Solubility Of Anthracene Research Articles

Solubility of Anthracene in Binary Alcohol + 2-Pentanol and Alcohol + 4-Methyl-2-pentanol Solvent Mixtures

Experimental solubilities are reported for anthracene dissolved in 16 binary mixtures containing either 2-pentanol or 4-methyl-2-pentanol with 1-propanol, 2-propanol, 1-butanol, 2-butanol, 1-pentanol, 1-octanol, 2-methyl-1-propanol and 3-methyl-1-butanol at 25 °C. Results of these measurements are used to test two mathematical representations based upon the combined nearly ideal binary solvent (NIBS)/Redlich−Kister equation and modified Wilson model. For the 16 systems studied, both equations were found to provide an accurate mathematical representation of the experimental data, with an overall average absolute deviation between measured and calculated values being 0.3% and 0.5% for the combined NIBS/Redlich−Kister and modified Wilson equations, respectively.

A Recirculating Equilibrium Procedure for Determining Organic Compound Solubility in Supercritical Fluids. Anthracene in Carbon Dioxide

An instrumental recirculation technique was developed to measure the solubility of organic compounds and thus their potential extractability, in supercritical fluids over the pressure range of 80−500 bar. Anthracene, whose solubility is well defined, was chosen as a model compound to be used in evaluating the recirculation technique. Its solubility in supercritical carbon dioxide was measured at 40, 50, and 60 °C using an off-line spectroscopic technique. The solubility data were found to have good precision and to agree with published results. Anthracene solubility increased with pressure but was more enhanced by higher temperature. An upper crossover pressure of the isotherms due to retrograde vaporization that agreed with theory was found at 142.2 bar.

Solubility of Anthracene and Pyrene in Binary Alcohol + Alcohol Solvent Mixtures

Article on the solubility of anthracene and pyrene in binary alcohol + alcohol solvent mixtures.

Solubility of Anthracene in Binary Alcohol + 2-Ethyl-1-hexanol Solvent Mixtures

Experimental solubilities are reported for anthracene dissolved in seven binary mixtures containing 2-ethyl-1-hexanol with 1-propanol, 2-propanol, 1-butanol, 2-butanol, 1-octanol, 2-methyl-1-propanol, and 3-methyl-1-butanol at 25 C. Results of these measurements are used to test two mathematical representations based upon the combined nearly ideal binary solvent (NIBS)/Redlich-Kister equation and modified Wilson model. For the seven systems studied, both equations were found to provide an accurate mathematical representation of the experimental data, with an overall average absolute deviation between measured and calculated values on the order of 0.6%. solvent mixtures. Results of these measurements are used to further test the descriptive abilities of several previously derived expressions. Experimental Methods Anthracene (Aldrich, 99.9+%) was used as received. 2-Ethyl-1-hexanol (Aldrich, 99+%), 1-propanol (Aldrich, 99+%, anhydrous), 2-propanol (Aldrich, 99+%, anhydrous), 1-butanol (Aldrich, HPLC, 99.8+%), 2-butanol (Aldrich, 99+%, anhydrous), 2-methyl-1-propanol (Aldrich, 99+%, anhydrous), 3-methyl-1-butanol (Aldrich, 99+%, anhy- drous), and 1-octanol (Aldrich, 99+%, anhydrous) were stored over both anhydrous sodium sulfate and molecular sieves before being fractionally distilled. Gas chromato- graphic analysis showed solvent purities to be 99.7 mol % or better. Karl Fischer titration gave water contents (mass1 mass %) of <0.01% for all seven alcohols used. Binary solvent mixtures were prepared by mass so that composi- tions could be calculated to 0.0001 mole fraction. Excess solute and solvent were placed in amber glass bottles and allowed to equilibrate in a constant tempera- ture water bath at (25.0 f 0.1) C for at last 3 days (often longer). Attainment of equilibrium was verified by repeti- tive measurements after a mimimum of three additional days and by approaching equilibrium from supersaturation by preequilibrating the solutions at a higher temperature. Aliquots of saturated anthracene solutions were trans- ferred through a coarse filter into a tared volumetric flask to determine the amount of sample and diluted quantita- tively with methanol. Concentrations were determined spectrophotometrically at 356 nm on a Bausch and Lomb Spectronic 2000. Experimental anthracene solubilities in the seven binary alcohol + 2-ethyl- 1-hexanol mixtures studied are listed in Table 1. Numerical values represent the average of between four and eight independent deter- minations, with the measured values being reproducible to within f1.3%.

Solubilities of Phenols in Supercritical Carbon Dioxide

Equilibrium solubilities of pure anthracene at 50 °C, 1-naphthol at 35, 45, and 55 °C, and hydroquinone at 35 and 45 °C in supercritical carbon dioxide over a pressure range of about 85-300 bar have been measured using a supercritical fluid extractor coupled with an external high-pressure liquid chromatographer. The solubility results, along with those for other phenols reported in the literature, are correlated with the translated-modified Peng Robinson equation of state.

Self‐Association of Dexverapamil in Aqueous Solution

The pKaand intrinsic solubility of monomeric dexverapamil were determined from its pH–solubility profile to be 8.90 and 6.6 × 10−5M, respectively. The solubility of dexverapamil below pH 7.0 was higher than expected on the basis of the aforementioned values. This unusually high solubility is believed to be due to the self‐association of cationic dexverapamil. The apparent pKaof the self‐associated drug is estimated to be ∼7.99. The self‐association of dexverapamil hydrochloride is supported by the fact that it is surface active and that it increases the solubility of both naphthalene and anthracene in aqueous solutions. The dependence of the drug solubility on pH and the solubilization of naphthalene and anthracene as a function of ionized drug concentration suggest that the self‐associated dexverapamil is a cationic dimer.

Thermochemical investigations of hydrogen-bonded solutions Part 6. Comparison of mobile order theory versus Kretschmer-Wiebe association model for describing anthracene solubilities in binary hydrocarbon + alcohol solvent mixtures

A conventional nonelectrolyte self-associated solution model, which has led to successful descriptive equations for excess molar enthalpies and excess molar Gibbs free energies, is extended to systems containing an inert solute dissolved in binary hydrocarbon + alcohol solvent mixtures. An expression is derived for predicting the solubility of crystalline solutes from a prior knowledge of the solubility in the two pure solvents. Applications and limitations of the newly derived equation were assessed using published solubility data for anthracene in 30 different binary solvent systems containing 1-propanol, 2-propanol, 1-butanol, 2-butanol, or 1-octanol. The derived expression predicted the observed values to within an overall average absolute deviation of approximately 5.7% using zero adjustable “curve-fit” parameters. Mobile order theory, in comparison, provides comparable predictions, with deviations between predicted and experimental values being on the order of approximately 5.7%.

Solubility of Anthracene and Anthraquinone in Cyclohexanone + Carbon Dioxide

In the processing of an anthracene oil fraction from coal tar, a mixture of anthracene and anthraquinone is required to be separated to obtain products of high purity. The solubilities of anthracene and anthraquinone were measured in cyclohexanone + carbon dioxide as a function of the temperature and pressure of carbon dioxide at 291, 300, and 313 K and from 1.8--12.4 MPa. Average equilibrium solubilities and recoveries of both solids increased with increasing normalized concentration and pressure. The average separation factor of anthracene to anthraquinone, due to the effect of the mixed solvent, was 2.88 [+-] 1.91.

Solubility of Anthracene in Binary Alkane + 3-Methyl-1-butanol Solvent Mixtures

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTSolubility of Anthracene in Binary Alkane + 3-Methyl-1-butanol Solvent MixturesAnita I. Zvaigzne and William E. Jr. AcreeCite this: J. Chem. Eng. Data 1994, 39, 4, 708–710Publication Date (Print):October 1, 1994Publication History Published online1 May 2002Published inissue 1 October 1994https://doi.org/10.1021/je00016a015RIGHTS & PERMISSIONSArticle Views198Altmetric-Citations17LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (285 KB) Get e-Alerts Get e-Alerts

Thermochemical investigations of hydrogen-bonded solutions Part 5. Development of predictive equations for the solubility of anthracene in binary alcohol + alcohol mixtures based upon mobile order theory

Abstract The unconventional solution model of Mobile Order which had previously been shown to provide a very accurate thermodynamic description of anthracene solubilities and chemical potentials in binary hydrocarbon + alcohol solvent mixtures is extended to binary solvent systems containing two self-associating alcohol co-solvents. Expressions are derived for predicting the solubility of crystalline solutes from a prior knowledge of the solubility in the two pure alcohol solvents. Applications and limitations of the newly derived equations are assessed using anthracene solubilities in binary 2-propanol+l-1-propanol 1-butanol + 1-propanol, 2-butanol + 1-propanol, 1-octanol + 1-propanol, 1-butanol + 2-propanol, 2-butanol + 2-propanol, and 1-octanol + 2-butanol mixtures which are measured as part of the present study. The two most successful expressions permit each individual alcohol co-solvent to form homogeneous hydrogen-bonded complexes. Both equations predict the experimental anthracene solubilities to within an average absolute deviation of about ± 2%. Inclusion of terms to account for heterogeneous complex formation between two dissimilar alcohols has little effect on the predicted values.

Solubility of Anthracene in Binary Alkane + 2-Methyl-1-propanol Solvent Mixtures

Article on the solubility of anthracene in binary alkane + 2-methyl-1-propanol solvent mixtures.

Thermochemical Investigations of Hydrogen-Bonded Solutions: Part 4. Prediction of Liquid-Vapor Equilibria for Binary 2,2,4-Trimethylpentane + 1-Alkanol Mixtures Using Mobile Order Theory

Abstract The unconventional solution model of Mobile Order, which previously had been shown to provide a very accurate thermodynamic description of anthracene solubilities and chemical potentials in binary hydrocarbon + alcohol solvent mixtures, is extended to other thermodynamic excess properties. An expression is derived for predicting liquid-vapor equilibria of binary hydrocarbon + alcohol systems. Applications and limitations of the newly-derived predictive expression are assessed using published vapor pressure data for binary mixtures containing 2,2,4-trimethylpentane with 1-propanol, 1-butanol, 1-pentanol, 1-hexanol, 1-heptanol and 1-octanol.

Biological remediation of anthracene-contaminated soil in rotating bioreactors

Soil impregnated with anthracene was subjected to bacterial treatment as a model for remediation of soils contaminated with polycyclic aromatic hydrocarbons (PAHs). Roller bottles were used to simulate the mixing of solids in rotating drums. The soil was prepared as a 60 weight % slurry in salts medium, and inoculated with a mixed culture, selected for the ability to mineralize anthracene as its sole carbon source. The degradation of anthracene followed zero-order kinetics when it was well dispersed on the soil particles, consistent with a rate limitation by dissolution of solid hydrocarbon. Maximum degradation rates of 300 μg/g per day were achieved in repeated batch operation, using a 10% volume of soil slurry as the inoculum for the succeeding batch. Anthracene degradation activity was maintained through 18 such transfers on a 3- to 4-day cycle. The culture produced soluble compounds that enhanced the solubility of anthracene in aqueous solution. Soil components did not have a significant effect on growth or degradation. Degradation of anthracene ceased when the concentration in soil dropped to approx. 30 μg/g, from an initial value of 600 μg/g.

Thermochemical investigations of hydrogen-bonded solutions: development of a predictive equation for the solubility of anthracene in binary hydrocarbon

Acree W.E., Jr., Zvaigzne A.I. and Tucker S.A., 1994. Thermochemical investigations of hydrogen-bonded solutions: development of a predictive equation for the solubility of anthracene in binary hydrocarbon + alcohol mixtures based upon Mobile Order theory. Fluid Phase Equilibria, 92: 233-253. Experimental solubilities are reported for anthracene dissolved in twelve binary solvent mixtures containing either 2-propanol or 1-octanol with n-hexane, n -heptane, n -octane, cyclohexane, methylcyclohexane and 2,2,4-trimethylpentane at 25.0°C. Results of these measurements, along with previously published solubility data for anthracene in binary 1-propanol+alkane and 1-butanol + alkane mixtures, are used to test the limitations and applications of expressions derived from Mobile Order theory. The best descriptive equation expresses the logarithm of the volume fraction solubility in binary mixtures as a simple volume fraction average of the corresponding logarithm solubilities in the two pure solvents, and contains additional terms to represent contributions from nonspecific physical interactions between dissimilar solvent components, from molecular size disparity, and from the reduction in mobile disorder caused by the self-association by hydrogen bonding of the alcohol solvent. The newly derived expression predicts the observed anthracene solubilities to within an overall average deviation of ca. 4.4% using a single value of K c = 5000 for the self-association equilibrium constant.

Modeling of anthracene removal from soil columns by surfactant

Abstract In‐situ soil washing using surfactants shows great potential to remove hydrophobic organics from subsurface environments. Lab scale soil washing experiments were performed using sodium dodecylsulfate (SDS), an anionic surfactant, to remove anthracene, a highly hydrophobic compound. The formation medium chosen was fine sand. Anthracene solubility tests were conducted in batch reactors. The results showed that the solubility of anthracene increases linearly with an increase in SDS concentration above the critical micellar concentration. The kinetics of anthracene solubilization from contaminated sand in batch reactors was observed to follow the exponential Elovich equation. Column experiments were performed using either SDS solution or water to mobilize anthracene from contaminated soil. These experiments verified that SDS can be effective in removing anthracene from contaminated sand mainly due to the solubility increase by micellization. A mathematical model for soil washing was formulated using two sets of mass conservation equations for surfactant and anthracene distribution. The mixing‐cell concept was used to obtain solutions for column experiments.

Thermochemical investigations of hydrogen-bonded solutions: Part 2. Comparison of mobile order theory versus Mecke-Kempter association model for describing anthracene solubilities in binary hydrocarbon + alcohol

William E. Acree, Jr., Anita I. Zvaigzne and Sheryl A. Tucker, 1994. Thermochemical investigations of hydrogen-bonded solutions. Part 2. Comparison of Mobile Order theory versus Mecke-Kempter association model for describing anthracene solubilities in binary hydrocarbon + alcohol solvent mixtures. Fluid Phase Equilibria, 92: 1-17. A conventional non-electrolyte self-associated solution model, which has led to successful descriptive equations for excess molar enthalpies and excess molar Gibbs free energies, is extended to systems containing an inert solute dissolved in binary hydrocarbon + alcohol solvent mixtures. An expression is derived for predicting the solubility of crystalline solutes from a prior knowledge of the solubility in the two pure solvents. Applications and limitations of the newly derived equation were assessed using published solubility data for anthracene in 30 different binary solvent systems containing 1-propanol, 2-propanol, 1-butanol, 2-butanol or 1-octanol. The derived expression predicted the observed values to within an overall average absolute deviation of approximately 9.4 % using zero adjustable “curve-fit” parameters. Mobile Order theory, in comparison, provides slightly superior predictions, with deviations between predicted and experimental values being in the order of approximately 5.7%.

Thermochemical investigations of hydrogen-bonded solutions: Part 3. Development of expression for predicting excess enthalpies of ternary alcohol + two inert hydrocarbon systems based upon Mobile Order theory

William E. Acree, Jr., 1994. Thermochemical investigations of hydrogen-bonded solutions. Part 3. Development of expression for predicting excess enthalpies of ternary alcohol + two inert hydrocarbon systems based upon Mobile Order theory. Fluid Phase Equilibria, 92: 19-34. The unconventional solution model of Mobile Order, which has previously been shown to provide a very accurate thermodynamic description of anthracene solubilities and chemical potentials in binary hydrocarbon + alcohol solvent mixtures, is extended to other thermodynamic excess properties. An expression is derived for predicting excess molar enthalpies of ternary alcohol + two inert hydrocarbon systems from measured binary data. Applications and limitations of the newly derived predictive expression are assessed using published enthalpy data for ternary ethanol + n-hexane + n-decane, ethanol + n-hexane + n-dodecane, 1-propanol + n-hexane + n-decane and 1-propanol + n-hexane + n-dodecane systems.

Solubility of anthracene in binary alkane + 1-propanol and alkane + 1-butanol solvent mixtures

Article on the solubility of anthracene in binary alkane + 1-propanol and alkane + 1-butanol solvent mixtures.

Washing of hydrophobic organic from contaminated sand with a surfactant

The use of surfactants shows great potential for the removal of hydrophobic organics from soils by in-situ washing techniques. Lab-scale soil washing experiments were performed using sodium dodecylsulfate (SDS), an anionic surfactant, and anthracene, a highly hydrophobic compound. The results of this research show that the solubility of anthracene increases linearly with an increase in SDS concentration above the critical micellar concentration. Furthermore, SDS can be effective in removing anthracene from contaminated sand.

Solubility of Anthracene in Binary Alkane + Dimethyl Adipate and Alkane + Dibutyl Oxalate Solvent Mixtures

Abstract Experimental solubilities are reported for anthracene dissolved in three binary mixtures containing dimethyl adipate with cyclohexane, methylcyclohexane and n-heptane, and in six solvent mixtures containing dibutyl oxalate with n-hexane, n-heptane, n-octane, cyclohexane, methylcyclohexane and isooctane at 25°C. Results of these measurements are used to test two mathematical representations based upon the combined Nearly Ideal Binary Solvent (NIBS)/Redlich-Kister equations and Modified Wilson model. For the systems studied, the combined NIBS/Redlich-Kister equation was found to provide the better mathematical representation with deviations between experimental and back-calculated values being on the order of ± 3% or less.