•The solubility of ETD in four mono-solvents and three aqueous solvent mixtures was experimentally determined.•The experimental solubility data were correlated by five models.•The mixing thermodynamic properties in different solvents were also calculated.Solid-liquid equilibrium data of erythromycin thiocyanate dihydrate in four mono-solvents (methanol, ethanol, propan-1-ol and propan-2-ol) and three organic + water solvent mixtures (acetonitrile + water, acetone + water and ethanol + water) were determined by a gravimetric method under atmospheric pressure. The effects of content of organic solvents and temperature on the solubility were investigated and discussed. It was found that the content of organic solvents can significantly affect the solubility of erythromycin thiocyanate dihydrate. The modified Apelblat equation and NRTL model were applied to correlate the solubility data in mono-solvents. The GSM, two modified Jouyban-Acree models (the Van't-JA equation and the Apel-JA equation) and NRTL model were used to correlate the experimental data in three binary solvents systems. Computational results indicated that the AIC (Akaike's Information Criterion) values of two Jouyban-Acree models and NRTL model were lower than that of GSM in binary solvents mixtures, which means that the former three models are better for correlating the experimental solubility data. In addition, the mixing thermodynamic properties of erythromycin thiocyanate dihydrate in different solvents were also calculated based on the experimental solubility data and the NRTL model.Download high-res image (131KB)Download full-size image

•Solubility of 2-Cyano-4′-methylbiphenyl in eight pure solvents were determined by using UV spectrometer method.•The experimental solubility data of 2-Cyano-4′-methylbiphenyl were correlated and analyzed by three thermodynamic models.•Mixing thermodynamic properties of 2-Cyano-4′-methylbiphenyl were calculated and discussed.Solid–liquid equilibrium data of 2-Cyano-4′-methylbiphenyl (OTBN) are essential for the design and optimization of its production process. In this work, the solubility data of OTBN in pure solvents including 2-propanol, (R)-(−)-2-butanol (2-butanol, for short), methyl acetate, ethyl acetate, propyl acetate, butyl acetate, acetone and acetonitrile were determined in different temperature ranges from (268.05 to 303.25) K by using UV spectrometer method under atmospheric pressure. It was found that the order of OTBN solubility in these selected pure solvents at given temperature is acetone > methyl acetate > ethyl acetate > propyl acetate > butyl acetate > 2-butanol > 2-propanol and methyl acetate > acetonitrile > 2-butanol. In the temperature range investigated, the solubility data of OTBN increase with the increasing of temperature in all eight solvents. Furthermore, the modified Apelblat equation, the Wilson model and the NRTL model were applied to correlate the experimental solubility data. The correlated results are consistent with the experimental results. Finally, the mixing thermodynamic properties of OTBN in different solvents were calculated and analyzed based on the experimental solubility data and the Wilson model.

•The solubility of OTBNBr were determined in three kinds of binary solvents.•Three model were used to correlate the solubility data.•The Akaike’s Information Criterion (AIC) was used to choose the best mode.The solubility of 4′-bromomethyl-2-cyanobiphenyl (OTBNBr) in binary solvent mixtures of {acetone + (ethanol, n-propanol, and n-butanol)} was experimentally determined within the temperature range 278.15–313.15 K by using a gravimetrical method under atmospheric pressure (P = 0.1 MPa). The results show that the solubility of OTBNBr monotonously increases with increasing temperature and increasing mole fraction of acetone. The solubility of OTBNBr was correlated by the modified Apelblat equation, the van’t Hoff equation, and the CNIBS/R-K model. The Akaike’s Information Criterion (AIC) was used to choose the best model for correlating the solubility of OTBNBr. The preferred model is the modified Apelblat equation which has the lowest AIC value. Furthermore, the mixing thermodynamic properties (enthalpy, entropy, and Gibbs energy) of OTBNBr were also calculated in the selected solvent mixtures.

Polystyrene(PS)@SiO2 core-shell microbeads with large pore and large particle size were prepared via layer-by-layer(LBL)assembly technique for potential applications in nano-micro composites. Negative silica nanoparticles synthesized via modified Stöber method and cationic poly(diallyldimethylammonium chloride)were alternately adsorbed on the surface of microbeads. Zeta potential, size, and morphology of the microbeads were monitored during LBL assembly process to ensure the successful deposition of silica nanoparticles. The porous shell was characterized using nitrogen adsorption and desorption analyses, and the surface area, volume and diameter of the pores were derived. It is found that the porous shell thickness and the pore size can be tuned by changing the coating times of silica nanoparticles. Finally, PS@SiO2 core-shell microbeads with 5,μm PS solid core and 350,nm mesoporous shell(mean BJH pore diameter is ~27,nm)were used to load CdSe/ZnS quantum dots(QDs). The fluorescence microscopic image and the optical amplification of the QDs-embedded microbeads (QDBs)indicate that the as-prepared core-shell microbeads can provide adequate space for QDs and may be useful for further application of nano-micro composites.

•Ternary phase diagrams of (IMC + NCT)-methanol or methanol/ethyl acetate mixture at T = (298.15 and 313.15) K were measured.•The effects of temperature and introduced ethyl acetate on solid phase stability were discussed.•Solubility of (IMC + NCT) cocrystals was first correlated using a model considering solubility product and complexation.•Solubility of (IMC + NCT) cocrystals as a function of co-former concentration was evaluated.(Solid + liquid) equilibrium data for indomethacin (IMC) and nicotinamide (NCT) in both methanol (MeOH) and methanol/ethyl acetate (EA) mixture were determined using a static method at T = (298.15 and 313.15) K under atmospheric pressure. The 1:1 (IMC + NCT) co-crystal and IMC·MeOH were found in both systems under conditions investigated. The solubility of the 1:1 (IMC + NCT) co-crystal was correlated using a mathematical model consisting of both solubility product and a complexation process. Solubility of (IMC + NCT) co-crystals as a function of co-former (NCT) concentration was evaluated. It was found that temperature has a significant effect on the formation of methanol solvate in the systems investigated. Solvate formation could be suppressed either by increasing temperature or using solvent mixtures. Additionally, the solvent mixture could level out the solubility differences between IMC and NCT, resulting in larger and more symmetric regions for the (IMC + NCT) co-crystal, which would be helpful to the development of the co-crystallization process for the 1:1 (IMC + NCT) co-crystal.

The phase diagrams for ibuprofen (IBU) and nicotinamide (NCT) in both ethanol and ethanol/water mixtures were constructed at (298.15 and 313.15) K under atmospheric pressure using static method. It is revealed that employing solvent mixtures in cocrystallization could significantly affect the symmetry of phase diagrams. In pure ethanol, the two solutes dissolve incongruently and the diagrams are asymmetric, so excessive IBU is needed to isolate cocrystals. However, in ethanol/water mixtures (mass fraction of water was 0.30), the solubility difference between the two components can be leveled out, resulting in more symmetric phase diagrams which can enlarge the processing space for cocrystallization. The solubility of the 1:1 IBU–NCT cocrystal was evaluated as a function of NCT concentration based on the solubility product. These findings are of great importance to develop the cocrystallization process for manufacturing IBU–NCT cocrystal.

Only a few studies of heterosolvate are reported in the literature. In this article, heterosolvates of cefodizime sodium were prepared in water/ethanol binary solvent mixtures and characterized. Through thermal analysis and composition determination, we deduced that both water and ethanol molecules participated in the forming of crystal lattice. The general chemical name of heterosolvates may be defined as cefodizime sesquihydrate sesquiethanolate. Then, the studies on infrared ATR and Raman spectroscopy provided a strong evidence of intermolecular hydrogen bonds. Further, the crystal structure of solvates was analyzed by the powder X-ray diffraction data. The results indicated that the structure differences between solvate and raw material were mainly caused by the solvent effect, leading to forming solvation through intermolecular hydrogen bonding.

Ternary phase diagram data of 1,2-dihydroacenaphthylene-dibenzofuran mixtures in a series of alcohols, including methanol, ethanol, propan-2-ol, propan-1-ol, butan-1-ol, and pentan-1-ol were measured using a dynamic method at 308.15 and 313.15 K. The experimental data were correlated with the Wilson model (including pseudobinary systems), UNIQUAC model, and NRTL model. The results indicate that pseudobinary systems with the Wilson equation give a better description of the solubility of the ternary system. The eutectic point shifts toward dibenzofuran when the more polar methanol and ethanol are used. This shift may help achieve a more efficient separation of 1,2-dihydroacenaphthylene and dibenzofuran.

•The solubilities of the homologous series of C2–C10 dicarboxylic acids were determined in four selected solvents.•The experimental data were well correlated with the modified Apelblat equation.•The odd–even effect of solubility was found and explained.•The enthalpy, entropy and the molar Gibbs free energy of solution were predicted.The solubility of the homologous series of dicarboxylic acids, HOOC(CH2)n−2COOH (n = 2 to 10), in ethanol, acetic acid, acetone and ethyl acetate was measured at temperatures ranging from (278.15 to 323.15) K by a static analytic method at atmospheric pressure. Dicarboxylic acids with even number of carbon atoms exhibit lower values of solubility than adjacent homologues with odd carbon numbers. This odd–even effect of solubility is attributed to the twist of molecules and interlayer packing in solid state as explained in our previous work. The alternation varies in different solvents, which is believed to be associated with the properties of solvents. Finally, the dissolution enthalpy, dissolution entropy and the molar Gibbs free energy were calculated using the fitting parameters of the modified Apelblat equation. The molar Gibbs free energy also showed apparent odd–even alternation in keeping with the alternation of solubility.

•Solubility of hydroxyacetic acid in mono-solvents and binary solvent mixtures was measured.•Modified Apelblat, NRTL and Wilson model were used to correlate the solubility data in pure solvents.•CNIBS/R-K and Jouyban-Acree model were used to correlate the solubility in binary solvent mixtures.•The mixing properties were calculated based on the NRTL model.The solubility of hydroxyacetic acid in five pure organic solvents and two binary solvent mixtures were experimentally measured from 273.15 K to 313.15 K at atmospheric pressure (p = 0.1 MPa) by using a dynamic method. The order of solubility in pure organic solvents is ethanol > isopropanol > n-butanol > acetonitrile > ethyl acetate within the investigated temperature range, except for temperature lower than 278 K where the solubility of HA in ethyl acetate is slightly larger than that in acetonitrile. Furthermore, the solubility data in pure solvents were correlated with the modified Apelblat model, NRTL model, and Wilson model and that in the binary solvents mixtures were fitted to the CNIBS/R-K model and Jouyban-Acree model. Finally, the mixing thermodynamic properties of hydroxyacetic acid in pure and binary solvent systems were calculated and discussed.

•The solubilities of vanillyl alcohol in eight pure solvents were determined.•The capability of forming hydrogen bond was applied to explain the solubility data.•Dissolution thermodynamic properties of vanillyl alcohol were calculated and discussed.In this work, the solubility of vanillyl alcohol in eight pure solvents was measured by using a static gravimetric method over the temperature range from 293.15 K to 343.15 K. It was found that the solubility of vanillyl alcohol in ethanol is the highest while solubility in butyl acetate is the least among all the selected solvents. The solubility values increase with the temperature rise. The capability of vanillyl alcohol to form hydrogen bond with solvents was applied to explain the difference of solubility in these selected pure solvents. Furthermore, the modified Apelblat equation, the λh equation and the Wilson equation were used to correlate the experimental solubility. Finally, the thermodynamic properties of vanillyl alcohol in different pure solvents were investigated and are discussed based on the Wilson equation and the experimental solubility date.