•The solubility of myo-inositol in (water + acetic acid) binary solvent mixtures is reported.•The dissolution process is a nonspontaneous process.•Modified Apelblat equation assisted with Jouyban–Acree model can be used to describe the solution process of myo-inositol adequately.In this paper, we focused on solubility and solution thermodynamics of myo-inositol. By gravimetric method, the solubility of myo-inositol was measured in (water + acetic acid) binary solvent mixtures from 278.15 K to 333.15 K under atmosphere pressure. The solubility data were fitted using modified Apelblat equation, a variant of the combined nearly ideal binary solvent/Redich–Kister (CNIBS/R–K) model and Jouyban–Acree model. The three models were all proven to give good agreement with the experiment data, and modified Apelblat equation was the best. By means of van’t Hoff analysis, the enthalpy, entropy and Gibbs energy were calculated, which indicated that the dissolving process was nonspontaneous.

•A high selective colorimetric and ratiometric fluorescent probe based on 4-hydroxy-1, 8-naphthalimide.•The fluorescence change from blue to green when add F.•The color of probe change from colorless to yellow when add F.•The probe has a excellent selectivity for F− over other competitive anions.A high selective colorimetric and ratiometric fluorescent probe based on 4-hydroxy-1, 8-naphthalimide was designed and synthesized to detect fluoride ions (F−). The sensing behavior of this probe was studied by UV–visible and fluorescence spectroscopy. The probe displays an 110 nm red-shift of fluorescence emission and the color changes from colorless to yellow by virtue of the strong affinity of F− toward silicon which can act as a new visual sensor for F−.A high selective colorimetric and ratiometric fluorescent probe based on 4-hydroxy-1, 8-naphthalimide was designed and synthesized to detect fluoride ions (F−). The sensing behavior of this probe was studied by UV–visible and fluorescence spectroscopy. The probe displays an 110 nm red-shift of fluorescence emission and the color changes from colorless to yellow by virtue of the strong affinity of F− toward silicon which can act as a new visual sensor for F−.

The solubilities of dimethyl fumarate in methanol + water, ethanol + water, 1-propanol + water mixed solvents were measured within the temperature range 278.15–333.15 K at atmospheric pressure by the dynamic method. The solubility of dimethyl fumarate in those selected solvents increased with increasing temperature, but the rate of solubility is different. The semi-empirical Buchwski–Ksiazaczak λh equation and the modified Apelblat equation were used to correlate with the solubility. The RMSD (root–mean–square deviations) <2.7 and the RD (relative deviation) <6.39. By comparing the two models, Apelblat equation describes the solubility of dimethyl fumarate in selected solvents as a function of temperature well. The thermodynamic properties of the solution process, including the enthalpy, and entropy were calculated by the van’t Hoff analysis and they were positive.Highlights► The solubility of dimethyl fumarate in mixed solvents. ► The dissolution of dimethyl fumarate is an endothermic and entropy-driving process. ► γh equation describes the solubility of dimethyl fumarate in studied solvents well.

Data on corresponding solid–liquid equilibrium of succinic acid in different aqueous solvent mixtures was measured with temperature range from 278.15 K to 333.15 K under atmospheric pressure by employing the gravimetric method. The experimental results indicated that the solubility of succinic acid in the binary mixtures increases with increasing both temperature and mass fraction of organic solvents. The experimental data were well-correlated with the modified Apelblat equation, the λh equation and the van’t Hoff equation. In addition, the calculated solubilities showed good agreement with the experimental results. It was found that the modified Apelblat equation could obtain the better correlation results than the other two models. The standard enthalpy, standard entropy, and Gibbs free energy change of solution of succinic acid were calculated from the solubility data by using the modified Apelblat model. Moreover, the experimental data and model parameters would be useful for optimizing the process of purification of succinic acid in industry.Highlights► The solubilities of succinic acid in binary mixed solvents were measured over the temperature range of (278.15–333.15) K. ► The solubilities of succinic acid in mixed solvents increase with increasing organic solvent content at constant temperature. ► The solubilities calculated by the corresponding equation show good agreement with the experimental data. ► Solubility was determined by the gravimetric method.

•The solubility of dimethyl succinylsuccinate in pure and mixed solvents.•The dissolution of dimethyl succinylsuccinate is an endothermic and entropy-driving process.•Buchowski–Ksiazczak equation provides a more reasonable prediction in mixture solvent.•Apelblat equation provides a more reasonable prediction in pure solvent.The solubilities of dimethyl succinylsuccinate in tetrahydrofuran, acetic ether, acetone, acetonitrile, 1-propanol, ethanol and methanol pure solvents and tetrahydrofuran + methanol mixed solvents were measured within the temperature range 278.15 K to 333.15 K at atmospheric pressure. The solubility of dimethyl succinylsuccinate in those selected solvents increased with increasing temperature, and the dissolution in tetrahydrofuran is best. The semi-empirical Buchowski–Ksiazczak λh equation, the modified Apelblat equation and CNIBS/R-K equation were used to correlate with the solubility. In pure solvents the values of the sum of deviation (∑(%Dev)) for Apelblat and Buchowski–Ksiazczak λh equations are 1.1115 and 1.0383, respectively. In the tetrahydrofuran and methanol mixture, the sums of deviation (Σ(%Dev)) for Apelblat equation, Buchowski–Ksiazczak λh equation and CNIBS/R-K equation are 0.7587, 0.7059 and 1.4090, respectively. By comparing models, the solubilities predicted by Buchowski–Ksiazczak λh equation and Apelblat equation is reasonable in mixture solvent and pure solvent, respectively. The thermodynamic properties of the solution process, including the enthalpy, and entropy were calculated by the van’t Hoff analysis. The value of enthalpy and entropy were positive.

DSC studies show that a sample starts to melt at 190.6 °C with a high melting enthalpy of 343.4 J/g. Using a laser monitoring system, the solubility of γ-aminobutyric acid in aqueous ethanol solution was measured by a synthetic method at temperatures ranging from 288.2 to 313.2 K and at atmospheric pressure; these are important data for the crystallization process of γ-aminobutyric acid from its aqueous solution. The measured solubility was correlated with the Buchowski−Ksia̧zczak equation and the modified Apelblat equation. Then, the induction of γ-aminobutyric acid in ethanol was estimated at different temperatures. The study reveals that the induction period of γ-aminobutyric acid decreases with increasing supersaturation. Interfacial tension was estimated from the experimentally determined induction period values. Nucleation parameters were also investigated based on classical nucleation theory. The grown crystals were also subjected to structural and thermal studies.

Date on the solubility of urea l-tartaric acid in aqueous ethanol solution are essential for industrial design and further theoretical studies. Using a laser monitoring system, the solubility of urea l-tartaric acid in aqueous ethanol solution at different temperatures was measured using the synthetic method. For the temperature range investigated, the solubilities of urea l-tartaric acid in the solvents increased with increasing temperature. The solubility data were correlated with Apelblat equation and Buchowski–Ksiązczak λh equation. The Apelblat equation can regress the solubility data much better than Buchowski–Ksiązczak λh equation. This study provides valuable data for the mechanism and preparation of the available crystal form of urea l-tartaric acid.