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Henry's Law Constants

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Rolf Sander

Atmospheric Chemistry Division

Max-Planck Institute for Chemistry
Mainz, Germany

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Henry's Law Constants

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

R. Sander: Compilation of Henry's law constants (version 5.0.0) for water as solvent, Atmos. Chem. Phys., 23, 10901-12440 (2023), doi:10.5194/acp-23-10901-2023

The publication from 2023 replaces that from 2015, which is now obsolete. Please do not cite the old paper anymore.

Henry's Law Constants → Inorganic species → Nitrogen (N) → nitrogen

FORMULA:N2
CAS RN:7727-37-9
STRUCTURE
(FROM NIST):
InChIKey:IJGRMHOSHXDMSA-UHFFFAOYSA-N

Hscp d ln Hs cp / d (1/T) References Type Notes
[mol/(m3Pa)] [K]
6.4×10−6 1300 Burkholder et al. (2019) L 1)
6.4×10−6 1300 Burkholder et al. (2015) L 1)
6.4×10−6 1600 Warneck & Williams (2012) L
6.4×10−6 1300 Sander et al. (2011) L 1)
6.4×10−6 1300 Sander et al. (2006) L 1)
6.5×10−6 1200 Fernández-Prini et al. (2003) L 3)
6.5×10−6 1200 Battino et al. (1984) L
6.5×10−6 1200 Battino (1982) L 1)
6.4×10−6 1300 Wilhelm et al. (1977) L
5.4×10−6 Steward et al. (1973) L 14)
6.5×10−6 1400 Allott et al. (1973) L
6.3×10−6 1300 Himmelblau (1960) L 1)
6.4×10−6 1300 Rettich et al. (1984) M 56)
6.6×10−6 1300 Cosgrove & Walkley (1981) M 11)
5.5×10−6 Power & Stegall (1970) M 14)
6.4×10−6 1300 Murray et al. (1969) M 57)
6.5×10−6 1400 Morrison & Billett (1952) M 58)
6.6×10−6 Orcutt & Seevers (1937a) M
6.5×10−6 1100 Van Slyke et al. (1934) M
5.6×10−6 Grollman (1929) M 59)
6.4×10−6 1200 Fox (1909) M
6.3×10−6 2200 Braun (1900) M 60)
6.3×10−6 1300 Winkler (1891b) M 61)
6.7×10−6 1400 Bohr & Bock (1891) M
5.8×10−6 1200 Bunsen (1855a) M 43)
6.4×10−6 1300 Wauchope & Haque (1972) V
6.5×10−6 1300 Wauchope & Haque (1972) V
6.5×10−6 Pierotti (1965) T
7.2×10−6 Nunn (1958) C 12)
5.6×10−6 Hayer et al. (2022) Q 20)
6.4×10−6 1600 Battino et al. (2018) ?
6.3×10−6 1200 Yaws et al. (1999) ? 21)
5.7×10−6 Abraham & Weathersby (1994) ? 21)
6.3×10−6 1300 Dean & Lange (1999) ? 23) 62)

Data

The first column contains Henry's law solubility constant Hscp at the reference temperature of 298.15 K.
The second column contains the temperature dependence d ln Hs cp / d (1/T), also at the reference temperature.

References

  • Abraham, M. H. & Weathersby, P. K.: Hydrogen bonding. 30. Solubility of gases and vapors in biological liquids and tissues, J. Pharm. Sci., 83, 1450–1456, doi:10.1002/JPS.2600831017 (1994).
  • Allott, P. R., Steward, A., Flook, V., & Mapleson, W. W.: Variation with temperature of the solubilities of inhaled anaesthestics in water, oil and biological media, Br. J. Anaesth., 45, 294–300, doi:10.1093/BJA/45.3.294 (1973).
  • Battino, R.: IUPAC Solubility Data Series, Volume 10, Nitrogen and Air, Pergamon Press, Oxford, ISBN 0080239226 (1982).
  • Battino, R., Rettich, T. R., & Tominaga, T.: The solubility of nitrogen and air in liquids, J. Phys. Chem. Ref. Data, 13, 563–600, doi:10.1063/1.555713 (1984).
  • Battino, R., Rettich, T. R., & Wilhelm, E.: Gas solubilities in liquid water near the temperature of the density maximum, Tmax(H2O) = 277.13K, Monatsh. Chem. – Chem. Mon., 149, 219–230, doi:10.1007/S00706-017-2097-3 (2018).
  • Bohr, C. & Bock, J.: Bestimmung der Absorption einiger Gase in Wasser bei den Temperaturen zwischen 0 und 100∘, Ann. Phys., 280, 318–343, doi:10.1002/ANDP.18912801010 (1891).
  • Braun, L.: Über die Absorption von Stickstoff und von Wasserstoff in wässerigen Lösungen verschieden dissociierter Stoffe, Z. Phys. Chem., 33U, 721–739, doi:10.1515/ZPCH-1900-3349 (1900).
  • Bunsen, R.: Ueber das Gesetz der Gasabsorption, Liebigs Ann. Chem., 93, 1–50, doi:10.1002/JLAC.18550930102 (1855a).
  • Burkholder, J. B., Sander, S. P., Abbatt, J., Barker, J. R., Huie, R. E., Kolb, C. E., Kurylo, M. J., Orkin, V. L., Wilmouth, D. M., & Wine, P. H.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation No. 18, JPL Publication 15-10, Jet Propulsion Laboratory, Pasadena, URL https://jpldataeval.jpl.nasa.gov (2015).
  • Burkholder, J. B., Sander, S. P., Abbatt, J., Barker, J. R., Cappa, C., Crounse, J. D., Dibble, T. S., Huie, R. E., Kolb, C. E., Kurylo, M. J., Orkin, V. L., Percival, C. J., Wilmouth, D. M., & Wine, P. H.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation No. 19, JPL Publication 19-5, Jet Propulsion Laboratory, Pasadena, URL https://jpldataeval.jpl.nasa.gov (2019).
  • Cosgrove, B. A. & Walkley, J.: Solubilities of gases in H2O and 2H2O, J. Chromatogr., 216, 161–167, doi:10.1016/S0021-9673(00)82344-4 (1981).
  • Dean, J. A. & Lange, N. A.: Lange’s Handbook of Chemistry, Fifteenth Edition, McGraw-Hill, Inc., ISBN 9780070163843 (1999).
  • Fernández-Prini, R., Alvarez, J. L., & 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).
  • Fox, C. J. J.: On the coefficients of absorption of nitrogen and oxygen in distilled water and sea-water, and of atmospheric carbonic acid in sea-water, Trans. Faraday Soc., 5, 68–86, doi:10.1039/TF9090500068 (1909).
  • Grollman, A.: The solubility of gases in blood and blood fluids, J. Biol. Chem., 82, 317–325, doi:10.1016/S0021-9258(20)78278-5 (1929).
  • Hayer, N., Jirasek, F., & Hasse, H.: Prediction of Henry’s law constants by matrix completion, AIChE J., 68, e17 753, doi:10.1002/AIC.17753 (2022).
  • Himmelblau, D. M.: Solubilities of inert gases in water. 0∘C. to near the critical point of water, J. Chem. Eng. Data, 5, 10–15, doi:10.1021/JE60005A003 (1960).
  • Morrison, T. J. & Billett, F.: 730. The salting-out of non-electrolytes. Part II. The effect of variation in non-electrolyte, J. Chem. Soc., pp. 3819–3822, doi:10.1039/JR9520003819 (1952).
  • Murray, C. N., Riley, J. P., & Wilson, T. R. S.: The solubility of gases in distilled water and sea water — I. Nitrogen, Deep-Sea Res. Oceanogr. Abstr., 16, 297–310, doi:10.1016/0011-7471(69)90020-5 (1969).
  • Nunn, J. F.: Respiratory measurements in the presence of nitrous oxide: storage of gas samples and chemical methods of analysis, Br. J. Anaesth., 30, 254–263, doi:10.1093/BJA/30.6.254 (1958).
  • Orcutt, F. S. & Seevers, M. H.: A method for determining the solubility of gases in pure liquids or solutions by the Van Slyke-Neill manometric apparatus, J. Biol. Chem., 117, 501–507, doi:10.1016/S0021-9258(18)74550-X (1937a).
  • Pierotti, R. A.: Aqueous solutions of nonpolar gases, J. Phys. Chem., 69, 281–288, doi:10.1021/J100885A043 (1965).
  • Power, G. G. & Stegall, H.: Solubility of gases in human red blood cell ghosts, J. Appl. Physiol., 29, 145–149, doi:10.1152/JAPPL.1970.29.2.145 (1970).
  • Rettich, T. R., Battino, R., & Wilhelm, E.: Solubility of gases in liquids. XVI. Henry’s law coefficients for nitrogen in water at 5 to 50∘C, J. Solution Chem., 13, 335–348, doi:10.1007/BF00645706 (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., & 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, URL https://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., & Wine, P. H.: Chemical Kinetics and Photochemical Data for Use in Atmospheric Studies, Evaluation No. 17, JPL Publication 10-6, Jet Propulsion Laboratory, Pasadena, URL https://jpldataeval.jpl.nasa.gov (2011).
  • Steward, A., Allott, P. R., Cowles, A. L., & 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).
  • Van Slyke, D. D., Dillon, R. T., & Margaria, R.: Studies of gas and electrolyte equilibria in blood: XVIII. Solubility and physical state of atmospheric nitrogen in blood cells and plasma, J. Biol. Chem., 105, 571–596, doi:10.1016/S0021-9258(18)75528-2 (1934).
  • Warneck, P. & Williams, J.: The Atmospheric Chemist’s Companion: Numerical Data for Use in the Atmospheric Sciences, Springer Verlag, doi:10.1007/978-94-007-2275-0 (2012).
  • Wauchope, R. D. & Haque, R.: Aqueous solutions of nonpolar compounds. Heat-capacity effects, Can. J. Chem., 50, 133–138, doi:10.1139/V72-022 (1972).
  • Wilhelm, E., Battino, R., & Wilcock, R. J.: Low-pressure solubility of gases in liquid water, Chem. Rev., 77, 219–262, doi:10.1021/CR60306A003 (1977).
  • Winkler, L. W.: Die Löslichkeit der Gase in Wasser (zweite Abhandlung), Ber. Dtsch. Chem. Ges., 24, 3602–3610, doi:10.1002/CBER.189102402237 (1891b).
  • Yaws, C. L., Hopper, J. R., Wang, X., Rathinsamy, A. K., & Pike, R. W.: Calculating solubility & Henry’s law constants for gases in water, Chem. Eng., pp. 102–105 (1999).

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 (2023) for further details.

Notes

1) A detailed temperature dependence with more than one parameter is available in the original publication. Here, only the temperature dependence at 298.15 K according to the Van 't Hoff equation is presented.
3) The vapor pressure for water from Wagner & Pruss (1993) was used to calculate Hs.
11) Measured at high temperature and extrapolated to T⊖ = 298.15 K.
12) Value at T = 293 K.
14) Value at T = 310 K.
20) Calculated using machine learning matrix completion methods (MCMs).
21) Several references are given in the list of Henry's law constants but not assigned to specific species.
23) The partial pressure of water vapor (needed to convert some Henry's law constants) was calculated using the formula given by Buck (1981). The quantities A and α from Dean & Lange (1999) were assumed to be identical.
43) The paper by Bunsen (1855a) was written in German. English versions with the same data were published by Bunsen (1855b) and Bunsen (1855c).
56) The data from Rettich et al. (1984) were fitted to the three-parameter equation: Hscp= exp( −187.67959 +8903.42739/T +25.60079 ln(T)) mol m−3 Pa−1, with T in K.
57) The data from Murray et al. (1969) were fitted to the three-parameter equation: Hscp= exp( −174.95304 +8370.23274/T +23.67882 ln(T)) mol m−3 Pa−1, with T in K.
58) The data from Morrison & Billett (1952) were fitted to the three-parameter equation: Hscp= exp( −193.68170 +9249.62932/T +26.45116 ln(T)) mol m−3 Pa−1, with T in K.
59) Value at T = 311 K.
60) The data from Braun (1900) were fitted to the three-parameter equation: Hscp= exp( 291.66358 −11637.68204/T −46.44139 ln(T)) mol m−3 Pa−1, with T in K.
61) The data from Winkler (1891b) were fitted to the three-parameter equation: Hscp= exp( −164.15163 +7906.86992/T +22.05400 ln(T)) mol m−3 Pa−1, with T in K.
62) The data from Dean & Lange (1999) were fitted to the three-parameter equation: Hscp= exp( −163.64571 +7887.30463/T +21.97696 ln(T)) mol m−3 Pa−1, with T in K.

References cited in the notes can be found here.

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