Solubility of Anthracene in Binary Alcohol + 1-chlorobutane Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for anthracene dissolved in six binary alcohol + 1-chlorobutane solvent mixtures at 25°C. The alcohol cosolvents studied were 1-propanol, 2-propanol, 1-butanol, 2-butanol, 2-methyl-1-propanol and 3-methyl-1-butanol. Results of these measurements are used to test a mathematical representation based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister equation. For the six systems studied, the Combined NIBS/Redlich-Kister equation was found to mathematically describe the experimental data, with overall average absolute deviations between measured and calculated values being approximately\pm 0.4%.     

Solubility of Trans-Stilbene in Binary Alcohol + 1-Propanol Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for trans-stilbene dissolved in six binary alcohol + 1-propanol solvent mixtures at 25°C. The alcohol cosolvents studied were 2-propanol, 1-butanol, 2-butanol, 2-methyl-1-propanol, 1-pentanol and 3-methyl-1-butanol. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister and Modified Wilson equations. For the six systems studied, the Combined NIBS/Redlich-Kister equation was found to provide the better mathematical representation of the experimental data, with overall average absolute deviations between measured and calculated values being approximately ±0.4%. Slightly larger deviations were noted in the case of the Modified Wilson equation.     

Solubility of anthracene in binary toluene + alcohol solvent mixtures at 298.15 K

Experimental solubilities are reported for anthracene in eight binary toluene?+?alcohol solvent mixtures at 298.15?K. The alcohol solvents studied were 1-propanol, 1-butanol, 1-pentanol, 1-hexanol, 2-propanol, 2-butanol, 2-methyl-1-propanol and 3-methyl-1-butanol. Results of these measurements were used to test a mathematical representation based on the combined nearly ideal binary solvent (NIBS)/Redlich–Kister equation. For the eight systems studied, the combined NIBS/Redlich–Kister equation was found to accurately describe the experimental data, with an average absolute deviation between the measured and back-calculated values being approximately ±0.4%.     

Solubility of Anthracene in Binary Alkane+2-Methyl-2-Propanol Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for anthracene dissolved in four binary alkane + 2-methyl-2-propanol solvent mixtures at 25°C. The alkane cosolvents studied were n-heptane, cyclohexane, methylcyclohexane and 2,2,4-trimethylpentane. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister and Modified Wilson equations. For the four systems studied, the Combined NIBS/Redlich-Kister equation was found to provide the better mathematical representation of the experimental data, with overall average absolute deviations between measured and calculated values being approximately ±0.5%. Slightly larger deviations were noted in the case of the Modified Wilson equation.     

Solubility of Trans-Stilbene in Binary Alkane + 1-Butanol Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for trans-stilbene dissolved in six binary alkane + 1-butanol solvent mixtures at 25°C. The alkane cosoivents studied were hexane, heptane, octane, cyclohexane, methylcyclohexane and 2,2,4-trimethylpentane. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister and Modified Wilson equations. For the six systems studied, the Combined NIBS/Redlich-Kister equation was found to provide the better mathematical representation of the experimental data, with overall average absolute deviations between measured and calculated values being approximately ±0.6%. Slightly larger deviations were noted in the case of the Modified Wilson equation.     

Solubility of Trans-Stilbene in Binary Alkane + 1-Propanol Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for trans-stilbene dissolved in six binary alkane + 1-propanol solvent mixtures at 25°C. the alkane cosolvents studied were hexane, heptane, octane, cyclohexane, methylcyclohexane and 2,2,4-trimethylpentane. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister and Modified Wilson equations. for the six system studied, the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister equation provided the better mathematical representation of the experimental data, with an overall average absolute deviation between measured and calculated values being approximately 0.4%. Slightly larger deviations were noted in the case of the Modified Wilson equation.     

Solubility of Anthracene in Binary Alkane + 2-Ethoxyethanol Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for anthracene dissolved in six binary alkane + 2-ethoxyethanol solvent mixtures at 25°C. the alkane cosolvents studied were hexane, heptane, octane, cyclohexane, methylcyclohexane and 2,2,4-trimethylpentane. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister and Modified Wilson equations. for the six systems studied, the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister equation provided the better mathematical representation of the experimental data, with an overall average absolute deviation between measured and calculated values being approximately 0.4%. Slightly larger deviations were noted in the case of the Modified Wilson equation.     

Solubility of trans-Stilbene in Binary Alkane + 2-Propanol Solvent Mixtures at 298.2 K

Abstract

Experimental solubilities are reported for trans-stilbene dissolved in six binary alkane + 2-propanol solvent mixtures at 25[ddot]C. The alkane cosolvents studied were hexane, heptane, octane, cyclohexane, methylcyclohexane and 2,2,4-trimethylpentane. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister and Modified Wilson equations. For the six systems studied, both equations provided an accurate mathematical representation of the experimental data, with overall average absolute deviations between measured and calculated values being approximately ± 0.5%.     

Densities and Viscosities for the Binary Mixtures (2-Methyl-1-Chloropropane + Isomeric Butanol) at 298.15 and 313.15 K

Abstract

This paper reports excess volumes, V^E , and viscosity deviations, Δ\eta, for binary mixtures of 2-methyl-1-chloropropane with an isomer of butanol at the temperatures 298.15 K and 313.15 K. These properties were obtained from density and viscosity measurements. The results are correlated by means of a Redlich-Kister type equation, and interpreted in terms of molecular interactions. The systems show positive values of V^E except in a short range of compositions for mixtures containing primary butanols (1-butanol at both temperatures and 2-methyl-1-propanol at 298.15 K), whereas Δ\eta presents negative values at both temperatures over the whole composition range.     

Solubility of benzilic acid in select organic solvents at 298.15 K

Experimental solubilities are reported for benzilic acid dissolved in ethanol, 1-propanol, 1-butanol, 1-pentanol, 1-hexanol, 1-heptanol, 2-propanol, 2-butanol, 2-methyl-1-propanol, diethyl ether and methyl tert-butyl ether at 298.15?K. Results of these measurements reveal that the observed solubilities in the nine alcohol solvents fall within a fairly narrow mole fraction range of each other. Benzilic acid is also very soluble in the two ether solvents studied.     

Thermochemical investigations of hydrogen-bonded solutions. Part 11. Expressions for predicting anthracene solubilities in alcohol+alkoxyalcohol mixtures based on mobile order theory

Experimental solubilities are reported for anthracene dissolved in eight binary mixtures containing 2-ethoxyethanol with 1-propanol, 2-propanol, 1-butanol, 2-butanol, 2-methyl-1-propanol, 1-pentanol, 3-methyl-1-butanol and 1-octanol, and also in binary 1-pentanol+2-methoxyethanol and 2-methyl-1-propanol+2-propoxyethanol solvent systems at 25°C. Results of these measurements, combined with previously reported anthracene solubility data in 22 different alcohol +2-alkoxyethanol (2-methoxyethanol, 2-propoxyethanol and 2-butoxyethanol) solvent mixtures, are used to test the limitations and applications of expressions derived from Mobile Order theory. The first predictive expression assumes only formation of homogeneous self-associated hydrogen-bonded species, whereas the second equation includes additional terms to account for heterogeneous complex formation between the dissolved alcohol and 2-alkoxyethanol solvent molecules. Both equations predict the observed anthracene solubilities to within an average absolute deviation of about 3%.     

Oxidation of alcohols by dimethyldioxirane

The kinetics of oxidation of a series of monoatomic alcohols (methanol, 2-propanol, 2-butanol, 2-methyl-1-propanol, 2-chloroethanol, 1,3-dichloro-2-propanol, benzyl alcohol), hydroxyacetic acid, and 1,3-butandiol (ROH) by dimethyldioxirane (1) was studied. The reaction kinetics obeys the second order equationw=k[ROH][1]. The rate constants were measured in the range of 7–50†C, and the activation parameters were found. To describe the reaction rate constants as a function of the ROH structure, the two-parametric Taft equation was used, which takes into account both the polar and resonance substituent effects. Alcohol oxidation produces the corresponding carbonyl compounds,viz., ketones from secondary alcohols and aldehydes from primary alcohols, in yields of at least 80%. The results were explained by the competition of the molecular (oxenoid) and radical mechanisms. The introduction of electron-withdrawing substituents into the alcohol molecule increases the contribution of the radical channel of the reaction. Published inIzvestiya Akademii Nauk. Seriya Khimicheskaya, No. 8, pp. 1338–1343, August, 2000.     

(Solid + liquid) phase equilibria of binary mixtures containing N-methyl-2-pyrrolidinone and alcohol at atmospheric pressure

The (solid + liquid) equilibria of {N-methyl-2-pyrrolidinone + 1-propanol, or 2-propanol, or 1-butanol, or 2-methyl-1-propanol, or 2-methyl-2-propanol, or 1-pentanol} has been measured by a dynamic method. The experimental results have been correlated using the Wilson, UNIQUAC ASM and two modified NRTL equations. The root-mean-square deviations of the solubility temperatures for all the calculated values vary from (0.5 to 2.1) K and depend on the particular equation used. The specific interaction between the carbonyl group of the NMP molecule and the alcohol has been discussed.     

Excess molar enthalpies of methylformate + (1-propanol, 2-propanol, 1-butanol, 2-butanol and 1-pentanol) at T = 298.15 K, p = (5.0, 10.0) MPa, and methylformate + 1-propanol at T = 333.15 K, p = 10.0 MPa

A high pressure flow-mixing isothermal calorimeter is used to determine the excess molar enthalpies of methylformate + (1-propanol, 2-propanol, 1-butanol, 2-butanol and 1-pentanol) at T = 298.15 K and p = (5.0, 10.0) MPa, and methylformate + 1-propanol at T = 333.15 K and p = 10.0 MPa. The Redlich-Kister equation is fit to the experimental results.     

Complementary vapor pressure data for 2-methyl-1-propanol and 3-methyl-1-butanol at a pressure range of (15 to 177) kPa

The vapor pressure of pure 2-methyl-1-propanol and 3-methyl-1-butanol, components called congeners that are present in aroma of wine, pisco, and other alcoholic beverages, were measured with a dynamic recirculation apparatus at a pressure range of (15 to 177) kPa with an estimated uncertainty <0.2%. The measurements were performed at temperature ranges of (337 to 392) K for 2-methyl-1-propanol and (358 to 422) K for 3-methyl-1-butanol. Data were correlated using a Wagner-type equation with standard deviations of 0.09 kPa for the vapor pressure of 2-methyl-1-propanol and 0.21 kPa for 3-methyl-1-butanol. The experimental data and correlation were compared with data selected from the literature.     

Enzymatic esterification and phase behavior in ionic microemulsions with different alcohols

The esterification of hexanoic acid and 1-pentanol catalyzed by the lipase fromChromobacterium viscosum was studied at 298.2 K using different Winsor systems as reaction medium. The microemulsion systems consisted of brine and alkane stabilized by the anionic surfactant sodium dodecylsulphate and a short-chained alcohol. The alcohol acts both as a reactant and as a part of the reaction medium. Therefore, it is of great fundamental interest to know the phase behavior of the used microemulsion systems. Partial phase diagrams were determined and the efficiency of different alcohols on the transition from a Winsor I system to a Winsor III or a Winsor IV system with bicontinuous structure and further to a Winsor II system was investigated. The investigated alcohols were 2-methyl-1-propanol, 1-butanol, 2-butanol, 2-methyl-1-butanol, 3-methyl-1-butanol, 1-pentanol, 2-pentanol, 3-pentanol, 2-methyl-1-pentanol, 3-methyl-1-pentanol, 4-methyl-1-pentanol, and 1-hexanol. The aqueous medium consisted of 0.5 m NaCl(aq) or a phosphate buffer (pH=7) and the organic medium of octane or 2,2,4-trimethyl pentane. A long alkyl chain of the alcohol or a branching far from the hydroxyl group gives a more efficient cosurfactant and a transition from Winsor I to Winsor III or Winsor IV at lower alcohol contents. In the Winsor III system the yield of 1-pentyl hexanoate is twice as high as the yield in the bicontinuous Winsor IV system.     

Refractive Indices of the Ternary Mixtures Butanol + <Emphasis Type="Italic">n</Emphasis>-Hexane + 1-Chlorobutane

Refractive indices for the ternary mixtures formed by each one of the isomers of butanol (1-butanol, 2-butanol, 2-methyl-1-propanol and 2-methyl-2-propanol), with n-hexane and 1-chlorobutane, have been measured at 298.15 K. From these data the refractive index deviations were calculated and fitted by Cibulka’s equation, and the refractive index deviations were related to the corresponding excess volumes of the mixtures. Furthermore, several mixing rules were used to predict both refractive indices and excess volumes of the ternary mixtures from their densities or refractive indices. Electronic Supplementary Material  The online version of this article () contains supplementary material, which is available to authorized users.     

Solubility of ethyl-(2-hydroxyethyl)-dimethylammonium bromide in alcohols (C2–C12)

The solubilities of a novel third generation of the precursor of ionic liquids, named ethyl-(2-hydroxyethyl)-dimethylammonium bromide, C₂Br, in alcohols {ethanol, 1-butanol, 1-hexanol, 1-octanol, 1-decanol, 1-dodecanol, 2-butanol, 2-methyl-2-propanol (tert-butyl alcohol)} have been measured by a dynamic method from 240 to 440 K.The solubility of ethyl-(2-hydroxyethyl)-dimethylammonium bromide in primary alcohols decreases with an increase of the molecular weight of the alcohol from C₂ to C₁₂. The differences in solubilities between the primary and secondary alcohols are not significant. The solubility of C₂Br in tert-butyl alcohol is much lower than in 1-butanol and 2-butanol.The data were correlated by means of the UNIQUAC ASM, NRTL1 and NRTL2 equations, utilizing parameters derived from the (solid + liquid) equilibrium (SLE) data. The root-mean-square deviations of the solubility temperatures for all calculated data are from 2.36 to 7.17 K and depend on the particular equation used. In the calculations, the existence of a solid–solid first-order phase transition in pure C₂Br has also been taken into account.