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Solubility of meloxicam in {methanol + water} mixtures from 293.15 to 313.15 K has been determined and correlated by means of the Jouyban–Acree model. By using the van’t Hoff and Gibbs equations the respective apparent thermodynamic quantities for the dissolution and mixing processes, namely Gibbs energy, enthalpy, and entropy, were calculated. A non-linear enthalpy–entropy relationship was observed in the plot of enthalpy vs. Gibbs energy exhibiting negative but variable slopes in the composition region 0.00

The equilibrium solubility of gliclazide (3) in {Transcutol (1) + water (2)} mixtures at several temperatures was reported in the literature. However, no deep attempt was made to correlate gliclazi...

The all experimental solubility data of sulphamethazine in {acetonitrile (1) + water (2)} binary solvent mixtures at temperature range from (278.15 to 323.15) K have been carefully reanalysed. Then...

Experimental mole fraction solubility of lamotrigine (LTG) in ternary aqueous mixtures of two ionic liquids (ILs), 1-hexyl and 1-octyl-3-methylimidazolium bromide, [HMIm][Br] and [OMIm][Br] were reported at several temperatures T = (293.15 to 313.15) K. The van't Hoff and (Jouyban-Acree-van't Hoff, E-Jouyban-Acree-van't Hoff, e-NRTL, UNIQUAC and Wilson) models were used to correlate the solubility data. The comparison of the models with temperature and solvent composition dependencies shows that the Wilson model has the minimum ARD which are relatively close to those obtained from Jouyban-Acree-van't Hoff and E-Jouyban-Acree-van't Hoff models and maximum ARD belonged to the UNIQUAC model. The order of ARDs for these models is: Wilson

In the current study, the sildenafil citrate solubility is investigated in (2-propanol + water) binary mixtures at five different temperatures (293.2-313.2 K). The experimental solubility data are obtained from the shake-flask method and correlated with some linear and non-linear cosolvency models (i.e. the van't Hoff, CNIBS/Redlich-Kister, the Jouyban-Acree, the Jouyban-Acree-van't Hoff, the mixture response surface, Buchowski-Ksiazczak and the modified Wilson models). The accuracy of these cosolvency models is investigated with the mean relative deviations of the back calculated solubility data. The Gibbs energy, enthalpy and entropy as the apparent thermodynamic parameters are calculated utilizing the van't Hoff and Gibbs equations for sildenafil citrate in the (2-propanol + water) binary mixtures at T-hm (303.2 K). Moreover, the density values of sildenafil citrate are measured in the saturated mixtures and represented by the Jouyban-Acree model. (C) 2021 Elsevier B.V. All rights reserved.

Background: Meloxicam is a powerful analgesic and anti-inflammatory drug widely prescribed by physicians in current therapeutics. Because of the very low aqueous equilibrium solubility of meloxicam, this property has been studied in {2-propanol + water} mixtures from (293.15 to 313.15) K to expand the solubility database about pharmaceutical compounds in mixed solvents useful for homogeneous liquid dosage forms design. Methods: Flask shaken method and UV-vis spectrophotometry were used for meloxicam solubility determinations. Jouyban-Acree model was challenged for solubility correlation. The van’t Hoff and Gibbs equations were employed here to calculate the respective apparent standard thermodynamic quantities for the dissolution and mixing processes, namely Gibbs energy, enthalpy, and entropy. In addition, the inverse Kirkwood-Buff integrals were employed to compute the preferential solvation parameters of meloxicam by 2-propanol in the mixtures. Results: Meloxicam solubility increases with temperature arising and maximum solubilities are observed in the mixture of x1 = 0.70 at all temperatures. Jouyban-Acree model correlates the meloxicam solubility very well. Dissolution processes were endothermic in all cases and entropy-driven in the interval 0.20 ≤ x1 ≤ 1.00. Non-linear enthalpy–entropy relationship was observed in the plot of enthalpy vs. Gibbs energy exhibiting negative but variant slopes in the composition region 0.00 < x1 < 0.40 and variant negative and positive slopes in the other mixtures. Meloxicam is preferentially solvated by water in water-rich mixtures, it is apparently solvated by water in 2-propanol-rich mixtures, but it is preferentially solvated by 2-propanol in the composition interval of 0.19 < x1 < 0.78. Conclusion: Solid-liquid equilibrium of meloxicam in {2-propanol + water} mixtures has been studied at several temperatures as a contribution to preformulation studies of homogeneous liquid pharmaceutical dosage forms based on this drug.

The solubility of lamotrigine was measured in aqueous mixtures of ionic liquid, 1-octyl-3-methylimidazolium bromide [OMIm][Br] up to 0.9 mass fraction at T = (293.2–313.2) K. The λ-h and van’t Hoff models with temperature dependency and Jouyban-Acree-van’t Hoff, e-NRTL, UNIQUAC and Wilson models with temperature and solvent composition dependencies were used to correlate the experimental solubility data. The computed %ARDs show that the van’t Hoff equation is better than λ-h model and Jouyban-Acree-van’t Hoff model has the best agreement with the experimental data and the order of %ARDs for the used models is, Jouyban-Acree-van’t Hoff

Naproxen (NAP) is a widely used drug for the treatment of pain and inflammatory conditions. However, there is not the physicochemical information about this drug such as solubility, volumetric and compressibility properties in the presence of deep eutectic solvents (DES) as a new class of green solvents to overcome the low solubility of drugs. In this work, the solubility of NAP is studied in the solutions containing some choline chloride (ChCl) based DES at temperature ranges (298.15–313.15) K. The results indicate that the solubility increases with increasing the concentration of DES and temperature and DES containing malonic acid is the proper co-solvent. The experimental solubility values were correlated by the e-NRTL, Wilson and UNIQUAC models. In addition, the complex interactions between the components in the systems should be elucidated, therefore, the thermodynamic properties including volumetric and compressibility properties have been investigated using density and speed of sound measurements at T = 298.15 K. According to calculated thermodynamic parameters, strong interactions between NAP and DESs are observed which is in agreement with obtained solubility data.

The aim of this investigation was to study the solubility behavior of ketoconazole in the binary mixed solvents of N-methyl-2-pyrrolidone (NMP) and water within the temperature range of 293.2–313.2 K and develop mathematical models using five cosolvency models; i.e. van't Hoff equation, Yalkowsky model, Jouyban-Acree model, Jouyban-Acree-van't Hoff model and modified Wilson model. In addition, density of the solutions saturated with ketoconazole in various solvent compositions and temperatures was measured and the results were correlated according to the Jouyban–Acree model. Moreover, apparent thermodynamic quantities of ketoconazole dissolution process in the NMP/water mixtures, including entropy, enthalpy and Gibbs free energy were computed using van't Hoff and Gibbs equations. The modeling showed that the mean relative deviation (MRD%) of the back-calculated solubility data using the above mentioned models were 2.9%, 55.4%, 13.6%, 8.6% and 21.8% respectively.

The solubility of lamotrigine (LTG) was determined in {1-propanol (1) + water (2)} mixtures over a temperature range of 293.15 to 313.15 K. The measured data were correlated to cosolvency models namely Jouyban-Acree, Jouyban-Acree-van’t Hoff, combined nearly ideal binary solvent/Redlich-Kister (CNIBS/R-K), modified Wilson and Machatha models. Among the models, Jouyban-Acree with temperature and solvent composition dependencies has more accuracy rather than Jouyban-Acree-van’t Hoff model and CNIBS/R-K model with solvent composition dependency is more compatible with the experimental solubility data. Furthermore, the apparent standard molar Gibbs energy, entropy, and enthalpy of dissolution and mixing ΔHsoln∘, ΔSsoln∘, ΔGsoln∘, ΔHmix∘, ΔSmix∘ and ΔGmix∘ for LTG in the studied binary mixtures were calculated based on the van’t Hoff and Gibbs free energy equations which suggest that the dissolution process is more favourable in 1-propanol-rich mixtures and proceeds entropically. Finally, preferential ...

Minoxidil solubility in binary mixtures of propylene glycol + water at different temperatures has been performed by shake-flask method followed by spectrophotometry method. Four cosolvency models including the modified Wilson model, the Yalkowsky model, Jouyban-Acree model and Jouyban-Acree-van't Hoff model were used to correlate the measured solubility data. The correlation and prediction abilities of these models were compared by computing mean relative deviations (MRD%). Apparent thermodynamic properties of minoxidil dissolution such as enthalpy, entropy and Gibbs free energy were investigated through van't Hoff and Gibbs equations. Furthermore, preferential solvation parameters of minoxidil were calculated by means of the inverse Kirkwood-Buff integrals.

The equilibrium solubility at temperatures from (293.15 to 313.15) K, dissolution thermodynamics and preferential solvation of sulphadiazine (SD) in {acetonitrile (ACN) (1) + water (2)} mixtures is...

The aims of this study were to investigate the solubility behavior of lamotrigine (LTG) in the binary mixed solvents of 2-propanol and water within the temperature range of 293.2–313.2 K and correlate the experimental values by some mathematical models including the van't Hoff equation, Yalkowsky model, Jouyban-Acree model, Jouyban-Acree-van't Hoff model and the modified Wilson model. The density of the saturated solutions of LTG in various solvent compositions and temperatures was also measured and the results were represented mathematically with Jouyban-Acree model. Furthermore, the apparent thermodynamic properties of LTG dissolving, as well as the preferential solvation, in the investigated mixed solvents were calculated and the details were discussed.

The goal of this work was to study the solubilization and thermodynamic behavior of budesonide (BDS) in the aqueous mixtures of polyethylene glycol 400 (PEG 400) within the temperature range of 293.2–313.2 K by using a shake-flask method. The obtained molar solubility data were correlated by using some cosolvency models. The mean relative deviations (MRDs%) for back-calculated solubility data were employed to show the accuracy of the fitness. Furthermore, the apparent thermodynamic properties of dissolution of BDS in the binary mixtures of solvent including entropy, enthalpy and Gibbs free energy were computed using van't Hoff and Gibbs equations. Finally, by means of IKBI method was observed that BDS was preferentially solvated by PEG 400 in all the mixtures compositions.

The equilibrium solubility of triclocarban in {1,4-dioxane (1) + water (2)} mixtures at 293.15 K to 313.15 K was reported. Mole fraction solubility increases continuously from neat water to neat 1,4-dioxane at all temperatures. Solubility behavior was adequately correlated by means of a number of cosolvency models including the Jouyban-Acree model. Based on the Gibbs and van't Hoff equations the respective apparent thermodynamic quantities of dissolution were calculated. Non-linear enthalpy-entropy compensation analysis is observed indicating different dissolution mechanism with the variation in mixtures composition.

Equilibrium mole fraction solubility of vanillin in nine aqueous-ethanolic mixtures, as well as in neat water and neat ethanol, was determined at seven temperatures from T = 293.15 to T = 323.15 K. Vanillin solubility in these mixtures was adequately correlated with several well-known correlation models with the mean percentage deviations of 5.9 to 18.3%. Respective apparent thermodynamic functions, i.e. Gibbs energy, enthalpy, and entropy, for the dissolution, mixing and solvation processes, were computed using the van't Hoff and Gibbs equations. The enthalpy-entropy relationship for vanillin was non-linear in the plot of enthalpy vs. Gibbs energy of dissolution with positive slopes from neat water to the mixture of w(1) = 0.10 and the interval 0.50 < w(1) < 0.90 but negative in the interval 0.10 < w(1) < 0.50 and from w(1) = 0.90 to neat ethanol. Accordingly, in the first cases the vanillin transfer from more polar to less polar solvent systems is enthalpy-driven but entropy-driven for the last ones. Moreover, by means of the inverse Kirkwood-Buff integrals is observed that vanillin is preferentially solvated by water molecules in water-rich mixtures but preferentially solvated by ethanol molecules in mixtures of 0.23 < x(1) < 1.00.

In this research, the equilibrium mole fraction solubility of fluconazole (FLC) in some aqueous-ethanolic mixtures was determined at seven temperatures from (293.15 to 323.15) K. The respective apparent thermodynamic functions (Gibbs energy, enthalpy, and entropy) for the dissolution, mixing and solvation processes were computed using the van't Hoff and Gibbs equations. The enthalpy-entropy relationship for FLC was non-linear in the plot of enthalpy vs. Gibbs energy of solution with negative slope in the composition regions of 0.00

Equilibrium mole fraction solubility of coumarin in nine aqueous-ethanolic mixtures, as well as in neat water and neat ethanol, was determined at seven temperatures from (293.15 to 323.15) K. Coumarin solubility in was adequately correlated with several well-known correlation models with the mean percentage deviations of 5.1-10.8%. The respective apparent thermodynamic functions (Gibbs energy, enthalpy, and entropy) for the dissolution, mixing and solvation processes were computed using the van't Hoff and Gibbs equations. The enthalpy-entropy relationship for coumarin was non-linear in the plot of enthalpy vs. Gibbs energy of dissolution with negative slope from neat water to the mixture of w(1) = 0.10 but positive from this mixture to neat ethanol. Accordingly, in the first case the coumarin transfer from neat water to the mixture of w(1) = 0.10 is entropy-driven, which could be attributed to water molecules release originally bounded as "icebergs" around the non-polar groups of this drug. Otherwise, in mixtures of w(1) >= 0.10 the driving mechanism for the transfer of coumarin from the more polar solvent systems to those less polar is the enthalpy, probably owing the better drug solvation. Moreover, by means of the inverse Kirkwood-Buff integrals is observed that apparently coumarin is preferentially solvated by water molecules in water-rich mixtures but preferentially solvated by ethanol molecules in mixtures of 0.23 < x(1) < 1.00. (C) 2021 Elsevier B.V. All rights reserved.

This paper discusses sulfamerazine (SMR) solubility in Acetonitrile (MeCN) + Methanol (MeOH) cosolvents at nine temperatures (278.15–318.15 K). Herein, the maximum SMR solubility was reached in a cosolvent mixture at the highest studied temperature, and the minimum SMR solubility was reached in neat methanol at the lowest studied temperature. Using experimental data, thermodynamic functions were calculated for both the solution and mixture using the Gibbs and van’t Hoff equations, thus determining that the solution process is endothermic with entropic favoring. In addition, the preferential solvation parameters (δx3,1), calculated using the inverse Kirkwood-Buff integrals (IKBI) method, are reported; SMR is preferentially solvated by MeOH in MeOH-rich mixtures, and in intermediate and MeCN-rich mixtures, the δx3,1 values indicate that SMR is not preferentially solvated by any of the two solvents in the mixture (MeCN + MeOH). Finally, eight models were assessed (Apelblat, van’t Hoff, Yaws, λh, Weibull, NRTL, Wilson, and Wilson modified), with all presenting mean relative deviation percentages (MRD%) under 6%, which indicates a good correlation with the experimental data.

The solubility profile of codeine phosphate in the carbitol and 2-propanol mixtures at 293.2-313.2 K are determined and correlated with some developed cosolvency models. Moreover, the density values of codeine phosphate saturated solutions are also determined and fitted with the Jouyban-Acree model. The model accuracy is investigated by calculating the mean relative deviations (MRDs%). The thermodynamic parameters of codeine phosphate dissolution in the non-aqueous mixtures of carbitol and 2-propanol are also computed by using van't Hoff and Gibbs equations.

The reported experimental density and viscosity of polyethylene glycol 600 + methanol, ethanol, 1-propanol, and 2-propanol were mathematically represented using a simple and single mathematical model, namely, the Jouyban–Acree model. The results obtained revealed that one may accurately calculate the density, viscosity, and the physico-chemical properties derived from these values using a single mathematical model.

The molar solubility of budesonide (BDS) in some non-aqueous mono-solvents was experimentally determined within the temperature ranges from 293.2 to 313.2 K and successfully correlated and back-calculated with the modified van't Hoff equation. The Abraham general solvation parameter model was used to predict the partitions and saturation solubility of BDS in the investigated mono-solvents. Furthermore, the generated molar solubility data were used to calculate the apparent thermodynamic parameters of the dissolution process of BDS in all solvents according to van't Hoff and Gibbs equations and the derived values were correlated using Abraham solvation parameters.

The experimental solubility determination of bosentan (BST) in 1-propanol + water mixtures within temperature range, T = (293.15–313.15) K were performed by applying the shake-flask method. The solubility data were correlated by four cosolvency models, which are the Jouyban-Acree, Jouyban-Acree-van’t Hoff, modified Wilson, and Yalkowsky equations. The back-calculated solubility using the Jouyban-Acree-van’t Hoff equation presents better compatibility with the experimental data than those by the other models. Thermodynamic properties such as apparent molar enthalpy, entropy, and Gibbs free energy change of BST dissolution process in the binary (1-propanol + water) mixtures were also calculated which indicative of the inspontaneous process of dissolution.

The aim of this study is to develop the trained versions of Yalkowsky and Jouyban-Acree models for the prediction of drug solubility in the binary aqueous mixtures of methanol (MeOH) at various temperatures. To provide a full predictive model, the Abraham solvation parameters of solutes are combined with the proposed models. The solubility data of 41 drug and/or drug-like compounds with different polarities and structural features covering the total drug-like space are fitted by these models. The generally trained models provide reasonable estimation of the solubility behavior of drugs and can be helpful in the pharmaceutical industry.

Extended Hildebrand solubility approach (EHSA) was applied in this research to analyse the equilibrium solubility of sulphadiazine, sulphamerazine and sulphamethazine in some {1-propanol (1) + water (2)} mixtures at 298.15 K. Reported experimental solubilities and some fusion properties of these drugs were used for EHSA calculations. A good predictive character of EHSA (with mean deviations lower than 4.0%) was found by using regular polynomials in order five when correlating the interaction parameter (W) and the Hildebrand solubility parameter of solvent mixtures free of drug (δ1+2). Nevertheless, the predictive character of EHSA was almost the same as obtained when logarithmic drug solubilities (log x3) were correlated with δ1+2 by using a fifth-degree regular polynomial.

The aim of present study is to investigate the solubilization behavior and thermodynamics of clotrimazole (CLO) in the binary mixtures of ethanol and water within the temperature range, T = (293.2–313.2) K, by employing a shake-flask method. The generated solubility data are mathematically represented by using four cosolvency models (i.e. van't Hoff equation, Yalkowsky–Roseman model, Jouyban-Acree model and Jouyban-Acree–van't Hoff model). The models performance for correlative studies is illustrated by mean relative deviations (MRD). Moreover, apparent thermodynamic properties of CLO dissolution process in the investigated mixed solvents including entropy, enthalpy and Gibbs free energy are calculated using van't Hoff and Gibbs equations. Finally, preferential solvation of CLO by the mixture components based on the inverse Kirkwood–Buff integrals method is also analyzed.

The present work is devoted to the study of the caffeine dissolution process in the non-aqueous binary mixture of N-methyl-2-pyrrolidone + ethylene glycol mixture at a temperature range of T = (293.2 – 313.2) K. The generated solubility data are mathematically represented by using some cosolvency models (i.e. Jouyban-Acree, Jouyban-Acree-van’t Hoff, mixture response surface and the double log–log) and their accuracy is investigated by calculation of the mean relative deviations (MRD%) for back-calculated solubility data. The density values of caffeine saturated solutions are determined and represented by the Jouyban-Acree model. In another effort, the apparent thermodynamic properties of Gibbs free energy, standard enthalpy, and entropy of the dissolution process are computed using the Gibbs and van’t Hoff equations at Thm = 303.0 K and discussed.

The solid-liquid equilibrium of sildenafil citrate in the binary non-aqueous mixtures of propylene glycol and ethanol is investigated by a shake-flask technique at T = (293.2–313.2) K and atmospheric pressure. Some mathematical models such as the van’t Hoff, the mixture response surface, the Jouyban-Acree, the Jouyban-Acree-van’t Hoff and λh models are utilized for modeling the experimental solubility data and the mean relative deviations are employed to evaluate the accuracy of the fitness. Moreover, apparent thermodynamic properties of Gibbs free energy, standard enthalpy and entropy of the dissolution process are calculated and discussed.

The equilibrium solubility of sulfamerazine (SMR) in neat ethylene glycol (EG) and nineteen {(EG) (1) + water (2)} mixtures is reported at temperatures from (278.15 to 318.15) K. Mole fraction solubility of SMR (x3) increases with temperature arising and also increases with the EG proportion increasing. It varies from 1.71 × 10−5 in neat water to 7.78 × 10−4 in neat EG at 298.15 K. Solubility behavior was correlated by the extended log-linear model of Yalkowsky, the Jouyban-Acree model, and Jouyban-Acree-van’t Hoff model and the obtained mean percentage deviations are 80.1%, 6.7% and 6.6%, respectively. From the variation of solubility with temperature, the apparent thermodynamic analysis of dissolution and mixing processes was performed in all the mixtures and neat solvents. From inverse Kirkwood-Buff integrals (IKBI) calculations is observed that SMR exhibits low negative preferential solvation parameters by EG in water-rich mixtures. Otherwise, SMR is preferentially solvated by EG in the interval (0.24

Solubility profile for sildenafil citrate in the non-aqueous mixtures of 1-propanol and water is measured using a shake-flask method at different temperatures of 293.2 K, 298.2 K, 303.2 K, 308.2 K and 313.2 K and correlated employing some well-known cosolvency models (e.g. the CNIBS/Redlich-Kister, the Jouyban-Acree, the Jouyban-Acree-van’t Hoff, the modified Wilson and λh equation models) and the accuracy of the models is checked by the calculation of the mean relative deviations. The density values of sildenafil citrate saturated solutions are also investigated and represented by the Jouyban-Acree model. In another effort, to obtain apparent thermodynamic parameters of sildenafil citrate dissolution process, including ΔHo, ΔSo, and ΔGo, the Gibbs and van’t Hoff equations are applied.

The solubility and solution thermodynamic properties of mesalazine in the binary mixtures of a deep eutectic solvent (DES) and water are determined by a shake-flask method followed by spectrophotometry method in the temperature range of 293.2–313.2 K. The obtained solubility data are correlated using some linear cosolvency models including the van’t Hoff equation, the Apelblat, Jouyban-Acree, Jouyban-Acree-van’t Hoff models. The accuracy of each used model is investigated by calculation of the mean relative deviations of the back-calculated solubility data. The apparent thermodynamic properties of mesalazine dissolution in the investigated mixtures are also computed based on the van’t Hoff and Gibbs equations.

The solubility knowledge of pharmaceutical compounds in pure solvents and solvent mixtures has a critical role in formulation, separation and purification in the pharmaceutical and chemical industries. In the article ahead, the solid–liquid equilibria measurements for solubility of caffeine in the non-aqueous binary mixtures of N-methyl-2-pyrrolidone (NMP) and isopropanol at different temperatures and atmospheric pressure is measured and the acquired data are fitted to some linear and non-linear cosolvency models including the van’t Hoff, the combined nearly ideal binary solvent/Redlich–Kister (CNIBS/R–K), Jouyban-Acree, Jouyban-Acree-van’t Hoff, and the modified Wilson models. The determined density data of caffeine saturated solutions as another physico-chemical property are also correlated with the Jouyban-Acree model and the results are discussed in detail. The mean relative deviations (MRD%) of the back-calculated solubility data aiming to study the accuracy of the applied models are computed. Moreover, the apparent thermodynamic properties of caffeine dissolution process are also calculated by using van’t Hoff and Gibbs equations.

The equilibrium solubility of a weakly water-soluble drug of naproxen (NAP) in ethylene glycol (EG) + water is determined by a shake-flask method in the temperature range of 293.2–313.2 K. Five models including Jouyban-Acree, Jouyban-Acree-van't Hoff, the mixture response surface, van't Hoff and the modified Wilson models are applied to mathematical modeling of the solubility data. The mean relative deviations is applied for the accuracy investigation of each model. Moreover, the Jouyban-Acree model is used to a numeric representation of the density of saturated mixtures at different temperatures. The respective apparent thermodynamic quantities of the dissolution and solvation processes, namely Gibbs energy, enthalpy, and entropy, are also calculated based on the van't Hoff and Gibbs equations. Further, preferential solvation parameters of NAP by EG molecules are estimated based on the inverse Kirkwood-Buff integrals.

*Akay, Sema ( Aksaray, Yazar ), Equilibrium mole fraction solubility of 5-fluorouracil (5-FU) in 19 aqueous-ethanolic mixtures, as well as in neat water and neat ethanol, was determined at seven temperatures from (293.15 to 323.15) K. 5-FU solubility in these mixtures was adequately correlated with several well-known correlation models. The respective apparent thermodynamic functions (Gibbs energy, enthalpy, and entropy) for the dissolution, mixing and solvation processes were computed using the van't Hoff and Gibbs equations. The enthalpy–entropy relationship for 5-FU was non-linear in the plot of enthalpy vs. Gibbs energy of solution with variant but positive slope in almost all the composition regions. Thus, the driving mechanism for 5-FU transfer processes was the enthalpy. In addition, by means of the inverse Kirkwood-Buff integrals is observed that apparently 5-FU is preferentially solvated by water molecules in water-rich mixtures but preferentially solvated by ethanol molecules in ethanol-rich mixtures.

The aims of the current study are solubility behavior investigation of phenytoin in the mixtures of 1-propanol and water at different temperatures and correlation of the generated data to some linear and non-linear cosolvency models. As another physico-chemical property, the density of phenytoin saturated solutions is also measured and the results are mathematically represented using the Jouyban-Acree model. The accuracy of applied models is checked by the computation of the mean relative deviations (MRD %). Moreover, the apparent thermodynamic properties of the phenytoin dissolution process are also calculated according to van't Hoff and Gibbs equations. It is observed that all the thermodynamic quantities, namely Gibbs energy, enthalpy and entropy changes, are positive in every solvent system. Furthermore, by means of the inverse Kirkwood-Buff integrals it is shown that phenytoin is preferentially solvated by water molecules in water-rich mixtures and preferentially solvated by 1-propanol molecules in the composition interval 0.19

The solubilities of budesonide (BDS) in binary aqueous mixtures of N-methyl-2-pyrrolidone at temperatures ranging from 293.2 to 313.2 K were determined and mathematically correlated by three cosolvency models, i.e. Jouyban–Acree model, Jouyban–Acree–van’t Hoff model and modified Wilson model. The solubilities were measured using the shake-flask method and the models wereused to fit the solubility data of BDS in the solvent mixtures. The obtained mean relative deviations (MRDs %) for cosolvency models trained using whole data points varied between 5.0% and 31.0%. Solubilities were also predicted by the generally trained version of the Jouyban–Acree model with the MRD of 37.0%. Furthermore, the apparent thermodynamic properties of dissolution process of BDS in all the mixed solvents were calculated according to van’t Hoff and Gibbs equations. Dissolution of BDS in these mixed solvents is an endothermic process.

The solubility of budesonide (BDS) in binary mixtures of ethanol and water at T = (293.2–313.2) K is determined and mathematically represented using two cosolvency models, i.e. Jouyban–Acree model and Jouyban–Acree–van’t Hoff model. The mean relative deviations for fitting the solubility data of BDS in binary mixtures of ethanol + water are 6.6% and 6.5%, respectively. Furthermore, the apparent thermodynamic properties, dissolution enthalpy, dissolution entropy, and Gibbs free energy change of dissolution process of BDS in all the mixed solvents were calculated according to van’t Hoff and Gibbs equations. Dissolution of BDS in these mixed solvents is an endothermic process.

Mathematical representations reported by Sun and coworkers for the modified version of the combined nearly ideal binary solvent (NIBS)/Redlich-Kister model are carefully examined in regards to the model's ability to predict the solubility of β-alanine dissolved in binary solvent mixtures and some recommendations were proposed. In addition, the preferential solvation parameter of β-alanine by the cosolvents in their binary aqueous mixtures were computed and discussed in details.

Extended Hildebrand solubility approach (EHSA) was applied to analyse the equilibrium solubility of sulphadiazine, sulphamerazine and sulphamethazine in some {methanol (1) + water (2)} mixtures at 298.15K. Reported experimental solubilities and some fusion properties of these drugs were used for EHSA calculations. A good predictive character of EHSA (with mean deviations lower than 4.0%) was found by using regular polynomials in order 4 when correlating the interaction parameter (W) and the Hildebrand solubility parameter of solvent mixtures free of drug (δ1+2). Nevertheless, the predictive character of EHSA was almost the same as obtained when logarithmic drug solubilities (log x3) were correlated with δ1+2.

Mathematical representations reported by Li et al. for a number of cosolvency models are carefully examined concerning the models’ abilities to predict the solubility of maltitol in binary aqueous mixtures of methanol and ethanol at various temperatures. Some further recommendations on computational methods are also provided to be employed in the future research works. Preferential solvation of the solution was also investigated to provide better understanding of the dissolution process.

Solubility is one of the most significant physicochemical properties of drugs, and improving the solubility of drugs is still a challenging subject in pharmaceutical sciences due to requirements of enhancing their bioavailability. Celecoxib, according to the biopharmaceutics classification system (BCS), is a class 2 drug, possessing low water solubility (

The experimental solubility data of fenofibrate in binary aqueous mixtures of ethanol and acetone has been reanalyzed. A correct mathematical derivation is provided for the correlation expression from a combination of the van’t Hoff and Jouyban–Acree models. Sun et al. used the expression in their study. However, it erroneously implied that the expression resulted from a simple transformation of the Jouyban–Acree model.

Experimental solubility of deferiprone (DFP) in N-methyl-2-pyrrolidone (NMP) + ethanol (EtOH) mixtures at 293.2, 298.2, 303.2 and 308.2 K was determined and mathematically represented using various models. The trained versions of the van’t Hoff equation, its combined version with log-linear model, Jouyban–Acree model and a combination of van’t Hoff + Jouyban–Acree model were reported to simulate DFP solubility in the binary mixture compositions at various temperatures. The mean percentage deviation (MPD) was used as an accuracy criterion. The obtained overall MPDs for back-calculated and predicted solubility of DFP in NMP + EtOH mixtures varied from 1.1% to 3.2% and 2.6% to 6.6%, respectively. Some of apparent thermodynamic quantities for the dissolution processes of DFP are also reported.

Mathematical representations reported by Yin and co-workers for the Combined Nearly Ideal Binary Solvent (NIBS)/Redlich–Kister model are carefully examined in regards to the model’s ability to predict the solubility of trimethoprim dissolved in binary aqueous-2-propanol and aqueous-ethanol solvent mixtures. The equation coefficients reported by Yin and co-workers were found to give calculated mole fraction solubilities in the two alcohol monosolvents that exceed unity. The narrow range of solvent composition over which the authors performed solubility measurements does not enable one to derive mathematical correlations for predicting the solubility of trimethoprim in the alcohol-rich solvent composition region.

Solubility of sildenafil citrate (SC) in binary aqueous mixtures of ethanol (EtOH) was studied at 293.2, 298.2, 303.2, 308.2 and 313.2 K. Density of the SC saturated solutions over the entire solvent composition and temperature range was measured using a pycnometer. The effect of solvent composition on solubility, enthalpy, entropy and Gibbs energy was studied according to van't Hoff and Gibbs equations. The experimental solubility and densities were used to estimate solubility in the investigated solvent system using the van't Hoff and Jouyban-Acree models.

Deep eutectic solvents (DESs) have recently been getting a great deal of attention in many fields of science and technology. The objective of this study was to peruse the solubility of indomethacin (IMC) as sparingly soluble drug in some tetrabutylammonium bromide (TBAB)-based DESs (TBAB/ethylene glycol and TBAB/glycerol). The shake flask method has been employed in this study at temperature ranges T = (298.15–313.15) K and atmospheric pressure (pP = 86.6 kPa). The results showed that the solubility of IMC in TBAB/ethylene glycol system was obtained approximately 17,000-fold more than its solubility in water. The solubility data were accurately correlated by the famous local composition activity coefficient models including e-NRTL and UNIQUAC. It was also our aim to evaluate Hansen solubility parameters in IMC solubility prediction. These parameters can help to predict the solvent performance during the manufacturing processes and will be useful in guessing solvent behavior in many other fields of effort. The experimental and the Hansen solubility parameters results are very well matched. In addition, the apparent thermodynamic properties of dissolution and mixing were studied in these solutions based on Van’t Hoff and Gibbs equations.

*Akay, Sema ( Aksaray, Yazar ) *Kayan, Berkant ( Aksaray, Yazar ), Author keywords Indexed keywords SciVal Topics Abstract In this research, the equilibrium mole fraction solubility of 2,4-dinitrotoluene (2,4-DNT) in some aqueous-ethanolic mixtures was determined at seven temperatures from (293.15 to 323.15) K. The respective apparent thermodynamic functions (Gibbs energy, enthalpy, and entropy of the dissolution processes) were computed using the van't Hoff and Gibbs equations. The enthalpy-entropy relationship for 2,4-DNT was non-linear in the plot of enthalpy vs. Gibbs energy of solution with negative slope in the composition region 0.00 ≤ w1 ≤ 0.40 but positive slope in the region 0.40 ≤ w1 ≤ 1.00. Therefore, the driving mechanism for 2,4-DNT transfer processes is the entropy in water-rich mixtures and the enthalpy in ethanol-rich mixtures. In addition, by means of the inverse Kirkwood-Buff integrals is observed that 2,4-DNT is preferentially solvated by water molecules in water-rich mixtures but preferentially solvated by ethanol molecules in the mixtures of 0.23 ≤ x1 ≤ 1.00.