Development of a correlation between the non-polar solubility parameter, refractive index and molecular structure. II. Aliphatic ethers and alcohols

Wingefors, Stig

doi:10.1002/jctb.280310171

Cited by 35 publications

(8 citation statements)

References 6 publications

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“…The existence of the solid−solid phase transition was observed for both solutes under study and was observed previously only for 2-methyl-1 H -imidazole 5 Molar Volume, V m , and Association Parameters for Alcohols V m (298.15 K)− Δ H alcoholcm 3 ·mol -1 a kJ·mol -1 K (298.15 K) 1-propanol 72.7 25.1 b 197 b 1-butanol 92.0 25.1 b 175 b 2-butanol 92.4 25.1 150 2-methyl-2-propanol 94.9 25.1 110 1-hexanol 125.3 25.1 c 120 c a From ref . b From ref .…”

Section: Resultssupporting

confidence: 66%

Solubility of Benzimidazoles in Alcohols

and

Bogel‐Łukasik

2003

J. Chem. Eng. Data

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The solid−liquid equilibrium (SLE) has been measured from 270 K to 445 K for 10 binary mixtures of benzimidazoles (benzimidazole and 2-methylbenzimidazole) with alcohols (1-propanol, 1-butanol, 2-butanol, 2-methyl-2-propanol, 1-hexanol) using a dynamic method. The melting point, enthalpy of fusion, and heat capacity change at the melting temperature were determined by differential scanning calorimetry (DSC). The solubility of benzimidazoles in alcohols (C3−C6) is higher than in water and in 1-octanol and generally decreases with an increase of the alkyl chain length of the alcohol. The intermolecular solute−solvent interaction is higher for the 1-alcohol than for the secondary or tertiary alcohol. The solubility of 2-methylbenzimidazole in alcohols (C3−C6) is higher than that of benzimidazole. Experimental results of solubility were correlated by means of the Wilson, UNIQUAC ASM, and NRTL 1 equations utilizing parameters derived from SLE results. The existence of a solid−solid first-order phase transition in benzimidazole and 2-methylbenzimidazole has been observed in the DSC measurements and has been taken into consideration in the solubility calculation. The best correlation of the solubility data has been obtained by the NRTL 1 equation.

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Section: Resultssupporting

confidence: 66%

Solubility of Benzimidazoles in Alcohols

and

Bogel‐Łukasik

2003

J. Chem. Eng. Data

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“…Thus, for instance Letcher and Govender 14 applied the method to mixtures of cyclic ethers with short alkanols, from methanol to propanol, and took n -heptane as the homomorph of the alkanol in every case. An additional problem is the disagreement found when reviewing as to the guidelines governing the selection of the apolar homomorph of a given molecule, ,− geometric considerations apart. Let us examine the simplest case, that of linear compounds.…”

Section: Theorymentioning

confidence: 99%

Thermodynamics of Mixing Tetrahydropyran with 1-Alkanols and Excess Enthalpies of Homomorphy-Related Systems

2007

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Densities (F) and volumetric heat capacities (C p /V) have been measured at 298.15 K over the whole mole fraction range for the binary mixtures {tetrahydropyran + 1-propanol, + 1-butanol, + 1-pentanol, + 1-hexanol, + 1-heptanol, + 1-octanol, + 1-nonanol, or + 1-decanol}. From experimental data, the excess molar isobaric heat capacities (C p E ) were calculated. Excess molar volumes (V E ) are reported for the systems containing 1-propanol, 1-butanol, 1-pentanol, and 1-decanol. In order to assess and compare the different degrees of hetero-association in these mixtures, the corresponding negative enthalpic contributions at equimolar fraction (H int ) have been calculated semiquantitatively by using the apolar homomorph concept. With this aim, excess molar enthalpies (H E ) of {tetrahydropyran + 1-pentanol, + 1-nonanol, or + 1-decanol}, {tetrahydropyran + decane}, and {cyclohexane + 1-pentanol, + 1-heptanol, + 1-nonanol, or + 1-decanol} have been measured at 298.15 K. The results are discussed in terms of molecular interactions. The various steps of W-shape concentration dependence found in the C p E point to the occurrence of local nonrandomness in THP + alkanol mixtures.

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“…In addition, a semiempirical relationship was proposed by Wingefors and Liljenzin , as δ d = K d n D 2 − 1 n D 2 + 2 ( 1 + a V m + b V m 2 ) ∑ g i j where K d , a , and b are the empirical constants relating to the molecular structures, and g ij is the structural parameters determined by the molecular structures (∑ g ij ∼ 0.92–1). Wingefors and Liljenzin confirmed the practicality of eq using the data of aliphatic hydrocarbons, ethers, and alcohols. , We noticed that the plot of δ d versus ( n D 2 – 1)/( n D 2 + 2) for each type of liquids shows a linear correlation (Figure S9, SI), with an R 2 of ∼0.861 for nonpolar liquids, ∼0.692 for polar liquids, and ∼0.772 for H-bonded liquids. Commonly, a / V m ≪ 1, b / V m 2 ≪ 1, and ∑ g ij ≈ 1 .…”

Section: Resultsmentioning

confidence: 99%

“…Some fundamental physical properties of substances such as the relative dielectric constant (ε r ), refractive index ( n D ), and density (ρ) are closely related to the intermolecular interactions, similar to the cases of γ and δ parameters. − Therefore, there must exist some intrinsic correlations between the characteristic parameters (γ and δ) and the fundamental physical quantities (ε r , n D , and ρ) for substances. ,, Several empirical (or semiempirical) equations relating γ t , δ t , and δ d to ε r and n D have been proposed for liquids so far, − but their accuracy and applicability are limited (see Results and Discussion). We noticed that almost all of the equations previously proposed do not involve density, an important physical quantity of substances.…”

Section: Introductionmentioning

confidence: 99%

Correlations of Surface Free Energy and Solubility Parameters with Dielectric Constant, Refractive Index, and Density for Liquids

Wang,

Hou

2024

J. Phys. Chem. B

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There should be some intrinsic correlations between the surface free energy (γ) and solubility (δ) parameters, called characteristic parameters here, of substances with their fundamental physical properties such as the refractive index ( n D), relative dielectric constant (εr), and density (ρ) because they are all related to intermolecular interactions. Understanding the correlations between characteristic parameters and fundamental physical quantities is of great fundamental and practical importance. In the current work, possible relationships between the characteristic parameters (γ and δ) and the physical quantities (n D, εr, and ρ) were explored by a trial-and-error fitting method based on the data of 92 liquids (including 14 nonpolar, 37 polar, and 41 hydrogen-bonded liquids). The γ parameters include total (γt), dispersive (γd), and polar (γp) ones, and the δ parameters include the Hildebrand parameter (δt) and the Hansen-dispersive (δd), polar (δp), and hydrogen-bonded (δh) ones. For each characteristic parameter, its relationship with the physical quantities was established. The applicability of the so-obtained relationships was confirmed using the data of another 66 liquids as an external data set. The empirical relationships can be used to estimate the characteristic parameters of liquids from their easily measurable physical quantities.

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Development of a correlation between the non-polar solubility parameter, refractive index and molecular structure. II. Aliphatic ethers and alcohols

Cited by 35 publications

References 6 publications

Solubility of Benzimidazoles in Alcohols

Solubility of Benzimidazoles in Alcohols

Thermodynamics of Mixing Tetrahydropyran with 1-Alkanols and Excess Enthalpies of Homomorphy-Related Systems

Correlations of Surface Free Energy and Solubility Parameters with Dielectric Constant, Refractive Index, and Density for Liquids

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