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Solubility data in water of ethane, propane, isobutane, n-butane, n-pentane, and n-hexane have been obtained as a function of temperature in vapor−liquid−liquid equilibrium (VLLE) conditions. The minimum temperature of experiments is 288 K, while the maximum temperature, for each system, is lower than the critical temperature of the corresponding hydrocarbon. New solubility vs temperature correlations are given herein for the studied hydrocarbons in water. Henry's law and activity coefficients at infinite dilution are deduced from the experimental solubility data. Good agreement is found with available literature data.

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Recently, we have published the solubility data of ethane and propane in aqueous diethanolamine (DEA) and methyldiethanolamine (MDEA) solutions at different concentrations (Mokraoui et al., J. Chem. Eng. Data 2013, 58, 2100−2109. In this work, new measurements are provided for longer aliphatic light hydrocarbons, namely, isobutane, n-butane, n-pentane, and n-hexane. The same concentrations of alkanolamines (w DEA = 0.35, w MDEA = 0.25, and w MDEA = 0.50) have been considered in three phases coexisting conditions. MDEA has shown more affinity than DEA for a given weight-based concentration. Within the temperature window explored in this paper (293−353) K, the solubility increases with the amine concentration but it decreases with an increase in the hydrocarbon molecular size. Furthermore, the higher is the carbon atom number of the hydrocarbon, the smaller is the solubility dependence with temperature.

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