Henry's Law Constants

Rolf Sander

Atmospheric Chemistry Division

Max-Planck Institute for Chemistry
Mainz, Germany

Errata

Contact, Imprint, Acknowledgements

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 Please do not cite the old paper anymore.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 → Rare gases (He, Ne, Ar, Kr, Xe, Rn) → neon

FORMULA:	Ne
CAS RN:	7440-01-9
STRUCTURE (FROM NIST):
InChIKey:	GKAOGPIIYCISHV-UHFFFAOYSA-N

$H_{s}^{cp}$	$d ln H_{s}^{cp} / d (1/ T)$	References	Type	Notes
[mol/(m³Pa)]	[K]
4.5×10⁻⁶	430	Fernández-Prini et al. (2003)	L	3)
4.4×10⁻⁶	470	Abraham and Matteoli (1988)	L
4.5×10⁻⁶	470	Clever (1979a)	L	1)
4.4×10⁻⁶	450	Wilhelm et al. (1977)	L
4.5×10⁻⁶	440	Krause and Benson (1989)	M
4.4×10⁻⁶	510	Crovetto et al. (1982)	M
4.3×10⁻⁶		Power and Stegall (1970)	M	14)
4.5×10⁻⁶	460	Morrison and Johnstone (1954)	M	193)
4.6×10⁻⁶	37	Lannung (1930)	M	194)
6.6×10⁻⁶	-990	von Antropoff (1910)	M
4.5×10⁻⁶	510	Wauchope and Haque (1972)	V
8.8×10⁻⁶		Pierotti (1965)	T
4.5×10⁻⁶		Hayer et al. (2022)	Q	20)
3.4×10⁻⁶	250	Linnemann et al. (2020)	Q	33)
4.7×10⁻⁶	470	Linnemann et al. (2020)	Q	33) 191)
3.6×10⁻⁶		Warr et al. (2015)	Q	12)
4.5×10⁻⁶	470	Yaws et al. (1999)	?	21)
4.4×10⁻⁶		Abraham and Weathersby (1994)	?	21)
4.5×10⁻⁶	550	Dean and Lange (1999)	?	23) 195)
4.4×10⁻⁶		Abraham et al. (1990)	?

Data

The first column contains Henry's law solubility constant

H_{s}^{cp}

at the reference temperature of 298.15 K.
The second column contains the temperature dependence

d ln H_{s}^{cp} / d
(1/ T)

, also at the reference temperature.

References

Abraham, M. H. & 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. & 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).
Abraham, M. H., Whiting, G. S., Fuchs, R., & 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.: IUPAC Solubility Data Series, Volume 1, Helium and Neon, Pergamon Press, Oxford, ISBN 0080223516 (1979a).
Crovetto, R., Fernández-Prini, R., & 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, 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).
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).
Krause, Jr., D. & 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).
Lannung, A.: The solubilities of helium, neon and argon in water and some organic solvents, J. Am. Chem. Soc., 52, 68–80, doi:10.1021/JA01364A011 (1930).
Linnemann, M., Nikolaychuk, P. A., noz Muñoz, Y. M. M., Baumhögger, E., & Vrabec, J.: Henry’s law constant of noble gases in water, methanol, ethanol, and isopropanol by experiment and molecular simulation, J. Chem. Eng. Data, 65, 1180–1188, doi:10.1021/ACS.JCED.9B00565 (2020).
Morrison, T. J. & Johnstone, N. B.: Solubilities of the inert gases in water, J. Chem. Soc., pp. 3441–3446, doi:10.1039/JR9540003441 (1954).
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).
von Antropoff, A.: The solubility of xenon, krypton, argon, neon, and helium in water, Proc. R. Soc. Lond. A, 83, 474–482, doi:10.1098/RSPA.1910.0036 (1910).
Warr, O., Ballentine, C. J., Mu, J., & Masters, A.: Optimizing noble gas-water interactions via Monte Carlo simulations, J. Phys. Chem. B, 119, 14 486–14 495, doi:10.1021/ACS.JPCB.5B06389 (2015).
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).
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 and Pruss (1993) was used to calculate H_s.
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 and Lange (1999) were assumed to be identical.
33)	Fitting the temperature dependence dlnH/d(1/T) produced a low correlation coefficient (r² < 0.9). The data should be treated with caution.
191)	Calculated employing molecular force field models for the solutes from Warr et al. (2015).
193)	The data from Morrison and Johnstone (1954) were fitted to the three-parameter equation: H_s^cp= exp( −171.84866 +7492.61303/T +23.58966 ln(T)) mol m⁻³ Pa⁻¹, with T in K.
194)	The data from Lannung (1930) were fitted to the three-parameter equation: H_s^cp= exp( −40.04033 +1266.80589/T +4.12574 ln(T)) mol m⁻³ Pa⁻¹, with T in K.
195)	The data from Dean and Lange (1999) were fitted to the three-parameter equation: H_s^cp= exp( −150.94728 +6639.96438/T +20.42365 ln(T)) mol m⁻³ Pa⁻¹, with T in K.

The numbers of the notes are the same as in Sander (2023). References cited in the notes can be found here.

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