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Chloroacetic acids

In organic chemistry, the chloroacetic acids (systematic name chloroethanoic acids) are three related chlorocarbon carboxylic acids:

As the number of chlorine atoms increases, the electronegativity of that end of the molecule increases, and the molecule adopts a progressively more ionic character: its density, boiling point and acidity all increase.

Acid Melting point Boiling point Density pKa
Acetic acid 16.5°C 118.1°C 1.05 4.76
Chloroacetic acid 61-63°C 189°C 1.58 2.87
Dichloroacetic acid 9.7°C 194°C 1.57 1.25
Trichloroacetic acid 57°C 196°C 1.63 0.77


CCl2= CHCl + 2H2O → CH2ClCOOH + 2HCl
  • Dichloroacetic acid is manufactured in small quantities by reducing trichloroacetic acid.
  • Trichloroacetic acid is made by the direct action of chlorine on ethanoic acid in the presence of a suitable catalyst.



All of these acids are unusually strong for organic acids, and should generally be treated with similar care as for strong mineral acids like hydrochloric acid. Even neutral salts however, tend to be significantly toxic, because the ions interfere in biological processes (such as the citric acid cycle) that normally process plain acetate ions. Interestingly, the chloroacetate anion is the most toxic, with a rat, oral LD50 of about 0.5 g/kg.

This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Chloroacetic_acids". A list of authors is available in Wikipedia.
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