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Pumukli
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Papaya,
Are you sure you titrated Na2CO3?
I mean was not your "standard" contaminated with either H2O (crystal water?) or NaHCO3?
Next time try to heat your Na2CO3 in a metal pan for a while say around 120 C before the titration. This way you can elimante both "contaminants",
water will evaporate and NaHCO3 would decompose to give Na2CO3.
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AlphaDecay
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My dad broke his mercury thermometer, but the Hg didn't spill anywhere, however it is stuck in the thin glass tube.
How can I extract it from the glass? Perhaps heating it? Im asking for help due to mercury toxicity, I don't want to poison anyone.
Sorry for english mistakes
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gdflp
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DON'T heat it. Mercury metal isn't that toxic but mercury vapor is extremely toxic. Try a syringe with a long end. You could also try to drill a
small hole in the other end of the thermometer, I suspect it isn't coming out because there is a way for air to get in.
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AlphaDecay
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Yes, the mercury tiny glass tube broke and the mercury is in contact with air, but it is too thin too use a syringe, and it doesn't fall from the
broken thermometer...
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gdflp
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You could try(carefully) breaking the other end so that the mercury will drain out. I assume you want the liquid mercury and not a mercury compound?
[Edited on 26-7-2014 by gdflp]
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AlphaDecay
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I thought of storing it as a metal to use later for making its compounds, but why the question? Imerse the glass with mercury in acid?
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TheChemiKid
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I would attempt carefully breaking the thermometer over a large necked glass container. The mercury and some glass will fall in, and the glass can
easily be separated.
When the police come
\( * O * )/ ̿̿ ̿̿ ̿'̿'̵͇̿̿з=༼ ▀̿̿Ĺ̯̿̿▀̿ ̿ ༽
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AlphaDecay
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Yes, this seems a safe and easy way to solve the problem!
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TheChemiKid
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Make sure that all of the mercury gets in the glass, and do the entire thing in a bucket, that way if there is a problem, any spills are contained.
When the police come
\( * O * )/ ̿̿ ̿̿ ̿'̿'̵͇̿̿з=༼ ▀̿̿Ĺ̯̿̿▀̿ ̿ ༽
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gdflp
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Quote: Originally posted by AlphaDecay  | | I thought of storing it as a metal to use later for making its compounds, but why the question? Imerse the glass with mercury in acid?
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Yes, you could just immerse the glass in nitric acid if you wanted to get mercury nitrate.
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AlphaDecay
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Another question: I've been thinking about doing a small scale Solvay Process. It consists of bubbling together ammonia and carbon dioxide together in
a flask with saturated sodium chloride solution. Then Sodium Bicarbonate should precipitate leaving ammonium chloride in solution, right? Ok, so my
doubt is if I bubble CO2 and NH3 together will they form ammonium carbonate?
(Sorry for English mistakes)
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Zyklon-A
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Yes, that's how it works I think. NH4CO3 is more soluble than Na2CO3, so the sodium salt precipitates.
NH4CO3 + NaCl (aq) → Na2CO3 ↓ + NH4Cl (aq)
[Edited on 29-7-2014 by Zyklon-A]
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gdflp
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No, it precipitates sodium bicarbonate before any ammonium carbonate can form. This is due to the ammonium bicarbonate being more soluble than the
sodium bicarbonate. Since a saturated solution of sodium chloride is used, the following occurs. NH3 + CO2 + H2O
--> NH4HCO3. The sodium bicarbonate will immediately precipitate because the solution is saturated with sodium ions. Since
there are no bicarbonate ions left in solution, no ammonium carbonate forms. If no sodium chloride is present, then ammonium carbonate will form
NH4HCO3 + NH3 --> (NH4)2CO3.
[Edited on 29-7-2014 by gdflp]
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bbartlog
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Are there any stable cuprous salts where the anion has a charge other than -1? For example, cuprous chloride and cuprous acetate exist (though the
latter is not trivial to synthesize). On the other hand, cuprous sulfate is nonexistent - it immediately disproportionates in to CuSO4 and Cu(0), and
this seems to be kind of typical of such salts. Are all the cuprous salts Cu(X), or does there exist some cuprous Cu2(X)??
The less you bet, the more you lose when you win.
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forgottenpassword
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Cuprous oxide, Cu2O
Cuprous acetylide, Cu2C2
Cuprous sulphide, Cu2S
Cuprous mercuric iodide, Cu2HgI4
Cuprous selenide, Cu2Se
Cuprous sulphite, Cu2SO3
Cuprous telluride, Cu2Te
[Edited on 4-8-2014 by forgottenpassword]
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bbartlog
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Cuprous oxide, obviously ... should have thought of that one! But the others I was unaware of. Thanks!
The less you bet, the more you lose when you win.
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gdflp
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I'm going to be running a workshop in about two weeks about creating a low cost dye-sensitized solar cell using titanium dioxide/anthocyanins. The
problem is that due to the expense of the ITO glass, only six pieces were ordered and I have to do a dry run right before I actually run the workshop.
My question is, if the dry run works, is there any way to clean off the fused titanium dioxide and iodine solution without harming the indium/tin
layer on the glass?
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Texium
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Filter Flask Pressure Rating Question
Ok, for some reason I've never been able to find this information despite a lot of various search terms.
What is the pressure that filter flasks (nice Pyrex ones) can normally handle? I've been very cautious with mine so far, but I just want to check and
make sure of the safe pressure range because I don't want to go imploding my fancy new flasks on my first few filtrations. (I already uglied up my formerly pristine Büchner funnel with carbon stains, and I don't want to risk worse stuff)
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gdflp
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From your previous picture, I assume you are using a hand pump. In that case or with an aspirator, I would be very surprised if you could get the
flask to implode no matter what you did. As long as the funnel is attached correctly, an electric pump can be connected to it with minimal to no risk
of anything occurring. The only possible chance you might have is if you stoppered the flask really tightly with the correct size stopper and
connected a strong vacuum pump to it and left it for a while.
[Edited on 8-8-2014 by gdflp]
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Texium
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Ok, thanks! I figured that the hand pump probably wouldn't cause any problems, I just wanted to make sure, particularly since I will probably get an
electric one some time in the future.
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arkoma
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Electrolysis with Cu anode, lead cathode in a split cell. NaCl electrolyte. Anodic liquid has a fine light green powdered compound in it insoluble
in water, vinegar, methanol, and ethyl acetate. Soluble in HCl. What the hell is it? I've got the chloride crystallizing ATM, but stumped on the
powder by-product.
Edit--add picture
from left to right Copper Acetate, Copper Acetylsalicylate, Copper Sulfate, and my "unknown"
[Edited on 8-15-2014 by arkoma]
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status, nationality, citizenship, etc" z-lib
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Texium
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It looks and sounds kinda like copper carbonate, but I'm not sure how that would happen, other than reaction with atmospheric CO2 at the
anode. Did it give off a lot of gas when added to HCl?
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arkoma
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No, not that I noticed, but used VERY small amount of powder and HCl. The chemistry came from one of Ledgard's books--he sez should be copper
hydroxide, but he tells fairy tales also. Does LOOK like carbonate.
From Ledgard's "King's Chemistry Survival Guide":
| Quote: | The bluish precipitate will be very finely divided cupric hydroxide, which is
very difficult to filter-off. |
"We believe the knowledge and cultural heritage of mankind should be accessible to all people around the world, regardless of their wealth, social
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ganger631
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Will neoprene coated latex gloves handle 95-98 conc sulfuric and conc nitric for a few minutes?
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Pyro
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perhaps,
it depends how thick they are.
also, do you mean immersion or just a few spatters?
all above information is intellectual property of Pyro.  |
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