| Pages:
1
2
3
4
5
6
..
30 |
bahamuth
Hazard to Others
Posts: 384
Registered: 3-11-2009
Location: Norway
Member Is Offline
Mood: Under stimulated
|
|
Blue compound from nitration attempt of isopentanol or n-pentanol.
Several years ago I tried to nitrate isopentanol, or n-pentanol with nitric acid and sulfuric acid and remember I got a beautiful blue compound in
solution, no attempts were done to try to isolate this.
Of what i think I remember I had the nitric acid mixed with the pentanol with stirring and added sulfuric acid WAY to quick, scorching and boiling of
the mix followed, and then it took on a deep but clear blue color.
IIRC I found something on the net then of a blue short chain nitroso compound that maybe was the culprit that formed under such conditions.
So my question is, do anyone know what it maybe was?
Any sufficiently advanced technology is indistinguishable from magic.
|
|
|
stygian
Hazard to Others
Posts: 242
Registered: 19-9-2004
Member Is Offline
Mood: No Mood
|
|
Which was it, iso or n-pentanol? I do recall reading of some secondary pseudonitrosite or nitroles or something that are blue.
The pseudo-nitrols, RR':C(NO)(NO 2), may be obtained by the action of nitrous acid on the secondary nitroparaffins; by the action of silver nitrite on
such bromnitrosoparaffins as contain the bromine and the nitroso group united to the same carbon atom (0. Piloty, Ber., 1902, 35, p. 3 0 93); and by
the action of nitrogen peroxide on ethereal solutions of ketoximes (R. Scholl, Ber., 1888, 21, p. 508; G. Born, Ber. 1896, 2 9, p. 93). They exhibit
an intense blue colour when in the liquid condition or dissolved in alkali and possess a very sharp smell. On oxidation with chromic acid they yield
dinitrohydrocarbons, and on reduction with hydroxylamine (in alkaline solution) or with potassium sulphydrate give ketoximes, RR': C: NOH (R. Scholl
and K. Landsteiner, Ber., 1896, 29, p. 87).
Perhaps some nitrous acid was formed to cause this reaction with the ketone also formed?
[Edited on 30-9-2010 by stygian]
|
|
|
Rogeryermaw
National Hazard
Posts: 656
Registered: 18-8-2010
Member Is Offline
Mood: No Mood
|
|
does freezing your benzene negatively affect it? i store most of my volatiles in a refrigerator and i guess it was a bit too low...
|
|
|
bahamuth
Hazard to Others
Posts: 384
Registered: 3-11-2009
Location: Norway
Member Is Offline
Mood: Under stimulated
|
|
| Quote: | Originally posted by stygian
Which was it, iso or n-pentanol? I do recall reading of some secondary pseudonitrosite or nitroles or something that are blue. |
Think it was iso-pentanol, but as I vaguely mentioned earlier, do not really remember...
Never tried to reproduce that peculiar reaction but could give it a try, as I now have an idea of what it might be...
Any sufficiently advanced technology is indistinguishable from magic.
|
|
|
1281371269
Hazard to Others
Posts: 312
Registered: 15-5-2009
Member Is Offline
|
|
I'm planning a titration against molar H2SO4 to find out the concentration of an ammonia solution.
According to Wiki, Phenolphthalein should be used for strong acid / strong base neutralisations. Both Phenolphthalein and an indicator called Neutral
Red are available from eBay. Whilst the former changes colour around pH 8.3-10, Neutral Red changes between 6.8 and 8, suggesting it would be more
accurate.
Which would be better to use?
|
|
|
not_important
International Hazard
Posts: 3873
Registered: 21-7-2006
Member Is Offline
Mood: No Mood
|
|
H2SO4 has two protons, the titration end point will depend on if you intent to titrate to bisulfate or sulfate. Ammonium sulfate when dilute has a pH
around 5.5 or so, the bisulfate obviously is lower.
|
|
|
crazyboy
Hazard to Others
Posts: 436
Registered: 31-1-2008
Member Is Offline
Mood: Marginally insane
|
|
Does anyone have experience using aqueous sodium metabisulfite to remove free iodine from compounds? I know sodium thiosulfate is often used for this
purpose but I don't have any so I was wondering if I could use sodium metabisulfite. I tested it by several milliliters of aqueous sodium
metabisulfite to some methanol with a pellet of iodine and it completely neutralized the color. Is there any reason why it would be a poor choice?
On a separate note, can welding gas be used as an inert gas in reactions of it is comprised of 75% argon 25% CO2? I am most concerned about the CO2, I
realize I *might* be able to scrub it with NaOH or KOH but is this necessary?
[Edited on 4-10-2010 by crazyboy]
|
|
|
smuv
National Hazard
Posts: 842
Registered: 2-5-2007
Member Is Offline
Mood: Jingoistic
|
|
Oxygen Tanks
Will welding gas suppliers fill rusty oxygen tanks? Pic of tanks in question attached.
@crazyboy: metabisulfite will work fine. About the inert gas, CO2 really limits the reactions that you can use the inert gas for. It seems you have
overcome the hurdle of obtaining a regulator and tank, can you not find a place that will fill with N2? As i recall both use the same regulator.
[Edited on 10-4-2010 by smuv]
"Titanium tetrachloride…You sly temptress." --Walter Bishop
|
|
|
Rogeryermaw
National Hazard
Posts: 656
Registered: 18-8-2010
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by smuv  | Will welding gas suppliers fill rusty oxygen tanks? Pic of tanks in question attached.
[Edited on 10-4-2010 by smuv] |
in my experience they will fill a tank as long as it is certified and within the certification date barring any obvious physical damage.
|
|
|
watson.fawkes
International Hazard
Posts: 2793
Registered: 16-8-2008
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by Rogeryermaw | | in my experience they will fill a tank as long as it is certified and within the certification date barring any obvious physical damage.
|
Agreed. I want to add that there do exist companies that will do hydrostatic tests on privately-owned
cylinders. Mostly this is done in-house by the big gas suppliers (e.g. Praxair), but they don't have a completely exclusive lock on that service.
|
|
|
crazyboy
Hazard to Others
Posts: 436
Registered: 31-1-2008
Member Is Offline
Mood: Marginally insane
|
|
| Quote: Originally posted by smuv |
It seems you have overcome the hurdle of obtaining a regulator and tank, can you not find a place that will fill with N2? As i recall both use the
same regulator.
[Edited on 10-4-2010 by smuv] |
Unfortunately, no. The tank contains shielding gas for welding, and while I could get it filled with pure nitrogen or argon, I wouldn't be able to use
it for welding.
|
|
|
Sedit
International Hazard
Posts: 1939
Registered: 23-11-2008
Member Is Offline
Mood: Manic Expressive
|
|
Sorry this isn't chemistry related but I didn't know where else to place it and did not want to start a new thread.
Does anyone have a good link for old newspapers?
I wish to read a few from the day of my birth but haven't come across anyplace that has them online yet, so if you know of any online microfilm so to
speak could you shoot me a link please, Thanks.
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
|
|
|
mewrox99
Hazard to Others
Posts: 321
Registered: 7-6-2010
Location: New Zealand
Member Is Offline
Mood: No Mood
|
|
Silly question. Is it possible to make hexamine perchlorate from hexamine and NH4ClO4
|
|
|
smuv
National Hazard
Posts: 842
Registered: 2-5-2007
Member Is Offline
Mood: Jingoistic
|
|
| Quote: Originally posted by crazyboy |
Unfortunately, no. The tank contains shielding gas for welding, and while I could get it filled with pure nitrogen or argon, I wouldn't be able to use
it for welding. |
I know welding gas suppliers sell argon/helium mixes. If you can use this for the welding you do and chemistry, it would be a good compromise, but
filling the tank will be a bit more expensive.
"Titanium tetrachloride…You sly temptress." --Walter Bishop
|
|
|
mnick12
Hazard to Others
Posts: 404
Registered: 30-12-2009
Location: In the lab w/ Dr. Evil
Member Is Offline
Mood: devious
|
|
Does anyone know if 5-hydroxyvanillin has a distinct odor?
The reason why I ask is I attempted the hydrolysis of 5-bromovanillin and the end product which is crystallizing from ethyl acetate has an odor
similar to vanillin (which it is contaminated with).
So after crystallizing from ethyl acetate the suppose-ed hydroxyvanillin was removed from the flask and placed into a small glass dish, the flask was
rinsed with 2x5ml of dcm which was then poured into the glass dish. Only some of the material dissolved in the dcm. Next I waited for the dcm to
evaporate, and I was rewarded with two distinct crystalline masses. The first being flaky cream colored crystals which seemed to be less soluble in
dcm, and the second being sticky yellow crystals which were stuck to the side of the dish. The odor is a pleasant one kind of like a cross between
vanilla and bubblegum.The mass of the two combine was 1.83gr from 2.00gr of bromovanillin
thanks
[Edited on 6-10-2010 by mnick12]
|
|
|
Pope
Harmless
Posts: 10
Registered: 14-10-2009
Member Is Offline
Mood: No Mood
|
|
How would one approach trying to separate an azeotropic mixture of Toluene/Methyl Ethyl Ketone, my goal is to completely separate and purify the
existing Toluene.
The components exist as - 430g Toluene: 410g MEK.
Thank you for your assistance, I have tried the search engine with little success.
|
|
|
woelen
Super Administrator
Posts: 7977
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
Is hexamine a stronger
base than NH3? I don't think so. So, I do not expect this to work. The only thing is that NH3 is a gas and that may be advantageous for you, but I
definitely do not expect a smooth reaction in which hexamine reacts with NH4ClO4 while NH3 escapes from the mix.
Something you could try is making the sulfate salt of hexamine (does that work, I don't know, try it) and mix a solution of that with a solution of
NH4ClO4. Many perchlorates of large cations have low solubility and could be precipitated out.
All of what I have written above is not well-proven, it is just some educated guessing, but you could give it a try.
|
|
|
mewrox99
Hazard to Others
Posts: 321
Registered: 7-6-2010
Location: New Zealand
Member Is Offline
Mood: No Mood
|
|
Found an ancient thread from 2002. This guy mixes HCl with NH4ClO4 and reacts hexamine with it. A precipitate forms that is highly flammable.
|
|
|
mnick12
Hazard to Others
Posts: 404
Registered: 30-12-2009
Location: In the lab w/ Dr. Evil
Member Is Offline
Mood: devious
|
|
Yeah I have made the suppose-ed hexamine perchlorate, when I made it was a fluffy white material which upon contact with fire burned with a luminous
blue-ish flame. The smoke was rather nasty lots HCl, and kinda stinky. I did this a few years ago and if I remember correctly I used NaClO4 and HCl to
generate perchloric acid, but I'm not sure it could have been NH4ClO4 and HNO3. I also made urea perchlorate in a similar manner its kinda boring
stuff, in my opionion it is about as interesting as urea nitrate.
|
|
|
Sedit
International Hazard
Posts: 1939
Registered: 23-11-2008
Member Is Offline
Mood: Manic Expressive
|
|
| Quote: Originally posted by Pope | How would one approach trying to separate an azeotropic mixture of Toluene/Methyl Ethyl Ketone, my goal is to completely separate and purify the
existing Toluene.
The components exist as - 430g Toluene: 410g MEK.
Thank you for your assistance, I have tried the search engine with little success. |
Sodium Metabisulfite will form a complex precipitating the MEK as an adduct. Repeated washes of the MeBn with Bisulfite solution should clear up your
problem.
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
|
|
|
dann2
International Hazard
Posts: 1523
Registered: 31-1-2007
Member Is Offline
Mood: No Mood
|
|
Hello,
Can anyone tell me how to make Aqua Regia.
I have been unable to find a definate answer with some saying it is 3:1 molar or 4:1 by weigh of 'concentrated' HCl and 'concentrate' Nitric acid.
They never specify what concentrated Nitric means and I gather it means the 70% stuff and not the 100% stuff. Also when moles of 'concentrate' HCl
are being referred to does it mean actual moles of HCl (one mole = 36.45 grams) and you must use the appropriate amount of 36% solution-in-water of
HCl or do you go with one mole of the actual solution in water (molecular weight I will have to figure out.
What ratio (by weight or volume) of 70% Nitric acid 37% Hydrochloric acid?
Or do you need 100% Nitric acid?
TIA,
Dann2
|
|
|
Picric-A
National Hazard
Posts: 796
Registered: 1-5-2008
Location: England
Member Is Offline
Mood: Fuming
|
|
| Quote: Originally posted by dann2 | Hello,
Can anyone tell me how to make Aqua Regia.
I have been unable to find a definate answer with some saying it is 3:1 molar or 4:1 by weigh of 'concentrated' HCl and 'concentrate' Nitric acid.
They never specify what concentrated Nitric means and I gather it means the 70% stuff and not the 100% stuff. Also when moles of 'concentrate' HCl
are being referred to does it mean actual moles of HCl (one mole = 36.45 grams) and you must use the appropriate amount of 36% solution-in-water of
HCl or do you go with one mole of the actual solution in water (molecular weight I will have to figure out.
What ratio (by weight or volume) of 70% Nitric acid 37% Hydrochloric acid?
Or do you need 100% Nitric acid?
TIA,
Dann2 |
Aqua Regia does not need to be made perfectly, any mix of conc nitric and hydrochloric acids will dissolve Au and Pt to some extent.
The perfect mix, as you say however, is 3:1, conc (36%) HCl to conc Nitric (70%) and the ratio is done by the solution in water, nothing to do with
moles, eg, 30ml HCl:10ml Nitric.
[Edited on 8-10-2010 by Picric-A]
|
|
|
dann2
International Hazard
Posts: 1523
Registered: 31-1-2007
Member Is Offline
Mood: No Mood
|
|
Thanks for reply.
I am dissolving Bismuth to make BiCl3:2H2O
Simply dissolve Bi metal and evaporate to obtain BiCl3.
Is it fair to assum that all Nitrate will evaporate (go away) and leave the Chloride?
Thats why I though I might need to get the ratio (of HCl to Nitric) close to correct.
Dann2
|
|
|
Picric-A
National Hazard
Posts: 796
Registered: 1-5-2008
Location: England
Member Is Offline
Mood: Fuming
|
|
| Quote: Originally posted by dann2 | Thanks for reply.
I am dissolving Bismuth to make BiCl3:2H2O
Simply dissolve Bi metal and evaporate to obtain BiCl3.
Is it fair to assum that all Nitrate will evaporate (go away) and leave the Chloride?
Thats why I though I might need to get the ratio (of HCl to Nitric) close to correct.
Dann2 |
As long as you keep to the 3:1 ratio (maybe add a little bit extra HCl to be sure) no nitrate will form as it is completly consumed according to;
HNO3 + 3 HCl → NOCl + 2 H2O + Cl2
You will only be left with the chloride.
|
|
|
solo
International Hazard
Posts: 3967
Registered: 9-12-2002
Location: Estados Unidos de La Republica Mexicana
Member Is Offline
Mood: ....getting old and drowning in a sea of knowledge
|
|
what is this compound called without the double bond between c1-c2
alpha-methyl cinnamaldehyde
Uploaded with ImageShack.us
[Edited on 13-10-2010 by solo]
It's better to die on your feet, than live on your knees....Emiliano Zapata.
|
|
|
| Pages:
1
2
3
4
5
6
..
30 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
