| 别名 |
Acetonitrile |
| Methyl cyanide |
| Ethanenitrile |
| 分析方法 |
EPA Method 8240B |
| EPA Method 8260A |
| 分子式 |
C2H3N |
| 用途 |
In organic synthesis as starting material for
acetophenone, alpha-naphthaleneacetic acid, thiamine,
acetamidine. To remove tars, phenols, & coloring matter from petroleum
hydrocarbons which are not soluble in acetonitrile.
To extract fatty acids from fish liver oils & other animals &
vegetable oils. Can be used to recrystallize steroids. As an
indifferent medium in physicochemical investigations.
Wherever a polar solvent having a rather high dielectric constant is
required. As medium for promoting reactions involving
ionization. As a solvent in non-aqueous titrations. As a
nonaqueous solvent for inorganic salts. Acrylic fibers;
pharmaceuticals; perfumes; nitrile rubber; ABS resins Acetonitrile is used
as a chemical intermediate in pesticide manufacture. Solvent for both
inorganic and organic compounds, including polymers. Starting material for
many types of nitrogen-containing compounds, eg, amides,
amines, higher molecular weight mono- and dinitriles;
halogenated nitriles; ketones; isocyanates; and heterocycles, eg, pyridines
and imidazolines A variety of lithium salts when dissolved
in anhydrous organic solvents, eg, acetonitrile from
electrolyte compositions for nonaqueous batteries. |
| 外观颜色 |
COLORLESS, LIMPID LIQUID |
| 嗅味 |
AROMATIC ODOR ; ETHER-LIKE ODOR |
| 沸点 |
81.6 DEG C AT 760 MM HG |
| 熔点 |
-45 DEG C |
| 分子量 |
41.05 |
| 密度 |
SP GR: 0.78745 @ 15 DEG C/4 DEG C |
| 味阈浓度 |
Low: 70.0 mg/cu m; High: 70.0 mg/cu m; Irritating: 875
mg/cu m |
| 敏感度 |
Immediately irritating to the eye. May cause skin
irritation. Vapor: irritating to eyes, nose and throat. Liquid: irritating
to skin and eyes. |
| 环境影响 |
Acetonitrile is released to the environment during its
manufacture and use, from shale oil retorting and
coal gasification, incineration of polyacrylonitrile, from automobile
exhaust and cigarette smoke. If released to soil,
aerobic biodegradation is likely to occur. Acetonitrile is
expected to be mobile in soil and may evaporate from soil
surfaces. Biodegradation is expected to be a major
loss process in water. Acclimatization increases the biodegradation rate
substantially. Volatilization may become competitive
with other loss processes particularly at shallow water
depths. Hydrolysis, photolysis, adsorption to suspended
particles and sediments and bioconcentration in
aquatic organisms are not likely to be important fate mechanisms.
Acetonitrile is likely to be unreactive towards
direct photolysis in air and the half-lives for its reaction with OH
radicals and ozone have been estimated to be 535 days and
860 days, respectively. Therefore, it will persist in
the troposphere for a long time and may be transported a long distance from
its source of emission. Wet deposition may remove
some of the atmospheric acetonitrile. Adequate data
regarding its typical concentrations in air, water and total diet sample are
not available to estimate intake from these exposure
routes. |
| 环境降解？
Environmental Fate |
TERRESTRIAL FATE: Although no conclusive study
demonstrating the biodegradability of acetonitrile in
grab soil samples is available, it can be inferred from the pure culture and
biodegradability studies in water that the compound may
biodegrade in soil. Photolysis studies in air(3,4)
and hydrolysis studies in water suggest that acetonitrile would not undergo
appreciable photolysis or hydrolysis in soil. Based on an
estimated Koc value of 16(1,6), acetonitrile would be
weakly sorbed to most soils. The high water solubility, moderately high
vapor pressure , and weak soil sorption of the compound
suggest that volatilization from soil surfaces and
leaching into groundwater would be important. AQUATIC FATE: A number of
biodegradation studies with sewage, activated sludge, and pure
cultures serving as microbial organisms have shown that
acetonitrile is biodegradable in water following
acclimatization, as long as its original concentration is not too high (eg,
500 mg/l). The decomposition of the compound (concn
0.1 to 25 mg/l) in Ohio River water was 20% in 5 days
and 40% in 12 days . Biodegradation was faster in water following
acclimatization. Photochemical studies in the vapor
phase(5,6) suggest that photodegradation in water may not be
important. Hydrolysis is unimportant at the pH range
normally present in natural waters . Based on the
value of 2.93X10-5 atm cu m/mole for Henry's Law constant (H) and the
relationship between H and volatility(6),
volatilization of the compound from water may not be rapid, but may
become competitive with other loss processes particularly at
shallow water depths. The high water solubility and
low Koc of acetonitrile would suggest that adsorption of the compound to
suspended solids and sediment in water and bioconcentration
in aquatic organisms would be unimportant.
ATMOSPHERIC FATE: The rate constant for the reaction of acetonitrile with OH
radicals in air has been determined to range from
1.9X10-14 to 4.94X10-14 cu cm/molecule-sec in the
temperature range 20 to 27 deg C(1-5). Based on a rate constant of 3X10-14
cu cm/molecule-sec and the average daily OH radicals
concn of 5X10 5 radicals/cu cm in the atmosphere , the
half-life of this reaction is 535 days. The rate constant
for the reaction of acetonitrile in air with ozone is
1.3X10-20 cu cm/molecule-sec(6). In a typical atmosphere where the average
daily ozone concn is 7.2X10 11 molecules/cu cm , the
half-life due to this reaction would be 860 days. The
photochemical smog studies also show that this compound is unreactive
towards photochemically-generated free radicals(8).
Acetonitrile is also unreactive towards direct
photolysis in the gas phase(7,9). EFFL: Acetonitrile was qualitatively
detected in shale oil wastewaters and wastewater from
coal gasification process(2,3). |
