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Henry's Law Constants

www.henrys-law.org

Rolf Sander

Atmospheric Chemistry Division

Max-Planck Institute for Chemistry
Mainz, Germany


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Henry's Law Constants

Notes

References

Errata

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 speciesNitrogen (N) → ammonia

FORMULA:NH3
CAS RN:7664-41-7
STRUCTURE
(FROM NIST):
InChIKey:QGZKDVFQNNGYKY-UHFFFAOYSA-N

Hcp d ln Hcp / d (1/T) Reference Type Notes
[mol/(m3Pa)] [K]
5.9×10−1 4200 Sander et al. 2011 L
5.9×10−1 4200 Sander et al. 2006 L
5.8×10−1 4400 Yoo et al. 1986 L
6.0×10−1 4200 Edwards et al. 1978 L
1.0×10−1 1500 Wilhelm et al. 1977 L
2.8×10−1 3200 Shi et al. 1999 M
6.0×10−1 4200 Clegg and Brimblecombe 1989 M
5.5×10−1 4100 Dasgupta and Dong 1986 M
7.7×10−1 Holzwarth et al. 1984 M
7.4×10−1 3700 Hales and Drewes 1979 M
5.6×10−1 4200 Dasgupta and Dong 1986 T
5.7×10−1 4100 Chameides 1984 T
6.1×10−1 Van Krevelen et al. 1949 X 20)
2.7×10−1 2100 Dean 1992 ? 6)
5.7×10−1 Abraham et al. 1990 ?
6.1×10−1 4100 Seinfeld 1986 ? 7)
5.8×10−1 4100 Hoffmann and Jacob 1984 ? 7)
5.2×10−1 Bone et al. 1983 ? 21)

References

  • 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.
  • Bone, R., Cullis, P., and Wolfenden, R.: Solvent effects on equilibria of addition of nucleophiles to acetaldehyde and the hydrophilic character of diols, J. Am. Chem. Soc., 105, 1339-1343, doi:10.1021/JA00343A044, 1983.
  • Chameides, W. L.: The photochemistry of a remote marine stratiform cloud, J. Geophys. Res., 89D, 4739-4755, doi:10.1029/JD089ID03P04739, 1984.
  • Clegg, S. L. and Brimblecombe, P.: Solubility of ammonia in pure aqueous and multicomponent solutions, J. Phys. Chem., 93, 7237-7248, doi:10.1021/J100357A041, 1989.
  • Dasgupta, P. G. and Dong, S.: Solubility of ammonia in liquid water and generation of trace levels of standard gaseous ammonia, Atmos. Environ., 20, 565-570, doi:10.1016/0004-6981(86)90099-5, 1986.
  • Dean, J. A.: Lange's Handbook of Chemistry, McGraw-Hill, Inc., 1992.
  • Edwards, T. J., Maurer, G., Newman, J., and Prausnitz, J. M.: Vapor-liquid equilibria in multicomponent aqueous solutions of volatile weak electrolytes, AIChE J., 24, 966-976, doi:10.1002/AIC.690240605, 1978.
  • Hales, J. M. and Drewes, D. R.: Solubility of ammonia in water at low concentrations, Atmos. Environ., 13, 1133-1147, doi:10.1016/0004-6981(79)90037-4, 1979.
  • Hoffmann, M. R. and Jacob, D. J.: Kinetics and mechanisms of the catalytic oxidation of dissolved sulfur dioxide in aqueous solution: An application to nighttime fog water chemistry, in: SO2, NO and NO2 Oxidation Mechanisms: Atmospheric Considerations, edited by Calvert, J. G., pp. 101-172, Butterworth Publishers, Boston, MA, 1984.
  • Holzwarth, G., Balmer, R. G., and Soni, L.: The fate of chlorine and chloramines in cooling towers, Wat. Res., 18, 1421-1427, doi:10.1016/0043-1354(84)90012-5, 1984.
  • Sander, S. P., Friedl, R. R., Golden, D. M., Kurylo, M. J., Moortgat, G. K., Keller-Rudek, H., Wine, P. H., Ravishankara, A. R., Kolb, C. E., Molina, M. J., Finlayson-Pitts, B. J., Huie, R. E., and Orkin, V. L.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation Number 15, JPL Publication 06-2, Jet Propulsion Laboratory, Pasadena, CA, http://jpldataeval.jpl.nasa.gov, 2006.
  • Sander, S. P., Abbatt, J., Barker, J. R., Burkholder, J. B., Friedl, R. R., Golden, D. M., Huie, R. E., Kolb, C. E., Kurylo, M. J., Moortgat, G. K., Orkin, V. L., and Wine, P. H.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation No. 17, JPL Publication 10-6, Jet Propulsion Laboratory, Pasadena, http://jpldataeval.jpl.nasa.gov, 2011.
  • Seinfeld, J. H.: Atmospheric Chemistry and Physics of Air Pollution, Wiley-Interscience Publication, NY, 1986.
  • Shi, Q., Davidovits, P., Jayne, J. T., Worsnop, D. R., and Kolb, C. E.: Uptake of gas-phase ammonia. 1. Uptake by aqueous surfaces as a function of pH, J. Phys. Chem. A, 103, 8812-8823, doi:10.1021/JP991696P, 1999.
  • Van Krevelen, D. W., Hoftijzer, P. J., and Huntjens, F. J.: Composition and vapor pressures of aqueous solutions of ammonia, carbon dioxide and hydrogen sulfide, Recl. Trav. Chim. Pays-Bas, 68, 191-216, 1949.
  • 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.
  • Yoo, K.-P., Lee, S. Y., and Lee, W. H.: Ionization and Henry's law constants for volatile, weak electrolyte water pollutants, Korean J. Chem. Eng., 3, 67-72, doi:10.1007/BF02697525, 1986.

Type

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.

Notes

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.
7) Several references are given in the list of Henry's law constants but not assigned to specific species.
20) Value given here as quoted by Betterton (1992).
21) Bone et al. (1983) gives Carter et al. (1968) as the source. However, no data were found in that reference.

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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