Acetone

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{{#if:Pungent, irritating, floralPungent, irritating, floralColorless liquid0.791 g cm−3[6]-0.04224.46-24.60 kPa (at 20 °C)24.2-10.21.359000.3075 cP178180631|! style="background: #F8EABA; text-align: center;" colspan="2" | Properties
Acetone[1]
Full structural formula of acetone with dimensions Skeletal formula of acetone
Ball-and-stick model of acetone Space-filling model of acetone
IUPAC name

2-Propanone

Systematic name

Propan-2-one[2]

Other names

Dimethyl ketone[3]

β-Ketopropane[3]
Propanone[4]
2-Propanone[3]

Dimethyl formaldehyde[5]

Identifiers
Abbreviations DMK
CAS number 67-64-1 7pxY
PubChem 180
ChemSpider 175 7pxY
UNII 1364PS73AF 7pxY
EC number 200-662-2
UN number 1090
KEGG D02311 7pxY
MeSH Acetone
ChEBI CHEBI:15347 7pxY
ChEMBL CHEMBL14253 7pxY
RTECS number AL3150000
Beilstein Reference 635680
Gmelin Reference 1466
3DMet B00058
Jmol-3D images Image 1
Molecular formula C3H6O
Molar mass 58.08 g mol−1
Structure
Coordination
geometry 		Triagonal planar at C2
Molecular shape Dihedral at C2
Dipole moment 2.91 D
Thermochemistry
Std enthalpy of
formation ΔfHo298 		-250.03-(-248.77) kJ mol−1
Std enthalpy of
combustion ΔcHo298 		-1.772 MJ mol−1
Standard molar
entropy So298 		200.4 J K−1 mol−1
Specific heat capacity, C 125.45 J K−1 mol−1
Hazards
GHS pictograms The flame pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS) The exclamation-mark pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)
GHS signal word DANGER
GHS hazard statements H225, H319, H336
GHS precautionary statements P210, P261, P305+351+338
EU Index 606-001-00-8
EU classification Flammable F Irritant Xi
R-phrases R11, R36, R66, R67
S-phrases (S2), S9, S16, S26
NFPA 704
3
1
0
Flash point −17 °C
Autoignition
temperature 		465 °C
Explosive limits 13.2–57.0%
Threshold Limit Value 1185 mg/m3 (TWA), 2375 mg/m3 (STEL)
LD50 3000 mg/kg (oral, mouse), 20000 mg/kg (dermal, rabbit), LC50 = 19000 mg/m3 (inhalation)
Related compounds
Related compounds Butanone

Isopropanol

 14pxY (verify) (what is: 10pxY/10pxN?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references
Not to be confused with Acetoin.

Acetone is the organic compound with the formula (CH3)2CO, a colorless, mobile, flammable liquid, the simplest example of the ketones.

Acetone is miscible with water and serves as an important solvent in its own right, typically as the solvent of choice for cleaning purposes in the laboratory. About 6.7 million tonnes were produced worldwide in 2010, mainly for use as a solvent and production of methyl methacrylate and bisphenol A.[7][8] It is a common building block in organic chemistry. Familiar household uses of acetone are as the active ingredient in nail polish remover and as paint thinner.

Acetone is produced and disposed of in the human body through normal metabolic processes. It is normally present in blood and urine. People with diabetes produce it in larger amounts. Reproductive toxicity tests show that it has low potential to cause reproductive problems. Due to the higher energy requirements in pregnant women, nursing mothers and children, they have higher levels of acetone. Ketogenic diets that increase acetone in the body are used to reduce epileptic attacks in infants and children who suffer from recalcitrant refractory epilepsy.

Biosynthesis

See also: ketosis
[icon] This section requires expansion. (December 2011)

Small amounts of acetone are produced in the body by the decarboxylation of ketone bodies. Since it is a byproduct of fermentation, acetone is a byproduct of the distillery industry.

Production

In 2010, the worldwide production capacity for acetone was estimated at 6.7 million tonnes per year.[9] With 1.56 million tonnes per year, the United States had the highest production capacity,[10] followed by Taiwan and mainland China. The largest producer of acetone is INEOS Phenol, owning 17% of the world's capacity, with also significant capacity (7-8%) by Mitsui, Sunoco and Shell in 2010.[9] INEOS Phenol also owns the world's largest production site (420,000 tonnes/annum) in Beveren (Belgium). Spot price of acetone in summer 2011 was 1100-1250 USD/tonne in the United States.[11]

Current method

Acetone is produced directly or indirectly from propylene. Approximately 83 % of acetone is produced via the cumene process,[8] as a result, acetone production is tied to phenol production. In the cumene process, benzene is alkylated with propylene to produce cumene, which is oxidized by air to produce phenol and acetone:

Overview of the cumene process

Other processes involve the direct oxidation of propylene (Wacker-Hoechst process), or the hydration of propylene to give 2-propanol, which is oxidized to acetone.[8]

Older methods

Previously, acetone was produced by the dry distillation of acetates, for example calcium acetate in ketonic decarboxylation. During World War I acetone was produced using acetone-butanol-ethanol fermentation with Clostridium acetobutylicum bacteria, which was developed by Chaim Weizmann (later the first president of Israel) in order to help the British war effort.[8] This acetone-butanol-ethanol fermentation was abandoned due to the small yields.[8]

Uses

About a third of the world's acetone is used as a solvent, and a quarter is consumed as acetone cyanohydrin. a precursor to methyl methacrylate.[7]

Laboratory uses

In the laboratory, acetone is used as a polar, aprotic solvent in a variety of organic reactions, such as SN2 reactions. The use of acetone solvent is critical for the Jones oxidation. It does not form an azeotrope with water (see azeotrope (data)).[12] It is a common solvent for rinsing laboratory glassware because of its low cost and volatility. Despite its common use as a supposed drying agent, it is not effective except by bulk displacement and dilution. Acetone can be cooled with dry ice to −78 °C without freezing; acetone/dry ice baths are commonly used to conduct reactions at low temperatures. Acetone is fluorescent under ultraviolet light, and its vapor may be used as a fluorescent tracer in fluid flow experiments.[13]

Solvent use

Acetone is a good solvent for most plastics and synthetic fibers including those used in laboratory bottles made of polystyrene, polycarbonate and some types of polypropylene.[14] It is ideal for thinning fiberglass resin, cleaning fiberglass tools and dissolving two-part epoxies and superglue before hardening. It is used as a volatile component of some paints and varnishes. As a heavy-duty degreaser, it is useful in the preparation of metal prior to painting; it also thins polyester resins, vinyl and adhesives. It is also useful for high reliability soldering applications to remove solder rosin after soldering is complete. This helps to prevent the Rusty bolt effect from occurring due to dirty solder contacts.

Many millions of kilograms of acetone are consumed in the production of the solvents methyl isobutyl alcohol and methyl isobutyl ketone. These products arise via an initial aldol condensation to give diacetone alcohol.[8]

2 (CH3)2CO → (CH3)2C(OH)CH2C(O)CH3

Acetone is used as a solvent by the pharmaceutical industry and as a denaturant in denatured alcohol.[15] Acetone is also present as an excipient in some pharmaceutical drugs.[16]

Storage of acetone

Although itself flammable, acetone is used extensively as a solvent for the safe transporting and storing of acetylene, which cannot be safely pressurized as a pure compound. Vessels containing a porous material are first filled with acetone followed by acetylene, which dissolves into the acetone. One liter of acetone can dissolve around 250 liters of acetylene.[17][18]

Methyl methacrylate synthesis

Acetone is used to synthesize methyl methacrylate. It begins with the initial conversion of acetone to acetone cyanohydrin:

(CH3)2CO + HCN → (CH3)2C(OH)CN

In a subsequent step, the nitrile is hydrolyzed to the unsaturated amide, which is esterified:

(CH3)2C(OH)CN + CH3OH → CH2=(CH3)CCO2CH3 + NH3

Bisphenol A synthesis

The third major use of acetone (about 20%)[7] is synthesizing bisphenol A. Bisphenol A is a component of many polymers such as polycarbonates, polyurethanes, and epoxy resins. The synthesis involves the condensation of acetone with phenol:

(CH3)2CO + 2 C6H5OH → (CH3)2C(C6H4OH)2 + H2O

Medical and cosmetic uses

Acetone is used in a variety of general medical and cosmetic applications and is also listed as a component in food additives and food packaging.

Acetone is commonly used in chemical peeling. Common agents used today for chemical peels are salicylic acid, glycolic acid, 30% salicylic acid in ethanol, and trichloroacetic acid (TCA). Prior to chemexfoliation, the skin is cleaned and excess fat removed in a process called defatting. Acetone, Septisol, or a combination of these agents is commonly used in this process.[citation needed]

Domestic and other niche uses

Acetone is often the primary component in cleaning agents such as nail polish remover. Acetone is a component of superglue remover and easily removes residues from glass and porcelain.

It is used as an artistic agent; when rubbed on the back of a laser print or photocopy placed face-down on another surface and burnished firmly, the toner of the image transfers to the destination surface.

Make-up artists use acetone to remove skin adhesive from the netting of wigs and moustaches by immersing the item in an acetone bath, then removing the softened glue residue with a stiff brush.

Safety

Flammability

The most hazardous property of acetone is its extreme flammability. At temperatures greater than acetone's flash point of −20 °C (−4 °F), air mixtures of between 2.5% and 12.8% acetone, by volume, may explode or cause a flash fire. Vapors can flow along surfaces to distant ignition sources and flash back. Static discharge may also ignite acetone vapors.[19] It auto-ignites at 465 °C (869 °F).

Acetone peroxide

Main article: acetone peroxide

When oxidized, acetone forms acetone peroxide as a byproduct, which is a highly unstable compound. It may be formed accidentally, e.g. when waste hydrogen peroxide is poured into waste solvent containing acetone. Due to its instability, it is rarely used, despite its easy chemical synthesis.

Health information

Acetone has been studied extensively and is generally recognized to have low acute and chronic toxicity if ingested and/or inhaled. Inhalation of high concentrations (around 9200 ppm) in the air caused irritation of the throat in humans in as little as 5 minutes. Inhalation of concentrations of 1000 ppm caused irritation of the eyes and of the throat in less than 1 hour; however, the inhalation of 500 ppm of acetone in the air caused no symptoms of irritation in humans even after 2 hours of exposure. Acetone is not currently regarded as a carcinogen, a mutagenic chemical or a concern for chronic neurotoxicity effects.[19]

Acetone can be found as an ingredient in a variety of consumer products ranging from cosmetics to processed and unprocessed foods. Acetone has been rated as a GRAS (Generally Recognized as Safe) substance when present in beverages, baked foods, desserts, and preserves at concentrations ranging from 5 to 8 mg/L. Additionally, a joint U.S-European study found that acetone’s "health hazards are slight."[citation needed]

Toxicology

Acetone is believed to exhibit only slight toxicity in normal use, and there is no strong evidence of chronic health effects if basic precautions are followed.[20]

At very high vapor concentrations, acetone is irritating and, like many other solvents, may depress the central nervous system. It is also a severe irritant on contact with eyes, and a potential pulmonary aspiration risk. In one documented case, ingestion of a substantial amount of acetone led to systemic toxicity, although the patient eventually fully recovered.[21] Some sources estimate LD50 for human ingestion at 1.159 g/kg; LD50 inhalation by mice is given as 44 g/m3, over 4 hours.[22]

Acetone has been shown to have anticonvulsant effects in animal models of epilepsy, in the absence of toxicity, when administered in millimolar concentrations.[23] It has been hypothesized that the high-fat low-carbohydrate ketogenic diet used clinically to control drug-resistant epilepsy in children works by elevating acetone in the brain.[23]

  • EPA EPCRA Delisting (1995). EPA removed acetone from the list of “toxic chemicals” maintained under Section 313 of the Emergency Planning and Community Right to Know Act (EPCRA). In making that decision, EPA conducted an extensive review of the available toxicity data on acetone and found that acetone "exhibits acute toxicity only at levels that greatly exceed releases and resultant exposures", and further that acetone "exhibits low toxicity in chronic studies".
  • Genotoxicity. Acetone has been tested in more than two dozen in vitro and in vivo assays. These studies indicate that acetone is not genotoxic.
  • Carcinogenicity. EPA in 1995 concluded, "There is currently no evidence to suggest a concern for carcinogenicity". (EPCRA Review, described in Section 3.3). NTP scientists have recommended against chronic toxicity/carcinogenicity testing of acetone because "the prechronic studies only demonstrated a very mild toxic response at very high doses in rodents".
  • Neurotoxicity and Developmental Neurotoxicity. The neurotoxic potential of both acetone and isopropanol, the metabolic precursor of acetone, have been extensively studied. These studies demonstrate that although exposure to high doses of acetone may cause transient central nervous system effects, acetone is not a neurotoxicant. A guideline developmental neurotoxicity study has been conducted with isopropanol, and no developmental neurotoxic effects were identified, even at the highest dose tested. (SIAR, pp. 1, 25, 31).
  • Environmental. When the EPA exempted acetone from regulation as a volatile organic compound (VOC) in 1995, EPA stated that this exemption would "contribute to the achievement of several important environmental goals and would support EPA’s pollution prevention efforts". 60 Fed. Reg. 31,634 (June 16, 1995). 60 Fed. Reg. 31,634 (June 16, 1995). EPA noted that acetone could be used as a substitute for several compounds that are listed as hazardous air pollutants (HAP) under section 112 of the Clean Air Act.

Environmental effects

Acetone evaporates rapidly, even from water and soil. Once in the atmosphere, it is degraded by UV light with a 22-day half-life. Acetone dissipates slowly in soil, animals, or waterways since it is sometimes consumed by microorganisms,[24] but it is a significant groundwater contaminant due to its high solubility in water. The LD50 of acetone for fish is 8.3 g/L of water (or about 0.8%) over 96 hours, and its environmental half-life is about 1 to 10 days. Acetone may pose a significant risk of oxygen depletion in aquatic systems due to the microbial activity consuming it.[25]

References

  1. ↑ Merck Index, 11th Edition, 58
  2. ↑ "Acetone – PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information. http://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=180.
  3. ↑ 3.0 3.1 3.2 "Acetone". NIST Chemistry WebBook. USA: National Institute of Standards and Technology. http://webbook.nist.gov/cgi/cbook.cgi?ID=67-64-1.
  4. ↑ Script error
  5. ↑ Script error
  6. ↑ "Acetone CHROMASOLV® Plus, for HPLC, ≥99.9%". Sigma-Aldrich. http://www.sigmaaldrich.com/catalog/ProductDetail.do?lang=en&N4=650501%7CSIAL&N5=SEARCH_CONCAT_PNO. Retrieved 15 September 2011.
  7. ↑ 7.0 7.1 7.2 Acetone, World Petrochemicals report, January 2010
  8. ↑ 8.0 8.1 8.2 8.3 8.4 8.5 Stylianos Sifniades, Alan B. Levy, “Acetone” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.
  9. ↑ 9.0 9.1 EO Camara Greiner and C Funada (june 2010). "CEH Marketing Research Report: ACETONE". Chemical Economics Handbook. SRI consulting. http://www.sriconsulting.com/CEH/Private/Reports/604.5000//. Retrieved March 2011.
  10. ↑ "Acetone Uses and Market Data". ICIS.com. October 2010. http://www.icis.com/v2/chemicals/9074858/acetone/uses.html. Retrieved 2011-03-21.
  11. ↑ http://www.icispricing.com/il_shared/Samples/SubPage132.asp
  12. ↑ What is an Azeotrope?
  13. ↑ Script error
  14. ↑ NALGENE Labware – Technical Data
  15. ↑ Script error
  16. ↑ Inactive Ingredient Search for Approved Drug Products, FDA/Center for Drug Evaluation and Research
  17. ↑ Mine Safety and Health Administration (MSHA) – Safety Hazard Information – Special Hazards of Acetylene
  18. ↑ History – Acetylene dissolved in acetone
  19. ↑ 19.0 19.1 Acetone MSDS
  20. ↑ Basic Information on Acetone
  21. ↑ Canadian Centre for Occupational Health and Safety. "Health Effects of Acetone". Archived from the original on 17 October 2008. http://ccohs.ca/oshanswers/chemicals/chem_profiles/acetone/health_ace.html. Retrieved 2008-10-21.
  22. ↑ Safety (MSDS) data for propanone
  23. ↑ 23.0 23.1 Script error
  24. ↑ Acetone, Agency for Toxic Substances and Disease Registry ToxFAQs, 1995
  25. ↑ Safety Data Sheet Acetone

External links

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M: MET

mt, k, c/g/r/p/y/i, f/h/s/l/o/e, a/u, n, m

k, cgrp/y/i, f/h/s/l/o/e, au, n, m, epon

m(A16/C10),i(k, c/g/r/p/y/i, f/h/s/o/e, a/u, n, m)

ar:أسيتون

be:Ацэтон bg:Ацетон bs:Aceton ca:Acetona cs:Aceton da:Acetone de:Aceton et:Atsetoon el:Προπανόνη es:Acetona eo:Acetono eu:Azetona fa:استون fr:Acétone ga:Aicéatón gl:Acetona ko:아세톤 hi:एसीटोन hr:Aceton io:Acetono id:Aseton it:Acetone he:אצטון kn:ಅಸಿಟೋನ್ kk:Ацетон la:Acetonum lv:Acetons lt:Acetonas lmo:Acetun hu:Aceton mk:Ацетон nl:Aceton ja:アセトン no:Aceton nn:Aceton pl:Aceton pt:Acetona ro:Acetonă ru:Ацетон sq:Acetoni simple:Acetone sk:Acetón sl:Aceton sr:Aceton fi:Asetoni sv:Aceton ta:அசிட்டோன் th:อะซิโตน tr:Aseton uk:Ацетон zh:丙酮


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