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Zyklon-A
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Try food-grade gloves. In a different thread I tried tested them, amazingly, they withstand even fuming nitric acid for over 20 minutes of contact.
Of course try it yourself before putting them on to be sure they are the same, but they should work fine.
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ganger631
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Few spatters
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ganger631
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Can you give me an example of a food grade gloves?
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Oscilllator
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The ones you buy at the supermarket for preparing food...
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Pyro
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they will be fine with a few spatters.
all above information is intellectual property of Pyro.  |
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Brain&Force
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Do you think my Samsung Galaxy S3 can handle being placed in a vacuum dessicator, so I can demonstrate air pressure with the phone's barometer app?
The screen can't crack and the phone should be able to remain powered on for the duration of the demo.
At the end of the day, simulating atoms doesn't beat working with the real things...
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forgottenpassword
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Is there some machine that can find the triple point(s) of an unknown pure substance automatically? Or is there a standard methodology for finding
triple points which is independent of the substance's identity?
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franklyn
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Acetylene tetrabromide ?
I'm sure this is a misprint. Ethylene terabromide or perbromide perhaps , or else Acetylene dibromide or perbromide.
wwwapps.tc.gc.ca/saf-sec-sur/3/erg-gmu/erg/guidepage.aspx/guide159/id1668/mnid1807
.
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PHILOU Zrealone
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Quote: Originally posted by franklyn  | I'm sure this is a misprint. Ethylene terabromide or perbromide perhaps , or else Acetylene dibromide or perbromide.
wwwapps.tc.gc.ca/saf-sec-sur/3/erg-gmu/erg/guidepage.aspx/guide159/id1668/mnid1807
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Acethylen tetrabromide...
Old chemical names/technical names looks a bit like alchemistry names and are sometimes misleading.
-You can have the addition product
CH2=CH2 + Br2 --> Br-CH2-CH2-Br (ethylene dibromide = 1,2-dibrom-ethane)
H-C#C-H + 2 Br2 --> Br2CH-CHBr2 (acethylene tetrabromide = 1,1,2,2-tetrabrom-ethane) (*)
-You can have the substitution product
Br2C=CBr2 (ethylene tetrabromide / perbrom-ethylene)
Br-C#C-Br (acethylene dibromide)
(*) I have some litters of that superheavy solvent (almost feels like mercury  ),
I got those for 1€/L
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
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HeYBrO
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Just a quick question... I was cleaning glassware with manganese dioxide stains on glassware with dilute hydrogen peroxide and 3-4 drops of conc.
sulphuric acid. One of the pipettes i was cleaning had a small amount (like a grain of sand or less) of potassium permanganate which formed some
bubbles which i presume was oxygen when it came into contact with the cleaning mix. However, there was a slight sulphurous odour, almost eggy (almost
like Sulphur dioxide), but not rancid and did not smell like rotten eggs. I guess it was kind of like the smell of sulphuric acid (sort of
sulphurous). Is there any chance i accidentally produced hydrogen sulphide? If so, should i be concerned? I had less than five minutes exposure, only
smelt it once or twice and i used small amounts of chemicals (~20-50 ml of 3% hydrogen peroxide , ~50 ml of distilled water and >0.5 ml of conc.
Sulphuric acid)
I don't think so but i just wanted to be sure.
EDIT: I don't know why I'm such a hypochondriac once I've been in the lab... I looked up the equation and forgot thats how you
titrate hydrogen peroxide.
2 KMnO4 + 3 H2SO4 + 5H2O2 = 2 MnSO4 + K2SO4 + 5O2 + 8H2O
[Edited on 23-8-2014 by HeYBrO]
[Edited on 23-8-2014 by HeYBrO]
[Edited on 23-8-2014 by HeYBrO]
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Texium
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From the description, it doesn't sound like hydrogen sulfide. If you had produced it, it would definitely smell of rotten eggs. I have produced it in
small amounts a few times, once on purpose and a couple times on accident, and the smell is quite potent even at low concentrations. As long as you
get away from it quickly and breath some fresh air, you're just fine. Even if you did produce hydrogen sulfide, if you didn't stick your nose right in
it, there shouldn't be a problem.
Edit: Ah, I see you answered your own question before I could reply.
[Edited on 8-23-2014 by zts16]
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HeYBrO
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Thanks.
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confused
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well, better to err on the side of caution than to totally disregard something potentially hazzardous
(within reason of course)
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solo
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...when using Oxone in many of its applications, I've often wondered, when they say x amount of oxone, do they mean the oxone as it comes with the two
other salts, since the active ingredient is only 48% of the whole, or do they mean of the active ingredient ....it's confusing. some clarification
please....solo
It's better to die on your feet, than live on your knees....Emiliano Zapata.
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DraconicAcid
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| Quote: Originally posted by arkoma | 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] |
That's impure copper(I) chloride.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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Amos
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Any cheap method of separating sodium nitrate and sodium chloride, particularly by solvent extraction?
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PHILOU Zrealone
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| Quote: Originally posted by DraconicAcid | | Quote: Originally posted by arkoma | 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] |
That's impure copper(I) chloride. |
Or copper hydroxychloride Cu(OH)Cl... I have some 200g in a glass jar and it has that colour, almost unsoluble in water.
It is also refered as copper oxychloride.
[Edited on 25-8-2014 by PHILOU Zrealone]
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
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DraconicAcid
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Wouldn't that react with vinegar, though?
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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PHILOU Zrealone
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Slowly especially with the 5-10% variant...much better with 80% acetic acid. Household vinegar dissolves metallic copper but you need air (O2) contact
with the copper and agitation for the acid to contact those parts and it takes weeks...actually acetic acid dissolves the hydroxy-oxy-carbonate layer
of the copper ...once naked it is oxydized again and reforms an hydrated-oxyd layer ...so atomic layer by atomic layer it is dissolved.
HCl conc (30%) on Cu(OH)Cl does the job very wel...you get CuCl2.
I use Cu(OH)Cl as colourizer for green-blue flame in some pyro mixes. It is not very stable with NaClO3 based pyro compositions owing to
hygroscopicity and bad interactions between Cu(2+) and ClO3(-)...so not storage advisable for long.
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
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PHILOU Zrealone
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You can play on the difference of solubility of both salts in water as a function of the temperature.
NaCl remains relatively constant while NaNO3 increases exponentially with T.
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
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Haber
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| Quote: Originally posted by Haber |
All of the product have now turned into a black dusty powder. Vanillin smell almost completely gone.
Even if it was 5-bromovanillic acid it shouldn't be black.
I'm very curious what has happened. Nobody who have any guess?
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I've discovered that this occured because of some kind of reaction with the metal on my thermometer probe.
Would be interesting to know what kind of reaction it was, if anyone have an guess, let me know
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gdflp
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Quick question, white phosphorus won't burn in carbon dioxide right? So if one wanted to convert white phosphorus(I don't have any currently but am
thinking of trying to make some using the current method in the phosphorus sticky thread) to red phosphorus, a flask could be charged with some white
phosphorus, flushed with CO2, and heated to convert to red phosphorus without ignition of the phosphorus occurring? If not, what is the
best way to convert white phosphorus to red phosphorus?
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elementcollector1
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| Quote: Originally posted by gdflp | | Quick question, white phosphorus won't burn in carbon dioxide right? So if one wanted to convert white phosphorus(I don't have any currently but am
thinking of trying to make some using the current method in the phosphorus sticky thread) to red phosphorus, a flask could be charged with some white
phosphorus, flushed with CO2, and heated to convert to red phosphorus without ignition of the phosphorus occurring? If not, what is the
best way to convert white phosphorus to red phosphorus? |
Place in flask with 0.5% wt. I2, flush with CO2 or other inert gas, and heat for 24 hours.
At least, that was what was told to me - I've never had the chance to try it, never having had any phosphorus to speak of.
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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learningChem
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Is it possible to reduce 3 nitrobenzoic acid to 3 aminobenzoic acid using the Fe/HCl method?
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Metacelsus
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It should work fine.
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