| Acetone[1] | |
|---|---|
|
Propan-2-one[2] |
|
| Identifiers | |
| Abbreviations | DMK |
| CAS number | 67-64-1 |
| PubChem | 180 |
| ChemSpider | 175 |
| UNII | 1364PS73AF |
| EC number | 200-662-2 |
| UN number | 1090 |
| KEGG | D02311 |
| MeSH | Acetone |
| ChEBI | CHEBI:15347 |
| ChEMBL | CHEMBL14253 |
| RTECS number | AL3150000 |
| Beilstein Reference | 635680 |
| Gmelin Reference | 1466 |
| 3DMet | B00058 |
| Jmol-3D images | Image 1 |
|
|
|
|
| Properties | |
| Molecular formula | C3H6O |
| Molar mass | 58.08 g mol−1 |
| Exact mass | 58.041864814 g mol−1 |
| Appearance | Colorless liquid |
| Odor | Pungent, irritating, floral |
| Density | 0.791 g cm−3[6] |
| Melting point |
-95--93 °C, 178-180 K, -139--136 °F |
| Boiling point |
56-57 °C, 329-330 K, 133-134 °F |
| log P | -0.042 |
| Vapor pressure | 24.46-24.60 kPa (at 20 °C) |
| Acidity (pKa) | 24.2 |
| Basicity (pKb) | -10.2 |
| Refractive index (nD) | 1.35900 |
| Viscosity | 0.3075 cP |
| Structure | |
| Coordination geometry |
Triagonal planar at C2 |
| Molecular shape | Dihedral at C2 |
| Dipole moment | 2.91 D |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
-250.03-(-248.77) kJ mol−1 |
| Std enthalpy of combustion ΔcH |
-1.772 MJ mol−1 |
| Standard molar entropy S |
200.4 J K−1 mol−1 |
| Specific heat capacity, C | 125.45 J K−1 mol−1 |
| Hazards | |
| MSDS | External MSDS |
| GHS pictograms | |
| 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 | F 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 | 500 ppm (TWA), 750 ppm (STEL) |
| LD50 | >2000 mg/kg, oral (rat) |
| Related compounds | |
| Related compounds | Butanone |
| Supplementary data page | |
| Structure and properties |
n, εr, etc. |
| Thermodynamic data |
Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| (verify) (what is: /?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
|
| Infobox references | |
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. Diabetic people 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.
Contents |
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.
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). The price of acetone varied in 2010 between $75 and $110/tonne in the United States and $90 and 100 in Western Europe.[9]
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:
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]
Previously, acetone was produced by the dry distillation of acetates, for example calcium acetate. 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]
About a third of the world's acetone is used as a solvent, and a quarter is consumed as a precursor to methyl methacrylate.[7]
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)).[11] 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.[12]
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.[13] 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]
Acetone is used as a solvent by the pharmaceutical industry and as a denaturant in denatured alcohol.[14] Acetone is also present as an excipient in some pharmaceutical drugs.[15]
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.[16][17]
Acetone is used to synthesize methyl methacrylate. It begins with the initial conversion of acetone to acetone cyanohydrin:
In a subsequent step, the nitrile is hydrolyzed to the unsaturated amide, which is esterified:
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:
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, lycolic 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.
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 be 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.
The most hazardous quality 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.[18] It auto-ignites at 465 °C (869 °F).
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. Acetone peroxide is more than ten times as sensitive to friction and shock as nitroglycerin. Due to its instability, it is rarely used, despite its easy chemical synthesis.
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.[18]
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."
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.[19]
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.[20] 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.[21]
Acetone has been shown to have anticonvulsant effects in animal models of epilepsy, in the absence of toxicity, when administered in millimolar concentrations.[22] 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.[22]
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,[23] 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.[24]
|
||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||