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DraconicAcid
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[*] posted on 20-8-2016 at 08:36


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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[*] posted on 23-8-2016 at 05:47


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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[*] posted on 23-8-2016 at 06:26


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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[*] posted on 23-8-2016 at 06:48
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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[*] posted on 23-8-2016 at 07:42


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.




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[*] posted on 23-8-2016 at 16:49


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 ?




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[*] posted on 23-8-2016 at 17:08


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.




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[*] posted on 23-8-2016 at 19:40


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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[*] posted on 23-8-2016 at 19:45


You want to play with acrolein??

Take care and good luck.




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[*] posted on 23-8-2016 at 20:16


Quote: Originally posted by j_sum1  
You want to play with acrolein??

Take care and good luck.


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]




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[*] posted on 23-8-2016 at 22:49


Quote: Originally posted by zwt  
Make an electroscope radiation meter and watch it droop.

I cannot assess the safety of this, x-rays scared even Edison.


I see, thank you. Is there anything else imaging-related I'd try?
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[*] posted on 24-8-2016 at 03:29


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?

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)




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[*] posted on 24-8-2016 at 03:55


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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[*] posted on 26-8-2016 at 14:39


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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[*] posted on 29-8-2016 at 20:38
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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[*] posted on 30-8-2016 at 06:02


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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[*] posted on 2-9-2016 at 10:37


Is there a possibility for a mixture of sodium hydroxide and magnesium metal, both powdered, to ignite spontaneously? :D
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[*] posted on 2-9-2016 at 12:03


Quote: Originally posted by Alice  
Is there a possibility for a mixture of sodium hydroxide and magnesium metal, both powdered, to ignite spontaneously? :D


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?




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[*] posted on 3-9-2016 at 02:38


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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[*] posted on 6-9-2016 at 12:18


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. :)




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[*] posted on 6-9-2016 at 14:52
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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[*] posted on 6-9-2016 at 17:44


No sadly it is no where even remotely that simple sadly!

Only way is distillation/boiling/SO3 addition.
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[*] posted on 6-9-2016 at 20:56


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]




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[*] posted on 12-9-2016 at 12:29


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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[*] posted on 12-9-2016 at 13:11


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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