Solid-liquid Equilibrium Data Research Articles

Crystallization Thermodynamics of α-Lactose Monohydrate in Different Solvents.

It is common to find that some of the lactose in dairy powders and pharmaceutical tablets is present in the unstable amorphous state. Therefore, their crystallization thermodynamics in different solvents are particularly important. In this paper, the solubility of α-lactose monohydrate (α-LM) in 15 mono-solvents such as ethanol, isopropanol, methanol, 1-propanol, 1-butanol, 2-butanol, isobutanol, 1-pentanol, isoamylol, 1-hexanol, 1-heptanol, 1-octanol, propanoic acid, acetonitrile, and cyclohexanone was evaluated by using the gravimetric method in the temperature ranges from 274.05 K to 323.05 K at constant pressure (1 atm). In the given temperature range, the solubility of α-LM in these solvents increased with the rising of temperature, the highest solubility of α-LM was found in methanol (2.37 × 104), and the lowest was found in 1-hexanol (0.80 × 105). In addition, the increase of α-LM solubility in isopropanol was the largest. The sequence at 298.15 K was: methanol > 1-butanol > isopropanol > ethanol > 1-propanol > 1-heptanol > isobutanol > propionic acid > 1-pentanol > 1-octanol > acetonitrile > isoamylol > 2-butanol > cyclohexanone > 1-hexanol. Solvent effect analysis shows that the properties of α-LM are more important than those of solvents. The Apelblat equation, λh equation, Wilson model, and NRTL model were used to correlate the experimental values. The root-mean-square deviation (RMSD) and relative average deviation (RAD) of all models were less than 2.68 × 10−2 and 1.41 × 10−6, respectively, implying that the fitted values of four thermodynamic models all agreed well with the experimental values. Moreover, the thermodynamic properties of the dissolution process (i.e., dissolution Gibbs free energy (ΔdisG), molar enthalpy (ΔdisH), and molar entropy (ΔdisS)) for α-LM in selected solvents were determined. The results indicate that ΔdisH/(J/mol) (from 0.2551 to 6.0575) and ΔdisS/(J/mol/K) (from 0.0010 to 0.0207) of α-LM in these solvents are all positive, and the values of ΔdisH and ΔdisS. ΔdisG/(J/mol) (from −0.0184 to −0.6380) are all negative. The values were observed to decrease with rising temperatures, implying that α-LM dissolution is an endothermic, entropy-driven, and spontaneous process. The solid–liquid equilibrium data and dissolution thermodynamics of α-LM were obtained, which provide a basis for industrial production.

Solubility determination, model correlation and preferential solvation of methyldopa in binary mixed solvents from 278.15 K to 323.15 K

As an antihypertensive drug, methyldopa (MD) plays a vital role in for clinical treatment of moderate, severe or malignant hypertension, especially for secondary hypertension, pregnancy-induced hypertension, heart failure combined with hypertension and other diseases. The solid-liquid equilibrium data of MD was determined. The four binary mixtures were composed of the mixtures of three green organic solvents (methanol, ethanol and isopropanol) + water and DMF + water in this experiment, and HPLC was used to detect the mole fraction solubility of MD (T = 278.15–323.15 K). The maximum mole fraction solubility data of MD (x = 1.35E−01) is related to pure DMF (T = 323.15 K) and the minimum value (x = 1.41E−06) is related to pure water (T = 278.15 K). When the organic solvent in the binary solvent is an alcohol solvent, the mole fraction solubility of MD is negatively correlated with the carbon chain length of the alcohol solvent and positively correlated with the polarity of the alcohol solvent. In addition, five thermodynamic models were used to validate and predict experimental data and deviation analysis, the largest mean square deviation value (RMSD) is only 9.76E−04, indicating that the experimental data has superior correlation with the five models used and the data is real and reliable. Simultaneously, the KAT model was used to analyze the effect of solvent effect on its mole fraction solubility during MD dissolution, the results are demonstrated that among multiple factors that affect solvent effects in the KAT model, the ability of the solvent to receive hydrogen bonds (α) and the size of the polarity (π∗) promote the dissolution of MD, but the main influence on the MD solvent effect is the cavity term demonstrating the solvent-solvent molecular interaction energy, and the contribution rates of these three items to the total solvent effect are 7.92%, 16.01% and 50.16%, respectively.

Current Trends in Predictive Methods and Electrolyte Equations of State.

Over the past 20–30 years, the development of thermodynamic models for electrolyte solutions has experienced remarkable progress. While in the first half of the 20th century, the thermodynamic models were essentially based on the continuum electrostatic approach, nowadays equations of state and predictive methods have been adapted to deal with electrolyte solutions. Given this panorama, in this mini-review, the recent advances in predictive methods and electrolyte equations of state are examined, as well as their performance in predicting activity coefficients and solid–liquid phase equilibrium data. Although this mini-review aims to shed light on the current progress in predictive methods and electrolyte equations of state, it also provides valuable references and information to the several models and theories that form the backbone of the thermodynamics of electrolyte solutions.

Solid-liquid equilibrium measurements using DSC for three binary mixtures of 2-methylbenzoic acid + 3-methylbenzoic acid, 2-methoxybenzoic acid + 3-methylbenzoic acid, and N-phenylacetamide + benzamide

This study reports the solid-liquid equilibrium (SLE) data for three binary mixtures of 2-methylbenzoic acid + 3-methylbenzoic acid, 2-methoxybenzoic acid + 3-methylbenzoic acid, and N-phenylacetamide + benzamide. These phase equilibrium data were measured using the Differential Scanning Calorimetry (DSC). The solidus and liquidus temperatures for each binary mixture at various compositions are presented. All three binary mixtures show the simple eutectic behavior. The eutectic temperatures and compositions for these binary mixtures were determined using the fractional transformation method. The fractional transformation is defined as the fraction of the mixture that is liquefied during the heating process using DSC. The fractional transformation data at the eutectic point, denoted as the eutectic fraction, were evaluated from the experimental DSC results over various time intervals during the measurements. A triangular plot of the eutectic fractions against various compositions of a binary mixture effectively illustrated the eutectic point condition. The liquidus curves for each binary system were correlated using the Wilson and NRTL (Non-Random Two-Liquid) activity coefficient models. The optimally fitted model parameters for each binary mixture are presented in this study. Satisfactory correlation results are also demonstrated for all binary systems.

Solubility, MD simulation, thermodynamic properties and solvent effect of perphenazine (Form I) in eleven neat organic solvents ranged from 278.15 K to 318.15 K

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(△solG°, △solH° and △solS°) 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.

Solid-Liquid Equilibrium and Phase Diagram of Organic System Forming Simple Eutectic

The study of phase diagram guided with solid-liquid equilibrium (SLE) data at different molar composition in two component systems serve as a basic roadmap for the material synthesis, and also provide in-depth study of physicochemical and thermochemical properties of synthesized materials. The solid-liquid equilibrium data of binary organic system, acetanilide – acetamide (ACN-ACT) is determined by thaw melt method. The system exhibits simple eutectic type phase diagram at 0.20 molar composition of ACN with congruent melting temperature 52oC.

Solubility Measurement and Thermodynamic Correlation of Diacetone Acrylamide in 15 Pure Solvents from 272.05 to 323.65 K

For the design, optimization, and control of the solution crystallization process of diacetone acrylamide (DAAM), solid–liquid equilibrium data in various solvents are critical. In this work, the solubility of DAAM in 15 pure solvents, such as methanol, ethanol, n-propanol, isopropanol, n-butanol, 1-hexanol, isobutanol, n-pentanol, isopentanol, 2-butanone, acetone, ethyl acetate, 2-pentanone, acetonitrile, methyl acetate, and ethyl formate, is analyzed by a gravimetric method under ambient pressure and temperatures ranging from 272.05 to 323.65 K. The solubility values in all of the solvents are positively correlated with temperature. The solubility of DAAM can be satisfactorily correlated by the Apelblat equation, λh equation, nonrandom two-liquid (NRTL) model, and Wilson model, and the calculated solubility agrees well with the measured results. The obtained maximum relative average deviation (RAD) and root-mean-square deviation (RMSD) are 2.44 × 10–2 (n-propanol, NRTL model) and 2.40 × 10–2 (methanol, λh equation), respectively. The most suitable model is the Apelblat equation.

Solid-liquid equilibrium of 3,3-dilauryl thiodipropionate/lauryl alcohol in melt crystallization and model based process design

Melt crystallization is a promising and widely used method for obtaining pure compounds. Nonetheless, separation of 3,3-dilauryl thiodipropionate (DLTP) has not yet been realized by melt crystallization. Solid-liquid equilibrium is the fundamental for the separation process design. In this work, we evaluated the feasibility of the purification of DLTP from the DLTP/lauryl alcohol (LA) binary mixture by melt crystallization technique. For this purpose, the solid-liquid equilibrium data were measured using differential scanning calorimetry (DSC) technique. The experimental data were correlated by Wilson, Margules-3-suffix and Non-Random Two-Liquid (NRTL) activity coefficient models to obtain the binary parameters of the three models. Eutectic composition and temperature were calculated using NRTL model, which were xLA = 0.961 (molar fraction) and 295.79 K, respectively. On the basis of the solid–liquid equilibrium, the multistage countercurrent separation configurations were proposed for the separation of the binary system. The formulated Mixed Integer Nonlinear Programming (MINLP) problem was solved using the branch-and-bound algorithm. The conceptual designs for multistage countercurrent configuration were derived based on MINLP optimization by comparing results at various conditions. Results showed that at least 3 crystallization stages with keff ≤ 0.4 are required to obtain the 99% (mass fraction) DLTP product within the initial concentration range from10% to 30% (mass fraction).

Solid–Liquid Phase Equilibrium of Isophthalonitrile in 16 Solvents from T = 273.15 to 324.75 K and Mixing Properties of Solutions

The solid–liquid equilibrium of isophthalonitrile (IPN) in 16 solvents (methanol, ethanol, n-propanol, isopropanol, acetone, ethyl acetate, acetonitrile, chloroform, cyclohexanone, cyclopentanone, methyl acetate, ethyl formate, 2-pentanone, tetrahydrofuran, toluene, and diethyl ether) was measured by using a static equilibrium method at temperatures T = 273.15–324.75 K under atmospheric pressure. The results demonstrated that the solubility of IPN in these 16 monosolvents increased with increasing temperature. The largest solubility values of IPN were found in cyclopentanone, and the lowest were in isopropanol. The values of solubility in ketones were much larger than those in esters and alcohols. In alcohols, the solubility ranked as methanol > ethanol > n-propanol > isopropanol, and the sequence was identical to that of the solvent polarities. The polarity of the solvent is an important factor influencing the solubility profiles of IPN in alcohols, despite that the conclusion is not supported by other kinds of solvents studied. Moreover, the Apelblat equation, λh equation, Wilson model, and nonrandom two-liquid model were used to correlate the experimental values. The calculated values of four models all provided good fitting results with the experimental data, and the values of root-mean-square deviation and relative average deviation (RAD) were no more than 6.84 × 10–4 and 6.84 × 10–3, respectively. Furthermore, the thermodynamic properties of the mixing process for IPN in selected solvents were calculated, that is, mixing Gibbs energy (ΔmixG), molar enthalpy (ΔmixH), and molar entropy (ΔmixS). The results indicated that the mixing process of IPN was a spontaneous and entropy-driven process. The solid–liquid equilibrium data and solution thermodynamics would be helpful for the synthesis and purification of IPN in the industry.

Solubility Determination and Thermodynamic Correlation of 3-Amino-2-methylbenzoic Acid in 12 Monosolvents from 288.15 to 328.15 K

A gravimetric method is adopted to measure the solid–liquid equilibrium of 3-amino-2-methylbenzoic acid in different solvents, including methanol, ethanol, 1-propanol, isopropyl alcohol, 1-butanol, isobutyl alcohol, 2-butanol, methyl acetate, ethyl acetate, propyl acetate, water, and acetonitrile. Moreover, the experiment is carried out at atmospheric pressure, and the temperature range is from 288.15 to 328.15 K. The solid–liquid equilibrium of 3-amino-2-methylbenzoic acid in all used solvents increases with increasing temperature. In alcohol solvents, except for isopropyl alcohol and 2-butanol, the solubility of 3-amino-2-methylbenzoic acid is positively related to the polarity of the solvent, which follows the “like dissolves like” rule. Because isopropyl alcohol and 2-butanol possess a high hydrogen bond acceptor propensity, this leads to a different solubility behavior. In nonalcohol solvents, the solid–liquid equilibrium of 3-amino-2-methylbenzoic acid also follows the “like dissolves like” rule. Among all 12 solvents, the solid–liquid equilibria of 3-amino-2-methylbenzoic acid in water and acetonitrile are lower than those in alcohols and esters. In addition, the solid–liquid equilibrium data of 3-amino-2-methylbenzoic acid were related by the modified Apelblat equation, van’t Hoff equation, and λh equation. Furthermore, all relevant results show consistency with the solid–liquid equilibrium data of 3-amino-2-methylbenzoic acid.

Measurements and Thermodynamic Modeling of Solid–Liquid Equilibria Data for the Ternary (KCl + PEG8000 + H2O) System at 288.2, 298.2, and 308.2 K

Measurements and Thermodynamic Modeling of Solid–Liquid Equilibria Data for the Ternary (KCl + PEG8000 + H2O) System at 288.2, 298.2, and 308.2 K

Determination and correlation of binary molten solid–liquid equilibria of tetramethyl biphenyl isomers

Three binary molten phase diagrams of three isomers of tetramethyl biphenyl (TMB) were constructed by differential scanning calorimetry (DSC) at 101.3 kPa. Our results reveal that the tetramethyl biphenyl isomers binary system presents a eutectic behaviour that lays a solid foundation for its separation technology. Meanwhile, the thermodynamic model such as Wilson, NRTL and Ideal model were employed to correlate the phase equilibrium data of the tetramethyl biphenyl isomers. The results show the ideal model can describe two binary phase behaviour of 2,2′,3,3′-Tetramethyl biphenyl (TMB1) + 3,3′,4,4′-Tetramethyl biphenyl (TMB3) well while it isn't suitable for TMB1 + 2,3′,3,4′-Tetramethyl biphenyl (TMB2) and TMB3 + TMB2 systems. The best correlation of the solid–liquid equilibrium data has been obtained by the NRTL equation. Besides, the mixing thermodynamic properties were calculated by NRTL model to gain more insights into the phase behaviour of the binary melt eutectic systems. Then, we discuss the co-effect of temperature and low melting point components on the binary phase melting mechanism. At last, non-linear enthalpy–entropy compensation analysis indicated different dissolution mechanism with the variation in mixtures composition.

Experimental measurement – correlation of solubility and dissolution thermodynamics study of itraconazole in pure monosolvents at various temperatures

The information about the solubility and thermodynamic properties of solution is important for pharmaceutically important processes, formulation development, and further theoretical studies. In the present study, the solid–liquid equilibrium (solubility) for itraconazole (ITC) was determined experimentally in 14 monosolvents at temperatures between 293.15 K and 318.15 K under pressure of 0.1 MPa. The mole fraction solubilities were found to increase with increasing temperatures and followed inverse trend with the polarity of selected solvents. Besides, KAT-LSER analysis was performed to study the effect of solvent. The results revealed that the solute–solvent interaction (43.94%) was much higher than that of solvent–solvent interaction (16.59%). Thermodynamic based models like van’t Hoff equation, modified Apelblat equation, Buchowski–Ksiazaczak equation, and polynomial empirical equation were applied to fit and correlate the experimental solubilities. Overall relative average deviation and overall root-mean square deviation () were observed to be minimum with the empirical polynomial equation and attained the values of 0.0033 and 0.0047, respectively. Furthermore, theoretical ideal solubilities, activity coefficients, and thermodynamic properties of dissolution including molar enthalpy, molar entropy, molar Gibbs free energy, and excess enthalpy were estimated. Ideal solubilities were projected considerably higher than experimental solubilities at each studied temperature. Thermodynamic properties of dissolution indicated that the dissolution was not a spontaneous process; observed to be endothermic ( and enthalpy driven Such solid–liquid equilibrium data of ITC will be of immense help in process and formulation development in pharmaceutical sciences.

Solid-liquid equilibrium, structural features and separation process of ammonium potassium dihydrogen phosphate solid solution

• Solid-liquid equilibrium of the NH 4 + , K + //H 2 PO 4 − -H 2 O system at 283.15 K and 313.15 K was investigated. • By characterization determined infinite substitutional solid solutions. • Two solid solutions are analyzed by FTIR, TG-DSC, EDS (mapping). • A multistage purification process was developed and proved feasibility for AQ-SS. Solid-liquid equilibrium for NH 4 H 2 PO 4 + KH 2 PO 4 + H 2 O ternary system was investigated at 283.15 K and 313.15 K, which revealed complete mixed crystals in the solid phase. By analysis of XRD and the formation rule of the substituted solid solution, it is further confirmed infinite substitutional solid solution. Then, from the analysis of FT-IR, TG-DSC and mapping of [K 0.78 (NH 4 ) 0.22 ]H 2 PO 4 and [K 0.11 (NH 4 ) 0.89 ]H 2 PO 4 solid solution, we can conclude that two solid solutions are similar, but the absorption position have slight shift to low wave number direction as the increasing of K + content; the homogeneous distribution of K + and NH 4 + elements. Finally, applying the experimental solid-liquid equilibrium data, multistage fractional crystallization experiment to obtain the purity of the KH 2 PO 4 is close to 97% after five times operation and purity of the NH 4 H 2 PO 4 reaches about 98% after four times operation, which proves multistage fractional purification is verified as an effective purification method for AQ-SS.

Multicomponent Solid–Liquid Equilibrium of 1,3,5-Triformylbenzene—A Key Intermediate for Porous Organic Cages: Solubility Determination and Correlation in Different Solvent Systems

The multicomponent solid–liquid equilibrium data for 1,3,5-triformylbenzene, a key intermediate for the synthesis of porous organic cages, in 12 neat solvents (water, methanol, ethanol, n-propanol,...

Solid–Liquid Phase Equilibria of Mn2+,NH4+//SO42–,Cl––H2O and Its Subsystems (Mn2+,NH4+//Cl––H2O, Mn2+//SO42–,Cl––H2O) at T = 303.15 K

In this study, the solid–liquid equilibrium data of the quaternary system Mn2+,NH4+//SO42–,Cl––H2O and its two ternary subsystems (Mn2+,NH4+//Cl––H2O and Mn2+//SO42–,Cl––H2O) were measured by the isothermal dissolution method. For the two ternary systems, the solubility of the equilibrium liquid phase was determined. In the Mn2+,NH4+//Cl––H2O system, there are two invariant points and five crystallization regions. In the Mn2+//SO42–,Cl––H2O system, there are one invariant point and three crystallization regions. The solubility data of the quaternary system Mn2+,NH4+//SO42–,Cl––H2O were measured in the experiment. According to the theory of translation, the number of invariant points and crystallization zones of the quaternary system are predicted. The predicted results are the same as the experimental results, both of them have the same number of co-saturation points and crystallization zones. There are four invariant points and six crystallization regions in the quaternary system. It provides a theoretical basis for the water–salt system containing the quaternary system.

Automated measurement of pH-dependent solid-liquid equilibria of itaconic acid and protocatechuic acid

Crystallization is a highly selective unit operation capable of separating target molecules from complex media. Its design requires precise solid-liquid equilibrium (SLE) data. The SLE of platform chemicals like carboxylic acids in complex aqueous media depends on temperature, pH value as well as on present side components, but predominantly, only the solubility for different temperatures is reported. This work presents a novel automated method for the determination of the pH- and temperature-dependent SLE in complex media using readily available laboratory equipment. Taking the example of itaconic acid, the pH-dependent solubility for different temperatures is measured and validated with results obtained from the classic excess solid method along with literature data. Using the automated setup, the influence of different loadings of sodium chloride on the SLE of itaconic acid is investigated and a correlation between solubility and concentration of the electrolyte is derived. The SLE data acquired for protocatechuic acid in fermentation medium demonstrates the applicability of the method for the determination of comprehensive SLE in multicomponent mixtures without the requirement of specific analytical methods for the target compound. The resulting SLE data can be used for a more precise design and techno-economic evaluation of crystallization processes in biotechnological production routes.

Phase Equilibria of the Ternary Systems Potassium Sulfate + Polyethylene Glycol (PEG6000/10,000) + Water at 288.2, 298.2 and 308.2 K: Experimental Determination and Correlation

The phase equilibrium data were determined for the ternary systems potassium sulfate + polyethylene glycol (PEG6000/10,000) + water at 288.2, 298.2 and 308.2 K. Only solid–liquid equilibrium exists for the ternary system K2SO4 + PEG6000/10,000 + H2O at 288.2 and 298.2 K, the solubility, density, and refractive index were measured by using the isothermal dissolution equilibrium method. The solid–liquid equilibrium and liquid–liquid equilibrium exist simultaneously for the ternary system K2SO4 + PEG6000/10,000 + H2O at 308.2 K, the corresponding compositions of binodal curve and tie-line were obtained experimentally by using the turbidimetric method. Results show that the solubility of K2SO4 decreases as the content of PEG increases in the PEG–H2O mixed solvents. Meanwhile, as the molar mass of PEG increased, the liquid–liquid equilibrium formed more easily and the liquid–liquid equilibrium area was larger. In addition, the modified Pitzer model was used to calculate the solid–liquid equilibrium data for systems K2SO4 + PEG6000/10,000 + H2O at 288.2, 298.2 and 308.2 K.

Experimental determination and modelling of the co-solvent and antisolvent behaviour of binary systems on the dissolution of pharma drug; L-aspartic acid and thermodynamic correlations

Solid-liquid equilibrium (SLE) data and thermodynamic properties play an important role to understand the crystallization phenomenon as it became an important step for purification and separation to get a required specific product. In this study, solubility of L-aspartic acid (L-ASP) in different binary mixtures (formic acid/trimethylamine(TMA)/methanol/iso-propylalcohol(IPA) + water) were carried out at temperatures from 283.15 to 328.15 K. The experimental data was generated using the gravimetric and titrimetric method. For a binary system, the solubility of L-ASP increased with increasing temperature. The effect of solvent on mole fraction solubility of L-ASP decreased with increasing methanol/IPA mole fraction in mixture, whereas solubility increased with increased formic acid/TMA fractions in mixture. The order of solubility for binary solvents systems as follows: TMA + water > formic acid + water > methanol + water > IPA + water. Different thermodynamic models like Apelblat equation, Apelblat-Jouyban-Acree model, NRTL model, and general single model were applied to correlate the experimental data. It was found that Apelblat equation and general single model was the best-fit for correlating solubility of L-ASP in binary mixtures with average relative deviation (ARD) less than 2% and root mean square deviation (RMSD) are below 5.3E-04. It can also be concluded that formic acid and TMA act as co-solvent in dissolution of L-ASP in their respective binaries, wheras methanol and IPA exhibited anti-solvent effect in the aqueous solution. The generated SLE data would be helpful in technological research for production of drugs in purification and separation process.

Solubility and solution thermodynamics of isobutyramide in 15 pure solvents at temperatures from 273.15 to 324.75 K

Being an important synthetic monomer, isobutyramide (IBA) is employed as an intermediate for the synthesis of organic dyes and pharmaceuticals. It is well known that investigation of the solubility behavior of drugs and intermediates has become an extensive research topic in pharmaceutical development. In this work, the solid-liquid equilibrium (SLE) data of IBA in fifteen solvents, including methanol, ethanol, n-propanol, isopropanol, n-butanol, isobutanol, acetonitrile, chloroform, acetone, ethyl formate, methyl acetate, cyclohexanone, cyclopentanone, tetrahydrofuran and 2-butanone was measured with a static gravimetric method with the temperature ranging from 273.15 to 324.75 K under atmospheric pressure. The solubility of IBA increases with the rising temperature in all selected solvents. The ranking of solubility in various solvents is not in accordance with the order of solvent physicochemical properties, namely polarity index, dipole moment, dielectric constant and solubility parameter. The modified Apelblat equation, λh equation, nonrandom two-liquid (NRTL) model and the Wilson model were used to correlate the experimental data. Maximum root-mean-square deviation (RMSD) and relative average deviation (RAD) were 7.157 × 10−3 and 1.80%, respectively. The λh equation presented less effective correlating results compared with other three models. The dissolution properties of IBA, including Gibbs energy (△disG), molar enthalpy (△disH) and molar entropy (△disS) were determined based on the Wilson model and the solubility data. Positive values of the dissolution enthalpy and entropy illustrated that the dissolution process of IBA in selected solvents are endothermic and entropy-driven.