4-Nitroaniline - Misplaced Pages

InChI=1S/C6H6N2O2/c7-5-1-3-6(4-2-5)8(9)10/h1-4H,7H2Key: TYMLOMAKGOJONV-UHFFFAOYSA-N
InChI=1/C6H6N2O2/c7-5-1-3-6(4-2-5)8(9)10/h1-4H,7H2Key: TYMLOMAKGOJONV-UHFFFAOYAW

SMILES

c1cc(ccc1N)N(=O)=O

Properties

Chemical formula

C₆H₆N₂O₂

Molar mass

138.12 g/mol

Appearance

yellow or brown powder

Odor

faint, ammonia-like

Density

1.437 g/ml, solid

Melting point

146 to 149 °C (295 to 300 °F; 419 to 422 K) (lit.)

Boiling point

332 °C (630 °F; 605 K)

Solubility in water

0.8 mg/ml at 18.5 °C (IPCS)

Vapor pressure

0.00002 mmHg (20°C)

Magnetic susceptibility (χ)

-66.43·10 cm/mol

Hazards

Occupational safety and health (OHS/OSH):

Main hazards

Toxic

GHS labelling:

Pictograms

Signal word

Warning

Hazard statements

H301, H311, H331, H373, H412

Precautionary statements

P260, P261, P264, P270, P271, P273, P280, P301+P310, P302+P352, P304+P340, P311, P312, P314, P321, P322, P330, P361, P363, P403+P233, P405, P501

NFPA 704 (fire diamond)

2 1 0

Flash point

199 °C (390 °F; 472 K)

Lethal dose or concentration (LD, LC):

LD₅₀ (median dose)

3249 mg/kg (rat, oral)
750 mg/kg (rat, oral)
450 mg/kg (guinea pig, oral)
810 mg/kg (mouse, oral)

NIOSH (US health exposure limits):

PEL (Permissible)

TWA 6 mg/m3 (1 ppm)

REL (Recommended)

TWA 3 mg/m

IDLH (Immediate danger)

300 mg/m

Safety data sheet (SDS)

JT Baker

Related compounds

2-Nitroaniline, 3-Nitroaniline

Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).

N verify (what is ?) Infobox references

Chemical compound

4-Nitroaniline, p-nitroaniline or 1-amino-4-nitrobenzene is an organic compound with the formula C₆H₆N₂O₂. A yellow solid, it is one of three isomers of nitroaniline. It is an intermediate in the production of dyes, antioxidants, pharmaceuticals, gasoline, gum inhibitors, poultry medicines, and as a corrosion inhibitor.

Synthesis

4-Nitroaniline is produced industrially via the amination of 4-nitrochlorobenzene:

ClC₆H₄NO₂ + 2 NH₃ → H₂NC₆H₄NO₂ + NH₄Cl

Below is a laboratory synthesis of 4-nitroaniline from aniline. The key step in this reaction sequence is an electrophilic aromatic substitution to install the nitro group para to the amino group. The amino group can be easily protonated and become a meta director. Therefore, a protection of the acetyl group is required. After this reaction, a separation must be performed to remove 2-nitroaniline, which is also formed in a small amount during the reaction.

Applications

4-Nitroaniline is mainly consumed industrially as a precursor to p-phenylenediamine, an important dye component. The reduction is effected using iron metal and by catalytic hydrogenation.

It is a starting material for the synthesis of Para Red, the first azo dye:

It is also a precursor to 2,6-dichloro-4-nitroaniline, also used in dyes.

Laboratory use

Nitroaniline undergoes diazotization, which allows access to 1,4-dinitrobenzene and nitrophenylarsonic acid. With phosgene, it converts to 4-nitrophenylisocyanate.

Carbon snake demonstration

When heated with sulfuric acid, it dehydrates and polymerizes explosively into a rigid foam.

In Carbon snake demo, paranitroaniline can be used instead of sugar, if the experiment is allowed to proceed under an obligatory fumehood. With this method the reaction phase prior to the black snake's appearance is longer, but once complete, the black snake itself rises from the container very rapidly. This reaction may cause an explosion if too much sulfuric acid is used.

Toxicity

The compound is toxic by way of inhalation, ingestion, and absorption, and should be handled with care. Its LD₅₀ in rats is 750.0 mg/kg when administered orally. 4-Nitroaniline is particularly harmful to all aquatic organisms, and can cause long-term damage to the environment if released as a pollutant.

References

^ NIOSH Pocket Guide to Chemical Hazards. "#0449". National Institute for Occupational Safety and Health (NIOSH).
"p-Nitroaniline". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
^ Booth, Gerald (2003-03-11). "Nitro Compounds, Aromatic". In Wiley-VCH (ed.). Ullmann's Encyclopedia of Industrial Chemistry (1 ed.). Wiley. doi:10.1002/14356007.a17_411. ISBN 978-3-527-30385-4.]
Mohrig, J.R.; Morrill, T.C.; Hammond, C.N.; Neckers, D.C. (1997). "Synthesis 5: Synthesis of the Dye Para Red from Aniline". Experimental Organic Chemistry. New York, NY: Freeman. pp. 456–467. Archived from the original on 2020-09-15. Retrieved 2007-07-18.
Williamson, Kenneth L. (2002). Macroscale and Microscale Organic Experiments, Fourth Edition. Houghton-Mifflin. ISBN 0-618-19702-8.
Starkey, E. B. (1939). "p-DINITROBENZENE". Organic Syntheses. 19: 40. doi:10.15227/orgsyn.019.0040.
Ruddy, A. Wayne; Starkey, Edgar B. (1946). "p-Nitrophenylarsonic Acid". Organic Syntheses. 26: 60. doi:10.15227/orgsyn.026.0060.
Shriner, R. L.; Horne, W. H.; Cox, R. F. B. (1934). "p-NITROPHENYL ISOCYANATE". Organic Syntheses. 14: 72. doi:10.15227/orgsyn.014.0072.
Sandin, R. B.; Drake, W. V.; Leger, Frank (1932). "2,6-Diiodo-p-Nitroaniline". Organic Syntheses. 12: 28. doi:10.15227/orgsyn.012.0028.
Poshkus, A. C.; Parker, J. A. (1970). "Studies on nitroaniline–sulfuric acid compositions: Aphrogenic pyrostats". Journal of Applied Polymer Science. 14 (8): 2049–2064. doi:10.1002/app.1970.070140813.
Summerlin, Lee R.; Ealy, James L. (1988). "Experiment 100: Dehydration of p-Nitroaniline: Sanke and Puff". Chemical Demonstrations: A Sourcebook for Teachers Volume 1 (2nd ed.). American Chemical Society. p. 171. ISBN 978-0-841-21481-1.
"Carbon Snake: demonstrating the dehydration power of concentrated sulfuric acid". communities.acs.org. 2013-06-06. Retrieved 2022-01-31.
Making a carbon snake with P-Nitroaniline, 7 April 2014, retrieved 2022-01-31
"4-Nitroaniline". St. Louis, Missouri: Sigma-Aldrich. December 18, 2020.

External links

Categories: