The mole fraction solubility data of N-carboxyphenoxy-L-2-phenylglycine in 11 neat solvents (methanol, water, isopropyl alcohol, ethanol, n-propyl alcohol, methyl acetate, ethyl acetate, acetone, dichloromethane, acetonitrile, and butanone) and a binary solvent mixture of ethanol + water were determined by the static gravimetric method at 283.15-323.15 K. From the solvent effect analysis, the solubility behavior was affected not only by polarity, but also by some other factors such as hydrogen bonding, cohesive energy density, and molecular structure. The solubility data of N-carboxyphenoxy-L-2-phenylglycine were correlated by using the two-dimensional modified Apelblat model and three-dimensional Apelblat-Jouyban - Acree model. The maximum values of root-mean-square deviation and relative average deviation were 100.98 x 10(-4) and 20.53%, respectively. The solubility calculated by the two models agreed well with the experimental values.

L-Cysteine methyl ester hydrochloride (one of the derivatives of L-cysteine) solubility in 14 monosolvents (methanol, ethanol, n-propanol, n-butanol, sec-butanol, isopropanol, isobutanol, ethyl acetate, 1,4-dioxane, acetonitrile, acetone, 2-butanone, n-pentanol, and dichloromethane) was determined by the static gravimetric method from 283.15 to 333.15 K under the atmospheric pressure. Meanwhile, its solubility in the binary solvent of ethanol + dichloromethane was measured from 283.15 to 303.15 K. From the experimental results, the solubility increased with increasing temperature. And three kinds of polymorphs appeared in the selected solvent systems, which are named alpha-form, beta-form, and gamma-form. Furthermore, from the results, the main factors affecting solubility are polarity, Hildebrand solubility parameter, and hydrogen-bonding interactions. Six thermodynamic models (the modified Apelblat model, Yaws model, Jouyban-Acree model, Machatha model, Apelblat-Jouyban-Acree model, and Apelblat-Machatha model) were used for correlating the solubility data. The Akaike information criterion method was used to evaluate the thermodynamic models.

The data on the solubility of L-thioproline in a mole fraction scale in nine individual solvents (water, methanol, ethanol, isopropanol, acetone, acetonitrile, dichloromethane, ethyl acetate, and 1,4-dioxane) and one binary solvent mixture of water + acetonitrile was measured by a static gravimetric method from 283.15 to 333.15 K. Whether or not a neat or binary solvent system is used, the solubility is nonlinearly positively correlated with the experimental temperatures. At a given temperature, the solubility presents an order of water > acetone approximate to 1,4-dioxane > dichloromethane approximate to ethanol approximate to ethyl acetate > methanol > isopropanol > acetonitrile, which is a result of the multiple influences of many factors related to intermolecular interactions. Four thermodynamic models, including the modified Apelblat, Yaws, Jouyban-Acree, and Apelblat-Jouyban-Acree models were employed for correlating the solubility data, and the results show a satisfactory fitting effect for each model.

The mole fraction solubility data of N-acetyl-L-proline in 16 neat solvents (water, methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, sec-butanol, n-pentanol, acetone, 2-butanone, acetonitrile, dichloromethane, methyl acetate, ethyl acetate, and 1,4-dioxane) covering a temperature range of 283.15-323.15 K were measured by the static gravimetric method. The polymorphism of N-acetyl-L-proline was investigated by the powder X-ray diffraction test and the patterns show that there are two polymorphs within the studied solid-liquid equilibrium systems. The increasing temperature shows a positive effect on N-acetyl-L-proline solubility in all of the solvents and the largest increasing rate is observed in acetonitrile with an increase of 16-fold. The solubility behavior was found to be influenced by five factors including polarity, hydrogen bonding, solvent-solvent interactions, molecular construction, and viscosity. Two thermodynamic models, i.e., the modified Apelblat model and the Yaws model, were used for the correlation of solubility data. To evaluate the fitting results, the average relative deviation (ARD) and root-mean-square deviation (RMSD), as well as the Akaike information criterion (AIC) and Akaike weights, were computed for each model.

The solubility data of L-arginine L-pyroglutamate were determined by the static gravimetric method from 283.15 to 323.15 K in nine pure solvents (water, methanol, ethanol, isopropanol, acetone, acetonitrile, dichloromethane, ethyl acetate, and n-hexane) and a water + ethanol binary solvent system. According to experimental results, solubility was positively correlated with temperature. In the selected solvent systems, three different polymorphs denoted as alpha-form, beta-form, and gamma-form were found. In addition, from the data analysis results, the polarity, hydrogen bonding, Hildebrand solubility parameters, and the molecular structure affected the dissolution equilibrium. Two thermodynamic models including the modified Apelblat model and the Yaws model were used to correlate the solubility data. Meanwhile, these models were evaluated by the Akaike information criterion method.

The solubility (mole fraction) of ethyl L-thiazolidine-4-carboxylate hydrochloride in 15 individual solvents including water, methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, sec-butanol, acetone, 2-butanone, acetonitrile, dichloromethane, methyl acetate, ethyl acetate, and 1,4-dioxane, as well as one binary mixed solvent of ethanol + methyl acetate from 283.15 to 323.15 K was measured by a static gravimetric method. The solid phase of ethyl L-thiazolidine-4-carboxylate hydrochloride in the investigated solvent systems was characterized by the powder X-ray diffraction test. The rising temperature exhibits a positive effect on the ethyl L-thiazolidine-4-carboxylate hydrochloride solubility in pure solvents, while a cosolvency phenomenon was observed in the binary solvent. The solubility behavior in pure solvents was found to be influenced by the mutual effect of six factors including polarity, hydrogen-bonding interaction, solvent-solvent interactions, molecular structures, steric effects, and solvent viscosity. In addition, the measured solubility data were fitted utilizing two thermodynamic models, i.e., the modified Apelblat model and the Apelblat-Jouyban-Acree model.

The data on the solubility of Boc-L-proline in 14 monosolvents, namely, water, ethanol, methanol, n-propyl alcohol, isopropyl alcohol, n-butyl alcohol, isobutyl alcohol, sec-butyl alcohol, acetone, acetonitrile, butanone, ethyl acetate, methyl acetate, and dichloromethane (DCM), were measured by a static gravimetric method covering the temperature range of 283.15-323.15 K. The equilibrated solid phase of Boc-L-proline in all the solvent systems was characterized via the test of X-ray powder diffraction. The solubility values in all the solvents are positively correlated with the temperature. The dissolution behavior was affected by the combined effects of four factors consisting of solvent polarity, formation of hydrogen bonds, solvent-solvent intermolecular interactions (represented by cohesive energy density), and molecular structures of solvents and the solute. Additionally, the Yaws model and modified Apelblat model were utilized to fit the data of solubility, and the values of Akaike information criterion as well as Akaike weights were calculated to evaluate the relative applicability of the two solubility models. The results show that the Yaws model could give a better correlation result for the solubility data than the model of modified Apelblat.

The multicomponent solid-liquid equilibrium data for 1,3,5-triformylbenzene, a key intermediate for the synthesis of porous organic cages, in 12 neat solvents (water, methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, sec-butanol, n-pentanol, acetone, acetonitrile, and 1,4-dioxane) and the binary solvent mixture of acetone + water were measured by the static gravimetric method within the temperature range from 283.15 to 323.15 K. In both neat and binary solvent systems, the solubility values increased with the increase in temperature. Analysis of the data showed that the solubility behavior was mainly affected by the properties of solute and solvents. Six thermodynamic models, i.e., the modified Apelblat model, Yaws model, simplified Jouyban-Acree model, Machatha model, Apelblat-Jouyban-Acree model, and Apelblat-Machatha model, were used for correlating the obtained solubility data mathematically. The Yaws model could give a better fitting result for the solubility in pure solvents (the maximum ARD is 10.761 x 10(-2)), and the correlation result of Machatha model is the best for the binary solvent system (the largest ARD is 5.699 x 10(-2)). To evaluate the models for correlating the solubility data, the Akaike information criterion values and Akaike weights were calculated for each thermodynamic model.

DL-Homocysteine thiolactone hydrochloride (one of the derivatives of L-cysteine) solubility in nine neat solvents (methanol, ethanol, isopropanol, ethyl acetate, 1,4-dioxane, acetonitrile, acetone, 2-butanone, and dichloromethane) were determined by the static gravimetric method at the atmospheric pressure from 283.15 to 323.15 K. At the same time, the solubility in the methanol + acetonitrile binary solvent system was determined. From the result of the experiments, the solubilities all increased with the increase of the temperature. And the polarity is one of the important factors affecting solubility. The three-dimensional (3D) Apelblat-Jouyban-Acree model and the Apelblat-Machatha model were used for correlating the solubility data, and the values calculated by the two thermodynamic models were in good agreement with the experimental data.

N-Acetylglycine solubility in 12 monosolvents (water, methanol, ethanol, n-propanol, i-propanol, n-butanol, i-butanol, s-butanol, n-pentanol, acetone, acetonitrile, and 1,4-dioxane) were determined by the static gravimetric method within the temperature range from 283.15 to 333.15 K under an ambient pressure of 98.8 kPa. In the meantime, the binary solvent mixture (methanol + acetonitrile) of different ratios was measured from 283.15 to 323.15 K. Analysis of the neat solvent data showed that the solubility behavior was influenced by the polarity, hydrogen bond, molecular structures, molecular steric hindrance, and so on. The KAT-LSER model was used to perform the multiple linear regression analysis on a pure solvent system to reveal the solvent effect on solubility. When the solvent composition was constant, a positive correlation of N-acetylglycine solubility with experimental temperature was found in all investigated pure and mixed solvent systems. At a given temperature, inflection points were found in the solubility curves for binary solvent systems as the mole fraction of methanol increased, which may be attributed to the cosolvency phenomenon. Six thermodynamic models, including the modified Apelblat, Yaws, Jouyban-Acree, Machatha, Apelblat-Jouyban-Acree, and Apelblat-Machatha models, were employed for fitting the solubility data.

The equilibrium solubility of N-benzylglycine in 11 pure solvents (methanol, ethanol, n-propyl alcohol, isopropyl alcohol, n-butyl alcohol, acetone, acetonitrile, dichloromethane, ethyl acetate, 1,4-dioxane, and water) and one binary water + ethanol solvent mixture was measured by a static gravimetric method covering the temperature range of (283.15-323.15) K. The polymorphism of N-benzylglycine was characterized via the powder X-ray diffraction test and the results indicate that no crystal form transition occurred during the dissolution process in all solvents studied. When the solvent composition is constant, the solubility of N-benzylglycine in all neat solvents and solvent mixtures is positively correlated with the experimental temperature. With the increase of the mole fraction of water at a certain temperature, the solubility curve of the binary water + ethanol solvent mixtures shows an inflection point, which may be the result of the synergistic solvation effects. The KAT-LSER model equation was used to analyze the mixed solvent system by multiple linear regression analysis to reveal the interactions between solute-solvent and solvent-solvent. In addition, the modified Apelblat model and the Apelblat-Jouyban-Acree model were utilized to correlate the solubility data.

The mole fraction solubility data of trans-4-hydroxy-L-proline in 16 neat solvents (water, methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, sec-butanol, n-pentanol, acetone, 2-butanone, acetonitrile, dichloromethane, methyl acetate, ethyl acetate, and 1,4-dioxane) and a binary solvent mixture of water + acetonitrile were determined by the static gravimetric method from 283.15 to 333.15 K. In both neat and binary solvent systems, the solubility values increased with the increase of temperature. Analysis of the data showed that the solubility behavior was influenced by the polarity, hydrogen bond, cohesive energy density, and molecular structures. Six thermodynamic models, including the modified Apelblat, Yaws, Jouyban-Acree, Machatha, Apelblat-Jouyban-Acree, and Apelblat-Machatha models, were employed for fitting the solubility data. In addition, these models were assessed for classification by the Akaike information criterion values and Akaike weights.

The equilibrium solubilities of myo-inositol in five monosolvents (water, methanol, ethanol, isopropanol, acetone) and four binary solvent systems (water + methanol, water + ethanol, water + isopropanol, water + acetone) were determined using the static gravimetric method from 283.15 to 323.15 K under the ambient pressure of 98.8 kPa. The KAT-LSER model was used to perform the multiple linear regression analysis on mixed solvent systems to reveal the solvent effect on solubility. The Hansen solubility parameter was employed to reveal the solubility behavior of myo-inositol. Three thermodynamic models, including the modified Apelblat, Jouyban-Acree, and Apelblat-Jouyban-Acree models, were employed for fitting the solubility data.

The mole fraction solubility data of L-phenylalanine benzyl ester hydrochloride in 11 neat solvents including, methanol, ethanol, n-propanol, n-butanol, n-pentanol, i-butanol, i-propanol, water, acetone, acetonitrile, and ethyl acetate, as well as one binary mixed solvent of methanol + acetone were measured using the static gravimetric method at a temperature interval of "T = 283.15-323.15 K" and a pressure of "p = 98.8 kPa". The powder X-ray diffraction test was employed to identify the solid-phase characterization of L-phenylalanine benzyl ester hydrochloride in the investigated solvent systems. At constant solvent composition, the solubility was positively correlated with temperature. In the selected monosolvents, the solubility of L-phenylalanine benzyl ester hydrochloride was restricted by multiple factors, and the following order was obtained: methanol > ethanol > n-propanol > n-butanol > n-pentanol > i-butanol > i-propanol > acetone > acetonitrile > ethyl acetate (except for water, which intersects with other solvents). In addition, the modified Apelblat model and the Apelblat-Jouyban-Acree model were employed to fit the solubility data.

The equilibrium solubility of beta-arbutin (ARB) in 12 pure (including water, methanol, ethanol, n-propanol, isopropanol, sec-butanol, n-pentanol, acetone, acetonitrile, ethyl acetate, dichloromethane, and 1,4-dioxane) and 4 binary (water + acetone, water + isopropanol, methanol + acetonitrile, and methanol + ethyl acetate) solvent systems was measured by the gravimetric method at different temperatures under atmospheric pressure. The experimental results indicated that the solubility of ARB increased with the increase of temperature and the content of positive solvent and decreased with the increase of antisolvent composition. The ARB monohydrate was obtained from water and binary solvents containing water, and the cosolvency phenomenon was found in the mixed solvents of water + acetone, water + isopropanol, and methanol + acetonitrile. In addition, the modified Apelblat model, the JouybanAcree model, and the ApelblatJouybanAcree model were used to correlate the experimental solubility data, and the values of average relative deviations and root-mean-square deviations between the experimental and calculated solubilities were no more than 11.534 x 10(-2) and 18.472 x 10(-4), respectively. The calculated values of the three thermodynamic models were in good agreement with the experimental solubility data.

Experimental solubility data of D(-)-salicin in twelve neat solvents (methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, n-pentanol, acetone, acetonitrile, 1,4-dioxance, ethyl acetate, and water) and four binary solvents (water + ethanol, water + acetone, water + isopropanol, and water + methanol) in the temperature range from 283.15 to 323.15 K under atmosphere pressure were determined using the gravimetric method. When the solvent composition was constant, a positive correlation of D(-)-salicin solubility with experimental temperature was found in all investigated pure and mixed solvent systems. At a given temperature, inflection points were found in the solubility curves for binary solvent systems as the mole fraction of water increased, which may be attributed to the cosolvency phenomenon. For the monosolvents, the solubility of D(-)-salicin may be affected by certain factors, such as polarity, steric effects, dipolaritypolarizability, hydrogen bonds, and so on. The KAT-LSER model was used to perform the multiple linear regression analysis on pure and mixed solvent systems to reveal the solutesolvent and solventsolvent interactions. Finally, the modified Apelblat model, the JouybanAcree model, and the ApelblatJouybanAcree model were utilized to correlate the solubility data.

The solubility of moroxydine hydrochloride was determined by the gravimetrical method (temperature from 283.15 to 323.15 K, pressure at 101.325 kPa) in 12 pure solvents (water, methanol, ethanol, 1-propanol, 1-butanol, 2-methyl-1-propanol, 2-propanol, 1-pentanol, 2-butanol, acetonitrile, ethyl acetate, and acetone) and a binary system (water + 2-propanol). The results of this experiment suggested that the solubility data of moroxydine hydrochloride increased with increasing mole fraction of water and experimental temperature in all investigated neat and mixed solvent systems. The moroxydine hydrochloride solubility order in the 12 neat solvents was shown as water > methanol > ethanol > 1-propanol > 1-butanol > 2-methyl- 1 - propanol > 2-propanol > 1-pentanol > 2-butanol > acetonitrile approximate to ethyl acetate approximate to acetone. For polar protic solvents except for 1-pentanol, the main factor influencing the solubility behavior was the polarity. While it was affected by complicating factors in polar aprotic solvents. The fitting results of the moroxydine hydrochloride solubility data obtained by the modified Apelblat, Jouyban-Acree, and Apelblat-Jouyban-Acree models were all satisfactory.

Experimental solubility data of D-ribose in four binary (2-propanol + 1-hexane, ethanol + 1-hexane, methanol + dichloromethane, and ethanol + dichloromethane) and twelve pure (1-hexane, dichloromethane, ethyl acetate, acetonitrile, acetone, 2-methyl-1-propanol, 1-butanol, 2-propanol, 2-butanol, 1-propanol, ethanol, and methanol) solvent systems were measured at different temperatures under the atmospheric pressure by using the gravimetric method. The experimental results showed that the solubility of D-ribose increased with the increase of temperature and the content of positive solvent, and decreased with the increase of antisolvent composition. The dissolution behavior of D-ribose in pure solvents was mainly affected by the solvent types and solvent properties, and the solvent effect on D-ribose solubility was further examined by the KAT-LSER model. The solubility data were correlated by the modified Apelblat, Jouyban-Acree, and Apelblat-Jouyban-Acree models. The calculated values of the three thermodynamic models were in good agreement with the experimental data.

Monosodium fumarate solubility in 12 monosolvents (water, methanol, ethanol, 1-propanol, 1-butanol, 1-pentanol, 2-propanol, 2-methyl- 1-propanol, ethyl acetate, 1,4-dioxane, acetonitrile, and acetone) and four binary solvents (water + methanol, water + ethanol, water + 2-propanol, and water + acetone) was determined by the gravimetric method from 283.15 to 323.15 K. The solubility order in pure solvents was water > methanol > ethyl acetate > 1,4-dioxane > ethanol > 1-propanol > 1-butanol > acetonitrile > 1-pentanol > 2-propanol > acetone > 2-methyl- 1 -propanol. Also, it was positively related to experimental temperature and solvent composition for all solvent systems. According to the solubility results, the dissolution behavior of monosodium fumarate in pure solvents was mainly affected by the solvent properties including polarity, hydrogen bond acidity (alpha), hydrogen bond basicity (beta), bipolar/polarizability (pi*) and Hildebrand solubility parameter (delta(H)). The modified Apelblat, Jouyban-Acree, and Apelblat-Jouyban-Acree models were used to correlate the solubility data, and the values calculated by the three thermodynamic models were found to agree well with the experimental data.

Experimental solubility data of sodium naphthalene-1,5-disulfonate in five neat solvents (water, methanol, ethanol, 2-propanol, acetone) and three binary solvent systems (water + ethanol, water + 2-propanol, water + acetone) at different temperatures from 283.15 to 323.15 K were determined by the gravimetric method. The experimental results showed that three kinds of polymorphs appeared in the investigated solvent systems, and the solubility of sodium naphthalene-1,5-disulfonate all increased with increasing temperature and water content. According to the data measured, water was suitable to be the positive solvent, while methanol was considered to be a less-effective antisolvent due to its relatively large dissolving capacity. By means of our research, the solubility of sodium naphthalene-1,5-disulfonate in the neat solvents had a relation with the polarity of the solvents. The solubilities of sodium naphthalene-1,5-disulfonate were fitted by the modified Apelblat, Jouyban-Acree, van't Hoff-Jouyban-Acree, and Apelblat-Jouyban-Acree models. The results showed that the four models can predict the experimental values very well.