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Author: Subject: The Short Questions Thread (4)
Volanschemia
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[*] posted on 26-3-2015 at 14:54


The pool treatment tablets are either Calcium Hypochlorite or Trichloroisocyanuric Acid, and I think most are the latter.

I seem to recall reading somewhere about this. I think the reaction of the acid and the Hydrogen Peroxide evolves Singlet Oxygen, which is the electronically excited state of O2. When it comes down off it's high, so to speak, it emits red light.

It's a pretty interesting reaction which I will have to try out one day.




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[*] posted on 26-3-2015 at 16:04


Quote: Originally posted by Argentum  
Something I've seen but can't find anywhere

When mixing H2O2 with pool water treatement pills it gave a red chemiluminiscence, am I right?

If I am, what is the reagent in the pills? (I think trichloroisocianuric acid, but can't remember)


Almost certainly TCCA or NaDCCA. The red glow is given off by singlet oxygen formed from the decomposition of a peroxyhypochlorous acid species produced in the reaction.

If the effect was quite strong and not much foam was produced, it is most likely NaDCCA. TCCA produces the same effect, but with more foaming (from my experience) and a weaker glow.

Edit: I forgot that calcium hypochlorite produces this effect too. However, I think the effect is short-lived as compared to that from the other two chemicals.

[Edited on 27-3-2015 by blargish]




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The Volatile Chemist
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[*] posted on 27-3-2015 at 08:23


I'm pretty sure W. Oelen has some stuff on his site about it, maybe in the physics section.



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[*] posted on 5-4-2015 at 18:02


Please explain how to convert a sulfate into a hydrochloride?
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[*] posted on 6-4-2015 at 03:25


@Badboy39560 - It might help to be more specific. Different oxidations states of metals can make this more or less a different operation.



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The Volatile Chemist
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[*] posted on 10-4-2015 at 16:00


For a general answer, add a hypochlorite salt to a solution of sulfate, but there are so many exceptions, that that generalization isn't useful. What's the salt?



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[*] posted on 10-4-2015 at 16:16


Quote: Originally posted by The Volatile Chemist  
For a general answer, add a hypochlorite salt to a solution of sulfate, but there are so many exceptions, that that generalization isn't useful. What's the salt?


He said "hydrochloride", not "hypochlorite". Methinks it is the hydrochloride of some alkaloid he's trying to make.

Deprotonate it with some base, extract the neutral alkaloid into some organic solvent, then add hydrochloric acid.




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The Volatile Chemist
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[*] posted on 10-4-2015 at 17:26


No, no, see, you're suppose to give them two 'possible routes, one being the legitimate route, and one obviously not (i.e. heat with dilute bromine-water) :)



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[*] posted on 26-4-2015 at 19:54


Is camphor readily soluble in xylenes? I searched, but wasn't able to find anything on the subject. Due to its high solubility in most common organic solvents, it seems like it would be, I'd just like to know for certain. Thanks.



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[*] posted on 27-4-2015 at 05:10


According to an old 1905 book, <i>Transactions of the Wisconsin Academy of Sciences, Arts, and Letters, Volume 15, Part 1</i> (from Google Books), "camphor is very soluble in toluene," so I assume it would be in xylenes.





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[*] posted on 30-4-2015 at 15:39
from 36-37 question, you are correct


Quote: Originally posted by The Volatile Chemist  
Quote: Originally posted by quantumcorespacealchemyst  
What is the white frost on glass from being near HCl(aq)? It is wipable, smells odd and forms even near sealed acid containers. It seems to certainly be from HCl gas. What it is, I don't know.

[Edited on 22-2-2015 by quantumcorespacealchemyst]

I get it all the time on things in my lab when evaporating HCl solutions. I think it's condensed HCl, or a salt of Cl-, that is, if you have ammonia vapors nearby or something.


yes, you are correct.
i could not understand how it happened, not thinking about the blue solution of ammonia and copper salts i had been saving sealed in a yogurt container with saran wrap under the lid . i just checked it and most of the water is evaporated.

:P
thanks
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[*] posted on 1-5-2015 at 07:23


what salt from human urine is insoluble in water and pure etanol?
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[*] posted on 7-5-2015 at 09:29


Quote: Originally posted by pneumatician  
what salt from human urine is insoluble in water and pure etanol?

None normally, hence the reason why urine, which is water based, is transparent.




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[*] posted on 7-5-2015 at 10:57
ATX power supply question


Can I use the +12V and +3.3V outputs on an ATX power supply to make an 8.7V output? Current would flow out of the 12V output and into the 3.3V output. (I have a Peltier cooler that I want to run that only accepts 8.3 to 8.8 volts, and draws 4 amps.) I don't want to ruin my ATX power supply by experimentation.

Edit: More research says that my power supply should be able to handle it.

Edit 2: Testing shows that the power supply just shuts off when I try to do it (probably some protection mechanism).

Edit 3: Even more research says that it is only possible if the 3.3V output is driving something that uses more than 4 amps. (The 3.3V output cannot sink current, only source it.) However, running the Peltier cooler off 5 volts works well enough for my purposes, I've found out.

[Edited on 7-5-2015 by Cheddite Cheese]
[Edited on 7-5-2015 by Cheddite Cheese]

[Edited on 8-5-2015 by Cheddite Cheese]




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[*] posted on 9-5-2015 at 17:04


Quote: Originally posted by gdflp  
Quote: Originally posted by pneumatician  
what salt from human urine is insoluble in water and pure etanol?

None normally, hence the reason why urine, which is water based, is transparent.


so now I have one and one problem! :o
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[*] posted on 9-5-2015 at 17:08


Quote: Originally posted by Cheddite Cheese  
Can I use the +12V and +3.3V outputs on an ATX power supply to make an 8.7V output?


the fast, best and cheap is to buy a voltage reductor, this come in a integrated circuit like a transistor with 3 pins. perhaps not of 8,7v but 9v... but in reality electronics have a wide range of tolerance!!! :cool:
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[*] posted on 11-5-2015 at 22:34


question

is there any feasible way I can convert dichloroisocyanuric acid to sodium dichloroisocyanurate?


thanks:)
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[*] posted on 11-5-2015 at 23:13


Before I had any idea what I was doing, I managed to make a very small amount of potassium dichlorocyanurate from TCCA and KOH. I got some of the characteristic purple copper complex I was aiming for but extremely small amounts. It turns out this family of chemicals is a bit weird and there are multiple side reactions and alternate reactions. The dichloro milecule was merely an intermediate on the way to something else.
So, I guess it would be possible but might be tricky. woelen explained it rather well when I asked a similar question. He did some extensive work on these chemicals about 6-8 years ago. Good info is on the board but you will have to search. You might start by searching on me (oct last year) and see where that takes you.
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Ramium
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[*] posted on 12-5-2015 at 00:05


thanks. it sounds tricky so i'll probably just buy the sodium dichloroisocyanurate
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[*] posted on 16-5-2015 at 22:55


europium(III) 6,6,7,7,8,8,8-heptafluoro-2,2-methyl-3,5-octanedionate‏

Is this the correct systematic name for EuFOD?

Eufod.png - 13kB




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[*] posted on 17-5-2015 at 04:01


Brain&Force - I don't think so. Ligands have special naming conventions and that doesn't appear to follow them (to me). I never cared much for hugely esoteric molecules and the names of them though. Anyways, if you wanna get inundated, http://en.wikipedia.org/wiki/IUPAC_nomenclature_of_inorganic...



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[*] posted on 19-5-2015 at 11:16



I reacted 2g of sulphur and 1g of aluminium - thermite reaction - and got 1.9g of slag/product. I'm wondering what happened to the 1.1g that's missing. Maybe part of the sulphur is vaporizing instead of reacting with the aluminium?
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[*] posted on 19-5-2015 at 11:58


Some is vaporizing. Some may be combining with oxygen. Suggestion: Figure out the stoichiometry of the reaction. Likely aluminum is the limiting factor. Find out how many moles you started with, and how many moles of Al2S3 you would expect at 100% yield.

I would guess that any unreacted sulfur did volatilize and the slag is alumina.
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[*] posted on 19-5-2015 at 12:33


Thanks Digga!

I was assuming 2Al + 3S → Al2S3
roughly 2x27 + 3x32 ~ 54/96

so I used 1/3 Al 2/3 S - that's where the 1g/2g mix came from. Now I was thinking that if part of the S vaporizes, maybe I should use an excess of it?
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[*] posted on 19-5-2015 at 12:46


Quote: Originally posted by learningChem  

Now I was thinking that if part of the S vaporizes, maybe I should use an excess of it?


That doesn't happen, in my experience. Stoichiometric ratio is good.





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