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• Musk xylene in ten organic solvents at temperatures ranging from 278.15 K to 313.15 K was measured. • Analysis of musk xylene by XRD. • Wilson model, NRTL model, Vant't Hoff equation, modified Apelblat equation, and λh equation are used to correlate the solubility of musk xylene in different solvents. • The mixed Gibbs energy, enthalpy and entropy were calculated according to Wilson model. In this study, isothermal saturation method was used to measure and correlate the solubility of musk xylene in ten organic solvents at temperatures ranging from 278.15 K to 313.15 K , including methanol, ethanol, isopropanol, n-butanol, cyclohexane, n-hexane, n-heptane, N,N-dimethylacetamide, ethyl acetate, tetrahydrofuran. The experimental results show that the solubility of musk xylene in the selected solvent increases with increasing temperature. The experimental data were correlated by five thermodynamic models, and the results showed that each model can give a satisfactory correlation. In addition, the three kinds of mixed thermodynamic properties of Gibbs energy, enthalpy and entropy of musk xylene in selected solvents were determined by solubility data and Wilson model. It can be seen that the dissolution of musk xylene in a given solvent is spontaneous and entropy driven. Exploring the solubility of musk xylene in different organic solvents and the thermodynamics of dissolution can not only provide basic data for industrial crystallization separation, but also have great significance for its own crystallization and theoretical research. [ABSTRACT FROM AUTHOR]

In this research, solid-liquid equilibrium for the ternary system (2-naphthaldehyde + o -phthalic anhydride + 1,4-dioxane) was measured at 283.15 K, 293.15 K and 303.15 K, respectively. Three isothermal phase diagrams of the system were plotted using the values of the experimental solubility. Pure 2-naphthaldehyde and o -phthalic anhydride were formed at (283.15, 293.15 and 303.15) K, and were determined by Schreinemaker’s wet residue method. The crystallization region of o -phthalic anhydride was found to be much larger than that of 2-naphthaldehyde at a certain temperature. The experimental solubility at multiple temperatures was correlated by the NRTL and Wilson models. The NRTL model was more accurate than the Wilson model in this system. The diagram of density versus component was also constructed. [ABSTRACT FROM AUTHOR]

• Isothermal saturation method was used to measure the solubility of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone in eight pure solvents and two binary solvents at temperatures ranging from 273.15 K to 308.15 K. • Analysis of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone by DSC and XRD. • Van't Hoff model, modified Apelblat model, NRTL model, Wilson model, Jouyban − Acree model, Sun model were used to correlate the solubility of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone. • Hansen solubility parameter was used to reveal the solubility behavior of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone. • The thermodynamic properties (Δ sol H°, Δ sol S°, Δ sol G°, %ξ H and %ξ TS) were discussed by van't Hoff equation. In this work, the solubility of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone was measured and correlated by isothermal saturation method in eight pure solvents (isopropyl alcohol, n -octanol, ethyl acetate, acetonitrile, ethanol, acetone, cyclohexane, methanol) and two binary solvents (isopropyl alcohol + ethyl acetate, ethanol + acetonitrile) at temperatures ranging from 273.15 K to 308.15 K. The results show that the solubility of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone in the selected solvent is positively correlated with temperature. The experimental solubility data were correlated by six thermodynamic models, including Van't Hoff equation, modified Apelblat equation, NRTL model, Wilson model, Jouyban − Acree model and Sun model. The values of RAD and RMSD showed that these models fit the solubility data well. Besides, Hansen solubility parameter was used to reveal the solubility behavior of 1-(4-tert-butyl-2,6-dimethylphenyl)ethenone. Finally, the thermodynamic propertie Δ sol H○, Δ sol S○, Δ sol G○, %ξ H and %ξ TS were calculated by van't Hoff equation. The results showed Δ sol H○, Δ sol G○, Δ sol S○, are all positive values, indicating that the dissolution process in selected solvents was entropy-driven and endothermic. [ABSTRACT FROM AUTHOR]

• Solubility of 2,3-dichloropyridine in 14 pure solvents were measured. • Solubility modeling was realized by seven thermodynamic models. • Hansen solubility parameters were employed to explain solubility behaviors. • Solvent effect was studied by MEPs, Hirshfeld surface analysis and DFT calculation. • Thermodynamic properties were discussed by Van't Hoff equation. The solid–liquid equilibrium data of 2,3-dichloropyridine(23DCP) in 14 pure solvents were measured making use of the laser dynamic monitoring at 278.15/283.15/288.15 K − 313.15 K with 0.1 MPa. The findings of this study showed that the solubility increase of 23DCP in 14 pure solvents had a positive relation with temperature, and the solubility order was 1,4-dioxane > dichloromethane > n-butyl acetate > ethyl acetate > methyl acetate > acetonitrile > n-butanol > isobutyl alcohol > n-propanol > isopropanol > ethanol > cyclohexane > methanol > n-hexane. The solubility data of 23DCP was operated by seven models (Van't Hoff, modified Apelblat, λh, Yaws, NRTL, NRTL-SAC, Wilson) to correlate. And the average ARD values were 1.684 %,1.058 %, 1.031 %, 0.905 %, 0.937 %, 1.012 %, 2.062 % and the average 103RMSD values were 1.978, 1.396, 1.542, 1.221, 1.758, 1.658 and 1.883, respectively. In addition, Hansen solubility parameters were well evaluated to appraise the miscibility of 23DCP in 14 pure solvents. And the interactions between molecules were studied by means of molecular electrostatic potential surface, Hirshfeld surface analysis and density functional theory calculation. Finally, according to Van't Hoff equation, Δ sol G °, Δ sol H ° and Δ sol S ° of 23DCP in 14 pure solvents were got. Δ sol H ° and Δ sol S ° were bigger than zero, representing that this was a dissolution process of endothermic and entropy increase. [ABSTRACT FROM AUTHOR]

• Solubility data of 1,4-cyclohexanedione in ten pure solvents were measured. • Experimental data were correlated by five thermodynamic models. • Dissolution mechanism of 1,4-cyclohexanedione in ten pure solvents was investigated. • Thermodynamic properties were discussed by Wilson model. As an important raw material in industrial production, the solubility studies of 1,4-cyclohexanedione (14CHD) in organic solvents may be of assistance in improving crystallization efficiency and yield in industry. Therefore, this work deeply explored the dissolution behavior of 14CHD by using the isothermal saturation method, model fitting and density functional theory (DFT) calculation. Firstly, we selected ten pure organic solvents that are environmentally friendly to measure the solubility of 14CHD at the temperature range of 278.15 ∼ 313.15 K under standard atmospheric pressure. According to the measurement results, the solubility of 14CHD increases with temperature, and there are some differences among the solubility of 14CHD in various solvents. For instance, it has a highest solubility in acetonitrile (x 1 = 0.5331) at 313.15 K while has the lowest solubility (x 1 = 6.757 × 10-4) in cyclohexane at 283.15 K. Whereafter, the measured solubility data was correlated by Van't Hoff equation, modified Apelblat equation, λh model, Yaws model and Wilson model. Among them, Yaws model represents the most accurate fitting outcomes. At the same time, the study results of mixing thermodynamic properties on the basis of Wilson model suggest that the dissolution processes of 14CHD in ten organic solvents are entropy-driven and spontaneous. Afterwards, in order to explain the large difference in solubility of 14CHD in ten organic solvents, we found that the dissolution of 14CHD depends mostly on the polarity (π) and cohesive energy density (CED), viewed from the physicochemical factors of solvents. Furthermore, we further studied intermolecular interactions between 14CHD and ten solvents through molecular electrostatic potential surface (MEPS) analysis and DFT methods. Results display that alcoholic and non-alcoholic solvents molecules have different sites of action with 14CHD and the absolute values orders of interaction energies of alcoholic and non-alcoholic solvents are all consistent with corresponding solubility laws. The solvent–solute interaction plays an important role in the solubilities of 14CHD. [ABSTRACT FROM AUTHOR]