The solubility of low-molecular-weight hydrocarbons in non-volatile liquids

Ashworth, Anthony J.; Everett, D. H.

doi:10.1039/tf9605601609

Cited by 98 publications

(26 citation statements)

References 2 publications

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“…In Abraham's solvation model [14,28,29] the partition coefficient is the sum of the terms corresponding to the different solute-stationary phase interactions, according to the equation:…”

Section: Theorymentioning

confidence: 99%

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Interactions between 33 solutes and four cyano-containing stationary phases: gas chromatographic activity coefficients and the solvation parameter model

Santiuste

Takács²

2003

Analytical and Bioanalytical Chemistry

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Infinite-dilution gas-liquid chromatographic activity coefficients at 393.15 K (with their thermal and athermal components) and derived excess partial molar Gibbs energies, enthalpies, and entropies have been determined for each of 33 solutes of different polarity on four stationary phases with cyano groups, using retention data taken from the literature. The strongest interactions predicted by the solvation model are the dipolarity/polarizability, the acidic solute-basic stationary phase interaction, and nonpolar cavity formation and dispersion. These interactions were compared with those evaluated from the solute activity coefficients; the effect of the solute connectivity index and dipole moment on nonpolar and polar interactions, respectively, is discussed. The dependence of the thermal activity coefficient on nonpolar interactions, and the influence of stationary phase polarity on the four solute-stationary phase interactions, were evaluated. The nonpolar interaction increases with increasing connectivity and with increasing athermal activity coefficient. The dipolarity/polarizability interaction increases with increasing solute dipole moment. Finally, polar interactions increase with increasing stationary phase polarity whereas the nonpolar interaction is independent of stationary phase polarity.

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“…In Abraham's solvation model [14,28,29] the partition coefficient is the sum of the terms corresponding to the different solute-stationary phase interactions, according to the equation:…”

Section: Theorymentioning

confidence: 99%

“…Gas chromatography is a valuable analytical technique of proved power for studying the physicochemical properties of analytes, especially thermodynamic magnitudes, with the advantage of its readiness as compared with other techniques [1, 2,3,4,5].…”

Section: Introductionmentioning

confidence: 99%

Interactions between 33 solutes and four cyano-containing stationary phases: gas chromatographic activity coefficients and the solvation parameter model

Santiuste

Takács²

2003

Analytical and Bioanalytical Chemistry

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“…Some of them are quite elaborate and require detailed information about the physical properties of solute and solvent molecules. Based on quasi-lattice theory, Everett and co-workers (29,30) have explained the deviation from Raoult's law as due to combination of two completely independent factors, namely disparity in molecular size of solute and solvent (combinatorial or configurational term or the athernlal part) and secondly, due to difference in intermolecular forces (the thermal part).…”

Section: Methodsmentioning

confidence: 99%

Studies on thermodynamics of solution by gas chromatography: solubility measurements of hydrocarbons in cycloalkanols

Kuchhal¹,

Mallik²,

Gupta³

1977

Can. J. Chem.

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Activity coefficients at infinite dilution have been determined by gas–liquid chromatography for nine hydrocarbons solutes in cyclopentanol, cyclohexanol, cycloheptanol, benzyl alcohol, and n-heptanol at 25 °C. Experimental results for cyclopentane and cyclohexane in cycloalkanols compare favourably with the values obtained by extrapolation to infinite dilution of activity coefficient data calculated from Benson et al.'s static (vapour–liquid equilibrium) measurements. Some characteristics of the solute–solvent interaction in the systems are discussed in light of statistical approaches (thermal and athermal contributions).

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“…According to solution theories [4], the solute activity coefficient (yj) based on mole fraction consists of an athermal term and a thermal term. At infinite dilution, in terms of the Flory-Huggins equation for the athermal term and the Hildebrand-Scatchard equation for the thermal term, this may be expressed [5] as…”

Section: Introductionmentioning

confidence: 99%

Calculation of Aqueous Solubility of Organic Compounds

Tewari

Miller

Wasik

1982

J. RES. NATL. BUR. STAN.

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The aqueous solubility of 14 organic solutes has been calculated from their octanoL/water partition coefficient and from their solute activity coefficient in octanol at infinite dilution. The solute activity coefficients were calculated from the Flory-Huggins and Hildebrand-Scatchand (FH-HS) equations and were found to be in good agreement with the activity coefficients detennined from GC specific retention volume measurements. The calculated solubilities were in good agreement with the experimental solubilities.

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The solubility of low-molecular-weight hydrocarbons in non-volatile liquids

Cited by 98 publications

References 2 publications

Interactions between 33 solutes and four cyano-containing stationary phases: gas chromatographic activity coefficients and the solvation parameter model

Interactions between 33 solutes and four cyano-containing stationary phases: gas chromatographic activity coefficients and the solvation parameter model

Studies on thermodynamics of solution by gas chromatography: solubility measurements of hydrocarbons in cycloalkanols

Calculation of Aqueous Solubility of Organic Compounds

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