The dissociation constant and henry's law constant of HCl in aqueous solution
1986; Elsevier BV; Volume: 20; Issue: 12 Linguagem: Inglês
10.1016/0004-6981(86)90079-x
ISSN1878-2442
AutoresSimon L. Clegg, Peter Brimblecombe,
Tópico(s)Thermodynamic properties of mixtures
ResumoDescriptions of the solubility of HC1 in water involving Raoult's Law have been shown to be inappropriate. Henry's Law constants (KH) 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 KH. A critical evaluation of experimental data yields KH equal to 2.04 × 106mol2kg−2atm−1 at 25°C for HCl. The solubility of weak acids, such as HF, is also discussed.
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