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Junbo Gong - One of the best experts on this subject based on the ideXlab platform.

  • Experimental and Modeling Studies on the Solubility of d-Pantolactone in Four Pure Solvents and Ethanol–Water Mixtures
    Journal of Chemical & Engineering Data, 2015
    Co-Authors: Cui Huang, Zhiping Xie, Yujia Qin, Junbo Gong
    Abstract:

    The solubility of d-pantolactone in water, ethanol, methanol, ethyl acetate, and ethanol–water mixtures was determined at temperatures between (278.15 and 318.15) K using a digital densitometer by a static method. The measured solubility data were correlated with Apelblat Equation, van’t Hoff Equation, nonrandom two liquid model, and Wilson model. The results indicate that the Wilson model is the most suitable model in pure solvents and the Apelblat model is the best model in ethanol–water mixtures.

  • Measurement and Correlation of the Solubility of Penicillin V Potassium in Ethanol + Water and 1‑Butyl Alcohol + Water Systems
    2015
    Co-Authors: Tingting Wei, Chen Wang, Junbo Gong
    Abstract:

    The solubility of penicillin V potassium (PVK) in binary ethanol + water and 1-butyl alcohol + water solvent mixtures was measured at temperatures ranging from (278.15 to 313.15) K. The solubility in ethanol + water was measured by a static analytical method while in 1-butyl alcohol + water a dynamic method was adopted. It was found that the solubility of PVK increased with increasing temperature as well as the increase of the initial mole fraction of water. The modified Apelblat Equation, the CNIBS/R-K Equation, the combined version of the Jouyban-Acree and van’t Hoff model, and the hybrid model were used to correlate the solubility data in ethanol + water solvent mixtures, among which the CNIBS/R-K Equation gave the best correlation results. The experimental solubility data in 1-butyl alcohol + water were correlated well by the van’t Hoff Equation and the modified Apelblat Equation. The dissolution enthalpy, entropy, and Gibbs energy of PVK in these solvent mixtures were obtained based on the van’t Hoff Equation

  • measurement and correlation of the solubility of l carnitine in different pure solvents and ethanol acetone solvent mixture
    Journal of Chemical & Engineering Data, 2014
    Co-Authors: Dengqiong Sun, Riju Ren, Weiqiang Dun, Haihong Zhang, Lijun Zhao, Li Zhang, Wenqing Zhang, Junbo Gong
    Abstract:

    A gravimetric method was used to determine the solubility of l-carnitine in different pure solvents and ethanol–acetone solvent mixture. The solubility in different pure solvents were then correlated by the modified Apelblat Equation, λh Equation and the modified van’t Hoff Equation, with the modified van’t Hoff Equation presenting the best consistence. Meanwhile, to illustrate the effect of ethanol or acetone on the change of the solubility, a new parameter defined as influence coefficient was introduced and the coefficient of acetone depending on temperature and molar faction of acetone was depicted. In addition, the changes for enthalpy, entropy and Gibbs free energy were calculated by the modified van’t Hoff Equation. It can be drawn that the changes for enthalpy and entropy in a solvent mixture decrease to a minimum before consequent increasing with increasing molar faction of acetone. Furthermore, the change for Gibbs free energy shows a linear relationship with natural logarithm of the solubility.

  • Measurement and Correlation of the Solubility of l-Carnitine in Different Pure Solvents and Ethanol–Acetone Solvent Mixture
    Journal of Chemical & Engineering Data, 2014
    Co-Authors: Dengqiong Sun, Weiqiang Dun, Haihong Zhang, Lijun Zhao, Li Zhang, Wenqing Zhang, Ren Riju, Junbo Gong
    Abstract:

    A gravimetric method was used to determine the solubility of l-carnitine in different pure solvents and ethanol–acetone solvent mixture. The solubility in different pure solvents were then correlated by the modified Apelblat Equation, λh Equation and the modified van’t Hoff Equation, with the modified van’t Hoff Equation presenting the best consistence. Meanwhile, to illustrate the effect of ethanol or acetone on the change of the solubility, a new parameter defined as influence coefficient was introduced and the coefficient of acetone depending on temperature and molar faction of acetone was depicted. In addition, the changes for enthalpy, entropy and Gibbs free energy were calculated by the modified van’t Hoff Equation. It can be drawn that the changes for enthalpy and entropy in a solvent mixture decrease to a minimum before consequent increasing with increasing molar faction of acetone. Furthermore, the change for Gibbs free energy shows a linear relationship with natural logarithm of the solubility.

  • Determination of the Solubility, Dissolution Enthalpy, and Entropy of Pioglitazone Hydrochloride (Form II) in Different Pure Solvents
    Industrial & Engineering Chemistry Research, 2013
    Co-Authors: Mengying Tao, Junbo Gong, Zhao Wang, Hongxun Hao, Jingkang Wang
    Abstract:

    The solubility of pioglitazone hydrochloride (Form II) in N,N-dimethylacetamide, methanol, dimethyl sulfoxide, and acetic acid was determined at temperatures ranging from 283.15 to 323.15 K. The experimental data were correlated with the modified Apelblat Equation, λh Equation, van’t Hoff Equation, ideal model, Wilson model, and nonrandom two-liquid model. Calculation results show that the λh Equation, van’t Hoff Equation, and the ideal model are more suitable in determining the solubility of pioglitazone hydrochloride (Form II) compared with the other three models. By using the van’t Hoff Equation, the dissolution enthalpy, entropy, and molar Gibbs free energy of pioglitazone hydrochloride (Form II) are predicted in different solvents.

Hongxun Hao - One of the best experts on this subject based on the ideXlab platform.

  • Solid-liquid equilibrium of l-alanyl-l-glutamine form II in methanol + water and isopropanol + water systems
    Journal of Molecular Liquids, 2016
    Co-Authors: Yongli Wang, Fuhong Yuan, Qiaoyin Huang, Hongxun Hao
    Abstract:

    Abstract Solid–liquid equilibrium data of L-alanyl-L-glutamine (Ala-Gln) are important for development of industrial crystallization technology of Ala-Gln. In this paper, the solubility data of one polymorph of Ala-Gln (form II) in binary methanol + water and isopropanol + water solvents mixtures from 278.15 to 313.15 K were determined by using a dynamic method under atmospheric pressure. The modified Apelblat Equation, the van't Hoff Equation, the modified CNIBS/R-K model and the modified Jouyban–Acree model were used to correlate the experimental solubility data, respectively. Computational results showed that the Jouyban–Acree model has the lowest AIC (Akaike's Information Criterion) value in both binary solvents mixtures, which means that the Jouyban–Acree model is better for correlating the experimental solubility data. In addition, the thermodynamic properties of the dissolution process, including the standard Gibbs energy change, the standard enthalpy and standard entropy of dissolution of Ala-Gln form II, were also calculated by the van't Hoff Equation.

  • Thermodynamic equilibrium of 4-hydroxy-2,5-dimethyl-3(2H)-furanone in different solvent systems
    The Journal of Chemical Thermodynamics, 2016
    Co-Authors: Yongli Wang, Hongxun Hao, Guan Wang, Cui Huang, Qiuxiang Yin
    Abstract:

    Abstract Crystalline state 4-hydroxy-2,5-dimethyl-3(2H)-furanone with high purity was prepared by recrystallization. Powder X-ray diffraction pattern (PXRD) and differential scanning calorimetry (DSC) were used to identify and characterize the samples. The solubility of 4-hydroxy-2,5-dimethyl-3(2H)-furanone samples in six pure solvents and one kind of binary solvent system from (283.15 to 318.15) K was determined by using a gravimetric method under atmospheric pressure. To extend the application range of the experimental solubility data, the modified Apelblat Equation, the van’t Hoff Equation and the λh Equation were used to correlate the experimental solubility in the pure solvents. For the correlation of binary solvent systems, the CNIBS/R-K model and Jouyban–Acree model were used instead. According to the Akaike Information Criterion (AIC), the λh Equation was found to be better for pure solvent systems and the Jouyban–Acree model was confirmed to be better for binary solvent systems. In addition, the dissolution thermodynamic properties of 4-hydroxy-2,5-dimethyl-3(2H)-furanone were also calculated by the van’t Hoff Equation.

  • determination and correlation of cefuroxime acid solubility in acetonitrile water mixtures
    The Journal of Chemical Thermodynamics, 2014
    Co-Authors: Guan Wang, Hongxun Hao, Yongli Wang, Qinghua Luan, Huihui Wang
    Abstract:

    Abstract The solubility of cefuroxime acid in (acetonitrile + water) mixtures was experimentally determined at temperatures from (278.15 to 313.15) K by using a dynamic method at atmospheric pressure. The solubility increased with the increasing of temperature, and it reached the maximum at acetonitrile molar fraction of 0.713 at constant temperature. The experimental solubility data were correlated well by using the modified Apelblat Equation, the λ h Equation and the van’t Hoff Equation, respectively. The Akaike’s Information Criterion (AIC) was used to select the best model for correlating the solubility of cefuroxime acid. Furthermore, the dissolution enthalpy, entropy and Gibbs free energy change of cefuroxime acid were also calculated by using the van’t Hoff Equation.

  • Determination and correlation of cefuroxime acid solubility in (acetonitrile + water) mixtures
    The Journal of Chemical Thermodynamics, 2014
    Co-Authors: Guan Wang, Hongxun Hao, Yongli Wang, Qinghua Luan, Huihui Wang
    Abstract:

    Abstract The solubility of cefuroxime acid in (acetonitrile + water) mixtures was experimentally determined at temperatures from (278.15 to 313.15) K by using a dynamic method at atmospheric pressure. The solubility increased with the increasing of temperature, and it reached the maximum at acetonitrile molar fraction of 0.713 at constant temperature. The experimental solubility data were correlated well by using the modified Apelblat Equation, the λ h Equation and the van’t Hoff Equation, respectively. The Akaike’s Information Criterion (AIC) was used to select the best model for correlating the solubility of cefuroxime acid. Furthermore, the dissolution enthalpy, entropy and Gibbs free energy change of cefuroxime acid were also calculated by using the van’t Hoff Equation.

  • Determination of the Solubility, Dissolution Enthalpy, and Entropy of Pioglitazone Hydrochloride (Form II) in Different Pure Solvents
    Industrial & Engineering Chemistry Research, 2013
    Co-Authors: Mengying Tao, Junbo Gong, Zhao Wang, Hongxun Hao, Jingkang Wang
    Abstract:

    The solubility of pioglitazone hydrochloride (Form II) in N,N-dimethylacetamide, methanol, dimethyl sulfoxide, and acetic acid was determined at temperatures ranging from 283.15 to 323.15 K. The experimental data were correlated with the modified Apelblat Equation, λh Equation, van’t Hoff Equation, ideal model, Wilson model, and nonrandom two-liquid model. Calculation results show that the λh Equation, van’t Hoff Equation, and the ideal model are more suitable in determining the solubility of pioglitazone hydrochloride (Form II) compared with the other three models. By using the van’t Hoff Equation, the dissolution enthalpy, entropy, and molar Gibbs free energy of pioglitazone hydrochloride (Form II) are predicted in different solvents.

Abdallah Dahmani - One of the best experts on this subject based on the ideXlab platform.

  • solid liquid equilibria and purity determination for binary n alkane naphthalene systems
    Thermochimica Acta, 2006
    Co-Authors: Kamel Khimeche, Yacine Boumrah, Mokhtar Benziane, Abdallah Dahmani
    Abstract:

    Abstract Mixtures of heavy aromatics with high aliphatics are important in the formation of asphaltenes in the oil industry. This work reports binary solid–liquid equilibria for naphtalene + eicosane, +pentacosane, +hexatriacontane mixtures by differential scanning calorimetry. Results are compared with those from modified UNIFAC (Larsen and Gmehling versions) and ideal predictions. Finally, we determine the purity according to van’t Hoff Equation. Results are in good agreement with values given by ultraviolet spectrophotometry.

  • Solid–liquid equilibria and purity determination for binary n-alkane + naphthalene systems
    Thermochimica Acta, 2006
    Co-Authors: Kamel Khimeche, Yacine Boumrah, Mokhtar Benziane, Abdallah Dahmani
    Abstract:

    Abstract Mixtures of heavy aromatics with high aliphatics are important in the formation of asphaltenes in the oil industry. This work reports binary solid–liquid equilibria for naphtalene + eicosane, +pentacosane, +hexatriacontane mixtures by differential scanning calorimetry. Results are compared with those from modified UNIFAC (Larsen and Gmehling versions) and ideal predictions. Finally, we determine the purity according to van’t Hoff Equation. Results are in good agreement with values given by ultraviolet spectrophotometry.

Hongyuan Wei - One of the best experts on this subject based on the ideXlab platform.

  • Solid–Liquid Phase Equilibrium of Nicotinamide in Different Pure Solvents: Measurements and Thermodynamic Modeling
    Industrial & Engineering Chemistry Research, 2014
    Co-Authors: Leping Dang, Hongyuan Wei
    Abstract:

    The solubility of nicotinamide in water, methanol, ethanol, 2-propanol, n-butanol, and ethyl acetate at temperatures ranging from 288.15 K to 318.15 K was measured via a static gravimetric analytic method, and the melting temperature and fusion enthalpy of nicotinamide were obtained using differential scanning calorimetry. The experimental solubility data were correlated by the modified Apelblat Equation, the van’t Hoff Equation, the λh (Buchowski) Equation, and the Wilson model; the van’t Hoff Equation shows the best agreement. Furthermore, the dissolution enthalpy and dissolution entropy of nicotinamide in the corresponding solvents were predicted.

  • Solid–liquid equilibrium of 1-hydroxyethane-1,1-diphosphonic acid in different solvents
    Fluid Phase Equilibria, 2013
    Co-Authors: Xiangyang Zhang, Xiaowu Yang, Lin Hao, Hongyuan Wei
    Abstract:

    Abstract The solubilities of 1-hydroxyethane-1,1-diphosphonic acid in five different solvents including ethanol, isopropyl alcohol, n-propyl alcohol, acetone and acetic acid were determined at temperatures ranging from 288.45 to 327.95 K at atmospheric pressure using a gravimetric method. Van’t Hoff Equation was used to correlate the experimental solubility data. The calculated values of van’t Hoff Equation were found to be in good agreement with the experimental data. Further, the dissolution enthalpy and entropy of HEDP in the corresponding solvents were predicted.

Yongli Wang - One of the best experts on this subject based on the ideXlab platform.

  • Solid-liquid equilibrium of l-alanyl-l-glutamine form II in methanol + water and isopropanol + water systems
    Journal of Molecular Liquids, 2016
    Co-Authors: Yongli Wang, Fuhong Yuan, Qiaoyin Huang, Hongxun Hao
    Abstract:

    Abstract Solid–liquid equilibrium data of L-alanyl-L-glutamine (Ala-Gln) are important for development of industrial crystallization technology of Ala-Gln. In this paper, the solubility data of one polymorph of Ala-Gln (form II) in binary methanol + water and isopropanol + water solvents mixtures from 278.15 to 313.15 K were determined by using a dynamic method under atmospheric pressure. The modified Apelblat Equation, the van't Hoff Equation, the modified CNIBS/R-K model and the modified Jouyban–Acree model were used to correlate the experimental solubility data, respectively. Computational results showed that the Jouyban–Acree model has the lowest AIC (Akaike's Information Criterion) value in both binary solvents mixtures, which means that the Jouyban–Acree model is better for correlating the experimental solubility data. In addition, the thermodynamic properties of the dissolution process, including the standard Gibbs energy change, the standard enthalpy and standard entropy of dissolution of Ala-Gln form II, were also calculated by the van't Hoff Equation.

  • Thermodynamic equilibrium of 4-hydroxy-2,5-dimethyl-3(2H)-furanone in different solvent systems
    The Journal of Chemical Thermodynamics, 2016
    Co-Authors: Yongli Wang, Hongxun Hao, Guan Wang, Cui Huang, Qiuxiang Yin
    Abstract:

    Abstract Crystalline state 4-hydroxy-2,5-dimethyl-3(2H)-furanone with high purity was prepared by recrystallization. Powder X-ray diffraction pattern (PXRD) and differential scanning calorimetry (DSC) were used to identify and characterize the samples. The solubility of 4-hydroxy-2,5-dimethyl-3(2H)-furanone samples in six pure solvents and one kind of binary solvent system from (283.15 to 318.15) K was determined by using a gravimetric method under atmospheric pressure. To extend the application range of the experimental solubility data, the modified Apelblat Equation, the van’t Hoff Equation and the λh Equation were used to correlate the experimental solubility in the pure solvents. For the correlation of binary solvent systems, the CNIBS/R-K model and Jouyban–Acree model were used instead. According to the Akaike Information Criterion (AIC), the λh Equation was found to be better for pure solvent systems and the Jouyban–Acree model was confirmed to be better for binary solvent systems. In addition, the dissolution thermodynamic properties of 4-hydroxy-2,5-dimethyl-3(2H)-furanone were also calculated by the van’t Hoff Equation.

  • determination and correlation of cefuroxime acid solubility in acetonitrile water mixtures
    The Journal of Chemical Thermodynamics, 2014
    Co-Authors: Guan Wang, Hongxun Hao, Yongli Wang, Qinghua Luan, Huihui Wang
    Abstract:

    Abstract The solubility of cefuroxime acid in (acetonitrile + water) mixtures was experimentally determined at temperatures from (278.15 to 313.15) K by using a dynamic method at atmospheric pressure. The solubility increased with the increasing of temperature, and it reached the maximum at acetonitrile molar fraction of 0.713 at constant temperature. The experimental solubility data were correlated well by using the modified Apelblat Equation, the λ h Equation and the van’t Hoff Equation, respectively. The Akaike’s Information Criterion (AIC) was used to select the best model for correlating the solubility of cefuroxime acid. Furthermore, the dissolution enthalpy, entropy and Gibbs free energy change of cefuroxime acid were also calculated by using the van’t Hoff Equation.

  • Determination and correlation of cefuroxime acid solubility in (acetonitrile + water) mixtures
    The Journal of Chemical Thermodynamics, 2014
    Co-Authors: Guan Wang, Hongxun Hao, Yongli Wang, Qinghua Luan, Huihui Wang
    Abstract:

    Abstract The solubility of cefuroxime acid in (acetonitrile + water) mixtures was experimentally determined at temperatures from (278.15 to 313.15) K by using a dynamic method at atmospheric pressure. The solubility increased with the increasing of temperature, and it reached the maximum at acetonitrile molar fraction of 0.713 at constant temperature. The experimental solubility data were correlated well by using the modified Apelblat Equation, the λ h Equation and the van’t Hoff Equation, respectively. The Akaike’s Information Criterion (AIC) was used to select the best model for correlating the solubility of cefuroxime acid. Furthermore, the dissolution enthalpy, entropy and Gibbs free energy change of cefuroxime acid were also calculated by using the van’t Hoff Equation.