Picramide Synthesis Essay

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Names
Preferred IUPAC name
Other names

Picric acid[1]
Carbazotic acid
Phenol trinitrate
Picronitric acid
Trinitrophenol
2,4,6-Trinitro-1-phenol
2-Hydroxy-1,3,5-trinitrobenzene
TNP
Melinite

Identifiers

CAS Number

3D model (JSmol)

ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard100.001.696

PubChemCID

RTECS numberTJ7875000
UNII

InChI

  • InChI=1S/C6H3N3O7/c10-6-4(8(13)14)1-3(7(11)12)2-5(6)9(15)16/h1-2,10H Y
    Key: OXNIZHLAWKMVMX-UHFFFAOYSA-N Y
  • InChI=1/C6H3N3O7/c10-6-4(8(13)14)1-3(7(11)12)2-5(6)9(15)16/h1-2,10H

    Key: OXNIZHLAWKMVMX-UHFFFAOYAM

SMILES

  • O=[N+]([O-])c1cc(cc([N+]([O-])=O)c1O)[N+]([O-])=O

Properties

Chemical formula

C6H3N3O7
Molar mass229.10 g·mol−1
AppearanceColorless to yellow solid
Density1.763 g·cm−3, solid
Melting point122.5 °C (252.5 °F; 395.6 K)
Boiling point> 300 °C (572 °F; 573 K) Detonates

Solubility in water

12.7 g·L−1
Vapor pressure1 mmHg (195 °C)[2]
Acidity (pKa)0.38

Magnetic susceptibility (χ)

-84.34·10−6 cm3/mol
Hazards
Main hazardsexplosive

EU classification (DSD) (outdated)

TEF+
R-phrases(outdated)R1R4R11R23R24R25
S-phrases(outdated)S28S35S37S45
NFPA 704
Flash point150 °C; 302 °F; 423 K [2]
Lethal dose or concentration (LD, LC):

LDLo (lowest published)

100 mg/kg (guinea pig, oral)
250 mg/kg (cat, oral)
120 mg/kg (rabbit, oral)[3]
US health exposure limits (NIOSH):

PEL (Permissible)

TWA 0.1 mg/m3 [skin]

REL (Recommended)

TWA 0.1 mg/m3 ST 0.3 mg/m3 [skin][2]

IDLH (Immediate danger)

75 mg/m3[2]
Explosive data
Detonation velocity7,350 m·s−1 at ρ 1.70
RE factor1.20

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)
Infobox references

Picric acid is an organic compound with the formula (O2N)3C6H2OH. Its IUPAC name is 2,4,6-trinitrophenol (TNP). The name "picric" comes from the Greek πικρός (pikros), meaning "bitter", reflecting its bitter taste. It is one of the most acidicphenols. Like other highly nitrated organic compounds, picric acid is an explosive, which was once its primary use. It has also been used in medicine (antiseptic, burn treatments) and dyes.

History[edit]

Picric acid was probably first mentioned in the alchemical writings of Johann Rudolf Glauber in 1742. Initially, it was made by nitrating substances such as animal horn, silk, indigo, and natural resin, the synthesis from indigo first being performed by Peter Woulfe in 1771.[4] Its synthesis from phenol, and the correct determination of its formula, were successfully accomplished in 1841.[5] Not until 1830 did chemists think to use picric acid as an explosive. Before then, chemists assumed that only the salts of picric acid were explosive, not the acid itself. In 1871 Hermann Sprengel proved it could be detonated[6] and most military powers used picric acid as their main high explosive material. Picric acid is also used in the analytical chemistry of metals, ores, and minerals.

Picric acid was the first high explosive nitrated organic compound widely considered suitable to withstand the shock of firing in conventional artillery. Nitroglycerine and nitrocellulose (guncotton) were available earlier but shock sensitivity sometimes caused detonation in the artillery barrel at the time of firing. In 1885, based on research of Hermann Sprengel, French chemist Eugène Turpin patented the use of pressed and cast picric acid in blasting charges and artillery shells. In 1887 the French government adopted a mixture of picric acid and guncotton under the name Melinite. In 1888, Britain started manufacturing a very similar mixture in Lydd, Kent, under the name Lyddite. Japan followed with an "improved" formula known as shimose powder. In 1889, a similar material, a mixture of ammonium cresylate with trinitrocresol, or an ammonium salt of trinitrocresol, started to be manufactured under the name ecrasite in Austria-Hungary. By 1894 Russia was manufacturing artillery shells filled with picric acid. Ammonium picrate (known as Dunnite or explosive D) was used by the United States beginning in 1906. However, shells filled with picric acid become highly unstable if the compound reacts with metal shell or fuze casings to form metal picrates which are more sensitive than the parent phenol. The sensitivity of picric acid was demonstrated in the Halifax Explosion. Picric acid was used in the Battle of Omdurman,[7]Second Boer War,[8] the Russo-Japanese War,[9] and World War I.[10] Germany began filling artillery shells with TNT in 1902. Toluene was less readily available than phenol, and TNT is less powerful than picric acid, but improved safety of munitions manufacturing and storage caused replacement of picric acid by TNT for most military purposes between the World Wars.[7]

Efforts to control the availability of phenol, the precursor to picric acid, emphasize its importance in World War I. Germans are reported[by whom?] to have bought US supplies of phenol and converted it to acetylsalicylic acid, i.e., aspirin, to keep it from the Allies.[citation needed] At the time, phenol was obtained from coal as a co-product of coke ovens and the manufacture of gas for gas lighting. Laclede Gas reports being asked to expand production of phenol (and toluene) to support the war effort.[11] Both Monsanto[12] and Dow Chemical[13] undertook manufacture of synthetic phenol in 1915. Dow was the leading producer. Dow describes picric acid as “the main battlefield explosive used by the French. Large amounts [of phenol] also went to Japan, where it was made into picric acid sold to the Russians.”[this quote needs a citation]

Synthesis[edit]

The aromatic ring of phenol is highly activated towards electrophilic substitution reactions, and attempted nitration of phenol, even with dilute nitric acid, results in the formation of high molecular weight tars. In order to minimize these side reactions, anhydrous phenol is sulfonated with fuming sulfuric acid, and the resulting p-hydroxyphenylsulfonic acid is then nitrated with concentrated nitric acid. During this reaction, nitro groups are introduced, and the sulfonic acid group is displaced. The reaction is highly exothermic, and careful temperature control is required.

Uses[edit]

By far, the largest use has been in munitions and explosives. Explosive D, also known as Dunnite, is the ammonium salt of picric acid—more powerful but less stable than the more common explosive TNT (which is produced in a similar process to picric acid but with toluene as the feedstock). Picramide, formed by aminating picric acid (typically beginning with Dunnite), can be further aminated to produce the highly stable explosive TATB.

It has found some use in organic chemistry for the preparation of crystalline salts of organic bases (picrates) for the purpose of identification and characterization.

In metallurgy, a picric acid etch has been commonly used in optical metallography to reveal prior austenite grain boundaries in ferritic steels. The hazards associated with picric acid has meant it has largely been replaced with other chemical etchants. However, it is still used to etch magnesium alloys, such as AZ31.

Bouin solution is a common picric-acid-containing fixative solution used for histology specimens.[14] It improves the staining of acid dyes, but it can also lead to hydrolysis of any DNA in the sample.[15]

Clinical chemistry lab testing utilizes picric acid for the Jaffe reaction to test for creatinine. It forms a colored complex that can be measured using spectroscopy.[16]

In the early 20th century, picric acid was used to measure blood glucose levels. When glucose, picric acid and sodium carbonate are combined and heated, a characteristic red color forms. With a calibrating glucose solution, the red color can be used to measure the glucose levels added. This is known as the Lewis and Benedict method of measuring glucose.[17]

Much less commonly, wet picric acid has been used as a skin dye, or temporary branding agent. It reacts with proteins in the skin to give a dark brown color that may last as long as a month.

In the early 20th century, picric acid was stocked in pharmacies as an antiseptic and as a treatment for burns, malaria, herpes, and smallpox. Picric acid-soaked gauze was also commonly stocked in first aid kits from that period as a burn treatment. It was most notably used for the treatment of burns suffered by victims of the Hindenburgdisaster in 1937. Picric acid was also used as a treatment for trench foot suffered by soldiers stationed on the Western Front during World War I.[18]

Picric acid has been used for many years by fly tyers to dye mole skins and feathers a dark olive green. Its popularity has been tempered by its toxic nature.

Safety[edit]

Modern safety precautions recommend storing picric acid wet. Dry picric acid is relatively sensitive to shock and friction, so laboratories that use it store it in bottles under a layer of water, rendering it safe. Glass or plastic bottles are required, as picric acid can easily form metal picrate salts that are even more sensitive and hazardous than the acid itself. Industrially, picric acid is especially hazardous because it is volatile and slowly sublimes even at room temperature. Over time, the buildup of picrates on exposed metal surfaces can constitute a grave hazard.[19]

Picric acid gauze, if found in antique first aid kits, presents a safety hazard because picric acid of that vintage (60–90 years old) will have become crystallized and unstable, and may have formed metal picrates from long storage in a metal first aid case.

Bomb disposal units are often called to dispose of picric acid if it has dried out.[20][21][22][23][24][25][26][27]

Munitions containing picric acid may be found in sunken warships. The buildup of metal picrates over time renders them shock-sensitive and extremely hazardous. It is recommended that wrecks that contain such munitions not be disturbed in any way.[28] The hazard may subside when the shells become corroded enough to admit seawater as these materials are water-soluble.[28]

See also[edit]

References[edit]

Further reading[edit]

  1. ^ abNomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 691. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4. 
  2. ^ abcd"NIOSH Pocket Guide to Chemical Hazards #0515". National Institute for Occupational Safety and Health (NIOSH). 
  3. ^"Picric acid". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). 
  4. ^Peter Woulfe (1771) "Experiments to shew the nature of aurum mosaicum,"Philosophical Transactions of the Royal Society of London, 61 : 114–130. See pages 127–130: "A method of dying wool and silk, of a yellow colour, with indigo; and also with several other blue and red colouring substances." and "Receipt for making the yellow dye." — where Woulfe treats indigo with nitric acid ("acid of nitre").
  5. ^Auguste Laurent (1841) "Sur le phényle et ses dérivés" (On phenol and its derivatives), Annales de Chimie et de Physique, series 3, 3 : 195–228 ; see especially pages 221–228.
  6. ^Note:
    • In March 1871, Sprengel detonated picric acid at the gunpowder works of John Hall & Sons in Faversham in Kent, England.
    • Sprengel filed patents in Britain for "safety explosives" (i.e., stable explosives) on April 6, 1871 (no. 921) and on October 5, 1871 (no. 2642); in the latter patent, Sprengel proposed using picric acid dissolved in nitric acid as an explosive.
    • Hermann Sprengel (1873) "On a new class of explosives which are non-explosive during their manufacture, storage, and transport," Journal of the Chemical Society, 26 : 796–808.
    • Hermann Sprengel, The Discovery of Picric Acid (Melinite, Lyddite) "As a Powerful Explosive" ..., 2nd ed. (London, England: Eyre & Spottiswoode, 1903). This pamphlet is a collection of (splenetic) letters in which Sprengel defends his priority in the use of picric acid as a high explosive.
  7. ^ abBrown, G.I. (1998) The Big Bang: a History of Explosives Sutton Publishing ISBN 0-7509-1878-0 pp.151–163
  8. ^John Philip Wisser (1901). The second Boer War, 1899–1900. Hudson-Kimberly. p. 243. Retrieved 2009-07-22. 
  9. ^Dunnite Smashes Strongest Armor, The New York Times, August 18, 1907
  10. ^Marc Ferro. The Great War. London and New York: Routeladge Classics, p. 98.
  11. ^Beck, Bill (2007) Laclede Gas and St. Louis: 150 Years Working Together, 1857–2007, Laclede Gas Company, ISBN 978-0-9710910-1-6 p. 64
  12. ^Forrestal, Dan J. (1977), Faith, Hope & $5000: The Story of Monsanto, Simon & Schuster, ISBN 0-671-22784-X[2] p. 24
  13. ^Brandt, E.N. (1997), Growth Company: Dow Chemical's First Century, Michigan State University, ISBN 0-87013-426-4 p. 77, 97 and 244
  14. ^Carson, Freida L.; Hladik, Christa (2009). Histotechnology: A Self-Instructional Text (3 ed.). Hong Kong: American Society for Clinical Pathology Press. p. 19. ISBN 978-0-89189-581-7. 
  15. ^Llewellyn, Brian D (February 2009). "Picric Acid". StainsFile. Retrieved 28 September 2012. 
  16. ^Creatinine Direct Procedure, on CimaScientific
  17. ^"Measuring blood glucose levels in the 1920s". Tacomed.com. Retrieved 13 June 2017. 
  18. ^(1922) [1]History of the Great War - Surgery of the War, Vol. 1, Pg. 175.
  19. ^JT Baker MSDS
  20. ^"Bomb squad called to Dublin lab". irishtimes.com. Irish Times. 1 October 2010. Retrieved 22 July 2011. 
  21. ^"Unstable chemicals made safe by army". rte.ie. RTÉ News. 3 November 2010. Retrieved 22 July 2011. 
  22. ^"Army bomb disposal team make Kerry scene safe". irishexaminer.com. Irish Examiner. 22 November 2010. Retrieved 22 July 2011. 
  23. ^"Dangerous chemicals made safe". irishtimes.com. Irish Times. 23 November 2010. Retrieved 22 July 2011. 
  24. ^"Unstable chemicals made safe". irishtimes.com. Irish Times. 31 May 2011. Retrieved 22 July 2011. 
  25. ^"Chemicals Blown Up At Transfer Station". kcra.com. KCRA. 6 January 2011. Retrieved 22 July 2011. 
  26. ^RTÉ (11 March 2013). "Unstable chemical made safe at Thurles school". RTE.ie. RTÉ. Retrieved 11 March 2013. 
  27. ^Ralston, Nick (24 October 2013). "UTS chemical spill sees 5000 evacuated". Sydney Morning Herald. Retrieved 24 October 2013. 
  28. ^ abAlbright, p.78

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