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Over the past few years, eutectic solvents (ESs) have drawn the scientific community's attention because they are usually more environmentally friendly than traditional organic solvents. One of the applications of ESs is in the gas capture field, where they are considered promising absorbers to replace amine- (MEA, DEA, or MDEA processes), methanol- (Rectisol process), dimethyl ethers of polyethylene glycol- (Selexol process), N-methyl-2-pyrrolidone- (Purisol process), propylene carbonate- (Fluor solvent process), or morpholine-based (Morphysorb process) solvents on CO2 capture from the atmosphere. Although several studies have reported experimental gas solubility data in ESs, especially for CO2, only a few existing options are covered. In fact, resorting to experimental methods to obtain the solubility data seems unfeasible considering the vast number of possible eutectic mixtures. Therewith, theoretical predictions of gas solubility in ESs are valuable for the fast pre-screening of prospective solvents. In this work, the ability of the thermodynamic model COSMO-RS to represent solubility data of CO2, CH4, and H2S in 17 choline chloride-based (ChCl) ESs was evaluated. The experimental data were collected from the literature at different molar ratios, at 298.15 K or 313.15 K, and in the pressure range from 1 to 125 bar. COSMO-RS offers a qualitative description of these gases' solubility, which was expected due to the model's fully predictive character. To improve the CO2 and CH4 solubility data description, a temperature–pressure-dependent correction was applied to the COSMO-RS predictions for these gases, offering a global average relative deviation of 15%. [ABSTRACT FROM AUTHOR]

In this research, a new Lewis acid-based deep eutectic solvent (LA-DES) was synthesized using diphenhydramine hydrochloride and CoCl2·6H2O, (2[HDPH]:CoCl42−), and identified by FT-IR and 1HNMR techniques. The physicochemical properties of this LA-DES, such as thermal behavior, thermal stability, and solubility in common solvents were also investigated. The catalytic ability of 2[HDPH]:CoCl42− was ascertained in the efficient synthesis of a novel array of thiadiazolo[2,3-b]quinazolin-6-one scaffolds via a one-pot three-component reaction of dimedone/1,3-cyclohexanedione, aldehydes, and 5-aryl-1,3,4-thiadiazol-2-amines/3-(5-amino-1,3,4-thiadiazol-2-yl)-2H-chromen-2-one under solvent-free conditions. This catalyst was also successfully utilized for the synthesis of mono- and bis-thiadiazolo[2,3-b]quinazolin-6-ones from dialdehydes or bis-1,3,4-thiadiazol-2-amine. The simplicity of enforcement, short reaction time, avoidance of toxic organic solvents, scalability of the synthesis procedure, excellent atom economy, high reaction mass efficiency, and low E-factor are other outstanding advantages of this newly developed method. Furthermore, due to the convenient recovery and reuse of LA-DES, this protocol is economically justified and environmentally friendly. [ABSTRACT FROM AUTHOR]

Methods are examined for estimating the Hildebrand solubility parameter of a mixture of organic solvents using the characteristics of their structural elements. A procedure is proposed for calculating the solubility parameter for mixtures of solvents differing in composition and structure depending on the ratio of their components. These results enable us to predict the optimal solvent mixture composition for polymers with a known Hildebrand solubility parameter. The proposed method permits us to estimate the solubility of complex mixtures of hydrocarbons of petroleum origin such as the tar obtained as the vacuum residue of oil distillation when it is used as a polymer solvent. 1H NMR analysis results were used to determine the structural elements of a tar and calculate its Hildebrand solubility parameter. [ABSTRACT FROM AUTHOR]

The cholesterol-functionalized polycarbonate-based diblock copolymer, PEG113-b-P(MTC-Chol)30, forms pathway-dependent nanostructures via dialysis-based solvent exchange. The initial organic solvent that dissolves or disperses the polymer dictates a self-assembly pathway. Depending upon the initial solvent, nanostructures of disk-like micelles, exhibiting asymmetric growth and hierarchical features, are accessible from a single amphiphilic precursor. Dioxane and tetrahydrofuran (THF) molecularly dissolve the block copolymer, but THF yields disks, while dioxane yields stacked disks after dialysis against water. Dimethylformamide and methanol display dispersed disks and then form stacked disk structures after dialysis. The path-dependent morphology was correlated to solubility parameters, an understanding of which offers routes to tailor self-assemblies with limited sets of building blocks. [ABSTRACT FROM AUTHOR]

Abraham model solute descriptors are determined for vanillin and five select derivatives (o-vanillin, isovanillin, vanillic acid, vanillyl alcohol and ethylvanillin) based on experimental solubility and partition coefficient data that we were able to find in the published literature. The solute descriptor values reported in the current communication back-calculate the observed experimental data to within standard errors of 0.12 log units (or less). The calculated solute descriptors can be used to predict the solubility of the vanillin and the five select derivatives in additional organic mono-solvents and binary aqueous-ethanol solvent mixtures using published Abraham model correlations. [ABSTRACT FROM AUTHOR]

In this research, we studied, in detail, the behavior of common PNIPAM microgels, obtained through surfactant-free precipitation polymerization, in a number of organic solvents. We showed that many of the selected solvents serve as good solvents for the PNIPAM microgels and that the size and architecture of the microgels depend on the solvent chosen. Expanding the range of solvents used for PNIPAM microgel incubation greatly enhances the possible routes for microparticle functionalization and modification, as well as the encapsulation of water-insoluble species. In this demonstration, we successfully encapsulated water-insoluble Sudan III dye in PNIPAM microgels and prepared the aqueous dispersions of such composite-colored microparticles. [ABSTRACT FROM AUTHOR]

AB-polybenzimidazole (ABPBI) dissolution kinetics in an eco-friendly complex acid-free solvent based on dimethyl sulfoxide (DMSO), methanol and KOH, and the rheological behavior of their solutions are investigated. The optimal component ratio of solvent providing the complete ABPBI dissolution is determined. Methanol containing dissolved KOH contributes to the creation of a single-phase superbasic medium, which accelerates and improves the polymer solubility in a mixture with DMSO, significantly reducing the viscoelasticity of the resulting solution. The optimum methanol content is up to 60 wt.% related to DMSO. The polymer dissolution rate increases by 5 times in this composition. It found the polymer concentration of 9% is close to the dissolution limit due to the strong solution structuring, which is probably associated with an increase in the amount of water released during the KOH-methanol-DMSO interactions. As a result, the conditions for obtaining high concentrated solutions in a complex, mainly organic solvent for fiber spinning are developed. The viscoelastic properties of solutions are measured in the concentration range of 1–9% at temperatures of 20–50 °C. The flow activation energy for 7 and 9% solutions decreases by 1.5 and 2.3 times, respectively, as the content of methanol in the complex solvent increases from 10 to 60%. [ABSTRACT FROM AUTHOR]

Organic solvents of different polarities (polar, semipolar, and nonpolar) are typically used in extraction studies on medical devices for chemical characterization of their constituents (called extractables or leachables, E/L) potentially exposed to patients during clinical uses per ISO 10993-18 (2020). This study evaluates the difference in solubility of semipolar solvents relative to ethanol for a wide range of E/L in hydrophobicity to help the selection of semipolar solvents for extraction studies. The solvents studied include methanol, ethanol, 1-propanol, 2-propanol (IPA), acetonitrile (ACN), acetone, dioxane, dimethylacetamide (DMA), dimethylformamide (DMF), dimethyl sulfoxide (DMSO), and ethylene glycol. A quantitative analysis of solubility difference (relative to ethanol) among these commonly used semipolar organic solvents over a wide hydrophobicity range based on Abraham general solvation model is presented. These semipolar solvents are also classified according to their solvation properties. The results of the calculation include a slope parameter with respect to hydrophobicity ( log 10 P O / W to describe the solubility ratio changes with an increase in E/L hydrophobicity, and an intercept parameter to describe the relative solubility for more polar E/L compounds. The calculation results are also corroborated by other solvent strength parameters. A recommendation on the rational selection of semipolar solvents in extraction studies is finally provided based on the two parameters, extraction type, and instrumental analysis. [ABSTRACT FROM AUTHOR]

• Solubility of isophthalic acid (IPA) in four different binary solvent systems was determined. • The experimental data was correlated with four thermodynamic models. • Molecular electrostatic potential surface (MEPS) and Hirshfeld surface (HS) analysis were used to investigate the intermolecular interactions. • The dissolution of isophthalic acid (IPA) was a non-spontaneous, endothermic and entropy-driven process. The solubility of isophthalic acid (IPA) in four different binary solvent systems (water + methanol, water + ethanol, water + 1-propanol, and water + isopropanol) was measured by the gravimetric method at atmospheric pressure from 283.15 K to 323.15 K. Under certain solvent compositions, the solubility of IPA increased with increasing temperature. The trend of solubility under isothermal conditions setting differs as the mole fraction of organic solvent increases. The solubility of IPA in water + methanol and water + ethanol systems increased with the mole fraction of methanol or ethanol. In the system of water + 1-propanol and water + isopropanol, as the mole fraction of organic solvent increased, the solubility of IPA increased firstly and then decreased gradually. The Hansen solubility parameters of IPA and selected solvents were analyzed, the analysis showed that the miscibility of IPA with the selected solvent was the result of many factors. Molecular electrostatic potential surface (MEPS) and Hirshfeld surface (HS) analysis were used to investigate the intermolecular interactions. The solubility data were correlated using the Apelblat equation, van't Hoff equation, λh equation, and Jouyban–Acree model. Besides, the vant Hoff equation was employed to analyze the apparent thermodynamic properties of dissolving process including the Gibbs energy, enthalpy and entropy. All positive values indicated that the dissolving process of IPA was non-spontaneous, endothermic, and entropy-driven. [ABSTRACT FROM AUTHOR]

• The order of cyclosporine solubility was DEGME > ethanol > NMP > 1-butanol > water. • Solubility increased with solvent mass fraction in binary solvent mixed with water. • The solubility was mainly affected by the self-cohesiveness of the solvent. • The solvent effects can be used as a basis of pharmaceutical co-solvent selection. In this study, the solid–liquid equilibrium solubility of cyclosporine in 20 pure solvents and four binary mixtures at 298.15 K were determined using shake-flask technique. Solid-state characterization exhibited that no solvate formation or polymorphic transformation occurred during the dissolution of cyclosporine in any of the solvent systems investigated. The experimental solubilities of cyclosporine in 20 pure mono solvents were ranked as follows: DEGME (2.21 × 10−1) > ethanol (1.22 × 10−1) > NMP (1.15 × 10−1) = 1-butanol (1.15 × 10−1) > dichloromethane (1.07 × 10−1) > acetonitrile (1.02 × 10−1) > PEG 200 (9.78 × 10−2) > PEG 300 (9.12 × 10−2) > chloroform (8.98 × 10−2) > PEG 400 (8.11 × 10−2) > DMF (7.65 × 10−2) > 2-propanol (7.09 × 10−2) > 1-propanol (6.57 × 10−2) > methanol (6.14 × 10−2) > propylene glycol (6.08 × 10−2) > tetrahydrofuran (4.69 × 10−2) > DMSO (2.64 × 10−2) > acetone (1.28 × 10−2) > glycerol (1.35 × 10−5) > water (4.29 × 10−7). In the four binary solvents (DEGME + water, PEG 200 + water, PEG 300 + water, and PEG 400 + water), the mole fraction solubility of cyclosporine increased with increasing mass fractions of the four different organic solvents. Based on the Kamlet-Taft linear solvation energy relationship (KAT-LSER) model, the solubility of cyclosporine was mainly affected by the self-cohesiveness of the solvent, which is related to the interaction between the solvent and the solvent. Additionally, the solubility parameter was used to explain and understand the solubility of cyclosporine in four different binary solvents. To correlate the solubility data of cyclosporine, two models (the Yalkowsky Log-Linear and simplified CNIBS/R–K models) were applied. The calculated data based on two mathematical models and experimental mole fraction solubility data for cyclosporine could provide information for the separation, extraction, purification, crystallization, and selection of suitable a solvent system. [ABSTRACT FROM AUTHOR]

Many active pharmaceutical ingredients (APIs) in the pharmaceutical pipeline require bioavailability enhancing formulations due to very low aqueous solubility. Although spray dried dispersions (SDDs) have demonstrated broad utility in enhancing the bioavailability of such APIs by trapping them in a high-energy amorphous form, many new chemical entities (NCEs) are poorly soluble not just in water, but in preferred organic spray drying solvents, e.g., methanol (MeOH) and acetone. Spraying poorly solvent soluble APIs from dilute solutions leads to low process throughput and small particles that challenge downstream processing. For APIs with basic pKa values, spray solvent solubility can be dramatically increased by using an acid to ionize the API. Specifically, we show that acetic acid can increase API solubility in MeOH:H2O by 10-fold for a weakly basic drug, gefitinib (GEF, pKa 7.2), by ionizing GEF to form the transient acetate salt. The acetic acid is removed during drying, resulting in a SDD of the original GEF free base having performance similar to SDDs sprayed from solvents without acetic acid. The increase in solvent solubility enables large scale manufacturing for these challenging APIs by significantly increasing the throughput and reducing the amount of solvent required. [ABSTRACT FROM AUTHOR]

This research provides a thorough investigation into the solubility behavior and solution thermodynamics of l-threonine in significant organic solvent systems. The work was done on measuring the actual solubility and subsequently calculating overall transfer solvation free energetics (∆ G energetic 0 i) and transfer entropies (∆ S t 0 i) at a temperature of 298.15 K. These measurements were performed as l-threonine transitioned from water to different water-organic mixed solvents systems. The saturated solubilities of l-threonine were determined using the 'gravimetric method' at five equidistant temperatures namely 288.15 K, 293.15 K, 298.15 K, 303.15 K and 308.15 K. By analyzing the data on solubility, we further obtained the different energies involved in solvation related issues. In the case of single solvents, the nature of solubility of l-threonine was observed like: dimethylsulfoxide (DMSO) < acetonitrile (ACN) < N, N -dimethylformamide (DMF) < ethylene glycol (EG) < water (H 2 O), irrespective of the experimental conditions. Specifically, at 298.15 K, the solubilities of l-threonine in single solvents were found to be as follows: 0.8220 mol per kg of water, 0.3101 mol per kg of EG, 0.1337 mol per kg of DMF, 0.1107 mol per kg DMSO and 0.1188 mol per kg of ACN. This research critically examines the relationship between the experimental saturated solubility of l-threonine and the complex properties influencing its solvation energy in diverse aqueous organic solvent systems. [Display omitted] • Solubility of l-threonine in various cosolvent systems and temperatures: EG-water > DMF-water > ACN-water > DMSO-water. • L-threonine's hydrophilic nature influences its solubility and interactions in water-EG/DMF/DMSO/ACN binary solvent systems. • Solvent molecule dimerization and their relative stabilities impact interactions, as seen in obtained values. • The study provides valuable insights for further scientific research in this area. [ABSTRACT FROM AUTHOR]

In this research, a new Lewis acid-based deep eutectic solvent (LA-DES) was synthesized using diphenhydramine hydrochloride and CoCl2·6H2O, (2[HDPH]:CoCl42−), and identified by FT-IR and 1HNMR techniques. The physicochemical properties of this LA-DES, such as thermal behavior, thermal stability, and solubility in common solvents were also investigated. The catalytic ability of 2[HDPH]:CoCl42− was ascertained in the efficient synthesis of a novel array of thiadiazolo[2,3-b]quinazolin-6-one scaffolds via a one-pot three-component reaction of dimedone/1,3-cyclohexanedione, aldehydes, and 5-aryl-1,3,4-thiadiazol-2-amines/3-(5-amino-1,3,4-thiadiazol-2-yl)-2H-chromen-2-one under solvent-free conditions. This catalyst was also successfully utilized for the synthesis of mono- and bis-thiadiazolo[2,3-b]quinazolin-6-ones from dialdehydes or bis-1,3,4-thiadiazol-2-amine. The simplicity of enforcement, short reaction time, avoidance of toxic organic solvents, scalability of the synthesis procedure, excellent atom economy, high reaction mass efficiency, and low E-factor are other outstanding advantages of this newly developed method. Furthermore, due to the convenient recovery and reuse of LA-DES, this protocol is economically justified and environmentally friendly. [ABSTRACT FROM AUTHOR]

Acetylated xylans have great potential in fabricating functional film and coating materials, which need a good solubility/dispersibility and film formability in an easily evaporable solvent. However, the changes of film formability with degree of substitution by acetyls (DS Ac) in different solvent systems for xylans have not been extensively studied, which limit the application of acetylated xylans in film materials. In this study, acetylated xylans with DS Ac of 0–2 were prepared and the effects of acetyl groups on solubility/dispersibility, crystallinity and film formability of xylans in water and chloroform solvent systems were investigated. Due to the change of polarity, xylans with DS Ac of 0–0.62 are only soluble in water solvents, while xylans with DS Ac of 1.13–2 are only soluble in chloroform/ethanol (70/30 v/v) organic solvents. We have found that the film formability of acetylated xylans is highly related to their solubility and crystallization. Film formable xylans all had good solubility in the cast solvents. However, although with good solubility, xylans with DS Ac of 0–0.3 and DS Ac of 1.76–2 cannot form intact films, which is due to the forming of xylan hydrate crystals and xylan diacetate crystals. With the increase of DS Ac , the mechanical property of xylan film increases initially at low DS Ac and decreases at high DS Ac. This study provides theoretical basis for applying xylans and their derivatives in advanced functional film and coating materials with great biocompatibility and biodegradability. [ABSTRACT FROM AUTHOR]

Acetylated xylans have great potential in fabricating functional film and coating materials, which need a good solubility/dispersibility and film formability in an easily evaporable solvent. However, the changes of film formability with degree of substitution by acetyls (DS Ac) in different solvent systems for xylans have not been extensively studied, which limit the application of acetylated xylans in film materials. In this study, acetylated xylans with DS Ac of 0–2 were prepared and the effects of acetyl groups on solubility/dispersibility, crystallinity and film formability of xylans in water and chloroform solvent systems were investigated. Due to the change of polarity, xylans with DS Ac of 0–0.62 are only soluble in water solvents, while xylans with DS Ac of 1.13–2 are only soluble in chloroform/ethanol (70/30 v/v) organic solvents. We have found that the film formability of acetylated xylans is highly related to their solubility and crystallization. Film formable xylans all had good solubility in the cast solvents. However, although with good solubility, xylans with DS Ac of 0–0.3 and DS Ac of 1.76–2 cannot form intact films, which is due to the forming of xylan hydrate crystals and xylan diacetate crystals. With the increase of DS Ac , the mechanical property of xylan film increases initially at low DS Ac and decreases at high DS Ac. This study provides theoretical basis for applying xylans and their derivatives in advanced functional film and coating materials with great biocompatibility and biodegradability. [ABSTRACT FROM AUTHOR]

[Display omitted] • 1,3-dioxolane, dimethyl carbonate and butyl acetate are suitable solvents for dissolving PHBV. • PHBV solubility increases by increasing temperature. • PHBV solubility decreases with increasing HV content. • PHBV solubility sphere based on Hansen's method is proposed. For the first time, a quantitative analysis of the solubility of poly-3hydroxybutyrrate-co-3hydroxyvalerate (PHBV) in green solvents is proposed. The solubility of two commercial co-polymers, with hydroxyvalerate (HV) contents of 8 %mol and 12 %mol, in 1,3-dioxolane, dimethyl carbonate and butyl acetate was experimentally determined using chloroform as the benchmark and water as the control. The results showed a direct correlation between solubility and temperature, with a maximum at the boiling point of the solvent. For PHBV with an HV content of 8 %mol, solubilities of 265 mg mL−1 for 1,3-dioxolane and dimethyl carbonate and 274 mg mL−1 for butyl acetate were measured; for PHBV with an HV content of 12 %mol, solubilities of 225 mg mL−1, 197 mg mL−1 and 137 mg mL−1 for 1,3-dioxolane, dimethyl carbonate and butyl acetate were measured, respectively. Following Hansen's theory, the PHBV solubility sphere was defined to predict the solubility of the co-polymers in solvents qualitatively. The validation of the sphere was performed by the experimental results herein obtained. [ABSTRACT FROM AUTHOR]

Using non‐halogenated solvents to process organic solar cells is preferable because they are less harmful to human health. However, it is challenging to mitigate the delicate trade‐offs between solubility and pre‐aggregation of organic semiconductors to maintain similar high device efficiencies as those processed by chlorinated solvents. The need for rigorous control of the kinetics between processing temperature and delay time inevitably complicates device processing for achieving reproducible performance. Herein, the authors develop a facile method to achieve proper solubility and pre‐aggregation in non‐halogenated solvents by selecting suitable donor/acceptor materials and subtle tuning of solvent compositions. This results in films with a high degree of ordering and suitably sized phase separation. Solar cells derived from this process can achieve a high power conversion efficiency up to 18%, which is the highest value reported for non‐halogenated solvent processed devices. This impressive result is achieved through synergistically reduced non‐radiative loss and enhanced charge generation. [ABSTRACT FROM AUTHOR]

Efforts to improve the TALSPEAK (Trivalent Actinide Lanthanide Separation with Phosphorus-Reagent Extraction from Aqueous Komplexes) Process have considered, among other options, the replacement of the organic solvent employed with a room-temperature ionic liquid (RTIL). The solubility of certain extractants in RTILs has been shown to be limited, however, calling into question their potential as replacement solvents. A systematic investigation of the solubility of bis(2-ethylhexyl)phosphoric acid (HDEHP) in a series of pyridinium- and imidazolium-based ionic liquids has therefore been undertaken, with the objective of relating the extractant solubility to structural characteristics of the RTIL. HDEHP solubility is shown to increase with solvent molar volume, with both larger IL cations and anions favoring dissolution. [ABSTRACT FROM AUTHOR]

[Display omitted] • Solubility and solvation thermodynamics of L-phenylalanine in aqueous-EG/DMF/DMSO/ACN were investigated. • Solvents parameters are calculated and used to explain solvation parameters. • Explained weak force interactions between solute and solvent, including cavity formation and solvent–solute interactions. • Transfer chemical transfer Gibbs energies and entropies were discussed. • L-phenylalanine solubility was shown in comparative way in complex solvent environments. This research elucidates comprehensive insights into the dissolution nature and solvation energetics of L-phenylalanine across distinct solvent environments. Specifically, the investigation encompasses saturated solubility measurements and the subsequent derivation of overall transfer free energies (Δ G t 0 (i)) and entropies (Δ S t 0 (i)) at 298.15 K, of L-phenylalanine from an aqueous medium to aqueous solutions comprising protic ethylene glycol (EG), dipolar aprotic N,N -dimethylformamide (DMF), acetonitrile (ACN), and dimethyl sulfoxide (DMSO). In this study the 'gravimetric method' was used to find the saturated solubilities of L-phenylalanine at five equidistant temperatures (288.15 K to 308.15 K). These experimental solubility measurements serve as the foundational dataset for the subsequent determination of transfer energies. The investigated drenched or equilibrium solubility data was applied to ascertain the solvation energies. In case of pure solvent, we get the solubility trend of L-phenylalanine as follows: ACN < DMSO < DMF < EG < water, at any temperature. At 298.15 K, we found the solubilities of L- phenylalanine in pure solvents like water, EG, DMF, DMSO and ACN are 0.1675, 0.0911, 0.0888, 0.0850 and 0.0811 mol·kg−1 respectively. A pivotal facet of this study involves the examination of the correlation between the saturated solubility of L-phenylalanine and the intricate characteristics of its solvation energetics across diverse aqueous organic solvent systems. [ABSTRACT FROM AUTHOR]

[Display omitted] • Diphenylsulfoxide is an amphiphilic homolog of DMSO featuring enhanced hydrophobicity. • Diphenylsulfoxide surprisingly exhibits outstanding solubility in methanol and high solubility in acetonitrile. • The strong diphenylsulfoxide-methanol hydrogen bonding is a prerequisite for high solubility. • The partial molar volume of diphenylsulfoxide in acetonitrile is larger than that in methanol. Diphenylsulfoxide (Ph 2 SO) represents a noteworthy organic substance composed of bulky amphiphilic molecules. The chemical interest in Ph 2 SO arises from a peculiar combination of the strongly polar and strongly nonpolar moieties which are uniquely packed. The solubility of Ph 2 SO in conventional organic solvents is a cornerstone of its prospective applications. In the present work, the full concentration ranges of the possible homogeneous solutions of diphenylsulfoxide (Ph 2 SO) in acetonitrile (ACN) and methanol (MEOH) have been investigated by densitometry, UV–vis, FTIR spectroscopy, and quantum-chemical calculations. For the first time, we unraveled an outstanding solubility of Ph 2 SO in MEOH. The homogeneous solutions form up to the molality of 0.9 mol kg−1. This observation is unexpected from the conventional chemical wisdom because Ph 2 SO contains twenty-two non-polar interaction sites vs. two polar interaction sites. Based on the volumetric measurements, we revealed that the partial molar volumes of Ph 2 SO depend somewhat on solvent (MEOH, ACN) peculiarities. The effects of solvent on the spectral characteristics of diphenylsulfoxide have been considered. The numerical simulations based on the systematic potential landscape exploration corroborate the existence of several types of supramolecular species involving Ph 2 SO and solvent molecules simultaneously. The peculiar anisotropic Ph 2 SO-MEOH coupling, which is a strong hydrogen bonding, along with the small size of the solvent molecules is responsible for the recorded outstanding solubility in the methanol media. In turn, the performance of ACN is somewhat less encouraging notwithstanding the way higher dipole moment of its molecules. As an amphiphilic solute, Ph 2 SO may boost the solubilities of hydrophobic solutes by interfacing its coupling with polar media. The reported results inspire further explorations of Ph 2 SO to design task-specific liquid systems. [ABSTRACT FROM AUTHOR]

• Equilibrium solubilities of GuHCl in different binary solvents were investigated. • The molecule interactions of solvent-solvent and solute-solvent were researched through molecular dynamics simulation. • Five thermodynamic models were utilized to regress the observed solubility data. • Dissolution thermodynamic properties were calculated. Solubilities of guanidine hydrochloride (GuHCl) in organic solvents are of great importance for its development and optimization of industrial process. The study of the dissolution characteristics of GuHCl in DMF/2-meoxyethanol/methanol/NMP + n -propanol at different temperatures were experimentally investigated by using laser monitoring method. Results showed that GuHCl solubilities were observed to be increasing with the increment in experimental temperature and rising with higher mass fraction of DMF/2-meoxyethanol/methanol/NMP. Molecular dynamics (MD) simulation technique was utilized to reveal the microscopic behaviors of GuHCl and solvent mixtures and its effect on the dissolving capability of GuHCl in involved solvent systems. Also, five thermodynamic models were selected to regress the observed GuHCl equilibrium solubility. A comparison of the experimental values with corresponding estimated data indicated that the modified Apelblat equation provided the most excellent correlation in modelling GuHCl solubility. Finally, through the analyses of enthalpy change, entropy change and Gibbs free energy change, the dissolution thermodynamic features were evaluated. [ABSTRACT FROM AUTHOR]

• Solubility of CDON in twelve organic solvents was determined. • The dissolution order of CDON was analyzed by solvent effect. • Experimental solubility data were correlated with five thermodynamic models. • CDON dissolution was observed to be endothermic and entropy-driven. The solubility of cyclododecanone (CDON) was determined in twelve solvents containing acetonitrile, acetone, toluene, ethyl acetate, cyclohexane, 1,2-dichloroethane, methanol, ethanol, n -propanol, i -propanol, n -butanol and i -butanol. The temperature range for the remaining solvents used in the experiment was 278.15–313.15 K, except for cyclohexane (283.15–313.15 K). The CDON solubility in solvents measured increased with growing temperature. The CDON solubility varies considerably in different solvents. Among the single solvents selected, CDON was most soluble in 1,2-dichloroethane and least in acetonitrile. The solubility in 1,2-dichloroethane is about 2–3 times higher than in acetonitrile. The carbonyl oxygen of CDON readily combines with alcoholic solvents to form hydrogen bonds. Hansen solubility parameters (HSP) and the physiochemical properties of the solvents explain the solvent effect in diverse solvents. To understand CDON dissolution, the electrostatic potential energy surfaces of CDON and the solute–solvent interactions were analyzed at the molecular level on the basis of density functional theory (DFT). Analysis of solvation effects revealed that variations in the CDON dissolution are influenced by a combination of factors rather than a single one. In addition, the Van't Hoff equation, modified Apelblat equation, Yaws equation, λh equation, Wilson model and Jouyban model were utilized to correlate the experimentally obtained value. The computational data show that the ARD (0.88%) and RMSD (0.24%) of Wilson model are the smallest among the selected equations with the best correlation. The apparent thermodynamic properties of CDON dissolution were further accounted for Van't Hoff equation, and the CDON dissolution was observed to be endothermic and entropy-driven. [ABSTRACT FROM AUTHOR]

This study compares the solubility predictions of the Flory-Huggins based on the Hansen Solubility Parameters (FH-HSP) model with those of openCOSMO-RS and PC-SAFT for evaluating the screening capabilities of the Hansen solubility parameters (HSP) using the relative energy difference (RED). Two deep eutectic solvents, thymol + L-menthol (TM) and thymol + cyclohexanone (TC), and their precursors were investigated. The three models performed reasonably well in predicting the solubility of thymol and L-menthol in organic solvents but showed significant deviations in predicting the solubility of solid solutes in cyclohexanone. For solubility predictions in DES compared to available experimental data, the root-mean-square logarithmic deviation (RMSLD) values obtained with FH-HSP, openCOSMO-RS, and PC-SAFT were 0.86, 0.27, and 0.93, respectively. Using FH-HSP with HSP obtained from an ideal mixing rule of the parameters of pure compounds resulted in a deviation of 1.13. The screening assessment of the studied DES revealed a 70.4% match rate between the RED parameter and ln ⁡ γ i ∞ , with 6.9% false negatives. Using HSP obtained from the ideal mixing rule resulted in similar scores, with a 68.5% match rate and 10.4% false negatives. The results suggest that the HSP theory can aid DES screening processes by identifying promising DES-solute pairs, thus allowing the targeting of more robust methods of computational resources in smaller sets of compounds. • Experimentally calculated Hansen solubility parameters are able to capture solute-DES interactions tendency. • Hansen solubility parameters allow screening solute-DES interactions using the relative energy difference parameter. • Solubility calculations using Flory-Huggins and Hansen solubility parameters are not recommended if high accuracy is needed. [ABSTRACT FROM AUTHOR]

[Display omitted] • The solubility of 2-amino-6-chloropyrazine in different solvents were determined. • The solubility data were calculated by different thermodynamic models. • Apparent thermodynamic properties were obtained by van't Hoff plots. • Preferential solvation of 2-amino-6-chloropyrazine was investigated by IKBI method. • The solvent effect of 2-amino-6-chloropyrazine was analyzed by KAT-LSER model. Equilibrium solubility of 2-amino-6-chloropyrazine in ten pure solvents (methanol, ethanol, n -propanol, isopropanol, N,N -Dimethylformamide (DMF), acetonitrile, acetone, propylene glycol (PG), ethylene glycol (EG) and water) and four binary blends of ethanol/ n -propanol/PG/DMF plus water was experimentally measured by isothermal saturation method at 278.15 K to 323.15 K under p = 101.2 kPa. The maximum mole fraction of 2-amino-6-chloropyrazine in mono-solvents was obtained in neat acetone (5.053 × 10-2) at 323.15 K. For four binary mixed systems, the amount of 2-amino-6-chloropyrazine dissolved in DMF + water was more than other three systems. For pure solvent systems, the temperature was the only factor that affected the dissolution of 2-amino-6-chloropyrazine, while temperature and solvent composition were both the factors that affected the dissolution of 2-amino-6-chloropyrazine. The solubility data of 2-amino-6-chloropyrazine in pure solvents was correlated with apelblat model, van't Hoff model and Buchowski–Książczak λh model. The Jouyban-Acree model, Apelblat-Jouyban-Acree model and van't Hoff-Jouyban-Acree model were applied to calculate the solubility data of 2-amino-6-chloropyrazine in mixtures. The van't Hoff plots of the solubility of 2-amino-6-chloropyrazine was adopted as a method to show the relationship between ln × and 1 /T- 1 /T hm , which was the basis for calculating thermodynamic properties. The preferential solvation performance in mixed systems was estimated by the values of δx 1,3 , in 0.19 < x n-propanol/PG/DMF < 1 and 0.23 < x ethanol < 1, the 2-amino-6-chloropyrazine was preferentially dissolved in organic solvents. In contrast, the 2-amino-6-chloropyrazine was dissolved preferentially in water in other intervals. What's more, the solvent effect of 2-amino-6-chloropyrazine in mixed systems was obtained, the hydrogen bond interaction was the only factor that affects dissolution in alcohols + water and the solvent–solvent molecular interaction was dominant in DMF + water. [ABSTRACT FROM AUTHOR]

The emulsifiable concentrates containing harmful organic solvents such as benzene, toluene, xylene, etc. could pose potential risks to the ecological environment and human health due to their lowflash points, easy volatility, and high toxicity. This paper reviewed the usage of organic solvents inpesticide emulsifiable concentrates, highlighted their potential hazards, and introduced the research progress of organic solvents substitution by bio-based solvents, mineral-based solvents, and artificially synthetic solvents. These eco-friendly alternative solvents with low toxicity showed good potential in the application of emulsifiable concentrates. However, the selection of alternative solvents through experiments was time-consuming and labor-intensive. The application of COSMO-RS thermodynamic model wasbased on the theoretical prediction of pesticide solubility in alternative solvents, and was verified by experiments in the laboratory. It could accelerate the screening of alternative solvents with less timeand materials, which is helpful to the development of eco-friendly emulsifiable concentrates. [ABSTRACT FROM AUTHOR]

Understanding solubility behavior of organic crystalline materials is critical in the development of slurry-formulated plastic bonded composites. In the field of high explosives (HE), a common method for obtaining high density, greater than 95% theoretical maximum density, is to encapsulate HE in a polymer matrix resulting in the formation of plastic bonded explosive (PBX) prills which can then be pressed to high density parts. Prill formation is highly nuanced and requires understanding of particle size distributions, solvent, antisolvent, and binder system as well as interactions thereof. In an effort to create mock-HE that mimics HE in density and mechanical strength, solubility of candidate molecules was compared to cyclotetramethylenetetranitramine (HMX) in binder solvents relevant to prill formation. The results indicate that the mock candidates chosen for this study have different solubilities compared to HMX in water and both organic solvents, 2-butanone and ethyl acetate, investigated. With these solubility differences known, prills to match PBXs based on HMX can be formulated, pressed and tested. [ABSTRACT FROM AUTHOR]

The solubility behavior and solution chemistry of CL-20/MTNP (2,4,6,8,10,12-hexanitro-hexaaza-isowurtzitane/1-methyl-3,4,5-trinitropyrazole) energetic cocrystals in organic solvents were first investigated to offer some important information on thermodynamics. The phase solubility diagram (PSD) and eutectic point (Keu1) of three solvents were also determined. Moreover, the solubility behavior of CL-20/MTNP energetic cocrystals was explained using the solubility product and solution complexation theories. The solution complexation results indicated that the CL-20/MTNP cocrystal has the strongest complexation effect in ethanol. The Keu1 values were all below 1 in three studied solvents, suggesting that the CL-20/MTNP cocrystal was less soluble than the other two pure components. Furthermore, studying the solubility behavior and solution chemistry of the CL-20/MTNP cocrystals has provided further insights into the screening, preparation and scaling-up of energetic cocrystals. [ABSTRACT FROM AUTHOR]

• Musk xylene in ten organic solvents at temperatures ranging from 278.15 K to 313.15 K was measured. • Analysis of musk xylene by XRD. • Wilson model, NRTL model, Vant't Hoff equation, modified Apelblat equation, and λh equation are used to correlate the solubility of musk xylene in different solvents. • The mixed Gibbs energy, enthalpy and entropy were calculated according to Wilson model. In this study, isothermal saturation method was used to measure and correlate the solubility of musk xylene in ten organic solvents at temperatures ranging from 278.15 K to 313.15 K , including methanol, ethanol, isopropanol, n-butanol, cyclohexane, n-hexane, n-heptane, N,N-dimethylacetamide, ethyl acetate, tetrahydrofuran. The experimental results show that the solubility of musk xylene in the selected solvent increases with increasing temperature. The experimental data were correlated by five thermodynamic models, and the results showed that each model can give a satisfactory correlation. In addition, the three kinds of mixed thermodynamic properties of Gibbs energy, enthalpy and entropy of musk xylene in selected solvents were determined by solubility data and Wilson model. It can be seen that the dissolution of musk xylene in a given solvent is spontaneous and entropy driven. Exploring the solubility of musk xylene in different organic solvents and the thermodynamics of dissolution can not only provide basic data for industrial crystallization separation, but also have great significance for its own crystallization and theoretical research. [ABSTRACT FROM AUTHOR]

• Novel modeling approach utilizing the Pitzer model and the EOS ePC-SAFT advanced. • Pitzer model provided very accurate T-dependent osmotic coefficients and KSP. • ePC-SAFT advanced as robust modeling framework to model SLE in organic solvents. • Approach enabled modeling the T-dependent solubility of CSCL in organic solvents. • Hypothetical KSP enabled modeling the solubility of carbonates in organic solvents. The temperature-dependent solubility of salts in organic solvents is of particular interest in nearly water-free multi-component systems, such as chemical reactions at extreme conditions, e.g., carboxylation reactions or Suzuki-Miyaura reactions. In this work, a novel modeling approach is proposed, which utilizes the correlative Pitzer model and the equation of state ePC-SAFT advanced to model the temperature-dependent solubility of salts in organic solvents. The proposed approach was applied to model the temperature-dependent solubility of CsCl in the organic solvents methanol, ethanol, and N -methyl-2-pyrrolidone (NMP) over a temperature range from T = 273.15 K to T = 333.15 K. The Pitzer model was used to correlate accurately temperature-dependent osmotic coefficients (OC). Pitzer was then used to determine ePC-SAFT binary interaction parameters and to determine the thermodynamic solubility product K SP of the salts over the temperature. Missing OC data were measured in this work using vapor-pressure osmometer for Na 2 CO 3 and Cs 2 CO 3. The resulting K SP values do not depend on the solvent, and they were used as an input into ePC-SAFT to model the temperature-dependent solubility of salts in organic solvents. Excellent agreement was achieved for CsCl, and the approach was then transferred to carbonate salts (Na 2 CO 3 and K 2 CO 3), which form multiple hydrates with water. Hypothetical K SP values of the anhydrous form were determined via the van 't Hoff equation and successfully allowed modeling of the solubility of (anhydrous) Na 2 CO 3 and K 2 CO 3 in methanol, ethanol, and NMP. To conclude, a combination of accurate K SP values together with a robust thermodynamic model, such as ePC-SAFT advanced, can help to reduce the experimental burden in screening the solubility of salts in organic solvents over the temperature. [Display omitted] [ABSTRACT FROM AUTHOR]

• Solubility data of 1,4-cyclohexanedione in ten pure solvents were measured. • Experimental data were correlated by five thermodynamic models. • Dissolution mechanism of 1,4-cyclohexanedione in ten pure solvents was investigated. • Thermodynamic properties were discussed by Wilson model. As an important raw material in industrial production, the solubility studies of 1,4-cyclohexanedione (14CHD) in organic solvents may be of assistance in improving crystallization efficiency and yield in industry. Therefore, this work deeply explored the dissolution behavior of 14CHD by using the isothermal saturation method, model fitting and density functional theory (DFT) calculation. Firstly, we selected ten pure organic solvents that are environmentally friendly to measure the solubility of 14CHD at the temperature range of 278.15 ∼ 313.15 K under standard atmospheric pressure. According to the measurement results, the solubility of 14CHD increases with temperature, and there are some differences among the solubility of 14CHD in various solvents. For instance, it has a highest solubility in acetonitrile (x 1 = 0.5331) at 313.15 K while has the lowest solubility (x 1 = 6.757 × 10-4) in cyclohexane at 283.15 K. Whereafter, the measured solubility data was correlated by Van't Hoff equation, modified Apelblat equation, λh model, Yaws model and Wilson model. Among them, Yaws model represents the most accurate fitting outcomes. At the same time, the study results of mixing thermodynamic properties on the basis of Wilson model suggest that the dissolution processes of 14CHD in ten organic solvents are entropy-driven and spontaneous. Afterwards, in order to explain the large difference in solubility of 14CHD in ten organic solvents, we found that the dissolution of 14CHD depends mostly on the polarity (π) and cohesive energy density (CED), viewed from the physicochemical factors of solvents. Furthermore, we further studied intermolecular interactions between 14CHD and ten solvents through molecular electrostatic potential surface (MEPS) analysis and DFT methods. Results display that alcoholic and non-alcoholic solvents molecules have different sites of action with 14CHD and the absolute values orders of interaction energies of alcoholic and non-alcoholic solvents are all consistent with corresponding solubility laws. The solvent–solute interaction plays an important role in the solubilities of 14CHD. [ABSTRACT FROM AUTHOR]

[Display omitted] • COSMO-RS parameters are optimized based on solvent classification by σ-profile analysis. • The model predictions are evaluated by 1173 acetylene solubility data in pure and mixed solvents. • The model is available over a wide range of temperatures and pressures. • Acetylene-based liquid-phase synthesis of N-vinylpyrrolidone is designed preliminarily with the predicted solubility. Acetylene has been used directly to synthesize various vinyl compounds. To avoid the explosion risk of gas-phase acetylene during the reaction, it is more reliable to dissolve acetylene in the solvent(s) first, and then make it react in the liquid phase. Accordingly, the solubility of acetylene is the most essential information for the solvent selection and the reaction process design. This work makes efforts to accurately predict the acetylene solubility in many organic solvents over a wide range of temperatures and pressures by optimizing two parameters in COSMO-RS based on solvent classification by σ-profile analysis. The model predictions are evaluated by 1173 solubility data of acetylene and the average absolute relative deviation is 13.0%. This established theoretical method provides a large number of solubility data of acetylene for reference to guide the liquid-phase reaction process design, where the synthesis of N-vinylpyrrolidone is chosen as a case illustration. [ABSTRACT FROM AUTHOR]

A Russia vacuum residue (RVR) was ultrasonically extracted with 15 organic solvents, respectively. The soluble fractions (SFs) were analyzed with a gas chromatography/mass spectrometer (GC/MS). The results show that the extract yields of RVR largely increased with the decrease in the dielectric constant of solvents, i.e., RVR tends to dissolve in weakly polar and non-polar solvents. Most of GC/MS-detectable components in the SFs are chain alkanes and cyclanes. [ABSTRACT FROM AUTHOR]

Ion solvation extraction using ethers and ketones is industrially applied for the extraction and separation of Au(III) from acidic chloride media. Although these have been in practical use since the 1970s, requirements for valid extractants (solvents) have not been systematically clarified. In this study, the relationship between Au(III) extractability using various organic solvents and their Hansen solubility parameters (HSPs) was investigated. The extractability of the solvents increases with the increase of the polar forces (δ P) of the solvents, however, solvents with much higher δ P values are water-miscible and unsuitable for solvent extraction. Hence a HSP sphere with center coordinates at δ D = 17.73, δ P = 7.82, δ H = 2.48, where D, P and H represent dispersive, polar and hydrogen-bonding forces, was obtained from the results of extraction tests using 26 solvents, with the exclusion of HSPs for 25 water-miscible solvents. Twenty-four of the 26 solvents tested were properly classified as valid or invalid for the extraction of Au(III) using the Hansen sphere. The results suggest partial utility of the prediction of the extractability using HSPs. Dicyclohexylketone, which has HSPs within the sphere, was selected as a potential extractant: it showed sufficient extractability and selectivity for the extraction of Au(III). • Relationship between Au(III) extractability and solubility parameters was studied. • Dicyclohexylketone was selected as a potential extractant for Au(III). • Hansen solubility parameters are a useful tool to predict extractant behavior. [ABSTRACT FROM AUTHOR]

The solubility of florfenicol form A in eight pure organic solvents (propionic acid, ethanol, 1-propanol, 1-butanol, 2-propanol, 2-methyl-1-propanol, 3-methyl-1-butanol, and 2-ethyl-1-hexanol) and three binary solvents (dimethyl sulfoxide + ethanol, dimethyl sulfoxide + 1-propanol, and dimethyl sulfoxide + 1-butanol) was measured by a laser dynamic method at temperature from 283.15 to 323.15 K. The experimental results show that the mole fraction solubility of florfenicol in the pure solvents decreased according to the following order: ethanol > 1-propanol > 2-propanol > 1-butanol > 3-methyl-1-butanol > 2-methyl-1-propanol ≈ propionic acid > 2-ethyl-1-hexanol. The experimental results show that the mole fraction solubility of florfenicol form A in the binary solvents increased with the increase of temperature and dimethyl sulfoxide mass fraction. The experimental solubility data were well correlated with the four thermodynamic models: modified Apelblat equation, Λh equation, NRTL model equation, and Wilson model equation. The modified Apelblat model equation was regarded as the best one to fit the experimental values in the pure solvents. [ABSTRACT FROM AUTHOR]

Abraham model solute descriptors are determined for 4-nitropyrazole based on published solubility data for 4-nitropyrazole dissolved in binary aqueous-methanol and aqueous-ethanol solvent mixtures at 298.15 K. The calculated solute descriptors enable the solubility of 4-nitropyrazole to be estimated in more than 80 different organic solvents. Also calculated from the published solubility data are the preferential solvation parameters, obtained from the inverse Kirkwood–Buff integrals, for describing the solvent distribution around the dissolved 4-nitropyrazole solute molecule. [ABSTRACT FROM AUTHOR]

Solubility measurements were performed for the systems (11β)-11,17,21-trihydroxypregna-1,4-diene-3,20-dione (prednisolone) and (11β)-11,17,21-trihydroxypregn-4-ene-3,20-dione (hydrocortisone) in 10 solvents at atmospheric pressure within the temperature range, T = (293.2 to 328.2) K by employing combined digital thermal analysis and thermal gravimetric analysis (DTA/TGA) to determine liquid phase compositions at saturation. The maximum solubility for prednisolone and hydrocortisone was in N , N dimethylformamide at 328.2 K with x 1 = 0.0141 and x 1 = 0.0142 respectively. The lowest solubility was found to be prednisolone and hydrocortisone in water at 293.2 K with x 1 = 0.0000105 and x 1 = 0.0000115 respectively. The composition data was modelled using the Tsuboka-Katayma modified Wilson and NRTL activity coefficient models. There is satisfactory agreement between the experimental results and the models chosen. Furthermore, melting points and enthalpies of fusion of prednisolone and hydrocortisone were determined by combined DTA/TGA. The enthalpy of fusion and melting point of prednisolone and hydrocortisone was found to be 36,145 J·mol − 1 and 514.5 K and 33,900 J·mol − 1 and 486.1 K respectively. [ABSTRACT FROM AUTHOR]

[Display omitted] • Solubility of 2-aminoterephthalic acid is measured in 8 monohydroxy alcoholic solvents. • Van't Hoff and Buchowski model satisfactorily describe the data. • The KAT-LSER model was used to explore the solvation effect. • Dissolution entropy and enthalpy show a volcano-type relation with solvent boiling point. This research experimentally measured the solubility of 2-aminoterephthalic acid in eight pure alcoholic solvents – methanol, ethanol, 1-propanol, 1-butanol, 2-propanol, 2-butanol, 2-methyl-2-propanol, and 3-methyl-1-butanol – from 303.15 to 338.15 K at normal pressure p = 0.1 MPa by the excess solid method. The measured solubility of 2-aminoterephthalic acid in these pure organic solvents was found to increase with the rise of temperature in the following order: 3-methyl-1-butanol (lowest solubility) < 1-butanol < 2-butanol < 1-propanol < 2-methyl-2-propanol ≈ 2-propanol < ethanol < methanol (highest solubility). The experimental solubility was correlated by the Van't Hoff equation and the λh (Buchowski) equation. The apparent thermodynamic properties (Δ0G sol , Δ0H sol and Δ0S sol) were calculated by the Van't Hoff equation, from which it was concluded that the dissolution process is entropy-motivated and endothermal. In addition, the solvent effects on 2-aminoterephthalic acid solubility were studied by the KAT-LSER model, where the results showed that the polarizability accounts for 47.9 ± 4.2 % of the total solvent effect. A volcano-type relation between the dissolution entropy and enthalpy versus the solvent boiling point is reported, showing maximal values of 55.3 J mol−1 K−1 and 29.2 kJ mol−1, respectively, for intermediate molecular interactions of solute and solvent. [ABSTRACT FROM AUTHOR]

The knowledge of solubility and solution thermodynamics for 2-methyl-4-nitroaniline in different solvents is essential for its purification and further theoretical studies. In this work, the solid-liquid equilibrium for 2-methyl-4-nitroaniline in eleven pure organic solvents (methanol, ethanol, n -propanol, isopropanol, n -butanol, toluene, ethyl acetate, acetonitrile, 2-butanone, acetone and cyclohexane) was established with the isothermal saturation method at temperatures T = (278.15–313.15) K under pressure of 101.2 kPa, and the solubility of 2-methyl-4-nitroaniline in these solvents were determined by a high-performance liquid chromatography (HPLC). In general, the mole fraction solubility obeyed the following order from high to low in different solvents: 2-butanone > acetone > ethyl acetate > acetonitrile > methanol > ethanol > n -propanol > n -butanol > isopropanol > toluene > cyclohexane. The modified Apelblat equation, λh equation, Wilson model and NRTL model were employed to correlate the measured solubility values of 2-methyl-4-nitroaniline in the selected solvents. Results show that the largest values of RAD and RMSD obtained with the four models are no greater than 0.71% and 3.27 × 10 −4 , respectively. The modified Apelblat equation provided better results than the other three models. Furthermore, the mixing properties, including Gibbs energy, mixing enthalpy, mixing entropy, activity coefficient at infinitesimal concentration ( γ 1 ∞ ) and reduced excess enthalpy ( H 1 E, ∞ ) were computed. The dissolution process of 2-methyl-4-nitroaniline is spontaneous and favourable in the selected solvents. The solubility and associated models would be very useful for optimizing the separation process of the isomeric mixtures of 2-methyl-4-nitroaniline and 2-methyl-6-nitroaniline. [ABSTRACT FROM AUTHOR]

Several errors and shortcomings in the paper by Liu et al. (J. Solution Chem. 45:932-946, 2016) concerning the calculation of Abraham model solution descriptors of telmisartan are discussed. The authors' calculated solute descriptors give an unreasonable value for the water to 1-octanol partition coefficient of telmisartan, which is eight orders of magnitude smaller than values predicted by other methods. The correct computation methodology for determining solute descriptors from experimental solubility data is presented. [ABSTRACT FROM AUTHOR]

[Display omitted] • The solubility of Amphotericin B drug in six organic solvents is reported. • Empirical thermodynamic models for interpolating solubility are provided. • Solid form is characterized by PXRD, DSC, TGA, RP-HPLC, SEM, FTIR, UV–vis and Raman. • No signs of solute aggregation in equilibrated solutions is evidenced. • Negative activity coefficients related to positive solute interactions are at play. The solubility of amphotericin B (AmB) has been studied between temperatures of 298–343 K in a range of pure organic solvents including methanol, ethanol, isopropanol, butanol, acetone, tetrahydrofuran, and 1,4-dioxane. The initial solid form used in solubility determinations has been characterized by a series of techniques including powder X-ray diffraction (PXRD), scanning electron microscopy (SEM), Fourier transform infrared (FTIR) and Raman spectroscopy, thermogravimetric analysis and differential scanning calorimetry. Pure AmB melts at 444.5 K with an associated enthalpy of fusion of 177.2 kJ/mol. The equilibrated solids in suspension have been characterized by SEM and PXRD and additionally, the equilibrated saturated solutions have been characterized by in-situ UV–vis to probe the saturation and the aggregation state of AmB. In the explored solvents, in terms of mass ratio, the solubility has been found to be remarkably low, decreasing in the order: ethanol > tetrahydrofuran > butanol ≃ 1,4-dioxane ≃ isopropanol > acetone. The relative order of solubility obtained in the alcohols correlates well with their polarity, revealing important interactions of the solvents' hydroxyl group with the polyol chain and the micosamine sugar carboxylic moiety of amphotericin B. Except in dioxane and isopropanol, the obtained Van't Hoff enthalpies of solution reveal an inverse proportionality to the experimental molar fraction solubility values obtained experimentally, indicating a larger energy requirement to solvate AmB molecules. Aggregation of AmB in the equilibrated solutions was not detected in any of the solvents studied yet HPLC analyses revealed that the API degraded in methanol during the equilibration time for the solubility determinations. [ABSTRACT FROM AUTHOR]

• The solubility of NVP was determined in eleven pure solvents and three binary solvents. • Five models were used to correlate the experimental solubility. • Combine solute structure and solvent effect for analysis. • KAT-LSER model was employed to investigate the solute–solvent interactions. Nevirapine (NVP) is the first non-nucleoside reverse transcriptase inhibitor drug to be marketed for the treatment of HIV. The solubility of NVP under atmospheric pressure in eleven pure solvents and three mixtures was measured from 278.15 to 323.15 K. XRD and DSC were used to detect the crystal form and stability of NVP in this work. Overall, the solubility of NVP gradually increases as the temperature rises. In addition, under the same temperature conditions, the solubility of NVP increases with the ratio of the positive solvents in binary solvents. In the mixture (DMF + acetonitrile), when the proportion of DMF reaches 0.8, the solubility in the binary solvent is greater than that in pure DMF. The experimental data was fitted by five thermodynamic models (Buchowski-Ksiazaczak λh model, the Modified Apelblat model, Jouyban-Acree model, SUN model, and CNIBS/R-K model). Subsequently, the largest mean square deviation value (RMSD) is only 2.31E-04, which demonstrates that the correlation of the solubility data and the five models is relatively good. Additionally, KAT-LSER model was used to explore the effects of solute–solvent interactions on solubility at 298.15 K. The analysis results indicated that the dipolarity/polarizability ( π ∗ ) of pure solvents plays a crucial role in the dissolution of NVP and its proportion of the total solvent effect reaches 30.92 %. This research was explored and developed the important systems (1-propyl alcohol and DMF + acetonitrile) for the industrial crystallization purification of NVP. [ABSTRACT FROM AUTHOR]

• An isothermal saturation method was used to measure the solubility of BPS. • Three mathematical models were used to correlate the experimental solubility data. • The thermodynamic properties were calculated. The equilibrium solubility of 4,4′-dihydroxydiphenylsulfone (BPS) in ten neat organic solvents, including methanol, 2-butanol, acetonitrile, 2-butanone, cyclohexanone, formamide, N, N -dimethylformamide, ethyl formate, isopropyl acetate, and dimethyl carbonate at temperatures from 278.15 to 313.15 K under atmospheric pressure (101.3 × 10 3 Pa) was studied using an isothermal saturation method. In all studied solvents, the solubility of BPS increased with the increase in temperature. Three solubility fitting models, including the van't Hoff equation, modified Apelblat equation, and λh equation, were used to correlate the experimental solubility data. The maximum magnitudes of the relative average deviation (RAD%) and root mean square deviation (RMSD) were 5.27 % and 9.45 × 10-3. Generally, the magnitudes of the RAD% generated by the modified Apelblat equation were the smallest among the selected solubility fitting models. The thermodynamic properties of BPS, such as the apparent standard dissolution enthalpy (Δ H sol o), standard dissolution Gibbs energy (Δ G sol o), and standard dissolution entropy change (Δ S sol o), were calculated. The Δ H sol o is positive in all studied cases, indicating that the dissolution process of BPS is endothermic. The obtained solubility data and relevant thermodynamic studies have an important guiding significance for optimizing the crystallization and purification process of BPS. [ABSTRACT FROM AUTHOR]

Solubilities of CO2 have been measured in five low volatile organic solvents at temperatures ranging from 293.15 to 323.15 K with 10K intervals under a pressure of 0 to 600.0 kPa using an isochoric saturation method. These organic solvents were selected from γ-butyrolactone (GBL), butyl lactate (BL), 1,1,3,3-tetramethylurea (TMU), 1,3-dimethyl-2-imidazolidinone (DMI), and 1,3-dimethyl-3,4,5,6-tetrahydro-2(1H)-pyrimidinone (DMPU). Henry's constants and thermodynamic properties such as Gibbs free energy, enthalpy, and entropy of dissolution were derived from the corresponding solubility data. The gravimetric solubilities of CO2 in these solvents followed the sequence of TMU < DMI ≈ BL ≈ GBL < DMPU. The enthalpies of dissolution were all exothermal at each condition. Henry's constants of CO2 in these solvents were further compared with those in ionic liquids and other ordinary absorbents, and it was found that they were similar to that of CO2 in polyethylene glycol dimethyl ether (NHD), which is widely used in the present industry. [ABSTRACT FROM AUTHOR]

• The solubility data of palbociclib was measured in fourteen pure solvents. • The experimental values were determined using a laser monitoring method. • Solubility order was analysed by using the Hansen solubility parameter. • Enthalpy, entropy and Gibb energy of dissolution and mixing process were calculated and discussed well. The solubility of palbociclib in fourteen organic solvents (chlorobenzene (MCB), N,N-dimethylformamide (DMF), pyridine (Py), anisole (An), ethyl acetate (EA), dimethyl sulfoxide (DMSO), tetrahydrofuran (THF), acetone (DMK), water, toluene (PhMe), methanol (MeOH), o -xylene (OX), ethanol (EtOH) and m -xylene (MX)) was determined using a laser monitoring method at atmospheric pressure in this work. The measured temperature range for all selected solvents is 293.15 K to 333.15 K. The holistic solubility profile showed that palbociclib solubility in all measured solvents was proportional to the increasing of test temperature. It was also found that the mole-fraction solubility values of palbociclib in measured solvents exhibited a sequence of: Py > THF > DMSO > DMF > DMK > PhMe > MCB > MX > OX > EtOH > EA > An > MeOH > water. Four mathematical equations were employed to correlate the solubility data including the modified Apelblat equation, λh equation, NRTL equation and Wilson equation, with the modified Apelblat equation giving the best regression. Solubility order of palbociclib in fourteen solvents was analyzed by using the Hansen solubility parameter (HSP) and the solvent effect (solvent interaction) was investigated through correlating palbociclib solubility in selected solvents based on KAT-LSER model. Finally, the thermodynamic properties of Δ mix G , Δ mix H , Δ mix S , Δ dis H , Δ dis G and Δ dis S of palbociclib in different solvents were computed based on measured solubility values and Wilson equation. The results demonstrated that the dissolution process was entropy-driven and favorable process. [ABSTRACT FROM AUTHOR]

Dataon corresponding solid–liquid equilibria of sulfanilicacid in different organic solvents are essential for industrial designand further theoretical studies. In this study, the solubilities ofsulfanilic acid were measured in methanol, ethanol, 2-propanol, acetone,acetonitrile, formic acid, and acetic acid with the temperature rangeof (278.15 to 328.15) K by the analytical stirred-flask method underatmospheric pressure. For the temperature range investigated, thesolubility of sulfanilic acid in the solvents increased with increasingtemperature. The thermodynamic models, such as the van’t Hoffmodel, the modified Apelblat model, and the Buchowski–Ksiazaczakλhmodel were investigated to describe theexperimental data. It was found that the modified Apelblat model wasthe most suitable for predicting the solubility behavior of sulfanilicacid with increasing temperature. The calculated thermodynamic parametersindicated that in each studied solvent the dissolution process ofsulfanilic acid is endothermic. [ABSTRACT FROM AUTHOR]

• Solubility of perphenazine (Form I) in eleven neat organic solvents was measured. • The KAT-LSER model was adopted to analyze the solvent effect. • Four activity coefficient models (Margules, NRTL NRTL-SAC UNIQUAC) were chosen to correlate solubility data. • Molecular dynamics simulation was used to simulate the effect of solute-solvent interaction on the dissolution process. • Thermodynamic properties of the solution were calculated. Perphenazine has rather effective in the treatment of mental illness. In this work, the solid-liquid equilibrium data of perphenazine in eleven organic neat solvents were determined by laser dynamic method under the atmospheric pressure and temperature range of 278.15 K ∼ 318.15 K. The selected solvents were n-propanol, n-butyl alcohol, methyl acetate, ethyl acetate, n-propyl acetate, n-amyl acetate, N, N-dimethylformamide (DMF), N, N-dimethylacetamide (DMAC), acetone, 2-methoxyethanol, glycol ether, respectively. From the results, the solubility of perphenazine is all positively correlated with temperature. Separately, we have adopted the KAT-LSER model and molecular dynamics simulation to investigate the influence of solvent effects and solute-solvent interaction on solute solubility. Meanwhile, there were four activity coefficient models being used to correlate the solubility data and Average relative deviation of models are 4.13% (Margules model), 3.94% (NRTL model), 4.49% (NRTL-SAC model) and 3.06% (UNIQUAC model), respectively, all of which do not exceed 5%. It manifests that the four activity coefficient models can fit the experimental values well, in which the UNIQUAC model gives the best regression effect. Moreover, the apparent thermodynamic properties(△ sol G° , △ sol H° and △ sol S°) of perphenazine in various solvents were calculated by Van't Hoff equation. In accordance with the analysis and calculation of dissolution, the dissolution process is an endothermic entropy-driven process. This research can provide basic data for the crystallization process of perphenazine. [ABSTRACT FROM AUTHOR]

Solubilitiesof SO2in five selected inexpensive organicsolvents with low volatility were measured at temperatures from 303.2K to 333.2 K and pressures up to 120 kPa. The solvents include sulfolane(SUF), ethylene glycol (EG), propylene carbonate (PC), N-methylimidazole (NMI) and N-methylpyrrolidone (NMP).The obtained results indicated that the solubilities of SO2in the five organic solvents followed the sequence NMI > NMP> SUF> PC > EG. The absorption isotherms of SO2in SUF,EG,and PC showed ideal profiles, while those in NMI and NMP showed nonidealtypes. The Henry’s law constants of SO2in SUF,EG, and PC in terms of molality were calculated by drawing linearfit between SO2solubilities and SO2partialpressures. The interactions of SO2with NMI and NMP wereexamined through density functional theory (DFT) calculations, andthe solvent–solute complex formations were illustrated. Theexperimental solubilities of SO2in NMI and NMP were successfullycorrelated by a reaction equilibrium thermodynamic model (RETM) proposedbased on the DFT calculations. Subsequently, Henry’s law constants,reaction equilibrium constants, and heat of complex formation werealso calculated to evaluate the potential of applying these organicsolvents in SO2absorption. The performance of SO2absorption in these organic solvents were further compared withthat in ILs and results illustrated that NMI and NMP were good alternativesto IL for applying in SO2absorption. [ABSTRACT FROM AUTHOR]

• Solubility of Nintedanib in ten pure solvents was measured. • The RDF of Nintedanib in solvents was simulated and researched. • KAT-LSER model was applied to analyze the solvent effect. • Solubility data was correlated by five models. • Thermodynamic properties of the solution were calculated. The equilibrium solubility and thermodynamic properties of Nintedanib in solvents including methanol, ethanol, n-propanol, iso -propanol, n-butanol, iso -butanol, DMF, DMAC, 1,4-dioxane and dichlormethane have been reported. By using the laser monitoring method with T = (278.15–323.15) K and p = 101.3 kPa, experiments for determinations of the solubility were carried out, from which it was proved that the mole fraction solubility of Nintedanib increased distinctly when the experimental temperature increased. The order of Nintedanib solubility in the above ten solvents was proved to be as follows: dichlormethane > DMAC > DMF > 1,4-dioxane > methanol > n-propanol > ethanol > n-butanol > iso -butanol > iso -propanol. The maximum mole fraction solubility of Nintedanib in dichloromethane was acquired (0.1314, T = 308.15 K); meanwhile, the minimum mole fraction solubility of Nintedanib in iso -propanol was acquired as well (4.4462 × 10−5, T = 278.15 K). Afterward, by using MD simulation, the results of the solute–solvent interaction proved that the solubility of Nintedanib in various solvents could be greatly affected by the interaction of the solute and solvent molecules, which showed that the dissolution behavior of Nintedanib in organic solvents was intricate. It also demonstrated that the solvent–solute interaction could be affected by factors of hydrogen bond acidity and the hydrogen bond donor propensities of the solvents. All records of Nintedanib solubility were regressed by using λh model, modified Apleblat model, Van't Hoff model and Yaws model. After comparing the results, it showed that the average 100 ARD of the λh model was smaller than that of the other four models, which perfectly proved that the λh model was more suitable for connecting the solubility data. Moreover, Van't Hoff equation was adopted to calculate and study the apparent thermodynamic properties of Nintedanib in all the relevant solvents, from which the results indicated that the dissolution process of Nintedanib was a non-spontaneous and entropy-driven endothermic process. [ABSTRACT FROM AUTHOR]

[Display omitted] • [BMIM]/[TOMP] ionic liquids (ILs) based on metal-EDTA complexes were synthetized. • The thermal behaviour of metal-EDTA ILs was investigated through TGA and DSC. • The solubility of metal-EDTA ILs in several solvents was tested. • Metal-EDTA ILs redox properties were assessed in aqueous/organic environments. Two series of ionic liquids (ILs) consisting in metal-EDTA complex anions ([MEDTA], with V, Cr, Mn, Fe and Co as metal center) and 1-butyl-3-methylimidazolium ([BMIM]) or trioctylmethylphosphonium ([TOMP]) cations have been prepared via a new synthetic approach based on the related acidic EDTA complexes (HMEDTA). A strong influence of both the coordinated metal and the cation type on the thermal behavior of the obtained ILs was assessed through DSC and TGA, while the solubility features were found to be primarily affected by the cation nature. The observed solubility results for [TOMP] series ILs in organic solvents showed the preparation of ILs as an effective way to solubilize metal-EDTA complexes into non-aqueous solutions, opening new investigation potential and applicative perspectives. The electrochemical properties of the synthesized ILs have been studied both in aqueous and non-aqueous environments, providing insights on the strong solvent effect on metal-EDTA complexes electrochemistry and, for many of the ILs, showing promising characteristics for electrochemical applications both in water and in organic solvents. [ABSTRACT FROM AUTHOR]