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DraconicAcid
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Quote: Originally posted by Velzee  | | Hmm..could oxalic acid be used to produce nitric acid, or would it just be oxidized as HNO3 is produced? |
Depends on what concentration you want. I assume you mean to react calcium nitrate with oxalic acid in a precipitation reaction, to leave nitric acid
in solution, or something to that effect. It will probably work fine if the concentration is less than 1 mol/L or so.
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math
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Which (safe) experiments could be done with a veterinary X-ray generator (plus phosphor screens), apart imaging objects conventionally (projecting
their shadow in radiographs)?
Thank you
[Edited on 23-8-2016 by math]
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zwt
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Make an electroscope radiation meter and watch it droop.
I cannot assess the safety of this, x-rays scared even Edison.
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Sulaiman
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Which of these has general or interesting use ?
I am planning to make a 'fruity' ester following videos by NileRed and others,
the alcohols are not cheap, for me, with p&p, price per litre;
1-propanol £11.95
Benzyl Alcohol £14.25
1-octanol £24.20
1-nonanol £266.10
2-pentanol n/a
are any of the first three generally useful/interesting ?
EDIT: math
You could investigate different doses on biological specimens,
living plants, seeds, bugs, muscle tissue ....
[Edited on 23-8-2016 by Sulaiman]
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DraconicAcid
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| Quote: Originally posted by Sulaiman | I am planning to make a 'fruity' ester following videos by NileRed and others,
the alcohols are not cheap, for me, with p&p, price per litre;
1-propanol £11.95
Benzyl Alcohol £14.25
1-octanol £24.20
1-nonanol £266.10
2-pentanol n/a |
I avoid benzyl anything as much as I can, and I'd expect propyl esters to be more volatile and fragrant than the octyl ones.
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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Texium
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Threads Merged
23-8-2016 at 08:15 |
Texium
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Threads Merged
23-8-2016 at 08:21 |
Sulaiman
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Thanks.
I did a little research on the alcohols and propanol seems to be quite useful, and it is the cheapest.
Since a litre of 99.9% n-propanol is £12 incl. p&p
I wonder if there are syntheses where it can be used as a substitute for dry ethanol ?
CAUTION : Hobby Chemist, not Professional or even Amateur
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DraconicAcid
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| Quote: Originally posted by Sulaiman | Thanks.
I did a little research on the alcohols and propanol seems to be quite useful, and it is the cheapest.
Since a litre of 99.9% n-propanol is £12 incl. p&p
I wonder if there are syntheses where it can be used as a substitute for dry ethanol ? |
As a solvent, it will probably be an excellent substitute for ethanol. It won't dissolve ionic compounds as well as ethanol, but I doubt it would
make much difference for most reactions.
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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Velzee
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1,3-propanediol can be produced by the hydration of acrolein. If this is so, can the reverse reaction occur? And if so, how would one go about it?
Check out the ScienceMadness Wiki: http://www.sciencemadness.org/smwiki/index.php/Main_Page
"All truth passes through three stages. First, it is ridiculed. Second, it is violently opposed. Third, it is accepted as being self-evident."
—Arthur Schopenhauer
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j_sum1
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You want to play with acrolein??
Take care and good luck.
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Velzee
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Oh, no.. I better read the MSDS before anything... I didn't read up on the safety much because it's past midnight and I can barely keep my eyes open
EDIT: Looks like I'm not touching acrolein.
[Edited on 8/24/2016 by Velzee]
Check out the ScienceMadness Wiki: http://www.sciencemadness.org/smwiki/index.php/Main_Page
"All truth passes through three stages. First, it is ridiculed. Second, it is violently opposed. Third, it is accepted as being self-evident."
—Arthur Schopenhauer
"¡Vivá Cristo Rey!"
—Saint José Sánchez del Río |
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math
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I see, thank you. Is there anything else imaging-related I'd try?
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PHILOU Zrealone
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| Quote: Originally posted by Velzee | | 1,3-propanediol can be produced by the hydration of acrolein. If this is so, can the reverse reaction occur? And if so, how would one go about it?
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Acrolein is CH2=CH-CH=O if you add water it would lead to HO-CH2-CH2-CH=O and if you add more water then to HO-CH2-CH2-CH(-OH)2 thus not to
1,3-propandiol...
To get 1,3-propandiol you also need a reduction (a partial hydrogenation).
Usually acrolein can be acheived in the lab from 1,2,3-propantriol (glycerine/glycerol)... and mild acid catalyst (NaHSO4).
HO-CH2-CHOH-CH2OH --> HO-CH2-CH=CH-OH + H2O
HO-CH2-CH=CH-OH <----> HO-CH2-CH2-CH=O (enol-keton equilibrium)
HO-CH2-CH2-CH=O --> CH2=CH-CH=O + H2O (favourized by the conjugation of the CC double link and the CO double link)
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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j_sum1
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Nilered has a recent video on acrolein from glycerine.
Fun to.watch but not fun to do.
As for the diol, I don't know. I have lots to learn. But undoubtedly there is a procedure. You might try prepchem.com.
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math
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Could a small license-free 60Co (or any other radioactive isotope of any kind) sample be used to obtain radiographs of objects comparable to those
obtained by using a X-ray tube and phosphor plates?
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RogueRose
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Activated carbon's "selection" of what it can absorb
I've always wondered how AC works and what compounds will be absorbed by it.
So if there is some ammonium sulfate (say 1g/L) in water and the water is run through an AC filter, will it remover the AmmSulf? What about the same
(1g/L) with a common chloride salt - Na, K, Mg or Ca?
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aga
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Activated carbon is basically carbon with a VAST surface area for atoms/molecules to get adsorbed onto.
Commercially they dose the AC with other chemicals to make them adsorb specific chemicals for specific applications.
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Texium
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Threads Merged
30-8-2016 at 06:04 |
Alice
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Is there a possibility for a mixture of sodium hydroxide and magnesium metal, both powdered, to ignite spontaneously? 
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Hegi
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| Quote: Originally posted by Alice | | Is there a possibility for a mixture of sodium hydroxide and magnesium metal, both powdered, to ignite spontaneously? |
Yeah there is a possibility for the metal particles to ignite spontaneously, if the size is really small and surface area high, it´s called
pyrophoricity.
Did it happen to you?
Our webpage has been shut down forever cause nobody was willing to contribute. Shame on you all!!!
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Alice
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Thanks for the answer! No, nothing happend. I'm asking beforehand. I knew Mg powder is pyrophoric, the point is, if the mixture is somehow
super-pyrophoric, for example due to the hygroscopicity of NaOH. Maybe it was a stupid question, because "powder" can mean a lot, and I should find
out in some micro-scale experiment. On the other hand it's possible having ten times nothing and ignition in the eleventh trial. However, the case I
was asking for is just a hypothetic worst case scenario compared to what I actually want to find out. 
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Hegi
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| Quote: Originally posted by Alice | | Thanks for the answer! No, nothing happend. I'm asking beforehand. I knew Mg powder is pyrophoric, the point is, if the mixture is somehow
super-pyrophoric, for example due to the hygroscopicity of NaOH. Maybe it was a stupid question, because "powder" can mean a lot, and I should find
out in some micro-scale experiment. On the other hand it's possible having ten times nothing and ignition in the eleventh trial. However, the case I
was asking for is just a hypothetic worst case scenario compared to what I actually want to find out. |
I think there´s no such a reaction. I never heard of it. 
Our webpage has been shut down forever cause nobody was willing to contribute. Shame on you all!!!
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PTeLuM
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Drying Sulfuric Acid to produce an anhydrous reagent
Does anyone know of economical and reliable ways to dry 93% sulfuric acid drain cleaner? Would drying with anhydrous magnesium sulfate work, or maybe
molecular sieves?
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XeonTheMGPony
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No sadly it is no where even remotely that simple sadly!
Only way is distillation/boiling/SO3 addition.
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Texium
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6-9-2016 at 20:03 |
greenlight
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I have a portable fumecabinet I have been using that I purchased from a high school which was upgrading to wall mounted fumehoods.
It has a large new activated carbon filter in it and I have clocked 33 hours on it so far mainly with acid fumes.
Does anyone have any idea how long these filters last before they reach their full absorbtion level and need replacing?
[Edited on 7-9-2016 by greenlight]
The only use for an atomic bomb is to keep somebody else from using one.
George Wald
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ficolas
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I wanted to make food grade sodium acetate to use as a condiment, so I took vinegar, and sodium bicarbonate. I added some sodium bicarbonate to the
vinegar until it stopped bubbling, then boiled the solution down. I got very contaminated sodium acetate, that tasted nicelly, but the vinegar I used
wasnt distilled (keeping it food-grade), so it had some organic planty stuff that burned and ruined the sodium acetate (Im not eating brown shiet)
What can I do to stop this from happening?
I didnt use stoichiometric amounts because I dont know the concentration of acetic acid in the vinegar, and I currently have no good way of
tritrating it (Only ph paper, I would need to use up a ton of them for a shitty tritation)
Or I could just use salt and vinegar as a condiment but that aint as fun.
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Sulaiman
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I'm guessing here but you could weigh out an ammount of sodium bicarbonate,
add vinegar until no fizzing (the last bit goes slowly, don't add vinegar too fast near the end)
you can work out the weight of sodium acetate produced,
look up the solubility and boil down only to that ammount then cool and hopefully collect moderately pure crystals.
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