|Preferred IUPAC name
|Systematic IUPAC name
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||78.49 g/mol|
|Density||1.104 g/ml, liquid|
|Melting point||−112 °C (−170 °F; 161 K)|
|Boiling point||52 °C (126 °F; 325 K)|
|Reacts with water|
|GHS signal word||Danger|
|H225, H302, H314, H318, H335, H402, H412|
|P210, P233, P240, P241, P242, P243, P260, P261, P264, P270, P271, P273, P280, P301+312, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P312, P321, P330, P363, P370+378, P403+233|
|Flash point||4 °C (39 °F; 277 K)|
|390 °C (734 °F; 663 K)|
Related acyl chlorides
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
- (CH3CO)2O + HCl → CH3COCl + CH3CO2H
Acetyl chloride is produced in the laboratory by the reaction of acetic acid with chlorodehydrating agents such as PCl3, PCl5, SO2Cl2, phosgene, or SOCl2. However, these methods usually give acetyl chloride contaminated by phosphorus or sulfur impurities, which may interfere with the organic reactions.
When heated, a mixture of dichloroacetyl chloride and acetic acid gives acetyl chloride. It can also be synthesized from the catalytic carbonylation of methyl chloride. It also arises from the reaction of acetic acid, acetonitrile, and hydrogen chloride.
Acetyl chloride is not expected to exist in nature, because contact with water would hydrolyze it into acetic acid and hydrogen chloride. In fact, if handled in open air it releases white "smoke" resulting from hydrolysis due to the moisture in the air. The smoke is actually small droplets of hydrochloric acid and acetic acid formed by hydrolysis.
Acetyl chloride is used for acetylation reactions, i.e., the introduction of an acetyl group. Acetyl is an acyl group having the formula-C(=O)-CH3. For further information on the types of chemical reactions compounds such as acetyl chloride can undergo, see acyl halide. Two major classes of acetylations include esterification and the Friedel-Crafts reaction.
Acetic acid esters and amide
Frequently such acylations are carried out in the presence of a base such as pyridine, triethylamine, or DMAP, which act as catalysts to help promote the reaction and as bases neutralize the resulting HCl. Such reactions will often proceed via ketene.
- Merck Index, 11th Edition, 79.
- Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. pp. 796–797. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4.
- Gerhardt, Charles (1852) "Ueber wasserfreie organische Säuren" (On anhydrous organic acids), Annalen der Chemie und Pharmacie, 83 : 112–116.
- Gerhardt, Charles (1853) "Untersuchungen über die wasserfreien organischen Säuren" (Investigations into anhydrous organic acids), Annalen der Chemie und Pharmacie, 87 : 57–84 ; see especially pp. 68–71.
- Hosea Cheung, Robin S. Tanke, G. Paul Torrence “Acetic Acid” in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a01_045
- Leo A. Paquette (2005). "Acetyl chloride". Handbook of Reagents for Organic Synthesis, Activating Agents and Protective Groups. John Wiley & Sons. p. 16. ISBN 978-0-471-97927-2.
- US 4352761
- Charles Merritt, Jr and Charles E. Braun "9-Acetylanthracene" Org. Synth. 1950, 30, 2. doi:10.15227/orgsyn.030.0001