Ethyl acetoacetate
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| Preferred IUPAC name
Ethyl 3-oxobutanoate | |
Other names
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3D model (JSmol)
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| ChEMBL | |
| ChemSpider | |
| ECHA InfoCard | 100.005.015 |
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PubChem CID
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| UNII | |
| UN number | 1993 |
CompTox Dashboard (EPA)
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| Properties | |
| C6H10O3 | |
| Molar mass | 130.14 g/mol |
| Appearance | Colourless liquid |
| Odor | Fruit or rum |
| Density | 1.021 g/cm3, liquid |
| Melting point | −45 °C (−49 °F; 228 K) |
| Boiling point | 180.8 °C (357.4 °F; 453.9 K) |
| 2.86 g/100 ml (20 °C) | |
| Acidity (pKa) |
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| −71.67×10−6cm3/mol | |
| Hazards | |
| GHS labelling:[1] | |
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| Warning | |
| H319 | |
| P305+P351+P338 | |
| NFPA 704 (fire diamond) | |
| Flash point | 70 °C (158 °F; 343 K) |
| Related compounds | |
Related esters
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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The organic compound ethyl acetoacetate (EAA) is the ethyl ester of acetoacetic acid. It is a colorless liquid. It is widely used as a chemical intermediate in the production of a wide variety of compounds.
Preparation
At large scale, ethyl acetoacetate is industrially produced by treatment of diketene with ethanol.[2]
The small scale preparation of ethyl acetoacetate is a classic laboratory procedure.[3] It involves Claisen condensation of ethyl acetate. Two moles of ethyl acetate condense to form one mole each of ethyl acetoacetate and ethanol.
Preparation of ethyl acetoacetate
Reactivity
Ethyl acetoacetate is subject to keto-enol tautomerism. In the neat liquid at 33 °C, the enol consists of 15% of the total.[4] The enol is moderately acidic. Thus ethyl acetoacetate behaves similarly to acetylacetone:[5]
- CH3C(O)CH2CO2Et + NaH → CH3C(O)CH(Na)CO2Et + H2
The resulting carbanion undergoes nucleophilic substitution. Ethyl acetoacetate is often used in the acetoacetic ester synthesis, comparable to diethyl malonate in the malonic ester synthesis or the Knoevenagel condensation. After its alkylation and saponification, thermal decarboxylation is also possible.[6] Like acetylacetone, ethyl acetoacetate affords ketoenolate complexes[7]
The dianion of ethylacetoacetate is also a useful building block, except that the electrophile adds to the terminal carbon. The strategy can be depicted in the following simplified form:[5]
- CH3C(O)CH(Na)CO2Et + BuLi → LiCH2C(O)CH(Na)CO2Et + BuH
- LiCH2C(O)CH(Na)CO2Et + RX → RCH2C(O)CH(Na)CO2Et + LiX
Reduction of ethyl acetoacetate gives ethyl 3-hydroxybutyrate.[8]
Ethyl acetoacetate transesterifies to give benzyl acetoacetate via a mechanism involving acetylketene. Ethyl (and other) acetoacetates nitrosate readily with equimolar sodium nitrite in acetic acid, to afford the corresponding oximinoacetoacetate esters. A dissolving-zinc reduction of these in acetic acid in the presence of ketoesters or beta-diketones constitute the Knorr pyrrole synthesis, useful for the preparation of porphyrins.
See also
Two ketals of ethyl acetoacetate are used in commercial fragrances.[9]
- Fructone (CH3C(O2C2H4)CH2CO2C2H5), the ethylene glycol ketal
- Fraistone (CH3C(O2C2H3CH3)CH2CO2C2H5), the propylene glycol ketal
References
- ^ Record in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2021-12-19.
- ^ Riemenschneider, Wilhelm; Bolt, Hermann M. (2005). "Esters, Organic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a09_565.pub2. ISBN 3527306730.
- ^ J. K. H. Inglis and K. C. Roberts (1926). "Ethyl Acetoacetate". Organic Syntheses. 6: 36. doi:10.15227/orgsyn.006.0036.
- ^ Jane L. Burdett; Max T. Rogers (1964). "Keto-Enol Tautomerism in β-Dicarbonyls Studied by Nuclear Magnetic Resonance Spectroscopy. I. Proton Chemical Shifts and Equilibrium Constants of Pure Compounds". J. Am. Chem. Soc. 86: 2105–2109. doi:10.1021/ja01065a003.
- ^ a b Jin, Yinghua; Roberts, Frank G.; Coates, Robert M. (2007). "Stereoselective Isoprenoid Chain Extension with Acetoacetate Dianion: [(E, E, E)-Geranylgeraniol from (E, E)-Farnesol". Organic Syntheses. 84: 43. doi:10.15227/orgsyn.084.0043.
- ^ Carey, Francis A. (2006). Organic Chemistry (Sixth ed.). New York, NY: McGraw-Hill. ISBN 0-07-111562-5.
- ^ . doi:10.1107/S010827010001249X.
{{cite journal}}: Cite journal requires|journal=(help); Missing or empty|title=(help) - ^ . doi:10.1021/ja01375a082.
{{cite journal}}: Cite journal requires|journal=(help); Missing or empty|title=(help) - ^ Panten, Johannes; Surburg, Horst (2016). "Flavors and Fragrances, 3. Aromatic and Heterocyclic Compounds". Ullmann's Encyclopedia of Industrial Chemistry. pp. 1–45. doi:10.1002/14356007.t11_t02. ISBN 978-3-527-30673-2.