Solubility and solution thermodynamics of hippuric acid in various solvents from 298.15 K to 328.15 K

Baluja, Shipra; Alnayab, Elham Abdullah Mo; Hirapara, Asmita

doi:10.1016/j.molliq.2017.04.122

Cited by 18 publications

(7 citation statements)

References 18 publications

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“…Although 2-butanol has the smaller value of dielectric constant than that of isobutanol, the solubility of N -acetyl- l -leucine in 2-butanol is larger than that in isobutanol. The reason may be that dissolution is a complex process and cannot be described clearly with only one parameter. , The formation of hydrogen bonds may be another vital factor that affects solubility. The greater hydrogen bond acceptor propensities may cause the apparently higher solubility of N -acetyl- l -leucine in 2-butanol than in isobutanol.…”

Section: Resultsmentioning

confidence: 99%

“…The reason may be that dissolution is a complex process and cannot be described clearly with only one parameter. 30,31 The formation of hydrogen bonds may be another vital factor that affects solubility. The greater hydrogen bond acceptor propensities may cause the apparently higher solubility of N-acetyl-L-leucine in 2-butanol than in isobutanol.…”

Section: Resultsmentioning

confidence: 99%

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Solubility Measurement, Correlation, and Thermodynamic Analysis of N-Acetyl-l-leucine in 12 Pure Organic Solvents from 283.15 to 323.15 K

Guo

Wang

et al. 2020

J. Chem. Eng. Data

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The solubility of N-acetyl-l-leucine in 12 mono organic solvents (methanol, ethanol, n-propanol, 2-propanol, 1-butanol, isobutanol, 2-butanol, methyl acetate, ethyl acetate, propyl acetate, acetone, and acetonitrile) was determined by the gravimetric method over the temperatures ranging from 283.15 to 323.15 K at 0.1 MPa. The solubility of N-acetyl-l-leucine in each experimental solvent increases with increasing temperature. Moreover, the solubility is an order of magnitude higher in alcohol solvents than in other solvents, which is mainly attributed to the hydrogen bond formation. In addition, the experimental solubility data are correlated by three models, including the modified Apelblat equation, λh equation, and the nonrandom two-liquid (NRTL) model. All of the average relative deviation % values are less than 3.72%, which indicates that the three models have satisfactory correlations. Furthermore, the mixing thermodynamic properties of N-acetyl-l-leucine in 12 mono solvents including Δmix G 0, Δmix H 0, and Δmix S 0 are calculated based on the NRTL model, indicating that the mixing process was spontaneous.

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Section: Resultsmentioning

confidence: 99%

Section: Resultsmentioning

confidence: 99%

Solubility Measurement, Correlation, and Thermodynamic Analysis of N-Acetyl-l-leucine in 12 Pure Organic Solvents from 283.15 to 323.15 K

Guo

Wang

et al. 2020

J. Chem. Eng. Data

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“…The negative or positive values of Δ S o sol are related to both the solvent and the solute's functional groups. The presence of these groups can cause existing various forces such as electrostatic force and hydrogen bonds, which may influence the dissolving process .…”

Section: Resultsmentioning

confidence: 99%

Thermodynamic Models and Central Composite Design for Calcium Sulfate Dihydrate Solubility

2020

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The solubility of calcium sulfate dihydrate (gypsum) was measured in HCl solutions in the presence of Cr 3+ and Fe 3+ ions at various temperatures. The results indicate that the solubility of gypsum is fairly dependent on the concentrations of HCl and impurities, i.e., Cr 3+ and Fe 3+ ions. The experimental data were analyzed by applying the Buchowski-Kiazczak (lh) model and the modified Apelblat model. Some thermodynamic parameters, such as the standard molar dissolution enthalpy, the standard molar Gibbs energy, and the entropy of solutions, were calculated by Van't Hoff analysis and Gibbs equation. The influences of the concentrations of both HCl and impurities, i.e., Cr 3+ and Fe 3+ ions, and temperature on the gypsum solubility were examined by applying the central composite design.

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“…The modified Apelblat equation, which is a commonly applied empirical correlation equation, describes the relationship between the mole fraction solubility data and the absolute temperature. − The equation is expressed as follows where x 1 refers to the mole solubility fraction of solute probenecid, T is the absolute temperature (K), and a , b , and c are empirical regression parameters which are determined using least-squares fitting of the experimental mole fraction solubility values and the absolute temperature. The mathematical method was nonliner regression, and the objective function is expressed as follows where x i refers to the mole solubility of probenecid obtained from the experimental measurement and x i cal refers to the calculated mole solubility.…”

Section: Resultsmentioning

confidence: 99%

Solubility Measurement and Correlation of Probenecid in 12 Pure Organic Solvents and Thermodynamic Properties of Mixing of Solutions

et al. 2019

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The solubility data of probenecid in 12 different organic solvents including methanol, methyl acetate, ethanol, ethyl acetate, n-propanol, n-butanol, butyl acetate, n-pentanol, isopropanol, isobutanol, acetone, and methyl tert-butyl ether was measured using the gravimetric method over the temperatures range from 283.15 to 323.15 K at 0.1 MPa. The acetone had much higher solubility to probenecid than to other solvents. Three models, including the modified Apelblat equation, the van’t Hoff model, and the nonrandom two-liquid (NRTL) model, were applied to correlate the measured solubility data. The correlation results were evaluated by the average relative deviation (ARD). All of the ARD values were less than 4.522%, which indicated that the three models have a satisfactory correlation. The thermodynamic properties of mixing of probenecid in 12 pure organic solvents including the enthalpy of mixing, Gibbs energy of mixing, and entropy of mixing were calculated by the NRTL model using the correlation results.

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Solubility and solution thermodynamics of hippuric acid in various solvents from 298.15 K to 328.15 K

Cited by 18 publications

References 18 publications

Solubility Measurement, Correlation, and Thermodynamic Analysis of N-Acetyl-l-leucine in 12 Pure Organic Solvents from 283.15 to 323.15 K

Solubility Measurement, Correlation, and Thermodynamic Analysis of N-Acetyl-l-leucine in 12 Pure Organic Solvents from 283.15 to 323.15 K

Thermodynamic Models and Central Composite Design for Calcium Sulfate Dihydrate Solubility

Solubility Measurement and Correlation of Probenecid in 12 Pure Organic Solvents and Thermodynamic Properties of Mixing of Solutions

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