Anthranilic acid

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Anthranilic acid
Skeletal formula of anthranilic acid
Ball-and-stick model of the anthranilic acid molecule
Preferred IUPAC name
2-Aminobenzoic acid[1]
Systematic IUPAC name
2-Aminobenzenecarboxylic acid
Other names
  • Anthranilic acid
  • o-Aminobenzoic acid
  • 2-Aminobenzoic acid
  • Vitamin L1
  • Anthranilate (conjugate base)
3D model (JSmol)
ECHA InfoCard 100.003.898
EC Number
  • 204-287-5
RTECS number
  • CB2450000
Molar mass 137.138 g·mol−1
Appearance white or yellow solid
Odor odorless
Density 1.412 g/cm3
Melting point 146 to 148 °C (295 to 298 °F; 419 to 421 K)[3]
Boiling point 200 °C (392 °F; 473 K) (sublimes)
0.572 g/100 mL (25 °C)
Solubility very soluble in chloroform, pyridine
soluble in ethanol, ether, ethyl ether
slightly soluble in trifluoroacetic acid, benzene
log P 1.21
Vapor pressure 0.1 Pa (52.6 °C)
Acidity (pKa)
  • 2.17 (carboxyl; H2O)
  • 4.85 (amino; H2O)[2]
-77.18·10−6 cm3/mol
1.578 (144 °C)
-380.4 KJ/mol
Safety data sheet External MSDS
GHS pictograms GHS05: CorrosiveGHS07: Harmful
GHS Signal word Danger
H318, H319
P264, P280, P305+351+338, P310, P337+313
NFPA 704 (fire diamond)
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
Flash point > 150 °C (302 °F; 423 K)
> 530 °C (986 °F; 803 K)
Lethal dose or concentration (LD, LC):
1400 mg/kg (oral, rat)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Anthranilic acid (o-aminobenzoic acid, 2-aminobenzoic acid, 2-AA, 2AA, AA)[4][5] is an aromatic acid with the formula C6H4(NH2)(CO2H) and has a sweetish taste.[6] The molecule consists of a benzene ring, ortho-substituted with a carboxylic acid and an amine. As a result of containing both acidic and basic functional groups, the compound is amphoteric. Anthranilic acid is a white solid when pure, although commercial samples may appear yellow. The anion [C6H4(NH2)(CO2)], obtained by the deprotonation of anthranilic acid, is called anthranilate. Anthranilic acid was once thought to be a vitamin and was referred to as vitamin L1 in that context, but it is now known to be non-essential in human nutrition.[7]


Although not usually referred to as such, it is an amino acid. Solid anthranilic acid consists of both the amino-carboxylic acid and the zwitterionic ammonium carboxylate forms.[8]


Many routes to anthranilic acid have been described. Industrially it is produced from phthalic anhydride, beginning with amination:

C6H4(CO)2O + NH3 + NaOH → C6H4(C(O)NH2)CO2Na + H2O

The resulting sodium salt of phthalamic acid is decarbonylated via a Hofmann rearrangement of the amide group, induced by hypochlorite:[9]

C6H4(C(O)NH2)CO2Na + HOCl → C6H4NH2CO2H + NaCl + CO2

A related method involves treating phthalimide with sodium hypobromite in aqueous sodium hydroxide, followed by neutralization.[10] In the era when indigo dye was obtained from plants, it was degraded to give anthranilic acid.

Anthranilic acid was first obtained by base-induced degradation of indigo.[11]


Anthranilic acid is biosynthesized from chorismic acid. It is the precursor to the amino acid tryptophan via the attachment of phosphoribosyl pyrophosphate to the amine group.

Anthranilate is the biosynthetic precursor to the amino acid tryptophan.


Industrially, anthranilic acid is an intermediate in the production of azo dyes and saccharin. It and its esters are used in preparing perfumes to mimic jasmine and orange, pharmaceuticals (loop diuretics, such as furosemide) and UV-absorber as well as corrosion inhibitors for metals and mold inhibitors in soy sauce.

Anthranilic acid can be used in organic synthesis to generate benzyne,[12] which can undergo various reactions, including a rapid dimerization to form biphenylene. It reacts with phosgene to give isatoic anhydride, a versatile reagent.[13]

Chlorination of anthranilic acid gives the 2,4-dichloro derivative.[14]

Anthranilate-based insect repellents have been proposed as replacements for DEET.

Fenamic acid is a derivative of anthranilic acid,[15]:235 which in turn is a nitrogen isostere of salicylic acid, which is the active metabolite of aspirin.[15]:235 Several non-steroidal anti-inflammatory drugs, including mefenamic acid, tolfenamic acid, flufenamic acid, and meclofenamic acid are derived from fenamic acid or anthranilic acid and are called "anthranilic acid derivatives" or "fenamates".[16]:17

Otto Eisleb patented some agents that are excellent local anesthetics: U.S. Patent 2,073,099 and considerably stronger than analogous agents of the para-series (according to the patent).

Safety and regulation[edit]

It is also a DEA List I Chemical because of its use in making the now-widely outlawed euphoric sedative drug methaqualone (Quaalude, Mandrax).[17]

See also[edit]


  1. ^ "Front Matter". Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 748. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4.
  2. ^ Haynes, William M., ed. (2016). CRC Handbook of Chemistry and Physics (97th ed.). CRC Press. pp. 5–89. ISBN 978-1498754286.
  3. ^ IPCS
  4. ^ Acton, Q. Ashton (2013). Aminobenzoic Acids—Advances in Research and Application (2013 ed.). Atlanta: ScholarlyEditions. p. 23. ISBN 9781481684842 – via Google Books.
  5. ^ Hardy, Mark R. (1997). "Glycan Labeling with the Flurophores 2-Aminobenzamide and Antranilic Acid". In Townsend, R. Reid; Hotchkiss, Jr., Arland T. (eds.). Techniques in Glycobiology. Marcel Dekker, Inc. p. 360. ISBN 9780824798222 – via Google Books.
  6. ^ The Merck Index, 10th Ed. (1983), p.62., Rahway: Merck & Co.
  7. ^ Davidson, Michael W. (2004). "Anthranilic Acid (Vitamin L)]". Florida State University. Retrieved November 20, 2019.
  8. ^ Brown, C. J. (1968). "The crystal structure of anthranilic acid". Proceedings of the Royal Society of London. Series A. Mathematical and Physical Sciences. 302 (1469): 185–199. Bibcode:1968RSPSA.302..185B. doi:10.1098/rspa.1968.0003.
  9. ^ Maki, Takao; Takeda, Kazuo (2000). "Benzoic Acid and Derivatives". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a03_555. ISBN 3527306730..
  10. ^ Vogel's Textbook of Practical Organic Chemistry, 4th Ed., (B. S. Furniss et al., Eds.) (1978), p.666, London: Longman.
  11. ^ Sheibley, Fred E. (1943). "Carl Julius Fritzsche and the discovery of anthranilic acid, 1841". Journal of Chemical Education. 20 (3): 115. Bibcode:1943JChEd..20..115S. doi:10.1021/ed020p115.
  12. ^ Logullo, F. M.; Seitz, A. H.; Friedman, L. (1973). "Benzenediazonium-2-carboxy- and Biphenylene". Organic Syntheses.; Collective Volume, 5, p. 54
  13. ^ Wagner, E. C.; Fegley, Marion F. (1947). "Isatoic anhydride". Organic Syntheses. 27: 45.
  14. ^ Atkinson, Edward R.; Murphy, Donald M.; Lufkin, James E. (1951). "dl-4,4',6,6'-Tetrachlorodiphenic Acid". Organic Syntheses. 31: 96.
  15. ^ a b Sriram D, Yogeeswari P. Medicinal Chemistry, 2nd Edition. Pearson Education India, 2010. ISBN 9788131731444
  16. ^ Auburn University course material. Jack DeRuiter, Principles of Drug Action 2, Fall 2002 1: Non-Steroidal Antiinflammatory Drugs (NSAIDS)
  17. ^ Angelos SA, Meyers JA (1985). "The isolation and identification of precursors and reaction products in the clandestine manufacture of methaqualone and mecloqualone". Journal of Forensic Sciences. 30 (4): 1022–1047. PMID 3840834.