Sodium chloroacetate is the organic compound with the formula CH2ClCO2Na. A white, water-soluble solid, it is the sodium salt of chloroacetic acid. Many of its uses are similar to those of the parent acid. It is prepared by treating chloroacetic acid with sodium carbonate.[1][2]
| |
| Names | |
|---|---|
| Preferred IUPAC name
Sodium chloroacetate | |
| Other names
sodium monochloroacetate
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.021.363 |
PubChem CID
|
|
| UNII | |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| C2H2ClNaO2 | |
| Molar mass | 116.48 g·mol−1 |
| Appearance | white solid |
| Density | 1.401 g/cm3 (25 °C) |
| soluble in water, ethanol, chloroform, ether and benzene | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
irritant to skin |
| does not ignite | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Uses edit
Chloroacetate is a good alkylating agent, serving as a reagent for affixing the -CH2CO2− group to a wide variety of even weak nucleophiles.
In terms of practical, commercial uses, it is used to convert cellulose to carboxymethylcellulose. It is a precursor to many herbicides dimethoate and benazoline (the salt itself is also used as a contact herbicide). It is a precursor to thioglycolic acid by reaction with sodium hydrosulfide. Reaction with cyanide salts gives cyanoacetate NCCH2CO2Na.[3] Cyanoacetate is a precursor to malonic acid.
Sodium chloroacetate is a common laboratory reagent in organic chemistry as illustrated by many entries in the book series Organic Syntheses. With bifunctional nucleophiles, sodium chloroacetate is a precursor to heterocycles.[4][5]
Reaction with sodium nitrite give nitroacetic acid.[6] With sodium ethoxide it gives ethoxyacetate.[7] With ethyl acetoacetate ethyl acetosuccinate is produced.[8]
Hydrolysis gives glycolic acid.[1]
References edit
- ^ a b Koenig, Günter; Lohmar, Elmar; Rupprich, Norbert (2000). "Chloroacetic Acids". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a06_537. ISBN 3527306730.
- ^ Nathan Weiner (1938). "Malonic Acid". Organic Syntheses. 18: 50. doi:10.15227/orgsyn.018.0050.
- ^ J. K. H. Inglis (1928). "Ethyl Cyanoacetate". Organic Syntheses. 8: 74. doi:10.15227/orgsyn.008.0074.
- ^ C. Ernst Redemann, Roland N. Icke, Gordon A. Alles (1947). "Rhodanine". Organic Syntheses. 27: 73. doi:10.15227/orgsyn.027.0073.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ C. F. H. Allen, J. A. VanAllan (1947). "Pseudothiohydantoin". Organic Syntheses. 27: 71. doi:10.15227/orgsyn.027.0071.
- ^ F. C. Whitmore, Marion G. Whitmore (1923). "Nitromethane". Organic Syntheses. 3: 83. doi:10.15227/orgsyn.003.0083.
- ^ Reynold C. Fuson, Bruno H. Wojcik (1933). "Ethoxyacetic Acid and Ethyl Ethoxyacetate". Organic Syntheses. 13: 42. doi:10.15227/orgsyn.013.0042.
- ^ Homer Adkins, Neville Isbell, Bruno Wojcik (1934). "Ethyl Acetosuccinate". Organic Syntheses. 14: 38. doi:10.15227/orgsyn.014.0038.
{{cite journal}}: CS1 maint: multiple names: authors list (link)
 | This article about an organic compound is a stub. You can help Wikipedia by expanding it. |