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Author: Subject: Does evaporation release ions into the air?
artemov
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[*] posted on 6-2-2021 at 20:04
Does evaporation release ions into the air?


Does slow evaporation, or even assisted evaporation (sun, low heat source, hot water bath, but NOT boiling), releases ions into the air?

I frequently slow evaporate (warm sunny room) to dry/crystallize salts like nickel and hexavalent chromium. Am I poisoning myself slowly?

According to nilered (11:15 mins) during the evaporation of acetone from his denatonium benzoate solution, he can taste the bitterness.
https://www.youtube.com/watch?v=GOw_I42eUpM
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Sulaiman
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[*] posted on 6-2-2021 at 21:05


I think that'
technically speaking, some dissolved salts will be carried by evaporating solvents,
partly by weak bonding/mechanical means,
and partly because all salts have some vapour pressure,

but it is negligible for non-boiling situations so I doubt that you are poisoning anyone.




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Fyndium
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[*] posted on 7-2-2021 at 02:17


When bubbles are formed, aerosol is created which carries some ions with it. I've witnessed this multiple times, at most simple way by noticing a smell of impurities in a distillate.

Slow evaporation without bubbling will generally emit extremely little ions. This is how ultra-pure reagents are distilled, anyway.
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[*] posted on 7-2-2021 at 03:58


I love these kinds of questions :)
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vano
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[*] posted on 10-2-2021 at 11:02


For example when i add sodium carbonate in selenous acid solution and when dioxide is generated it has smell. The smell is not pungent, though unpleasant. I can not describe the smell accurately but it feels different when you inhale. Maybe ions are to blame and therefore do not look like any other smell and that is what causes such a feeling



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Fyndium
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[*] posted on 10-2-2021 at 11:25


Effervescence indeed carries over ions, as it's not gas that comes over, but aerosol particles, which can carry over anything that a liquid can, as far as I'd believe. Make lead acetate from lead carbonate, inhale lead, or boil it down, inhale lead. Doing it in closed setup or still or evaporating it is the safe method.

They make ultra-pure reagents by sub-boiling point evaporation, likely in molecular distillation with a system that moves the input liquid and output condensate very close to each other to make the transfer rate reasonable, as evaporation would be prohibitively slow in passive mode.
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vano
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[*] posted on 10-2-2021 at 11:43


I think it is possible. Because there is not much distance between the person and the flask.There will usually be some research or this process is mentioned in some books.

[Edited on 10-2-2021 by vano]




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[*] posted on 22-8-2021 at 17:45


of course
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[*] posted on 22-8-2021 at 22:57


Awww, I remember making NaOH solutions as a lab tech. You can't see the NaOH getting into the air, but
your respiratory system can surely detect it. Nasty!
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[*] posted on 23-8-2021 at 11:26


Quote: Originally posted by zed  
Awww, I remember making NaOH solutions as a lab tech. You can't see the NaOH getting into the air, but
your respiratory system can surely detect it. Nasty!


It's less immediately noticable, but I believe your eyes are what take the hardest hit with NaOH and family:

Quote: Originally posted by BromicAcid  
Sodium hydroxide did a number on my eyes, always take care when working with bases. The effects were not immediately noticeable, I only realized in time that my eyesight had been shot.
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[*] posted on 24-8-2021 at 11:56


Any sort of evaporation can include dissolved substances.

Nickel is not nearly as toxic as chromium (VI) salts.
I would suggest covering the evaporating dish with something to reduce the amount that gets into the air and using good ventilation. Keeping in mind that hexavalent chromium salts will readily oxidize pretty much anything including dna.
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[*] posted on 12-9-2021 at 09:05


Quote: Originally posted by macckone  
Any sort of evaporation can include dissolved substances.

Nickel is not nearly as toxic as chromium (VI) salts.
I would suggest covering the evaporating dish with something to reduce the amount that gets into the air and using good ventilation. Keeping in mind that hexavalent chromium salts will readily oxidize pretty much anything including dna.


Dissolved salts don't evapourate at all, as long as there aren't any aerosoles from boiling it there is nothing to worry about. You'd be more likely to breath in nickel "evapourating" from a penny then a nickel salt solution.

However, you should be careful with evapourating acidic solutions of hexavalent chromium and maybe also pentavalent vanadium. With chloride ions in acidic conditions some hexavalent chromium could react to chromyl chloride (CrO2Cl2), which is a volatile red liquid. I had this happen once when I poured some HCl to a somewhat concentrated solution of dichromate, which caused some red vapour to come out of the solution. Vanadium is probably less likely to do that, but it can form similar compounds like vanadyl chloride (VOCl3).

[Edited on 12-9-2021 by theAngryLittleBunny]
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[*] posted on 16-9-2021 at 10:38


So why wouldn't a dissolved salt, such as mercuric chloride, evaporate at all?



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