Solubility of ammonia in pure aqueous and multicomponent solutions

Research output: Journal Publications and Reviews (RGC: 21, 22, 62)22_Publication in policy or professional journal

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Author(s)

  • S. L. Clegg
  • P. Brimblecombe

Detail(s)

Original languageEnglish
Pages (from-to)7237-7248
Journal / PublicationJournal of Physical Chemistry
Volume93
Issue number20
Publication statusPublished - 1989
Externally publishedYes

Abstract

The thermodynamic Henry's law constant (KH/mol kg-1 atm-1) of the weak electrolyte NH3 is described by the equation In (KH) = -8.09694 + 3917.507/T - 0.00314T, from 273 to 313 K. Measured NH3 solubilities in both pure aqueous and multicomponent solutions agree well with calculations using the Pitzer thermodynamic model to predict osmotic and activity coefficients. Partial pressure and heat of dilution data were used to determine the activity coefficient of NH3NH3). In pure aqueous solutions where dissociation is not significant this is given by γNH3 = exp(2mNH3λNH3,NH3), where λNH3,NH3 = 0.033161 - 21.12816/T + 4665.1461/T2 from 273 to 313 K. Ion-NH3 interaction parameters were obtained by using partial pressure, salt solubility, and partitioning data for the following ions at 298.15 K: Li+, Na+, K+, NH4 +, Mg2+, Ca2+, Sr2+, Ba2+, F-, Cl-, Br-, I-, OH-, CNS-, NO3 -, NO2 -, ClO3 -, ClO4 -, S2-, SO3 2-, CH3COO-, HCOO- and (COO)2 2-. Parameter values are found to be simply related to ion charge and size. © 1989 American Chemical Society.

Citation Format(s)

Solubility of ammonia in pure aqueous and multicomponent solutions. / Clegg, S. L.; Brimblecombe, P.

In: Journal of Physical Chemistry, Vol. 93, No. 20, 1989, p. 7237-7248.

Research output: Journal Publications and Reviews (RGC: 21, 22, 62)22_Publication in policy or professional journal