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| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Acetonitrile[2] | |||
| Systematic IUPAC name
Ethanenitrile[2] | |||
| Other names
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| Identifiers | |||
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3D model (JSmol) |
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| 741857 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider |
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| ECHA InfoCard | 100.000.760 
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| EC Number |
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| 895 | |||
| MeSH | acetonitrile | ||
PubChem CID |
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| RTECS number |
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| UNII | |||
| UN number | 1648 | ||
CompTox Dashboard (EPA) |
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| Properties | |||
| C2H3N | |||
| Molar mass | 41.053 g·mol−1 | ||
| Appearance | Colorless liquid | ||
| Odor | Faint, distinct, fruity | ||
| Density | 0.786 g/cm3 at 25°C | ||
| Melting point | −46 to −44 °C; −51 to −47 °F; 227 to 229 K | ||
| Boiling point | 81.3 to 82.1 °C; 178.2 to 179.7 °F; 354.4 to 355.2 K | ||
| Miscible | |||
| log P | −0.334 | ||
| Vapor pressure | 9.71 kPa (at 20.0 °C) | ||
Henry's law |
530 μmol/(Pa·kg) | ||
| Acidity (pKa) | 25 | ||
| UV-vis (λmax) | 195 nm | ||
| Absorbance | ≤0.10 | ||
| −28.0×10−6 cm3/mol | |||
Refractive index (nD) |
1.344 | ||
| 3.92 D | |||
| Thermochemistry | |||
Heat capacity (C) |
91.69 J/(K·mol) | ||
Std molar |
149.62 J/(K·mol) | ||
Std enthalpy of |
40.16–40.96 kJ/mol | ||
Std enthalpy of |
−1256.03 – −1256.63 kJ/mol | ||
| Hazards | |||
| GHS labelling: | |||
 
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| Danger | |||
| H225, H302, H312, H319, H332 | |||
| P210, P280, P305+P351+P338 | |||
| NFPA 704 (fire diamond) | |||
| Flash point | 2.0 °C (35.6 °F; 275.1 K) | ||
| 523.0 °C (973.4 °F; 796.1 K) | |||
| Explosive limits | 4.4–16.0% | ||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose) |
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LC50 (median concentration) |
5655 ppm (guinea pig, 4 hr) 2828 ppm (rabbit, 4 hr) 53,000 ppm (rat, 30 min) 7500 ppm (rat, 8 hr) 2693 ppm (mouse, 1 hr)[4] | ||
LCLo (lowest published) |
16,000 ppm (dog, 4 hr)[4] | ||
| NIOSH (US health exposure limits): | |||
PEL (Permissible) |
TWA 40 ppm (70 mg/m3)[3] | ||
REL (Recommended) |
TWA 20 ppm (34 mg/m3)[3] | ||
IDLH (Immediate danger) |
500 ppm[3] | ||
| Related compounds | |||
Related alkanenitriles |
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Related compounds |
DBNPA | ||
| Supplementary data page | |||
| Acetonitrile (data page) | |||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
Acetonitrile, often abbreviated MeCN (methyl cyanide), is the chemical compound with the formula CH3CN and structure H3C−C≡N. This colourless liquid is the simplest organic nitrile (hydrogen cyanide is a simpler nitrile, but the cyanide anion is not classed as organic). It is produced mainly as a byproduct of acrylonitrile manufacture. It is used as a polar aprotic solventinorganic synthesis and in the purification of butadiene.[5] The N≡C−C skeleton is linear with a short C≡N distance of 1.16 Å.[6]
Acetonitrile was first prepared in 1847 by the French chemist Jean-Baptiste Dumas.[7]
Acetonitrile is used mainly as a solvent in the purification of butadiene in refineries. Specifically, acetonitrile is fed into the top of a distillation column filled with hydrocarbons including butadiene, and as the acetonitrile falls down through the column, it absorbs the butadiene which is then sent from the bottom of the tower to a second separating tower. Heat is then employed in the separating tower to separate the butadiene.
In the laboratory, it is used as a medium-polarity non-protic solvent that is miscible with water and a range of organic solvents, but not saturated hydrocarbons. It has a convenient range of temperatures at which it is a liquid, and a high dielectric constant of 38.8. With a dipole moment of 3.92 D,[8] acetonitrile dissolves a wide range of ionic and nonpolar compounds and is useful as a mobile phase in HPLC and LC–MS.
It is widely used in battery applications because of its relatively high dielectric constant and ability to dissolve electrolytes. For similar reasons, it is a popular solvent in cyclic voltammetry.
Its ultraviolet transparency UV cutoff, low viscosity and low chemical reactivity make it a popular choice for high-performance liquid chromatography (HPLC).
Acetonitrile plays a significant role as the dominant solvent used in oligonucleotide synthesis from nucleoside phosphoramidites.
Industrially, it is used as a solvent for the manufacture of pharmaceuticals and photographic film.[9]
Acetonitrile is a common two-carbon building block in organic synthesis[10] of many useful chemicals, including acetamidine hydrochloride, thiamine, and 1-naphthaleneacetic acid.[11] Its reaction with cyanogen chloride affords malononitrile.[5]
Acetonitrile has a free electron pair at the nitrogen atom, which can form many transition metal nitrile complexes. Being weakly basic, it is an easily displaceable ligand. For example, bis(acetonitrile)palladium dichloride is prepared by heating a suspension of palladium chloride in acetonitrile:[12]
A related complex is tetrakis(acetonitrile)copper(I) hexafluorophosphate [Cu(CH3CN)4]+. The CH3CN groups in these complexes are rapidly displaced by many other ligands.
It also forms Lewis adducts with group 13 Lewis acids like boron trifluoride.[13]Insuperacids, it is possible to protonate acetonitrile.[14]
Acetonitrile is a byproduct from the manufacture of acrylonitrile. Most is combusted to support the intended process but an estimated several thousand tons are retained for the above-mentioned applications.[15] Production trends for acetonitrile thus generally follow those of acrylonitrile. Acetonitrile can also be produced by many other methods, but these are of no commercial importance as of 2002. Illustrative routes are by dehydration of acetamide or by hydrogenation of mixtures of carbon monoxide and ammonia.[16] In 1992[update], 14,700 tonnes (16,200 short tons) of acetonitrile were produced in the US.
Starting in October 2008, the worldwide supply of acetonitrile was low because Chinese production was shut down for the Olympics. Furthermore, a U.S. factory was damaged in Texas during Hurricane Ike.[17] Due to the global economic slowdown, the production of acrylonitrile used in acrylic fibers and acrylonitrile butadiene styrene (ABS) resins decreased. Acetonitrile is a byproduct in the production of acrylonitrile and its production also decreased, further compounding the acetonitrile shortage.[18] The global shortage of acetonitrile continued through early 2009.[needs update]
Acetonitrile has only modest toxicity in small doses.[11][19] It can be metabolised to produce hydrogen cyanide, which is the source of the observed toxic effects.[9][20][21] Generally the onset of toxic effects is delayed, due to the time required for the body to metabolize acetonitrile to cyanide (generally about 2–12 hours).[11]
Cases of acetonitrile poisoning in humans (or, to be more specific, of cyanide poisoning after exposure to acetonitrile) are rare but not unknown, by inhalation, ingestion and (possibly) by skin absorption.[20] The symptoms, which do not usually appear for several hours after the exposure, include breathing difficulties, slow pulse rate, nausea, and vomiting. Convulsions and coma can occur in serious cases, followed by death from respiratory failure. The treatment is as for cyanide poisoning, with oxygen, sodium nitrite, and sodium thiosulfate among the most commonly used emergency treatments.[20]
It has been used in formulations for nail polish remover, despite its toxicity. At least two cases have been reported of accidental poisoning of young children by acetonitrile-based nail polish remover, one of which was fatal.[22] Acetone and ethyl acetate are often preferred as safer for domestic use, and acetonitrile has been banned in cosmetic products in the European Economic Area since March 2000.[23]
| Compound | Cyanide, concentration in brain (μg/kg) | Oral LD50 (mg/kg) |
|---|---|---|
| Potassium cyanide | 700 ± 200 | 10 |
| Propionitrile | 510 ± 80 | 40 |
| Butyronitrile | 400 ± 100 | 50 |
| Malononitrile | 600 ± 200 | 60 |
| Acrylonitrile | 400 ± 100 | 90 |
| Acetonitrile | 28 ± 5 | 2460 |
| Table salt (NaCl) | — | 3000 |
| Ionic cyanide concentrations measured in the brains of Sprague-Dawley rats one hour after oral administration of an LD50 of various nitriles.[24] | ||
In common with other nitriles, acetonitrile can be metabolisedinmicrosomes, especially in the liver, to produce hydrogen cyanide, as was first shown by Pozzani et al. in 1959.[25] The first step in this pathway is the oxidation of acetonitrile to glycolonitrile by an NADPH-dependent cytochrome P450 monooxygenase. The glycolonitrile then undergoes a spontaneous decomposition to give hydrogen cyanide and formaldehyde.[19][20] Formaldehyde, a toxin and a carcinogen on its own, is further oxidized to formic acid, which is another source of toxicity.
The metabolism of acetonitrile is much slower than that of other nitriles, which accounts for its relatively low toxicity. Hence, one hour after administration of a potentially lethal dose, the concentration of cyanide in the rat brain was 1⁄20 that for a propionitrile dose 60 times lower (see table).[24]
The relatively slow metabolism of acetonitrile to hydrogen cyanide allows more of the cyanide produced to be detoxified within the body to thiocyanate (the rhodanese pathway). It also allows more of the acetonitrile to be excreted unchanged before it is metabolised. The main pathways of excretion are by exhalation and in the urine.[19][20][21]
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