Henry's Law Constants

Rolf Sander

Atmospheric Chemistry Division

Max-Planck Institute for Chemistry
Mainz, Germany


Henry's Law Constants




Contact, Impressum, Acknowledgements

When referring to the compilation of Henry's Law Constants, please cite this publication:

R. Sander: Compilation of Henry's law constants (version 4.0) for water as solvent, Atmos. Chem. Phys., 15, 4399-4981 (2015), doi:10.5194/acp-15-4399-2015

Henry's Law ConstantsInorganic speciesRare gases (He, Ne, Ar, Kr, Xe, Rn) → xenon

CAS RN:7440-63-3

Hcp d ln Hcp / d (1/T) Reference Type Notes
[mol/(m3Pa)] [K]
4.4×10−5 2200 Fernández-Prini et al. 2003 L 1)
4.3×10−5 2300 Abraham and Matteoli 1988 L
4.2×10−5 2200 Wilhelm et al. 1977 L
3.3×10−5 Steward et al. 1973 L 19)
4.3×10−5 2300 Krause and Benson 1989 M
4.2×10−5 2400 Crovetto et al. 1982 M
4.3×10−5 1900 Morrison and Johnstone 1954 M
4.3×10−5 2300 Clever 1979b X 5)
4.9×10−5 2500 Dean 1992 ? 6)
4.3×10−5 Abraham et al. 1990 ?


  • Abraham, M. H. and Matteoli, E.: The temperature variation of the hydrophobic effect, J. Chem. Soc. Faraday Trans. 1, 84, 1985-2000, doi:10.1039/F19888401985, 1988.
  • Abraham, M. H., Whiting, G. S., Fuchs, R., and Chambers, E. J.: Thermodynamics of solute transfer from water to hexadecane, J. Chem. Soc. Perkin Trans. 2, pp. 291-300, doi:10.1039/P29900000291, 1990.
  • Clever, H. L., ed.: IUPAC Solubility Data Series, vol. 2 of Krypton, Xenon and Radon , Pergamon Press, Oxford, England, 1979b.
  • Crovetto, R., Fernández-Prini, R., and Japas, M. L.: Solubilities of inert gases and methane in H2O and in D2O in the temperature range of 300 to 600 K, J. Chem. Phys., 76, 1077-1086, doi:10.1063/1.443074, 1982.
  • Dean, J. A.: Lange's Handbook of Chemistry, McGraw-Hill, Inc., 1992.
  • Fernández-Prini, R., Alvarez, J. L., and Harvey, A. H.: Henry's constants and vapor-liquid distribution constants for gaseous solutes in H2O and D2O at high temperatures, J. Phys. Chem. Ref. Data, 32, 903-916, doi:10.1063/1.1564818, 2003.
  • Krause, Jr., D. and Benson, B. B.: The solubility and isotopic fractionation of gases in dilute aqueous solution. IIa. solubilities of the noble gases, J. Solution Chem., 18, 823-873, doi:10.1007/BF00685062, 1989.
  • Morrison, T. J. and Johnstone, N. B.: Solubilities of the inert gases in water, J. Chem. Soc., pp. 3441-3446, doi:10.1039/JR9540003441, 1954.
  • Steward, A., Allott, P. R., Cowles, A. L., and Mapleson, W. W.: Solubility coefficients for inhaled anaesthetics for water, oil and biological media, Br. J. Anaesth., 45, 282-293, doi:10.1093/BJA/45.3.282, 1973.
  • Wilhelm, E., Battino, R., and Wilcock, R. J.: Low-pressure solubility of gases in liquid water, Chem. Rev., 77, 219-262, doi:10.1021/CR60306A003, 1977.


Table entries are sorted according to reliability of the data, listing the most reliable type first: L) literature review, M) measured, V) VP/AS = vapor pressure/aqueous solubility, R) recalculation, T) thermodynamical calculation, X) original paper not available, C) citation, Q) QSPR, E) estimate, ?) unknown, W) wrong. See Section 3.1 of Sander (2015) for further details.


1) Vapor pressure data for water from Wagner and Pruss (1993) was needed to calculate H.
5) Value given here as quoted by Lide and Frederikse (1995).
6) Only the tabulated data between T = 273 K and T = 303 K from Dean (1992) were used to derive H and its temperature dependence. Above T = 303 K, the tabulated data could not be parameterized very well. The partial pressure of water vapor (needed to convert some Henry's law constants) was calculated using the formula given by Sander et al. (1995). The quantities A and α from Dean (1992) were assumed to be identical.
19) Value at T = 310 K.

The numbers of the notes are the same as in Sander (2015). References cited in the notes can be found here.

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