The dissociation constant and henry's law constant of HCl in aqueous solution

S. L. Clegg; P. Brimblecombe

doi:10.1016/0004-6981(86)90079-X

The dissociation constant and henry's law constant of HCl in aqueous solution

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 language	English
Pages (from-to)	2483-2485
Journal / Publication	Atmospheric Environment (1967)
Volume	20
Issue number	12
Publication status	Published - 1986
Externally published	Yes

Link(s)

DOI	DOI https://doi.org/10.1016/0004-6981(86)90079-X Final Published version
	Check@CityULib
Link to Scopus	https://www.scopus.com/record/display.uri?eid=2-s2.0-0000415193&origin=recordpage
Permanent Link	https://scholars.cityu.edu.hk/en/publications/publication(dc9cd14a-dc77-4f67-ba8a-efd23d26b5c5).html

Abstract

Descriptions of the solubility of HC1 in water involving Raoult's Law have been shown to be inappropriate. Henry's Law constants (K_H) for reactions of the form: HX_(g) = H_(aq) ⁺+X_(aq) ^- are recommended for strong acids on both theoretical and practical grounds. Solubilities of strong acids in electrolyte mixtures can be calculated using activity coefficient models and appropriate values of K_H. A critical evaluation of experimental data yields K_H equal to 2.04 × 10⁶mol²kg^-2atm^-1 at 25°C for HCl. The solubility of weak acids, such as HF, is also discussed. © 1986.