Diachrynic
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Dense, metallic liquid - supposed mercury - hit or shit?
Today I found in the shed in an old shelf a jar with a very dense, metallic liquid, which got me excited and a bit terrified - did I find some old
mercury? The jar was unlabeled though, so I'm completely unaware of what it's backstory is.
So, I am pretty sure it is mercury - is there any other dense, metallic liquid?
It not shiny; not at all. Pprobably highly contaminated with other stuff.
I live in Germany. I didn't find anything about mercury being illegal, but please correct me if I'm wrong.
Now, my question is: Can a moron like me with two left hands handle it safely? If, then how? Or better bring it to a disposal facility? Is it worth
the effort to purify it because it's really impossible to get here?
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UC235
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That's mercury. It does tend to get scummy over time. IIRC, the preferred way to clean it is to let it drip through a pinhole in a filter paper cone
into a clean container. The oxides stick to the paper.
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S.C. Wack
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And things dissolved in it can be removed chemically without difficulty. Most people handle it like plutonium so we're sure you'll be fine as long as
the authorities are not interested in this shed.
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Diachrynic
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Thanks, so it is mercury.
Filtering it through a pinhole seems like a good idea.
What would be a chemical way to clean it? HCl?
Also, how do I protect myself from the fumes? Gloves, lab coat, that's fine, but do I need a respirator or something?
I need to buy a container for the mercury contaminated waste...
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Bert
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Mercury Poisoning
Metallic Mercury = Not benign, but can be handled by a careful person with little danger. Has been handled, prodded, poked bare handed and generally
oogled at by many people, including school children in my youth- AT SCHOOL. We floated the junior high school science teacher's Gold wedding ring in a
jar of it for fun, he put it back on again after. No discernible consequences in the next 4 years I was at that school...
Water soluble inorganic mercury salts = Rather more dangerous, but still can be handled and used CAREFULLY by a competent amateur, an ethical person
will have a procedure in place for disposing properly of any waste from use. NOT just dumping it down the drain or pouring it out in a field...
Organic mercury compounds = can be VERY dangerous. Some can go right through common nitril gloves, the Plutonium reputation comes largely from this
class. Industrial users have had some serious problems with large and enduring consequences. Probably not wise for most amateurs, how good is your
hood and where does the exhaust go?
For some background, Google: Minimata, Niigata, Basra poison grain disaster, "mad hatter", "Isaac Newton Mercury poisoning".
[Edited on 24-11-2017 by Bert]
[Edited on 24-11-2017 by Bert]
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chornedsnorkack
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Quote: Originally posted by Diachrynic  | Today I found in the shed in an old shelf a jar with a very dense, metallic liquid, which got me excited and a bit terrified - did I find some old
mercury? The jar was unlabeled though, so I'm completely unaware of what it's backstory is.
So, I am pretty sure it is mercury - is there any other dense, metallic liquid?
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The low melting metals are 3 groups:
alkali metal eutectics;
Ga alloys;
Hg and alloys.
Activity and density are grossly different.
Density of alkali metals tops at 1,9 of caesium. And that´s very reactive with air and water. NaK and anything that is mostly Na or K would also be
less dense than water.
Ga density is near 6. Pure metal freezes at 30 degrees, alloys lower.
Hg density is around 13,5.
These 3 liquids are not mutually miscible. With larger amounts of impurities, Hg forms solid amalgams.
So detecting difference between Hg and Ga? More than double the difference in density. And Ga wets glass, Hg does not.
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S.C. Wack
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Nitric acid.
https://www.sciencemadness.org/whisper/viewthread.php?tid=10...
You've been exposed to mercury vapor before if you've broken fluorescent lights. Do not heat.
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Bert
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DILUTE nitric acid, SHORT contact time. Best specify?
I have dissolved metallic Mercury in 68% Nitric acid (first step in a Mercury fulminate synthesis). Did not take long.
Rapopart’s Rules for critical commentary:
1. Attempt to re-express your target’s position so clearly, vividly and fairly that your target says: “Thanks, I wish I’d thought of putting it
that way.”
2. List any points of agreement (especially if they are not matters of general or widespread agreement).
3. Mention anything you have learned from your target.
4. Only then are you permitted to say so much as a word of rebuttal or criticism.
Anatol Rapoport was a Russian-born American mathematical psychologist (1911-2007).
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Diachrynic
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Unfortunately I don't have any nitric acid yet (but I plan do make some, someday).
Is there an alternative?
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ninhydric1
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It will dissolve in hot concentrated sulfuric acid.
The philosophy of one century is the common sense of the next.
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Diachrynic
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Yeah, but I don't want to dissolve the mercury. I want to clean it by dissolving the impurities and leaving the mercury behind.
That way I think I can avoid mercury salts for now. As Bert wrote, it's metallic form is safer that its salts, so I try to avoid those for now.
Also, I don't have sulfuric acid. Anyone knows a good source of sulfuric acid in Germany?
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metalresearcher
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| Quote: Originally posted by chornedsnorkack | | Quote: Originally posted by Diachrynic | Today I found in the shed in an old shelf a jar with a very dense, metallic liquid, which got me excited and a bit terrified - did I find some old
mercury? The jar was unlabeled though, so I'm completely unaware of what it's backstory is.
So, I am pretty sure it is mercury - is there any other dense, metallic liquid?
|
The low melting metals are 3 groups:
alkali metal eutectics;
Ga alloys;
Hg and alloys.
Activity and density are grossly different.
Density of alkali metals tops at 1,9 of caesium. And that´s very reactive with air and water. NaK and anything that is mostly Na or K would also be
less dense than water.
Ga density is near 6. Pure metal freezes at 30 degrees, alloys lower.
Hg density is around 13,5.
These 3 liquids are not mutually miscible. With larger amounts of impurities, Hg forms solid amalgams.
So detecting difference between Hg and Ga? More than double the difference in density. And Ga wets glass, Hg does not. |
And the first category is very light. NaK has a density of only 0.86 but is very reactive, more than individual Na or K.
ScienceMadness has a video with a gun shooting bullets of Na, K or NaK wrapped in plastic, real fun !
You can clean Hg with a method by a NileRed: https://www.youtube.com/watch?v=2ubw1bI8s5w
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ninhydric1
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If you want to clean it chemically, some HCl or dilute H2SO4 will be good enough. The pinhole is the simplest physical method IMO.
[Edited on 11-23-2017 by ninhydric1]
The philosophy of one century is the common sense of the next.
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chornedsnorkack
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A logical way to clean more active metal impurities out of mercury is displacement by mercury salts. Like:
Cu+Hg2(NO3)2=Cu(NO3)2+2Hg
But that leaves the less active metals.
How are impurities of less active metals removed from mercury? The appreciably (though to a small degree) soluble less active metals in liquid Hg at
low temperatures are Ag and Au. So how do you separate Ag and Au impurities? Especially Ag? It has reactivity close to that of Hg, so what would
dissolve just one?
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hyfalcon
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Distill your mercury away from the impurities.
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j_sum1
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Nice. But not for the inexperienced or faint of heart. And definitely not an area where you want to skimp on good equipment.
I understand that putting a cotton ball in a syringe and forcing the mercury through that is an effective way of filtering. You then want to have a
means for disposing of your filter material. That opens up a whole new bunch of issues.
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woelen
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Distilling is not an option. I have quite some experience with chemical experimenting and also with distillations, but distilling mercury in a
home/amateur setting is beyond reasonable. Only VERY few amateurs can do that safely.
If you don't have HNO3, nor H2SO4, then you can use high quality dilute acetic acid (not spiced and sweeted vinegar!) with a tiny amount amount of
H2O2 and drip your mercury in that. Take a coffee filter, make a tiny hole in it and carefully drip the mercury in that filter and let the drops fall
into the dilute acetic acid with a few tenths of percent of H2O2. Around 5% concentration of acid is OK.
Most of the solid crap on the surface of the mercury then remains behind in the filter, the droplets of mercury fall through the dilute acetic acid
and some metallic impurities dissolve. Also more crap which still sticks to the droplets dissolves. Let the metal sit at the bottom. You can lso store
it in this way. Simply pipette away 95% or so of the aqueous layer with the acid, then replace with distilled water and store it that way. The metal
then remains shiny and no vapor of mercury is released.
I would strongly advice you to work with the mercury above a big plastic tub. If you accidently spill droplets, then they do not fall onto your
desk, onto the floor and so on. Having droplets of mercury, contaminating your house is disastrous, it is VERY VERY hard to cleanup these droplets.
They break aprt in a zillion nearly invisible droplets which go into every wrinkle or crack of your floor, wood, concrete or whatever it falls
on.
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S.C. Wack
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My bad for not providing any hint as to how one might proceed, might as well delete my post then. Should I scan the book it came from and post that
too? It was my impression that prior permanganate treatment was essential, but not mentioning that at all is OK? (It makes the mercury finely divided,
if nothing else.)
Brauer implies that some dissolving of mercury in nitric acid is not necessarily undesirable. Furthermore, a yes we can conc. sulfuric and air setup
is drawn in both the German and English versions.
Battery electrolyte can be concentrated without fumes in the oven by gradual heating until it probably starts to darken i.e. from low 30's to 70-80's
%, in ovenware or a borosilicate beaker I'd set on cast iron.
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phlogiston
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Mercury can also be refined (purified) electrolytically. That might be a relatively non-hazardous means to purify it, since it does not require
heating and should get rid of non-noble impurities.
However, it does involved soluble mercury salts.
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"If a rocket goes up, who cares where it comes down, that's not my concern said Wernher von Braun" - Tom Lehrer |
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chornedsnorkack
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How efficient is Fe in reducing soluble Hg salts to metallic Hg?
Also, how good solvent for Hg is cold dilute H2SO4 with hydrogen peroxide?
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VSEPR_VOID
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https://www.youtube.com/watch?v=d6SahlAFV-w
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