Solubility measurement and modelling of 1,8-dinitronaphthalene in nine organic solvents from T=(273.15 to 308.15)K and mixing properties of solutions

Zhou, Guoquan; Du, Cunbin; Han, Sen; Meng, Long; Wang, Jian; Li, Rongrong; Zhao, Hongkun

doi:10.1016/j.jct.2015.07.010

Cited by 24 publications

(8 citation statements)

References 16 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…33 Modified Apelblat equation. The dependence of the mole fraction solubility of 4-(methylsulfonyl)benzaldehyde upon temperature in the studied solvents is correlated by the modified Apelblat equation, 25,29 which was expressed as eq 2.…”

Section: ■ Results and Discussionmentioning

confidence: 99%

“…In this work, the relationship between the temperature and mole fraction solubility of 4-(methylsulfonyl)benzaldehyde in the different solvents is described by modified Apelblat equation, , λh equation, , Wilson model, and NRTL model …”

Section: Results and Discussionmentioning

confidence: 99%

“…The experimental procedure of solubility determination was similar to those used in the publications. , A 20 mL aliquot of solvent was put into an Erlenmeyer flask (about 50 mL), and then excess 4-(methylsulfonyl)benzaldehyde was added into the solvent. The temperature of the Erlenmeyer flask was controlled by a jacketed vessel with water circulated through the outer jacket from a smart thermostatic water bath (model DZKW-4).…”

Section: Experimental Sectionmentioning

confidence: 99%

See 2 more Smart Citations

Solubility Modeling of 4-(Methylsulfonyl)benzaldehyde in Nine Organic Solvents at Elevated Temperatures

Cong

Han

et al. 2016

J. Chem. Eng. Data

Self Cite

View full text Add to dashboard Cite

The binary solid−liquid phase equilibrium for 4-(methylsulfonyl)benzaldehyde in methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, acetone, acetonitrile, toluene, and acetic acid were studied experimentally within the temperatures range from (283.15 to 318.15) K under 101.3 kPa by using a static equilibrium method. With the increase in temperature, the solubility of 4-(methylsulfonyl)benzaldehyde in these solvents increased. The solubility values from high to low obeyed the following order in different solvents: acetone > acetonitrile > acetic acid > methanol > ethanol > toluene > 1-butanol > 1-propanol > 2-propanol. The modified Apelblat equation, λh equation, Wilson model, and nonrandom two liquid model were employed to correlate the experimental solubility of 4-(methylsulfonyl)benzaldehyde in the nine solvents. The calculated solubility with the modified Apelblat equation provided better agreement than those with the other three models. Generally, the regressed results by the four thermodynamic models could be acceptable for 4-(methylsulfonyl)benzaldehyde in the studied solvents. The acquired solubility data could provide a theoretical basis for the purification of crude 4-(methylsulfonyl)benzaldehyde.

show abstract

Section: ■ Results and Discussionmentioning

confidence: 99%

Section: Results and Discussionmentioning

confidence: 99%

Section: Experimental Sectionmentioning

confidence: 99%

See 1 more Smart Citation

Solubility Modeling of 4-(Methylsulfonyl)benzaldehyde in Nine Organic Solvents at Elevated Temperatures

Cong

Han

et al. 2016

J. Chem. Eng. Data

Self Cite

View full text Add to dashboard Cite

show abstract

“…During the experimental process, the solubility of 4,4′-dihydroxydiphenyl sulfone in various solvents were determined by means of the gravimetric method. − The temperature was controlled by using a smart thermostatic water bath with a model of DZKW-4 and a standard uncertainty of 0.02 K. The quantities of the solvent, solute, and saturated liquid were determined by means of an analytical balance with a standard uncertainty of 0.0001 g.…”

Section: Methodsmentioning

confidence: 99%

Solubility Measurement and Modeling of 4,4′-Dihydroxydiphenyl Sulfone in Nine Organic Solvents from T = (278.15 to 313.15) K and Thermodynamic Property of Dissolution

et al. 2015

View full text Add to dashboard Cite

The solubility of 4,4′-dihydroxydiphenyl sulfone in acetonitrile, methanol, ethanol, n-propanol, isopropyl alcohol, acetone, 1-butanol, 2-methyl-1-propanol and ethyl acetate were determined at temperatures from (278.15 to 313.15) K under 101.3 kPa by using a gravimetric method. With the increase in temperature, the solubility of 4,4′-dihydroxydiphenyl sulfone in these solvents increased. The solubility values decreased according to the following order: acetone > acetonitrile > ethyl acetate >1-butanol > (methanol, ethanol, n-propanol, 2-methyl-1-propanol) > isopropyl alcohol. The obtained solubility data were correlated with three models, which corresponded to the modified Apelblat equation, λh equation, and Van't Hoff equation. The evaluated solubility values by the modified Apelblat equation agreed very well with those calculated by the other two models. In general, the regressed results with the three models were all within the acceptable limit for the solubility of 4,4′dihydroxydiphenyl sulfone in the selected solvents. Furthermore, the standard dissolution enthalpies per 1 mol of mixtures of 4,4′-dihydroxydiphenyl sulfone and solvent were evaluated in terms of the modified Apelblat equation. The dissolution process of 4,4′-dihydroxydiphenyl sulfone in these solvents was endothermic. The study concerning the solubility of 4,4′-dihydroxydiphenyl sulfone in the selected solvents and thermodynamic property of dissolution could provide fundamental data in the manufacturing and separating process of 4,4′-dihydroxydiphenyl sulfone.

show abstract

“…Solubility and thermodynamic properties are important physicochemical parameters which are useful in crystallization, purification, formulation development, and preformulation studies. − The solubility data and thermodynamic properties of veramoss are unavailable in the literature and are needed to control the supersaturation, particle size, and desired polymorphic form in the crystallization process . Therefore, much more attention should be paid to the solubility and thermodynamic parameters of veramoss.…”

Section: Introductionmentioning

confidence: 99%

Solubility and Thermodynamic Behavior of Veramoss in Different Pure Solvents and {Ethanol + Water} Mixtures from T = 283.15 to 333.15 K

Chen

et al. 2016

J. Chem. Eng. Data

View full text Add to dashboard Cite

The solubility of veramoss in n-butyl alcohol, ethanol, isopropanol, ethyl acetate, acetone, tetrahydrofuran, isoamyl alcohol, n-amyl alcohol, n-propyl alcohol, and DMF pure solvents and various {ethanol + water} mixtures at T = 283.15−333.15 K and atmospheric pressure was measured by using the dynamic method. The experiment solubility data showed that the solubility of veramoss increased with increasing temperature in all solvents selected and decreased with the rise of mole fraction of water in the binary solvent mixtures of {ethanol + water}. The modified van't Hoff equation and the Apelblat model were successfully used to correlate the experimental solubility in pure solvents while the modified Apelblat model, the van't Hoff equation, and the CNIBS/R model were applied to correlate the solubility in binary solvent mixtures, and all of the models provided good fitting to the data. Furthermore, the thermodynamic parameters (dissolving enthalpy, dissolving entropy, and Gibbs free energy) of veramoss in different solvents were also calculated based on the Wilson equation and experimental solubility data; the dissolving process of veramoss in all selected pure solvents was observed as an endothermic, nonspontaneous, and entropy-driven process and in the binary solvent mixtures of {ethanol + water} was observed as an endothermic, spontaneous, and entropy-driven process. The data of experimental solubility, correlation equations, and thermodynamic property can be used as essential data for a preliminary study of industrial applications.

show abstract

Solubility measurement and modelling of 1,8-dinitronaphthalene in nine organic solvents from T=(273.15 to 308.15)K and mixing properties of solutions

Cited by 24 publications

References 16 publications

Solubility Modeling of 4-(Methylsulfonyl)benzaldehyde in Nine Organic Solvents at Elevated Temperatures

Solubility Modeling of 4-(Methylsulfonyl)benzaldehyde in Nine Organic Solvents at Elevated Temperatures

Solubility Measurement and Modeling of 4,4′-Dihydroxydiphenyl Sulfone in Nine Organic Solvents from T = (278.15 to 313.15) K and Thermodynamic Property of Dissolution

Solubility and Thermodynamic Behavior of Veramoss in Different Pure Solvents and {Ethanol + Water} Mixtures from T = 283.15 to 333.15 K

Contact Info

Product

Resources

About