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alexleyenda
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Then I guess it would be friction, cork is good at creating heat with friction so it makes sense, thought i'm not sure it can create enough heat to
ignite H2. Anyways to me it's more plausible than static electricity as it takes quite a lot of static e to create a spark at my knowledge. Unless you
rub your cork in your hair for luck before you experiment I doubt it explains the ignition :p
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Pyro
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is rectapur (chemically pure, http://www.surechem.co.uk/pdf/chemicalCompweb14509.pdf) anhydrous AlCl3 supposed to look like this? I can tell 3 different colors...
and is it really necessary to grind it to a powder? My lab is kind of damp and the fumes...
all above information is intellectual property of Pyro.  |
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Zyklon-A
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Storing magnesium.
I got some Mg ribbon a few months ago, and put it in a ziplock bag, and then forgot about it. When I took it out, it was coated with a white powder
(MgO or Mg(OH)2), anyway I put it in very dilute HCl for about 5 mins. It's mostly shiny now, but I don't want that to happen again, so I
want to find a way to store it without it oxidizing anymore.
I put it in a glass jar and filled it with CO2, I know Mg reacts with CO2, but slower than air and only at high temps right?
Would this be affective for long time storage of magnesium?
(The jar of course was sealed.)
[Edited on 8-1-2014 by Zyklonb]
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Pyro
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Just protect it from damp air, in a jar or air tight bag. the oxidation is minimal, I have 2 rolls of Mg ribbon, one was lying around for a year, the
other was in an airtight bag. there isn't much difference between the two.
all above information is intellectual property of Pyro. |
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Zyklon-A
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Well I live in Texas, where it is very humid, and even though the bag was airtight ( I think), it still oxidized quite a bit.
But I guess the jar will work then?
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thebean
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I put my magnesium under mineral oil, it works fairly well.
My question would be about oxalic acid ester syntheses. Does the Fischer Esterification work? If I want to produce dimethyl oxalate or diethyl oxalate
will a simple reflux of the oxalic acid the alcohol and a sulfuric acid catalyst work?
"You need a little bit of insanity to do great things."
-Henry Rollins
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Crowfjord
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Answer @thebean:
Yep, pretty much. There is a synthesis on orgsyn.org that does just that if I remember correctly. I don't have the link off hand, but a structure
search for dimethyl oxalate brings it up.
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thebean
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Oh and one other question/conundrum.
I wanted to produce benzoic acid, so I took stoichiometric amounts of sodium benzoate and hydrochloric acid but I didn't see any sort of reaction. The
odor is the same and the crystals look untouched. What happened, what can I do to fix it, and if it isn't fixable without a lot of work is the sodium
benzoate salvageable?
"You need a little bit of insanity to do great things."
-Henry Rollins
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Crowfjord
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Benzoic acid is scarcely soluble in water, so the result isn't much of a surprise. The crystals are likely benzoic acid. I think you can extract with
a non polar solvent, dry with desiccant of your choice and evaporate to recover.
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DraconicAcid
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You should have dissolved it in water, then added the acid to get a precipitate.
If what you have is benzoic acid (as it should be), dissolve it in hot water (not boiling, or you'll hate the smell), and let it cool slowly to
crystallize. They should be white and feathery.
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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thebean
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I added approximately 400mls of water to a beaker if the acid is included so I should think it would work. If I remove some precipitate and put it in
hot water that should determine whether it is benzoic acid or not, yes?
"You need a little bit of insanity to do great things."
-Henry Rollins
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DraconicAcid
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400 mL of water should dissolve about 1.2 g of benzoic acid at RT, and 18 g at 90oC. How much did you add? Heat your solution, and if everything
dissolves, cool it slowly.
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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thebean
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I added .1 moles of sodium benzoate and .1 moles of HCl (actually a tiny bit more because excess HCl would be easier to deal with than benzoate).
"You need a little bit of insanity to do great things."
-Henry Rollins
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DraconicAcid
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That should give you about 12 g of benzoic acid, so getting it hot should dissolve it all nicely. Once it's dissolved, let it cool slowly to room
temp, then chill it in an ice bath for twenty minutes or so, then filter your acid out.
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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thebean
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Yeah my theoretical yield was just barely over 12 grams. I did the hot water test and it is definitely benzoic acid.
"You need a little bit of insanity to do great things."
-Henry Rollins
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plante1999
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Anyone got a good chemical engineering book? I already have perry.
I mean, a book that would be about design of plants. For example pipes and pumps and all the other chemical plant goodies.
Thanks
I never asked for this.
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Brain&Force
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Also, how can you tell if an oxide is nonstochiometric? I know MnO2 is and Tb4O7 may be, and they're both
brownish-black. I've also seen the color of Ho2O3 explained as being caused by stoichometric defects. Can such defects create
colors that subtle?
At the end of the day, simulating atoms doesn't beat working with the real things...
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DraconicAcid
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Quote: Originally posted by Brain&Force  | | Also, how can you tell if an oxide is nonstochiometric? I know MnO2 is and Tb4O7 may be, and they're both
brownish-black. I've also seen the color of Ho2O3 explained as being caused by stoichometric defects. Can such defects create
colors that subtle? |
Yes, they can. One class of defect is called an f-centre; the f stands for "farbe" or "colour", because it can turn an otherwise colourless compound
blue.
How to tell if it's nonstoichiometric? No idea....
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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Romain
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Hi,
I'm wondering if you can use gold electrodes to electrochemically make sulfuric acid form copper sulfate.
I don't have access (at all) to H2SO4, HCl, HNO3,... where I live so that would be very useful if I could make my own sulfuric acid.
I'd like to etch circuit boards with it (+ H2O2) so if it works I could restore my etchant for almost nothing.
I asked for platinum at my local bank but they only have gold... though I ordered a 1g gold bar anyway because I need some for my element collection.
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Zyklon-A
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I think so. HCl is sold at Home Depot FYI.
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Romain
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Ok thanks!
Also I live in Switzerland and very few chemicals are available here.
HCl, H2SO4, NaOH, acetone, 35% H2O2,... are readily available in France (and I live only 60km away from the border) though I need to bring them back
to Switzerland and I don't think it's legal...
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elementcollector1
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You can order 1g gold bars? How much do they cost?
Elements Collected:52/87
Latest Acquired: Cl
Next in Line: Nd
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alexleyenda
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He lives in switzerland, I don't know if they have any home depot. Anyways, usually you can find HCl in pool stores to lower the PH, you can also find
it in hardware stores near the paint thinners. Conc. Sulfuric acid is sold in hardware stores as drain cleaner and 35% sulfuric acid is sold in car
pieces shop as battery acid, you have to ask for it. You can concentrate it yourself ( very dangerous however).
HNO3 can be more tricky. At least here in Canada it's impossible to find , you have to make it yourself with nitrate salt like KNO3 (also banned but
obtainable from farms) and conc. H2SO4.
edit after I saw your post: Even where I told you they don't have it? That would be real chimicalphobia. And I know what you live, I often think about
going in the states to buy chemicals and bring them back but if they catch me at the border I'll be in deep trouble :p
[Edited on 11-1-2014 by alexleyenda]
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Zyklon-A
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Not that dangerous to concentrate H2SO4, as long as you do it outside and don't breath in the fumes, it takes a lot of energy though, boil it
>300C.
I never realized how lucky I am, in Texas I can get almost any chemical I want, (mostly online).
Does the border patrol search you when you cross?
[Edited on 12-1-2014 by Zyklonb]
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alexleyenda
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Really? I thought it heard you could not even have chemistry glassare in Texas. Anyways the danger with H2SO4 is that it boils at 320+ °C and that it
tends to splash as it bubbles, even with boiling chips. If 98% H2SO4 splashes on you, it's very bad. If 320°C 98% H2SO4 splashes on you, you're in
deep _____.
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