[*] posted on 19-11-2015 at 15:25


Quote: Originally posted by Pinkhippo11  
Copper phosphate finally dried out:
Are you sure that's copper phosphate? I've never seen it make crystals like that... or at all really. I've made it a couple times and it's always precipitated as a fine, blue powder.



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[*] posted on 19-11-2015 at 16:34


I made it by reacting copper carbonate with phosphoric acid and drying it slowly in a desiccator over sodium hydroxide.



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[*] posted on 19-11-2015 at 17:54


Perhaps it is a soluble acid salt then, like CuHPO4
Analyzing the ratio of phosphate ions to copper ions in it would clarify it.




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[*] posted on 20-11-2015 at 13:42


Nonetheless, very pretty. And if you can stoichiometrically analyze it (titration with NaOH?) then you've got a fine compound to vial. As long as it's all the same salt, of course...



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[*] posted on 20-11-2015 at 20:29


18514d56-4c5d-44aa-9ffa-63c2721f1da4_zpsdewfdojl.jpg - 366kB

first reflux in my new space. pecan shells in acetone.




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[*] posted on 21-11-2015 at 06:15


Cool 'hotplate' ! Wish mine had two plates, though I've seen ones with more too.
By the way, pretty pictures (1) ended at 40 pages. This thread has 40 now. Is it time for another, or did new software fix the problems with having a 40pg. thread?




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[*] posted on 24-11-2015 at 06:23


Just trying out my 'new' reconditioned Edwards 2 stage vacuum pump





IMG_0907.JPG - 203kB

[Edited on 24-11-2015 by plastics]
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[*] posted on 28-11-2015 at 08:58


Wow, very nice. Is that just the readout, or the entire device?
Did you purchase it new, or did you 'acquire' it used?




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[*] posted on 1-12-2015 at 18:40


The first pic is the flat alum crystal
The second one is a perfectly octahedral alum crystal :P
And the third one is sodium bicarbonate (baking soda crystal)

The crystals are homemade. :))

738372_559768857395932_1320046660_o.jpg - 102kB1606207_643642112341939_2064944133_o.jpg - 143kB10682377_789568847749264_1265765932151861459_o.jpg - 296kB
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[*] posted on 2-12-2015 at 12:32


Nice. What's the second crystal inside of?



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[*] posted on 3-12-2015 at 05:21


It is potassium alum crystal. :)
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[*] posted on 4-12-2015 at 13:51


Quote: Originally posted by CrystalCage  
It is potassium alum crystal. :)

He asked what you were storing the crystal in the second picture in
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[*] posted on 6-12-2015 at 00:12


Oh, my apologies. The red one holding the crystal is the plastic base from graduated cylinder (my graduated cylinder broke :'( ) contained in a glass jar.

https://static.fishersci.com/images/FS106312~wl.jpg


[Edited on 6-12-2015 by CrystalCage]
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[*] posted on 10-12-2015 at 07:45


Phosphorescent alkaline earth sulfides activated with bismuth.
From left to right:
BaS / SrS / CaS

phosphorescent sulfides.jpg - 1.1MB
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[*] posted on 10-12-2015 at 13:09


Quote: Originally posted by CrystalCage  

The second one is a perfectly octahedral alum crystal :P

Nice one! But I should warn you that putting do-not-eat bags with crystal defeats the purpose of putting it into sealed container.

For sulfates, most common problem is not absorption of moisture from air, but dehydration.
Alum is very stable, but in extremely dry environment it could start loosing water and turn into white powder. For storing crystals, I would recommend do the opposite: put into the sealed jar a piece of tissue, wet with saturated solution of the compound. It would create just right humidity level. Used this method to preserve uncoated crystal of ferric alum - works great, crystal has not changed for months.
Quote: Originally posted by CrystalCage  

And the third one is sodium bicarbonate (baking soda crystal)

I have very strong suspicion that it sesquicarbonate (trona), not bicarbonate. Did you grew it from hot solution? Interesting result, by the way.

[Edited on 10-12-2015 by Dmishin]
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[*] posted on 11-12-2015 at 08:23


The alum crystal is kept for 2 years in that conditions. But anyway, I will do your method in preserving my copper acetate crystal, which is still growing. :)

I grew that star-shaped crystal in a hot solution... But that crystal is very fragile. It crushed when I picked it up.
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[*] posted on 19-12-2015 at 11:00


I love element 29. reduced Cu, CuSO4, and CuAc across top, and crystallizing CuCl2 on the glass. My lil Kodak doesn't focus well close up *sigh* as the chloride is bee-you-ti-ful

100_1369.JPG - 2.3MB




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[*] posted on 20-12-2015 at 13:56


Element 28 is calling to me right about now...

here's some nickel sulfamate I'm probably going to use for electroplating. I just need to find a nickel electrode.

<img src="http://i.imgur.com/JHxrO6B.jpg" width=800>




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[*] posted on 20-12-2015 at 14:04


For small scale nickel electrodes, http://www.ebay.co.uk/itm/30PCS-Pure-99-96-Low-Resistance-Ni...
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[*] posted on 20-12-2015 at 14:49


Quote: Originally posted by Sulaiman  
For small scale nickel electrodes, http://www.ebay.co.uk/itm/30PCS-Pure-99-96-Low-Resistance-Ni...
been waiting for 1 1/2 months for delivery of those nickel strips.have to wait until jan, 01 2016 before i ask for money back.
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[*] posted on 21-12-2015 at 04:58


Quote: Originally posted by stibium  
Phosphorescent alkaline earth sulfides activated with bismuth.
From left to right:
BaS / SrS / CaS

@Stibium,
Magnificent!
How did you do/make those? Via United State Patent n°US2544507A or else?
How is that phosphorescence activated, sunlight, UV light/laser and how long exposure?
How long does the phosphorescence lasts?




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[*] posted on 22-12-2015 at 21:47


This evening I made some 3-nitrophthalic acid for future production of luminol. I noticed that one of the soluble byproducts of the nitration exhibits yellow-green fluorescence. I got a good picture of it:

Fluorescence.jpg - 559kB
My tablet's camera makes the fluorescence appear more yellow than it does in person, it's actually quite green. By any chance, does anyone know what the cause of it is?




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[*] posted on 23-12-2015 at 14:09


Quote: Originally posted by zts16  
This evening I made some 3-nitrophthalic acid for future production of luminol. I noticed that one of the soluble byproducts of the nitration exhibits yellow-green fluorescence. I got a good picture of it:


My tablet's camera makes the fluorescence appear more yellow than it does in person, it's actually quite green. By any chance, does anyone know what the cause of it is?

Could it be m-nitrophtalic acid or m-nitrophtalate anion?




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[*] posted on 23-12-2015 at 17:20


There's definitely a substantial amount of 4-nitrophthalic acid in that solution, but I don't know if that's what is causing the fluorescence. I haven't been able to find much out there about its properties. It might also be a trace amount of a dinitrophthalic acid, as I did unfortunately allow the temperature to rise too high for about half a minute during the nitration.



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