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Aniline
Aniline Aniline
General
Other names	Phenylamine Aminobenzene
Molecular formula	C6H7N
SMILES	NC1=CC=CC=C1
InChI	InChI=1/C6H7N/c7-6-4- 2-1-3-5-6/h1-5H,7H2
Molar mass	93.126 g/mol
Appearance	colorless liquid
CAS number	[62-53-3]
Properties
Density and phase	1.0217 g/ml, liquid
Solubility in water	3.6 g/100 mL at 20°C
Solubility in ethanol, acetone	Miscible
Melting point	−6.3 °C
Boiling point	184.13 °C
Basicity (p''K''b)	9.40
Viscosity	3.71 cP at 25 °C
Thermodynamic data
Standard enthalpy of formation Δf''H''oliquid	? kJ/mol
Standard enthalpy of combustion Δc''H''oliquid	-3394 kJ/mol
Standard molar entropy ''S''oliquid	? J.K−1.mol−1
Hazards
MSDS	External MSDS
EU classification	Toxic ('T') Carc. Cat. 3 Muta. Cat. 3 Dangerous for the environment ('N')
NFPA 704
R-phrases	, , , , , ,
S-phrases	, , , , , , ,
Supplementary data page
Structure and properties	''n'', ''εr'', etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Regulatory data	Flash point, RTECS number, etc.
Related compounds
Related aromatic amines	1-Naphthylamine 2-Naphthylamine
Related compounds	Phenylhydrazine Nitrosobenzene Nitrobenzene
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

'Aniline', 'phenylamine' or 'aminobenzene' is an organic compound with the formula C₆H₅NH₂. It is an organic chemical compound, specifically an aryl amine, consisting of a phenyl group attached to an amino group. The chemical structure of aniline is shown at the right. It is now used mainly in the manufacture of polyurethane, although it previously was mainly used more for dyes and drugs.

Contents

Production

Properties

Uses

History

Toxicology

References

External links

Production

Aniline is produced industrially in two steps from benzene:

First, benzene is heated with a concentrated mixture of nitric acid and sulfuric acid at 50 - 60 °C, where one hydrogen atom is displaced to give nitrobenzene. In this nitration reaction, nitric acid first reacts with sulfuric acid giving the electrophile ⁺NO₂ which is attracted towards the π-electron cloud of benzene. The ⁺NO₂ electrophile attacks the carbon atom, displacing a proton H⁺ from that particular carbon atom. Nitration is thus called an electrophilic substitution reaction.
Now a mixture of hydrogen gas and nitrobenzene vapors are heated at 600 °C in presence of a nickel catalyst. This gives aniline by reduction. Aniline obtained here is in the pure state.
Many derivatives of aniline can be prepared similarly. In commerce three brands of aniline are distinguished—aniline oil for blue, which is pure aniline; aniline oil for red, a mixture of equimolecular quantities of aniline and ortho- and para-toluidines; and aniline oil for safranine, which contains aniline and ortho-toluidine, and is obtained from the distillate (échappés) of the fuchsine fusion. Monomethyl and dimethyl aniline are colourless liquids prepared by heating aniline, aniline hydro-chloride and methyl alcohol in an autoclave at 220 °C. They are of great importance in the colour industry. Monomethyl aniline boils at 193-195 °C, dimethyl aniline at 192 °C.

Properties

Aniline is oily and, although colourless, it slowly oxidizes and resinifies in air, giving the sample a red-brown tint.
Like most volatile amines, it possesses a somewhat unpleasant odour of rotten fish, and also has a burning aromatic taste; it is a highly poison. It ignites readily, burning with a smoky flame.
Chemically, aniline is a weak base. Aromatic amines such as aniline are generally much weaker bases than aliphatic amines. Aniline reacts with strong acids to form 'anilinium' (or phenylammonium) ion (C₆H₅-NH₃⁺), and reacts with acyl halides such as acetyl chloride to form amides. The amides formed from aniline are sometimes called '''anilides''', for example CH₃-CO-NH-C₆H₅ is acetanilide.
The sulfate forms beautiful white plates. Although aniline is weakly basic, it precipitates zinc, aluminium and ferric salts, and on warming expels ammonia from its salts. Aniline combines directly with alkyl iodides to form secondary and tertiary amines. Boiled with carbon disulfide, it gives sulfocarbanilide (diphenyl thiourea), CS(NHC₆H₅)₂, which may be decomposed into phenyl isothiocyanate, C₆H₅CNS, and triphenyl guanidine, C₆H₅N=C(NHC₆H₅)₂. Reaction with sulfuric acid at 180° C produces sulfanilic acid, NH₂C₆H₄SO₃H. Anilides, compounds in which the amino group is substituted by an acid radical, are prepared by heating aniline with certain acids; antifebrin or acetanilide is thus obtained from acetic acid and aniline. The oxidation of aniline has been carefully investigated. In alkaline solution azobenzene results, while arsenic acid produces the
violet-colouring matter violaniline. Chromic acid converts it into quinone, while chlorates, in the presence of certain metallic salts (especially of vanadium), give aniline black. Hydrochloric acid and potassium chlorate give chloranil. Potassium permanganate in neutral solution oxidizes it to nitrobenzene, in alkaline solution to azobenzene, ammonia and oxalic acid, in acid solution to aniline black. Hypochlorous acid gives 4-aminophenol and para-amino diphenylamine.
Like phenols, aniline derivatives are highly susceptible to electrophilic substitution reactions. For example, sulfonation of aniline produces sulfanilic acid, which can be converted to sulfanilamide. Sulfanilamide is one of the sulfa drugs which were widely used as antibacterials in the early 20th century.
Aniline and its ring-substituted derivatives react with nitrous acid to form diazonium salts. Through these, the -NH₂ group of aniline can be conveniently converted to -OH, -CN, or a halide via Sandmeyer reactions.
It reacts with nitrobenzene to produce phenazine in the Wohl-Aue reaction.

Uses

Originally the great commercial value of aniline was due to the readiness with which it yields, directly or indirectly, valuable dyestuffs. The discovery of mauve in 1856 by William Henry Perkin was the first of a series of dyestuffs which are now to be numbered by hundreds. Reference should be made to the articles dyeing, fuchsine, safranine, indulines, for more details on this subject. In addition to its use as a precursor to dyestuffs, it is a starting-product for the manufacture of many drugs such as paracetamol (acetaminophen, Tylenol).
It is used to stain neural RNA blue in the Nissl stain.
Currently the largest market for aniline is preparation of methylene diphenyl diisocyanate (MDI), some 85% of aniline serving this market. Other uses include rubber processing chemicals (9%), herbicides (2%), and dyes and pigments (2%). ^[1]

History

Aniline was first isolated from the destructive distillation of indigo in 1826 by Otto Unverdorben (''Pogg. Ann.'', 1826, 8, p. 397), who named it crystalline. In 1834, Friedrich Runge (''Pogg. Ann.'', 1834, 31, p. 65; 32, p. 331) isolated from coal tar a substance which produced a beautiful blue colour on treatment with chloride of lime; this he named kyanol or cyanol. In 1841, C. J. Fritzsche showed that by treating indigo with caustic potash it yielded an oil, which he named aniline, from the specific name of one of the indigo-yielding plants, ''Indigofera anil'', anil being derived from the Sanskrit ''nīla'', dark-blue, and ''nīlā'', the indigo plant. About the same time N. N. Zinin found that on reducing nitrobenzene, a base was formed which he named benzidam. August Wilhelm von Hofmann investigated these variously prepared substances, and proved them to be identical (1855), and thenceforth they took their place as one body, under the name aniline or phenylamine.
Its first industrial-scale use was in the manufacture of mauveine, a purple dye discovered in 1856 by William Henry Perkin.
p-Toluidine, an aniline derivative, can be used in qualitative analysis to prepare carboxylic acid derivatives.

Toxicology

Aniline is toxic by inhalation of the vapour, absorption through the skin or swallowing. It causes headache, drowsiness, cyanosis, mental confusion and in severe cases can cause convulsions. Prolonged exposure to the vapour or slight skin exposure over a period of time affects the nervous system and the blood, causing tiredness, loss of appetite, headache and dizziness.^[2]
Oil mixtures containing rapeseed oil denatured with aniline have been clearly linked by epidemiological and analytic chemical studies to the toxic oil syndrome that hit Spain in the spring and summer of 1981, in which 20,000 became acutely ill, 12,000 were hospitalized, and more than 350 died in the first year of the epidemic. The precise etiology though remains unknown.
Some authorities class aniline as a carcinogen, although the IARC lists it in Group 3 (''not classifiable as to its carcinogenicity to humans'') due to the limited and contradictory data available.

References

1. ''Aniline producers price capacity market demand consumption production growth uses outlook'' n.d., The Chemical Market Reporter, Schnell Publishing Company. Retrieved January 12, 2002 from http://www.the-innovation-group.com/ChemProfiles/Aniline.htm
2. Muir, GD (ed.) 1971, ''Hazards in the Chemical Laboratory'', The Royal Institute of Chemistry, London.

External links

★ International Chemical Safety Card 0011

★ Computational Chemistry Wiki entry

★ Aniline electropolymerisation