Solubility and Thermodynamic Modeling of Sulfanilamide in 12 Mono Solvents and 4 Binary Solvent Mixtures from 278.15 to 318.15 K

Kodide, Kalyani; Asadi, Prashanth; Thati, Jyothi

doi:10.1021/acs.jced.9b00411

Cited by 19 publications

(20 citation statements)

References 43 publications

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“…The modified Apelblat model is another thermodynamic solubility model as a frequently-used semiempirical model, , which was derived from the Clausius-Clapeyron equation. Just as Buchowski-Ksiazczak λh model, it is also able to correlate the experimental mole fraction solubility of solute at different temperatures in pure solvents as eq where x 1 is the mole fraction solubility of the solute at temperature T ; T is the absolute temperature; A , B and C stand for model parameters of the modified Apelblat model.…”

Section: Thermodynamic Modelsmentioning

confidence: 99%

“…The modified Apelblat model is another thermodynamic solubility model as a frequently-used semiempirical model, 12,13 which was derived from the Clausius-Clapeyron equation. Just as Buchowski-Ksiazczak λh model, it is also able to correlate the experimental mole fraction solubility of solute at different temperatures in pure solvents as eq 7…”

Section: Modified Apelblat Modelmentioning

confidence: 99%

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Solubility of Benzanilide Crystals in Organic Solvents

2020

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The solubility of benzanilide in sixteen pure organic solvents, including N, N-dimethylformamide, tetrahydrofuran, butanone, acetone, ethyl acetate, dichloromethane, n-butanol, diethyl ether, n-propanol, acetonitrile, ethanol, methanol, isobutanol, isopropanol, toluene, and carbon tetrachloride, was measured at temperatures ranging from 274.15 to 313.15 K using the static equilibrium method at atmospheric pressure. The modified Apelblat model, Buchowski-Ksiazczak λh model, and Non Random Two Liquid (NRTL) model were used to correlate the experimental solubility data. It was found that in all these solvents the solubility of benzanilide increases in different pace as the temperature increases. The modified Apelblat model gave the best fit. Guided by the solubility data, preliminary experimental study was conducted for cooling crystallization of benzanilide in ethanol and n-propanol. The result indicated that the solvent, stirring speed and cooling rate all have significant impact on crystal morphology and particle size distribution.

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Section: Thermodynamic Modelsmentioning

confidence: 99%

Section: Modified Apelblat Modelmentioning

confidence: 99%

Solubility of Benzanilide Crystals in Organic Solvents

2020

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“…It is another empirical model to correlate the solubility with temperature. This equation is described as 14,15 x x h T T ln 1…”

Section: Methodsmentioning

confidence: 99%

“…It is another empirical model to correlate the solubility with temperature. This equation is described as , where T m /K is the melting point; λ and h are model parameters.…”

Section: Solid–liquid Phase Equilibrium Modelsmentioning

confidence: 99%

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

Guan

Yang

et al. 2021

J. Chem. Eng. Data

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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 (Δ mix G), molar enthalpy (Δ mix H), and molar entropy (Δ mix S). 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.

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“…In this work, the solubility data in mole fraction of NTZ were correlated by the modified Apelblat equation − and λ h equation. − The dependence of solubility results on the temperature T could be described using the modified Apelblat equation, which is expressed in eq . where x is the mole fraction solubility of NTZ in 12 organic solvents, R is the universal gas constant. A , B , and C are the adjustable equation parameters.…”

Section: Data Correlation With Semi-empirical Modelsmentioning

confidence: 99%

Solubility Determination of Nitazoxanide in Twelve Organic Solvents from T = 273.15 to 313.15 K

2020

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The objective of the present study was to study the solubility of nitazoxanide (NTZ) in 12 organic solvents such as methanol, ethanol, isopropanol, n-propanol, 1-butanol, ethyl acetate, toluene, acetonitrile, 1,4-dioxane, N-methyl-2-pyrrolidone (NMP), N,N-dimethylformamide (DMF), and 2-butanone by using the isothermal saturation method over a temperature range of 273.15–313.15 K under 101.3 kPa. Experimental solubility data of NTZ was fitted with the modified Apelblat and λh equations. The maximum mole fraction solubility of NTZ was found in NMP (1.127 × 10–1 at 313.15 K) followed by DMF (1.043 × 10–1 at 313.15 K), 1,4-dioxane (3.107 × 10–2 at 313.15 K), 2-butanone (2.286 × 10–2 at 313.15 K), ethyl acetate (3.99 × 10–3 at 313.15 K), acetonitrile (2.011 × 10–3 at 313.15 K), 1-butanol (6.17 × 10–4 at 313.15 K), isopropanol (5.80 × 10–4 at 313.15 K), n-propanol (5.25 × 10–4 at 313.15 K), ethanol (4.50 × 10–4 at 313.15 K), methanol (3.34 × 10–4 at 313.15 K), and toluene (2.91 × 10–4 at 313.15 K). The maximum values of relative average deviation (RAD) and root-mean-square deviation (RMSD) were 4.62% and 9.478 × 10–4, respectively, and were obtained in 2-butanone with the λh equation. Through the analysis of RAD and RMSD values, it was found that the calculated value of the modified Apelblat equation was closer to the experimental value. The solubility data obtained in the present study could be useful for optimizing the purification process of NTZ.

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Solubility and Thermodynamic Modeling of Sulfanilamide in 12 Mono Solvents and 4 Binary Solvent Mixtures from 278.15 to 318.15 K

Cited by 19 publications

References 43 publications

Solubility of Benzanilide Crystals in Organic Solvents

Solubility of Benzanilide Crystals in Organic Solvents

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

Solubility Determination of Nitazoxanide in Twelve Organic Solvents from T = 273.15 to 313.15 K

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