tert-Butyl chloride as a probe of the solvophobic effects

Abraham model correlations for solute transfer into 2-methoxyethanol from water and from the gas phase

“…Second, the published infinite dilution activity coefficient data (γ solute ∞ ) of Sedov et al [10,11] and Matteoli et al [12] that was retrieved from the published literature is converted to gas-to-2-methoxyethanol partition coefficients and water-to-2-methoxyethanol using standard thermodynamic relationships:…”

“…Experimental solubilities have been determined for acenaphthene, biphenyl, benzoic acid, 3-nitrobenzoic acid, 4-nitrobenzoic acid, 2-methoxybenzoic acid, 4-methoxybenzoic acid, 3,4-dimethoxybenzoic acid, 4-aminobenzoic acid, 4-chlorobenzoic acid, 3,5-dinitro-2-methylbenzoic acid, 2-methylbenzoic acid, 3-methylbenzoic acid, 4-chloro-3-nitrobenzoic acid, 2-chloro-5-nitrobenzoic acid, 2-hydroxybenzoic acid, acetylsalicylic acid, 3,4-dichlorobenzoic acid, benzil, salicylamide, trans-stilbene, benzoin, and 9-fluorenone dissolved in 2-methoxyethanol at 298 K. Abraham model log P and log K correlations have been derived by combining our measured molar solubilities with published activity coefficients [10][11][12], gas-to-liquid partition coefficients [13], and solubility data for hydrogen gas [14], carbon dioxide [15], anthracene [16], pyrene [17], 2-nitrobenzoic acid [18], 2-chlorobenzoic acid [18], 3-chlorobenzoic acid [18], and 4-nitroaniline [19]. The derived Abraham model correlations were validated using an external test set of log P and log K values for acetone, methanol, acetonitrile, butyl acetate, pyridine, 2-propanol, and dichloromethane which were measured as part of the current study.…”

Abraham model correlations for describing solute transfer into anhydrous 1,2-propylene glycol for neutral and ionic species

“…A search of the published literature found gas-to-liquid partition coefficient, [18] infinite dilution activity coefficient [19,20] and solubility data for a chemically diverse set organic solutes dissolved in anhydrous 1,2-propylene glycol. Castells and coworkers [18] reported the gas-to-propylene glycol partition coefficients measured at 290 K for 18 hydrocarbons (alkanes, alkenes and alkylbenzenes) and for acetone, diisopropyl ether and 3 chloroalkanes, as well as the enthalpy of solution data needed to correct the measured log K values to 298.15 K. Sedov et al [19,20] determined the infinite dilution activity coefficients of hexane, heptane, octane, benzene, toluene, ethylbenzene, oxylene, m-xylene, p-xylene, 2-chloro-2-methylpropane, fluorobenzene and chlorobenzene dissolved in propylene glycol based on a gas chromatographic headspace analysis method.…”

“…Castells and coworkers [18] reported the gas-to-propylene glycol partition coefficients measured at 290 K for 18 hydrocarbons (alkanes, alkenes and alkylbenzenes) and for acetone, diisopropyl ether and 3 chloroalkanes, as well as the enthalpy of solution data needed to correct the measured log K values to 298.15 K. Sedov et al [19,20] determined the infinite dilution activity coefficients of hexane, heptane, octane, benzene, toluene, ethylbenzene, oxylene, m-xylene, p-xylene, 2-chloro-2-methylpropane, fluorobenzene and chlorobenzene dissolved in propylene glycol based on a gas chromatographic headspace analysis method. The measured infinite dilution activity coefficients, γ 1 solute , were converted to log K values through Equation (3):…”

Solvation of apolar compounds in protic ionic liquids: the non-synergistic effect of electrostatic interactions and hydrogen bonds

“…8 The same is true for protic non-ionic solvents, where the solubility decreases with increasing concentration of intermolecular hydrogen bonds. 9 In addition, aprotic ionic liquids (AILs) are known to have very small vapor pressures and huge enthalpies of vaporization due to strong interactions between the ions. Hydrogen bonds in protic molecular solvents also decrease their volatility and increase the energy cost of vaporization, at least relative to aprotic solvents, which are often demonstrated using a comparison of water (T b = 373.15 K, D vap H = 44 kJ mol À1 at 298 K) with hydrogen sulfide (T b = 212.9 K, D vap H = 18.6 kJ mol À1 at 298 K) or various protic and aprotic organic compounds.…”