. 67,2213 (1989). We have measured the solubility of ammonia in chloroform at several pressures and at three temperatures (25,30, and 35°C). Results of these measurements have been analysed in terms of the Henry's law constant that applies to "simple" dissolution of the type B(g) = B(disso1ved) and the equilibrium constant K for the liquid phase complex-forming equilibrium represented by A + B = AB where A and B represent chloroform and ammonia, respectively. As expected on the basis of this analysis, ammonia is more soluble (same pressure and temperature) in chloroform than in carbon tetrachloride, where no hydrogen-bonded complex can be formed.Key words: gas solubility, hydrogen-bonded complexes, Henry's law constant, ammonia-chloroform complex, chloroformammonia complex. Mots clks : solubilit6 des gaz, complexes par liaisons hydrogknes, constante de la loi de Henry, complexe ammoniac-chloroforme, complexe chlorofome-ammoniac.[Traduit par la revue] Introduction Analyses of the thermodynamic properties of non-electrolyte solutions are generally made by comparing the measured properties with the properties the solution would have if it were ideal. Attempts are then made to explain the observed deviations in terms of some model (or theory) of solutions. As a first step in the development of such a model it is often convenient to separate the deviations from ideality into "physical" and