rokaro
Harmless
Posts: 3
Registered: 23-1-2004
Member Is Offline
Mood: No Mood
|
|
NH2Cl
Many are saying that you can form chloramine (NH2Cl) by reacting bleach with ammonia solution. Did anyone actually see it done or reported in serous
literature? Is the reaction occuring between vapors of NaOCl (Cl2 and H2O) and ammonia solution (NH3 and H2O) or in the aqueous phase ?
|
|
|
BromicAcid
International Hazard
Posts: 3245
Registered: 13-7-2003
Location: Wisconsin
Member Is Offline
Mood: Rock n' Roll
|
|
As far as I know that is believed to be one of the reaction intermediates in the formation of hydrazine from sodium hypochlorite and ammonia.
However, I don't think it can be isolated in this way, and even its role as a reaction intermediate in this reaction has been called into
question in recent time. Because although the reaction of NH2Cl with other chems can produce hydrazine, the actual amount of NH2Cl present in the
solution at any time is significantly smaller then should be expected, measured via spectroscopical data.
NaOCl is very unstable beyond the hexahydrate and therefore the reaction in a vapor phase is somewhat out of the question, usually the reaction of
sodium hyprochlorite and ammonia is preformed in aqueous solution. I believe chloroamine is formed by the reaction of gaseous ammonia with chlorine
at slightly elevated temperatures and pressures.
|
|
|
DDTea
National Hazard
Posts: 940
Registered: 25-2-2003
Location: Freedomland
Member Is Offline
Mood: Degenerate
|
|
I have made n-Chloramine by this route before. I can't say whether it was monochloramine or dichloramine, though. It does have a
"unique" smell however, different from that of Chlorine. Chlorine has a much more irritating odor, while Chloramine doesn't hurt much
too breathe (though I don't imagine it is very good for you). I can't sit here and tell you the quality of the product, however, because I
simply don't know.
|
|
|
Marvin
National Hazard
Posts: 995
Registered: 13-10-2002
Member Is Offline
Mood: No Mood
|
|
Equimolar solutions of ammonia and faintly alkaline hyperchlorite will go to chloramine rapidly and almost quantativly in the cold. Its stable for
fairly long periods.
|
|
|
Haggis
Hazard to Others
Posts: 238
Registered: 1-12-2002
Location: Mid-America.
Member Is Offline
Mood: Lacrymating
|
|
If I can remember, there is also, in some instances, hydrazine, and nitrogen trichloride formed as well as some others, however I do not remember the
situations in which these products are formed.
Chloramine is a cheaply and easily produced poisonous gas, although the latter quality is not very effective. It's simply the damage that it
does to lung tissue that makes it poisonous. Does anyone know what the hydrolysis products are?
I've had fleeting ideas about producing chloramine, then condensing the gas down using a dry ice/ acetone cooling mixture or the like to a
liquid, but realized I would have no where to store it, because the gas would more than likely leak out over time. Oh well.
Great ideas often receive violent opposition from mediocre minds.
<b> <a href=\"http://pgp.mit.edu:11371/pks/lookup?op=get&search=0xEE41A2B1\">PGP Key</a> </b> 0C0A 7486 B97F
92EE AE50 A98C A4F3 087E 8CE9 A782 |
|
|
Pyrovus
Hazard to Others
Posts: 241
Registered: 13-10-2003
Location: Australia, now with 25% faster carrier pigeons
Member Is Offline
Mood: heretical
|
|
I remember hearing that chloramine also is a suspected carcinogen!
|
|
|
Marvin
National Hazard
Posts: 995
Registered: 13-10-2002
Member Is Offline
Mood: No Mood
|
|
If hyperchlorite is in excess (more than about twice) and the solution acid enough, nitrogen trichloride can form.
If ammonia is in excess hydrazine can form but this is a slow reaction. With normal amounts of impurities this will mostly give off nitrogen gas
instead.
Keep the molar ratios the same, and you get chloramine in solution.
|
|
|
cyclonite4
Hazard to Others
Posts: 480
Registered: 16-11-2004
Location: is unknown
Member Is Offline
Mood: Amphoteric
|
|
It hydrolizes into Cl2, NH3, and Oxygen radicals in the lungs.
Here is some info from Wikipedia: http://en.wikipedia.org/wiki/Chloramine
I was actually looking for info on Ammonium Persulfate, and came by this wikipedia information, and then decided to search the forum to see if it had
any threads on chloramine to match info givien by wikipedia.
Apparently its also used for water purification, which gives me concerns about drinking tap water, because it is a supspected carcinogen.
\"It is dangerous to be right, when your government is wrong.\" - Voltaire
|
|
|
Theoretic
National Hazard
Posts: 776
Registered: 17-6-2003
Location: London, the Land of Sun, Summer and Snow
Member Is Offline
Mood: eating the souls of dust mites
|
|
"It hydrolizes into Cl2, NH3, and Oxygen radicals in the lungs."
It doesn't do that straight away, first it's NH2Cl + H2O <=> NH3 + HClO, then HClO shatters into a HCl molecule and an oxygen atom
(slowly, faster in sunlight, also disproportionates to HCl and HClO3), then HCl reacts with more HClO to foprm water and chlorine. Therefore, apart
from the things you said there's also the damaging action of HCl and HClO.
Chloramine is formed like this: NH3 + ClO- => NH2Cl + OH-.
|
|
|
gorkem
Harmless
Posts: 6
Registered: 20-12-2004
Member Is Offline
Mood: gorkem
|
|
NH2Cl+H2O
NH2Cl+H2O ----) NH3+ClO because it has amfoterik special.
|
|
|
cyclonite4
Hazard to Others
Posts: 480
Registered: 16-11-2004
Location: is unknown
Member Is Offline
Mood: Amphoteric
|
|
It's spelt "Amphoteric" 
\"It is dangerous to be right, when your government is wrong.\" - Voltaire
|
|
|
Theoretic
National Hazard
Posts: 776
Registered: 17-6-2003
Location: London, the Land of Sun, Summer and Snow
Member Is Offline
Mood: eating the souls of dust mites
|
|
"NH2Cl+H2O ----) NH3+ClO because it has amfoterik special."
1) It's NH2Cl + H2O <=> NH3 + HClO <=> NH4ClO, not NH2Cl+H2O ----) NH3+ClO (ClO is a radical)
2) Who has "amfoterik special"?
3) What is "amfoterik special"?
[Edited on 25-12-2004 by Theoretic]
|
|
|
Madandcrazy
Hazard to Others
Posts: 117
Registered: 11-5-2005
Member Is Offline
Mood: annoyed
|
|
I know chloroamin is soluble in H2O.
Eventually it is suitable for substitution or a further syntheses when it treated with HCl or Cl2 (Br2) in a closed vessel to nitrogentrichloride if it exist.
ClNH2 -->
Cl2NH -->
Cl3N
Interested to this, is chloroamin producible in low yield when
HCl is added to NH4OH solution and this is heated and the H2O is than evaporated ?
[Edited on 20-5-2006 by Madandcrazy]
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
