The solubility of mercaptosuccinic acid in water+ (methanol, ethanol, acetone) mixtures from (278.15 to 333.15K)

Kai, Yumei; Hu, Yonghong; Liu, Yan; Liang, Mengmeng; Yang, Wenge; Yu, Xi

doi:10.1016/j.fluid.2013.11.001

Cited by 18 publications

(6 citation statements)

References 12 publications

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“…This might be attributed to the fact that PTBBA, water, and methanol work as hydrogen donors and acceptors, the O−H•••O−H bond among PTBBA and water and methanol is much stronger for higher concentrations of methanol in methanol + water, resulting in the greater dissolution capacity, that is, more solubility. 8 A significant increase in the solubility of PTBBA was observed for acetic acid + PTBT; however, acetic acid with mass fraction of almost 0.2 (0.38 mole fraction in Figure 2c) showed the best dissolving capacity for PTBBA at each temperature. This effect is called the "maximum solubility effect".…”

Section: Resultsmentioning

confidence: 90%

“…Also, the acetic acid + water system shows more dissolution capacity for lower concentrations of acetic acid than the methanol + water system, whereas the methanol + water system exhibited more solubility of PTBBA for higher concentrations of methanol compared to the acetic acid + water system. This might be attributed to the fact that PTBBA, water, and methanol work as hydrogen donors and acceptors, the O–H···O–H bond among PTBBA and water and methanol is much stronger for higher concentrations of methanol in methanol + water, resulting in the greater dissolution capacity, that is, more solubility . A significant increase in the solubility of PTBBA was observed for acetic acid + PTBT; however, acetic acid with mass fraction of almost 0.2 (0.38 mole fraction in Figure c) showed the best dissolving capacity for PTBBA at each temperature.…”

Section: Resultsmentioning

confidence: 96%

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Measurement and Modeling of Solid–Liquid Equilibrium of para-tert-Butylbenzoic Acid in Acetic Acid/Methanol + Water and Acetic Acid + para-tert-Butyltoluene Binary Systems at Various Temperatures

et al. 2016

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In this work, experimental solubility data of para-tert-butylbenzoic acid in binary solvents of acetic acid + water (293.15 to 333.15) K, methanol + water (293.15 to 328.15) K, and acetic acid + para-tert-butyltoluene (293.15 to 323.15) K were studied over acetic acid/methanol mass fraction, w 2 (on solute free basis) of 0.1 to 0.6 at temperatures of 5 K intervals. The solubility measurements showed that acetic acid + para-tert-butyltoluene recorded higher solubility than acetic acid/methanol + water for the same mass fraction of acetic acid at each temperature. Moreover, solubility increases with increase in temperature for the studied binary systems and the acetic acid + para-tert-butyltoluene system presents a maximum solubility effect at mass fraction of 0.2 (0.38 mole fraction) of acetic acid. Several thermodynamic models such as Buchowski–Ksiazczak equation, the Van’t Hoff equation, the modified Apelblat equation and NRTL model were fitted to the experimental data and the optimum values of the regressed parameters were presented. The results indicate that the Van’t Hoff and Buchowski–Ksiazczak equation represent the experimental findings better compared to other models based on the average absolute percentage deviation (δAAPD).

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Section: Resultsmentioning

confidence: 90%

Section: Resultsmentioning

confidence: 96%

Measurement and Modeling of Solid–Liquid Equilibrium of para-tert-Butylbenzoic Acid in Acetic Acid/Methanol + Water and Acetic Acid + para-tert-Butyltoluene Binary Systems at Various Temperatures

et al. 2016

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“…The combined nearly ideal binary solvent/Redich–Kister (CNIBS/R–K) model is one of the theoretical models for calculating the solute solubility in binary solvents. − This equation is expressed as eq where x A and x B represent the initial mole fraction compositions of the binary solvents when the solute was not added. X A is the saturated mole solubility of APMC in ethyl acetate.…”

Section: Resultsmentioning

confidence: 99%

Experimental Determination and Thermodynamic Models for Solid–Liquid Equilibrium of 4-(4-Aminophenoxy)-N-methylpyridine-2-carboxamide in Pure and Binary Solvent Mixtures for T = (278.15–328.15) K

et al. 2018

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In this study, the solubility of 4-(4-aminophenoxy)-N-methylpyridine-2-carboxamide (APMC) in pure tetrahydrofuran, ethyl acetate, acetonitrile, n-butanol, n-propanol, ethanol, methanol, and three binary solvent mixtures (ethyl acetate + methanol, ethyl acetate + ethanol, and ethyl acetate + n-butanol) was first experimentally determined within the temperature range from (278.15 to 328.15) K under atmosphere pressure by the gravimetric method. The results reveal that the solubility of APMC increases with an increase in temperature in all of the solvents selected. The modified Apelblat equation and the Buchowski−Ksiazaczak λh equation were used to correlate the experimental solubility in pure solvents while the modified Apelblat equation, the CNIBS/R−K model, and the Jouyban−Acree model were applied to correlate the solubility in binary solvent mixtures. All of the models could be well applied, and the modified Apelblat equation stood out to be more suitable with a higher accuracy compared to that of the other three models.

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“…The value of AIC is given as follows: where κ is the number of parameters in the statistical model and L is the maximized value of the likelihood function for the estimated model.…”

Section: Resultsmentioning

confidence: 99%

Measurement and Correlation of the Solubility for Camptothecine in Different Organic Solvents

Zhi

Liu

et al. 2016

J. Chem. Eng. Data

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Dissolution thermodynamics of camptothecine in chloroform, methanol, ethanol, and {chloroform + (methanol or ethanol)} mixed organic solvents were studied and correlated. The solubility of camptothecine in the above solvents was measured over the temperature range of 275.76–328.42 K at around 3 K intervals at atmospheric pressure. Experimental results showed that the solubility of camptothecine in the mixtures solvents increased with the increasing temperature. The mole fraction solubility of camptothecine reached a maximum at the mole fraction of chloroform 0.8016 in chloroform + methanol mixed solvent and 0.8031 in chloroform + ethanol mixed solvent. The experimental solubility data were well-correlated by using the modified Apelblat equation, the λh equation, and the ideal equation, respectively. The λh equation was proved to be the best-fit model for correlating the solubility of camptothecine from the analysis of the Akaike’s Information Criterion (AIC).

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The solubility of mercaptosuccinic acid in water+ (methanol, ethanol, acetone) mixtures from (278.15 to 333.15K)

Cited by 18 publications

References 12 publications

Measurement and Modeling of Solid–Liquid Equilibrium of para-tert-Butylbenzoic Acid in Acetic Acid/Methanol + Water and Acetic Acid + para-tert-Butyltoluene Binary Systems at Various Temperatures

Measurement and Modeling of Solid–Liquid Equilibrium of para-tert-Butylbenzoic Acid in Acetic Acid/Methanol + Water and Acetic Acid + para-tert-Butyltoluene Binary Systems at Various Temperatures

Experimental Determination and Thermodynamic Models for Solid–Liquid Equilibrium of 4-(4-Aminophenoxy)-N-methylpyridine-2-carboxamide in Pure and Binary Solvent Mixtures for T = (278.15–328.15) K

Measurement and Correlation of the Solubility for Camptothecine in Different Organic Solvents

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