Acetic anhydride

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Acetic anhydride

Template:Longitem	Template:Unbulleted list
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RTECS number	Template:Unbulleted list
UN number	1715
Template:Longitem	Template:Chembox Elements/molecular formula
Molar mass	Template:Chem molar mass
Appearance	colorless liquid
Density	1.082 g cm−3, liquid
Melting point	Template:Chembox CalcTemperatures
Boiling point	Template:Chembox CalcTemperatures
Vapor pressure	4 mmHg (20 °C)
Template:Longitem	−52.8·10−6 cm3/mol
Template:Longitem	1.3901
Template:Longitem	−624.4 kJ/mol
Legal status	Template:Chembox Legal status/format
Template:Longitem	Propionic anhydride
Template:Longitem	Acetic acid Acetyl chloride

Acetic anhydride, or ethanoic anhydride, is the chemical compound with the formula Template:Chem2. Commonly abbreviated Template:Chem2, it is one the simplest anhydrides of a carboxylic acid and is widely used in the production of cellulose acetate and heroin, as well as a reagent in organic synthesis. It is a colorless liquid that smells strongly of acetic acid, which is formed by its reaction with moisture in the air.

Structure and properties

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Acetic anhydride in a glass bottle

Acetic anhydride, like most organic acid anhydrides, is a flexible molecule with a nonplanar structure. The C=O and C-O distances are 1.19 and 1.39 Å. The pi system linkage through the central oxygen offers very weak resonance stabilization compared to the dipole-dipole repulsion between the two carbonyl oxygens. The energy barriers to bond rotation between each of the optimal aplanar conformations are quite low.

Production

Acetic anhydride was first synthesized in 1852 by the French chemist Charles Frédéric Gerhardt (1816-1856) by heating potassium acetate with benzoyl chloride.

Acetic anhydride is produced by carbonylation of methyl acetate:

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The Tennessee Eastman acetic anhydride process involves the conversion of methyl acetate to methyl iodide. Carbonylation of the methyl iodide produces acetyl iodide, which reacts with acetate source to give the desired anhydride. Rhodium chloride in the presence of lithium iodide is employed as the catalyst. Because acetic anhydride is not stable in water, the conversion is conducted under anhydrous conditions.

To a decreasing extent, acetic anhydride is also prepared by the reaction of ketene (ethenone) with acetic acid at 45–55 °C and low pressure (0.05–0.2 bar).

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(ΔH = −63 kJ/mol)

The route from acetic acid to acetic anhydride via ketene was developed by Wacker Chemie in 1922, when the demand for acetic anhydride increased due to the production of cellulose acetate.

Due to its low cost, acetic anhydride is usually purchased, not prepared, for use in research laboratories.

Reactions

Acetic anhydride is a versatile reagent for acetylations, the introduction of acetyl groups to organic substrates. In these conversions, acetic anhydride is viewed as a source of Template:Chem2.

Acetylation of alcohols, amines, aromatics

Alcohols and amines are readily acetylated. For example, the reaction of acetic anhydride with ethanol yields ethyl acetate:

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Often a base such as pyridine is added to function as catalyst. In specialized applications, Lewis acidic scandium salts have also proven effective catalysts.

Aromatic rings are acetylated by acetic anhydride. Usually acid catalysts are used to accelerate the reaction. Illustrative are the conversions of benzene to acetophenone and ferrocene to acetylferrocene:

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Preparation of other acid anhydrides

Dicarboxylic acids are converted to the anhydrides upon treatment with acetic anhydride. It is also used for the preparation of mixed anhydrides such as that with nitric acid, acetyl nitrate.

Precursor to geminal diacetates

Aldehydes react with acetic anhydride in the presence of an acidic catalyst to give geminal diacetates. A former industrial route to vinyl acetate involved the intermediate ethylidene diacetate, the geminal diacetate obtained from acetaldehyde and acetic anhydride:

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Hydrolysis

Acetic anhydride dissolves in water to approximately 2.6% by weight. Aqueous solutions have limited stability because, like most acid anhydrides, acetic anhydride hydrolyses to give carboxylic acids. In this case, acetic acid is formed, this reaction product being fully water miscible:

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Enolate formation

Acetic anhydride forms the enolate in the presence of acetate as base. The enolate can be trapped by condensation with benzaldehyde. In the 19th century, this chemistry, the Perkin reaction, was used for the production of cinnamic acid:

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Lewis base properties

The carbonyl groups in acetic anhydride are weakly basic. A number of adducts are known, such as the derivative of titanium tetrachloride, TiCl₄((CH₃CO)₂O).

Applications

As indicated by its organic chemistry, acetic anhydride is mainly used for acetylations leading to commercially significant materials. Its largest application is for the conversion of cellulose to cellulose acetate, which is a component of photographic film and other coated materials, and is used in the manufacture of cigarette filters. Similarly it is used in the production of aspirin (acetylsalicylic acid), which is prepared by the acetylation of salicylic acid. It is also used as an active modification agent via autoclave impregnation and subsequent acetylation to make a durable and long-lasting timber.

Acetic anhydride is commonly used for the production of modified starches (E1414, E1420, E1422).

Legal status

Because of its use for the synthesis of heroin by the diacetylation of morphine, acetic anhydride is listed as a U.S. DEA List II precursor and is restricted in many other countries.

Safety

Acetic anhydride is an irritant and combustible liquid; it is highly corrosive to skin and any direct contact will result in burns. Because of its reactivity toward water and alcohol, foam or carbon dioxide are preferred for fire suppression. The vapour of acetic anhydride is harmful.

External links

• ICSC 0209
• NIOSH Pocket Guide to Chemical Hazards