Acetate

An acetate /ˈæsɪteɪt/ is a salt formed by the combination of acetic acid with a base (e.g. alkaline, earthy, metallic, nonmetallic or radical base). "Acetate" also describes the conjugate base or ion (specifically, the negatively charged ion called an anion) typically found in aqueous solution and written with the chemical formula C
2H
3O−
2. The neutral molecules formed by the combination of the acetate ion and a positive ion (called a cation) are also commonly called "acetates" (hence, acetate of lead, acetate of aluminum, etc.). The simplest of these is hydrogen acetate (called acetic acid) with corresponding salts, esters, and the polyatomic anion CH
3CO−
2, or CH
3COO−
.

For other uses, see Acetate (disambiguation).
Acetate
Names
IUPAC name
Acetate
Systematic IUPAC name
Ethanoate
Identifiers
3D model (JSmol)
ChemSpider
UNII
Properties
C
2H
3O−
2
Conjugate acid Acetic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Most of the approximately 5 billion kilograms of acetic acid produced annually in industry are used in the production of acetates, which usually take the form of polymers. In nature, acetate is the most common building block for biosynthesis. For example, the fatty acids are produced by connecting the two carbon atoms from acetate to a growing fatty acid.[1]

Nomenclature and common formula

When part of a salt, the formula of the acetate ion is written as CH
3CO−
2, C
2H
3O−
2, or CH
3COO−
. Chemists often represent acetate as OAc− or, less commonly, AcO−. Thus, HOAc is the symbol for acetic acid, NaOAc for sodium acetate, and EtOAc for ethyl acetate[2] (as Ac is common symbol for acetyl group CH3CO[3][4]).The pseudoelement symbol "Ac" is also sometimes encountered in chemical formulas as indicating the entire acetate ion (CH3CO2−). It is not to be confused with the symbol of actinium, the first element of the actinide series; context guides disambiguation. For example, the formula for sodium acetate might be abbreviated as "NaOAc", rather than "NaC2H3O2". Care should also be taken to avoid confusion with peracetic acid when using the OAc abbreviation; for clarity and to avoid errors when translated, HOAc should be avoided in literature mentioning both compounds.

Although its systematic name is ethanoate (/ɪˈθænoʊ.eɪt/), the common acetate remains the preferred IUPAC name.[5]

Salts
acetate anion

The acetate anion, [CH3COO]−,(or [C2H3O2]−) is one of the carboxylate family. It is the conjugate base of acetic acid. Above a pH of 5.5, acetic acid converts to acetate:[2]

CH3COOH ⇌ CH3COO− + H+

Many acetate salts are ionic, indicated by their tendency to dissolve well in water. A commonly encountered acetate in the home is sodium acetate, a white solid that can be prepared by combining vinegar and sodium bicarbonate ("bicarbonate of soda"):

CH3COOH + NaHCO3 → CH3COO−Na+ + H2O + CO2

Transition metals can be complexed by acetate. Examples of acetate complexes include chromium(II) acetate and basic zinc acetate.

Commercially important acetate salts are aluminium acetate, used in dyeing, ammonium acetate, a precursor to acetamide, and potassium acetate, used as a diuretic. All three salts are colourless and highly soluble in water.[6]

Esters
acetate ester

Acetate esters have the general formula CH3CO2R, where R is an organyl group. The esters are the dominant forms of acetate in the marketplace. Unlike the acetate salts, acetate esters are often liquids, lipophilic, and sometimes volatile. They are popular because they have inoffensive, often sweet odors, they are inexpensive, and they are usually of low toxicity.

Almost half of acetic acid production is consumed in the production of vinyl acetate, precursor to polyvinyl alcohol, which is a component of many paints. The second largest use of acetic acid is consumed in the production of cellulose acetate. In fact, "acetate" is jargon for cellulose acetate, which is used in the production of fibres or diverse products, e.g. the acetate discs used in audio record production. Cellulose acetate can be found in many household products. Many industrial solvents are acetates, including methyl acetate, ethyl acetate, isopropyl acetate, ethylhexyl acetate. Butyl acetate is a fragrance used in food products.[6]

Acetate in biology

Acetate is a common anion in biology. It is mainly utilized by organisms in the form of acetyl coenzyme A.[7]

Intraperitoneal injection of sodium acetate (20 or 60 mg per kg body mass) was found to induce headache in sensitized rats, and it has been proposed that acetate resulting from oxidation of ethanol is a major factor in causing hangovers. Increased serum acetate levels lead to accumulation of adenosine in many tissues including the brain, and administration of the adenosine receptor antagonist caffeine to rats after ethanol was found to decrease nociceptive behavior.[8][9]

Fermentation acetyl CoA to acetate

Pyruvate is converted into acetyl-coenzyme A (acetyl-CoA) by the enzyme pyruvate dehydrogenase. This acetyl-CoA is then converted into acetate in E. coli, whilst producing ATP by substrate-level phosphorylation. Acetate formation requires two enzymes: phosphate acetyltransferase and acetate kinase.[10]

The mixed acid fermentation pathway is characteristic of the family Enterobacteriaceae, which includes E. coli

      acetyl-CoA + phosphate → acetyl-phosphate + CoA

      acetyl-phosphate + ADP → acetate + ATP

Fermentation of acetate

Acetic acid can also undergo a dismutation reaction to produce methane and carbon dioxide:[11][12]

CH3COO− + H+ → CH4 + CO2   ΔG° = −36 kJ/mol

This disproportionation reaction is catalysed by methanogen archaea in their fermentative metabolism. One electron is transferred from the carbonyl function (e− donor) of the carboxylic group to the methyl group (e− acceptor) of acetic acid to respectively produce CO2 and methane gas.

Structures
gollark: Also random political debates?
gollark: ++remind 7w summary?
gollark: It is missing random bots, an unrelated discussion on some compiler, and C/Rust arguments.
gollark: It's not a good summary.
gollark: utter apiobee.

See also

References
  1. March, J. “Advanced Organic Chemistry” 4th Ed. J. Wiley and Sons, 1992: New York. ISBN 0-471-60180-2.
  2. Zumdahl, S. S. “Chemistry” Heath, 1986: Lexington, MA. ISBN 0-669-04529-2.
  3. International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. ISBN 0-85404-438-8. p. 63. Electronic version.
  4. Brimble, Margaret A.; Black, David StC.; Hartshorn, Richard; Rauter, Amélia P.; Sha, Chin-Kang; Sydnes, Leiv K. (10 November 2012). "Rules for abbreviation of protecting groups (IUPAC Technical Report)". Pure and Applied Chemistry. 85 (1): 310. doi:10.1351/PAC-REP-12-07-12.
  5. R-9.1 Trivial and semisystematic names retained for naming organic compounds Archived 2014-02-08 at the Wayback Machine, A Guide to IUPAC Nomenclature of Organic Compounds, IUPAC Commission on Nomenclature of Organic Chemistry
  6. Hosea Cheung, Robin S. Tanke, G. Paul Torrence "Acetic acid" in Ullmann's Encyclopedia of Industrial Chemistry Weinheim, Germany: Wiley-VCH, 2005. doi:10.1002/14356007.a01_045
  7. Nelson, D. L.; Cox, M. M. "Lehninger, Principles of Biochemistry" 3rd Ed. Worth Publishing: New York, 2000. ISBN 1-57259-153-6.
  8. Maxwell, Christina; et al. (2010). "Acetate Causes Alcohol Hangover Headache in Rats". PLoS ONE. 5 (12): e15963. Bibcode:2010PLoSO...515963M. doi:10.1371/journal.pone.0015963. PMC 3013144. PMID 21209842.
  9. 'Is coffee the real cure for a hangover?' by Bob Holmes, New Scientist, Jan. 15 2011, p. 17.
  10. Keseler, Ingrid M.; et al. (2011). "EcoCyc: a comprehensive database of Escherichia coli biology". Nucleic Acids Research. 39: D583–D590. doi:10.1093/nar/gkq1143. PMC 3013716. PMID 21097882.
  11. Ferry, J.G. (1992). "Methane from acetate". Journal of Bacteriology. 174 (17): 5489–5495. PMC 206491. Retrieved 2011-11-05.
  12. Vogels, G. D.; Keltjens, J. T.; Van Der Drift, C. (1988). "Biochemistry of methane production". In Zehnder A.J.B. (ed.). Biology of anaerobic microorganisms. New York: Wiley. pp. 707–770.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.