Jouyban Acree Equation Research Articles

Determination and correlation of the solubility of myricetin in ethanol and water mixtures from 288.15 to 323.15K

ABSTRACTThe solubility of myricetin (MY) is very important in regard to its extraction and purification, which was performed by an equilibrium method in the binary solvent system of ethanol and water in the temperature range 288.15 ~ 323.15 K and was determined by ultraviolet (UV-Vis) spectrophotometry at 375 nm. The experimental solubility values were correlated by four mathematical equations: a simplified universal equation (ideal model), modified Apelblat equation, equation and Jouyban–Acree equation. The modified Apelblat model is more suitable for predicting the solubility data of MY in the binary solvent system of ethanol and water at this experimental temperature range. The dissolution enthalpy and entropy of MY were evaluated by the Van’t Hoff and Gibbs−Helmholtz equations. The results illustrate that the dissolution process in binary system solvent mixtures is strongly dependent on solvent composition and temperature, and this process was endothermic and entropy driven.

Thermodynamic Models for Determination of the Solubility of Boc-(R)-3-Amino-4-(2, 4, 5-trifluorophenyl)butanoic acid in Different Pure Solvents and (Tetrahydrofuran + n-Butanol) Binary Mixtures with Temperatures from 280.15 to 330.15 K

A gravimetric method was taken to measure the solubility of the Boc-(R)-3-amino-4-(2,4,5-trifluorophenyl)butanoic acid under atmospheric pressure in methanol, ethanol, propanol, n-butanol, ethyl acetate, and tetrahydrofuran as well as in the (tetrahydrofuran + n-butanol) mixtures from 280.15 to 330.15 K.The experiment results have proved that the rising temperature leads to increased solubility of the Boc-(R)-3-amino-4- (2,4,5-trifluorophenyl)butanoic acid in all selected solvents. The solid–liquid equilibrium data in pure and mixed solvents is correlated with a series of equations, including the modified Apelblat equation, the Buchowski–Ksiazaczak λh equation, CNIBS/R–K equation and the Jouyban–Acree equation. During the study, the computational values were in good agreement with the experimental results according to the calculations based on all selected equations, however, the modified Apelblat equation stood out to be the higher suitable with the higher accuracy. The thermodynamic properties of the solution process, including the Gibbs energy, enthalpy, and entropy were calculated by the van’t Hoff equation. The calculated thermodynamic parameters indicated that in each studied solvent the dissolution process of Boc-(R)-3-amino-4-(2,4,5-trifluorophenyl)butanoic acid is endothermic.

Thermodynamic models for determination of the solubility of 4-(4-aminophenyl)-3-morpholinone in different pure solvents and (1,4-dioxane + ethyl acetate) binary mixtures with temperatures from (278.15 to 333.15) K

A gravimetric method was used to measure the solubility of the 4-(4-Aminophenyl)-3-morpholinone under atmospheric pressure in 1,4-dioxane, methanol, tetrahydrofuran, ethanol, ethyl acetate, n-propanol as well as in the (1,4-dioxane+ethyl acetate) binary mixtures from T=(278.15 to 333.15)K. The experiment results have proved that rising temperature leads to increased solubility of the 4-(4-aminophenyl)-3-morpholinone in all selected solvents. The (solid+liquid) equilibrium data in six pure solvents and binary mixtures were correlated with four equations, including the modified Apelblat equation, the Buchowski−Ksiazaczak λh equation, CNIBS/R–K equation and the Jouyban–Acree equation. During the research, the computational values were in good agreement with the experimental results according to the calculations based on all selected equations, and the modified Apelblat equation stood out to be the higher suitable with the higher accuracy. The thermodynamic properties of the solution process, including the Gibbs energy, enthalpy, and entropy were calculated by the van’t Hoff analysis. All values of %ξH are ⩾60.35% indicated that in each studied solvent the dissolution process of 4-(4-aminophenyl)-3-morpholinone is endothermic.

Thermodynamic Models for Determination of the Solubility of N-Acetylglycine in (Methanol+Acetonitrile) Binary Solvent Mixtures

N-Acetylglycine is an important organic chemical and pharmaceutical intermediate. The solubility of N-Acetylglycine in methanol+Acetonitrile was measured in the temperature ranging from 278.15 K to 333.15 K. In the processing of the experimental data, we use three kinds of equations. There are the Combined Nearly Ideal Binary Solvent/Redlich–Kister (CNIBS/R–K) equations and the simplified Jouyban–Acree equation. All equations can be well applied. The CNIBS/R–K equations are relatively better. We used the van’t Hoff equation to determine the thermodynamic properties of N-Acetylglycine further more, including the entropy, enthalpy, and Gibbs energy.

Measurement and Correlation of the Solubility of Vanillic Acid in Eight Pure and Water + Ethanol Mixed Solvents at Temperatures from (293.15 to 323.15) K

The solubility of vanillic acid in eight pure solvents, including ethanol, 1-propanol, 2-propanol, n-butanol, isobutanol, acetone, methyl acetate, water, and binary mixtures of water + ethanol have been measured at (293.15 to 323.15) K and atmospheric pressure by using a gravimetric method. The experimental solubility in the pure solvents was correlated by the modified Apelblat equation, van’t Hoff equation, λh equation, nonrandom two-liquid (NRTL) equation, universal quasichemical (UNIQUAC) equation, and Wilson equation. The solubility in the binary mixed solvents was correlated by the modified Apelblat equation and the Jouyban–Acree equation. The correlated values based on all the selected equations showed good agreement with the experimental values, and the correlated data of the modified Apelblat equation show the best agreement with the experimental data.

Measurement and correlation of the solubility of rivaroxaban (form I) in binary mixtures of ethyl acetate with tetrahydrofuran, N,N-dimethylformamide, and N,N-dimethylacetamide from T = (278.15 to 318.15) K

In this work, the solubility of rivaroxaban (form I) in binary solvent mixtures of ethyl acetate (EA) with N,N-dimethylformamide (DMF), N,N-dimethylacetamide (DMA) and tetrahydrofuran (THF) was firstly experimentally measured over the temperature range from (278.15 to 318.15)K. Then the measured solubility data were correlated with such semiempirical thermodynamic models as Jouyban–Acree (JA) equation and Buchowski (λh) equation. The crystal form of the residual solids in equilibrium with liquids was identified by powder X-ray diffraction (PXRD). The melting temperature and fusion enthalpy were determined using differential scanning calorimetry (DSC). The results show that, the solubility of rivaroxaban generally increases with the temperature and decreases with the increase in the content of EA in the binary solvent mixtures. Furthermore, when λh equation is used to correlate the solubility of rivaroxaban with the temperature in each solvent mixture, the average relative deviation (ARD) between the experimental and calculated values is about 0.0671, while it is about 0.0905 when JA equation is employed to correlate the solubility with the temperature and the composition of solvent mixtures simultaneously.

Thermodynamic models for determination of the solubility of omeprazole sulfide in (ethanol + ethyl acetate) binary solvent mixtures

The solubility of omeprazole sulfide in (ethanol+ethyl acetate) binary solvent mixtures was measured within the temperature range from 277.65 to 333.15K. The experimental data were fitted using CNIBS/R–K equation and the Jouyban–Acree equation, respectively. All the two equations were proven to give good representations of the experimental values. Computational results showed that the CNIBS/R–K equation was superior to the other equation. The thermodynamic properties of the solution process, including the Gibbs free energy, enthalpy and entropy, were calculated by the van’t Hoff analysis. The values of both the enthalpy change and the standard molar Gibbs free energy change of solution were positive, which indicated that the process was endothermic.

Solubility of dihydromyricetin in ethanol and water mixtures from 288.15 to 323.15 K

The solubility of dihydromyricetin in the binary system of ethanol and water was measured by using UV spectrophotometric method at the maximum absorption wavelength of 290nm from 288.15K to 323.15K. The solubility increases with temperature and mole fraction of ethanol in the binary system. The calculated solubility data of dihydromyricetin were computed by using three models, the modified Apelblat equation, the Buchowski–Książczak λH equation, and the Jouyban–Acree equation. The modified Apelblat equation and λH equation are more suitable for correlating experimental solubility data of dihydromyricetin. The activity coefficients were calculated based on the results of thermal properties of DMY (obtained by DSC), presenting good consistency with the solubility behavior. In this study, the enthalpy and entropy of a solution were evaluated using the van't Hoff equation. The course of dihydromyricetin dissolving in the binary system in the experimental temperature range was endothermic.

Thermodynamic Models for Determination of the Solubility of the (1:1) Complex of (Urea + l-Malic Acid) in (Methanol + Acetonitrile) Binary Solvent Mixtures

In this paper, we focused on solubility and solution thermodynamics of urea l-malic acid (1:1 solid state compound). By gravimetric method, the solubility of urea l-malic acid was measured in (methanol + acetonitrile) binary solvent mixtures in the temperature (from 278.15 K to 333.15 K). The solubility data were fitted using modified Apelblat model, a variant of the combined nearly ideal binary solvent/Redlich–Kister (CNIBS/R–K) model and Jouyban–Acree equation. Computational results showed that the modified Apelblat model has advantages than the other two models. In addition, we used van’t Hoff analysis and Gibbs equation to help later scholars understand the thermodynamic properties in the process of dissolving. The experimental data showed that acetonitrile could be used as effective antisolvents.

Temperature dependent solubility of sodium cyclamate in selected pure solvents and binary methanol + water mixed solvents

The solubility of the sodium cyclamate in water, methanol, formamide, formic acid, acetic acid, DMF, DMSO and binary methanol+water mixed solvents was measured over the temperature rang from 280K to 340K about 5K intervals by a laser technique under atmospheric pressure. The experimental results indicated that the solubility of sodium cyclamate in the pure and mixed solvents increased with increasing temperature and decreased with increasing mass fraction of methanol in the mixed solvents. The experimental data was correlated by the modified Apelblat model, modified Jouyban–Acree equation and three-parameter van’t Hoff equation. In addition, all the calculated values were in good agreement with all the experimental data in the temperature range studied. We also tried to calculate the thermodynamic functions (ΔHsol, ΔSsol).

Solubility of N-ethylcarbazole in ethanol+petroleum ether mixtures at various temperatures

The solubility of N-ethylcarbazole in (ethanol+petroleum ether) binary solvent mixtures was measured with the temperature changing from 280.15 K to 316.15 K. The experimental data matched the solvent/Redlich-Kister (CNIBS/R-K) equation and the Jouyban-Acree equation. Computational results showed the CNIBS/R-K equation was more suitable than the Jouyban-Acree equation. The solution process in the thermodynamic properties, including the Gibbs energy, enthalpy, and entropy, was calculated by the van’t Hoff analysis.

Thermodynamic analysis and correlation of solubility of disodium 5′-guanylate heptahydrate in aqueous ethanol mixtures

The solubility of disodium 5′-guanylate heptahydrate (5′-GMPNa2) in water-ethanol binary solvent mixtures was measured at temperatures ranging from 278.15K to 323.15K using a dynamic method. The solubility data were correlated by the Apelblat equation, the Combined Nearly Ideal Binary Solvent/Redlich–Kister (CNIBS/R–K) equation and the modified Jouyban–Acree equation, respectively. Results showed that a reasonable match with experimental data is obtained from the Apelblat equation and CNIBS/R–K equation, while the modified Jouyban–Acree equation contains parameters including both solvent composition and temperature. The thermodynamic functions Gibbs free energy, enthalpy and entropy of solution were also calculated based on solubility data of 5′-GMPNa2 determined in binary water+ethanol solvent mixtures by using van’t Hoff equation. The dissolving process is endothermic and the dissolution driving force converts from enthalpy-driving to entropy-driving.

Measurement and correlation of the solubility of 4-methylbenzoic acid in (methanol + acetic acid) binary solvent mixtures

Data on corresponding solid–liquid equilibrium of 4-methylbenzoic acid in (methanol+acetic acid) binary solvent mixtures are essential for industrial design and further theoretical studies. In this study, the solubility of 4-methylbenzoic acid was measured in (methanol+acetic acid) binary solvent mixtures in the temperature ranging from 283.15 to 333.15K by the analytical stirred-flask method under atmospheric pressure. The results obtained from these measurements were fitted using the modified Apelblat equation, the combined nearly ideal binary solvent/Redlich–Kister (CNIBS/R–K) equation and the Jouyban–Acree equation, respectively. All the equations were proven to give good representations of the experimental data. The experiment results indicated that the solubility of 4-methylbenzoic acid in the binary solvent increased with increasing temperature, decreases with increasing methanol content, but the increments with temperature differed from different methanol contents. The Redlich–Kister (CNIBS/R–K) equation was more accurate than the other two equations owning to its lowest value of the overall MD. In addition, the thermodynamic properties of the solution process, including the Gibbs energy, enthalpy, and entropy were calculated by the van't Hoff analysis. The experimental data and model parameters would be useful for optimizing the process of purification of 4-methylbenzoic acid in industry.

Solubility and solution thermodynamics of 2,3,4,5-tetrabromothiophene in (ethanol + trichloromethane) binary solvent mixtures

The solubility of 2,3,4,5-tetrabromothiophene in a (ethanol+trichloromethane) binary solvent mixture was measured in the temperature ranging from 278.15K to 322.15K. The results obtained from these measurements were fitted using the two variants of the combined nearly ideal binary solvent/Redlich–Kister (CNIBS/R–K) equation and the Jouyban–Acree equation, respectively. All the three equations were proven to give good representations of the experimental data. Computational results showed that the variant 2 of CNIBS/R–K equation was superior to the other two equations. In addition, the thermodynamic properties of the solution process, including the Gibbs energy, enthalpy, and entropy were calculated by the van’t Hoff analysis. The experimental results showed that ethanol could be used as effective anti-solvents in the crystallization process.

Solubility and solution thermodynamics of 2,3,4,5-tetrabromothiophene in (ethanol + tetrahydrofuran) binary solvent mixtures

The solubility of 2,3,4,5-tetrabromothiophene in (ethanol+tetrahydrofuran) binary solvent mixtures was measured within the temperature range from (278.15 to 322.15)K. The solubility increases with the rise of temperature, while it decreases with increasing ethanol content at constant temperature. The experimental data were fitted using the two variants of the combined nearly ideal binary solvent/Redlich–Kister (CNIBS/R–K) equation and the Jouyban–Acree equation, respectively. All the three equations were proven to give good representations of the experimental values. Computational results showed that the variant two of CNIBS/R–K equation was superior to the other two equations. The thermodynamic properties of the solution process, including the Gibbs free energy, enthalpy, and entropy, were calculated by the van’t Hoff analysis. The values of both the enthalpy change and the standard molar Gibbs free energy change of solution were positive, which indicated that the process was endothermic.

Solubility of ranitidine hydrochloride in solvent mixtures of PEG 200, PEG 400, ethanol and propylene glycol at 25 °C

Experimental solubilities of ranitidine hydrochloride in binary mixtures of ethanol (EtOH)-polyethylene glycol 200 (PEG 200), EtOH-polyethylene glycol 400 (PEG 400), EtOH-1, 2-propanediol (PG), PEG 200-PG and PG-PEG 400 and ternary mixtures of EtOH-PG-PEG 400 at 25°C are reported. The measured data were fitted to the Jouyban–Acree model and the mean percentage deviations (MPD) of back-calculated solubilities for EtOH-PG, EtOH-PEG 400, EtOH-PEG 200, PG-PEG 200 and PG-PEG 400 were 3.0%, 6.3%, 2.8%, 2.2% and 2.1, respectively, and the overall MPD was 3.3%. The corresponding MPD for solubility in PG-PEG 400-EtOH mixtures was 8.4%. Also, experimental densities of the saturated solutions were measured and then fitted to the Jouyban–Acree equation with the overall MPD of 1.5%.

Solubility of Thiotriazinone in Binary Solvent Mixtures of Water + Methanol and Water + Ethanol from (283 to 330) K

The solubility of thiotriazinone in water, methanol, ethanol, water + methanol, and water + ethanol has been measured under temperatures ranging from (283 to 330) K with a laser technique. The results of these measurements were correlated with semiempirical equations. The calculated results have showed fine representativity of experimental data. The stepwise regression method was used to simplify the modified Jouyban–Acree equation.