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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

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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 4.0) for water as solvent, Atmos. Chem. Phys., 15, 4399-4981 (2015), doi:10.5194/acp-15-4399-2015


Henry's Law ConstantsInorganic speciesSulfur (S) → sulfuric acid

FORMULA:H2SO4
CAS RN:7664-93-9
STRUCTURE
(FROM NIST):
InChIKey:QAOWNCQODCNURD-UHFFFAOYSA-N

Hscp d ln Hs cp / d (1/T) Reference Type Notes
[mol/(m3Pa)] [K]
Marti et al. (1997) M 76)
Ayers et al. (1980) M 77)
Gmitro and Vermeulen (1964) M 78)
Clegg et al. (1998) V 79)
1.3×1013 20000 Hoffmann and Calvert (1985) T
2.9×107 10000 Ayers (1983) T

References

  • Ayers, G. P.: Equilibrium partial pressures over (NH4)2SO4/H2SO4 mixtures, Aust. J. Chem., 36, 179–182, doi:10.1071/CH9830179 (1983).
  • Ayers, G. P., Gillett, R. W., & Gras, J. L.: On the vapor pressure of sulfuric acid, Geophys. Res. Lett., 7, 433–436, doi:10.1029/GL007I006P00433 (1980).
  • Clegg, S. L., Brimblecombe, P., & Wexler, A. S.: Thermodynamic model of the system H+-NH4+-SO42-NO3-H2O at tropospheric temperatures, J. Phys. Chem. A, 102, 2137–2154, doi:10.1021/JP973042R (1998).
  • Gmitro, J. I. & Vermeulen, T.: Vapor-liquid equilibria for aqueous sulfuric acid, AIChE J., 10, 740–746, doi:10.1002/AIC.690100531 (1964).
  • Hoffmann, M. R. & Calvert, J. G.: Chemical transformation modules for Eulerian acid deposition models. Volume II. The aqueous-phase chemistry, Tech. rep., NCAR, Box 3000, Boulder, CO 80307 (1985).
  • Marti, J. J., Jefferson, A., Cai, X. P., Richert, C., McMurry, P. H., & Eisele, F.: H2SO4 vapor pressure of sulfuric acid and ammonium sulfate solutions, J. Geophys. Res., 102D, 3725–3735, doi:10.1029/96JD03064 (1997).

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

76) Marti et al. (1997) give partial pressures of H2SO4 over a concentrated solution (e.g., 2.6×10−9 Pa for 54.1 weight-percent at 298 K). Extrapolating this to dilute solutions can only be considered an order-of-magnitude approximation for Hs.
77) Ayers et al. (1980) give partial pressures of H2SO4 over concentrated solutions at high temperatures. Extrapolating this to dilute solutions can only be considered an order-of-magnitude approximation for Hs.
78) Gmitro and Vermeulen (1964) give partial pressures of H2SO4 over a concentrated solution (e.g., 10−7 mmHg for 70 weight-percent at 298 K). Extrapolating this to dilute solutions can only be considered an order-of-magnitude approximation for Hs.
79) Clegg et al. (1998) estimate a Henry's law constant of 5×1011 atm−1 at 303.15 K for the reaction H2SO4(g) ↔ 2 H+(aq) + SO42−(aq) but don't give a definition for it. Probably it is defined as x2(H+)×x(SO42−)/p(H2SO4), where x is the aqueous-phase mixing ratio.

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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