Henry's Law coefficients of formic and acetic acids

Bryan J. Johnson, Eric Betterton, David Craig

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The Henry's law constants, K(H), Of dilute aqueous formic and acetic acids were determined experimentally as a function of concentration and temperature using a new counterflow packed-column technique. K(H) was found to be (8.91 ± 1.3) x 103 and (4.1 ± 0.4) x 103 M atm-1 at 25°C for HCOOH and CH3COOH, respectively. The reaction enthalpies, ΔH, were found to be -51 ± 2 kJ mol-1 and -52 ± 1 kJ mol-1 formic and acetic acid, respectively. These are in good agreement for with calculated thermochemical values. Whereas the K(H) values are in reasonably good agreement with certain other experimentally determined values, K(H) (HCOOH) is two to three times higher than calculated thermochemical values while K(H) (CH3COOH) is lower than the two calculated values. The 'best' experimental values appear to be (11 ± 2) x 103 M atm-1 and (7 ± 3) x 103 M atm-1 for HCOOH and CH3COOH, respectively.

Original languageEnglish (US)
Pages (from-to)113-119
Number of pages7
JournalJournal of Atmospheric Chemistry
Issue number2
Publication statusPublished - 1996



  • Acetic acid
  • Carboxylic acids
  • Formic acid
  • Henry's law

ASJC Scopus subject areas

  • Atmospheric Science
  • Environmental Science(all)
  • Environmental Chemistry

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