Solubility of Minoxidil in Methanol, Ethanol, 1-Propanol, 2-Propanol, 1-Butanol, and Water from (278.15 to 333.15) K

Yan, Hao; Li, Runyan; Li, Qiang; Wang, Jingkang; Gong, Junbo

doi:10.1021/je1012839

Cited by 27 publications

(11 citation statements)

References 7 publications

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“…In this work, the solubility of dicarboxylic acids was measured by a static analytic method similar to that described in the literature. 36 A thermostatic bath (type 501A, Shanghai Laboratory Instrument Works Co., Ltd., China) was used to keep each temperature with an uncertainty of ±0.05 K. An excess amount of drugs and solvent was added in a specially designed sealed dual-wall flask, stirring for 18 h under a stable temperature to reach the equilibrium. 37 After that, the suspension was settled down for 2 h. Then, upper clear solution was taken by a syringe, filtered through a 0.2 μm filer and poured into a Petri dish, which was evaporated fully in a vacuum drying oven at 363.15 K. After being dried, each sample was reweighed every 30 min until the values were unaltered.…”

Section: Methodsmentioning

confidence: 99%

Identification and Molecular Understanding of the Odd–Even Effect of Dicarboxylic Acids Aqueous Solubility

Zhang

Xie

Liu

et al. 2013

Ind. Eng. Chem. Res.

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The solubilities of the homologous series of dicarboxylic acids, HOOC−(CH 2 ) n−2 −COOH (n = 2−10), in water have been measured at temperatures ranging from 288.15 to 323.15 K by a static analytic method at atmospheric pressure. Dicarboxylic acids with even numbers of carbon atoms exhibit lower solubilities than acids with adjacent odd carbon numbers. The odd−even effect of solubility is most likely associated with the twist of the molecules, which influences the molecular packing in the solid state: the molecules stack with some offset in the cases of even (n = even) series, but without offset in the cases of odd (n = odd) series, whereas the carboxyl groups are twisted in even members. The interlayer packing is looser in odd members than that in even ones. The energies of intramolecular torsion were calculated using Materials studio 6.0 (Accelrys Software Inc.). Finally, the molar Gibbs energies were predicted, which also showed odd−even alternation.

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Section: Methodsmentioning

confidence: 99%

Identification and Molecular Understanding of the Odd–Even Effect of Dicarboxylic Acids Aqueous Solubility

Zhang

Xie

Liu

et al. 2013

Ind. Eng. Chem. Res.

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“…Amidst, formic acid has shown the highest solubility of L-GA, which is attributed to the formation of strong intermolecular hydrogen bonding. Comparing the solubility in alcohols, the solubility increases as nonpolarity of the antisolvents increases except for the 2-propanol, due to the stearic congestion of 2propanol in dissolution of L-GA. 23 The dissolution of L-GA was more pronounced at higher temperatures in the case of 2propanol than acetonitrile. The acetonitrile has shown the linear temperature dependency on dissolution of L-GA, as it shows lower solubility at higher temperature than 2-propanol.…”

Section: Validation Of the Experimental Techniquementioning

confidence: 97%

Measurement and Modeling of Solid–Liquid Equilibria of l-Glutamic Acid in Pure Solvents and Aqueous Binary Mixtures

et al. 2019

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The experimental solubility data of L-glutamic acid in pure water, formic acid, methanol, 1-propanol, 2-propanol, acetonitrile, and binary mixtures (formic acid + water, methanol + water, 2-propanol + water, acetonitrile + water) with different compositions were carried out at temperatures ranging from (283.15 to 328.15) K by the static analytic method. The solubility measurements showed that formic acid and its aqueous mixtures recorded a higher solubility than methanol + water, 2-propanol + water, and acetonitrile + water for the same composition at each temperature. Moreover, except formic acid the addition of methanol, 2-propanol, and acetonitrile to its aqueous mixtures resulted in the decrease in solubility of L-glutamic acid. The experimental data was fitted using different thermodynamic models such as the Buchowski−Ksiazczak equation, the Van't Hoff equation, the modified Apelblat equation, and the NRTL model, and the optimum values of the regressed parameters were obtained. The modified Apelblat equation, Buchowski−Ksiazczak equation, and NRTL activity coefficient model were fitted to the pure solvents solubility data, while the modified Apelblat, modified Apelblat−Jouyban−Acree, and NRTL models were used for the binary solvent systems. The results demonstrated formic acid as a cosolvent in the dissolution of L-glutamic acid in formic acid + water binary mixtures, while others exhibited an antisolvent effect on the solubilization of L-glutamic acid in their respective aqueous mixtures.

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“…ji ij (10) where g ij − g jj represents the Gibbs energy of intermolecular interaction, α ij refers an adjustable empirical constant between 0 and 1, and τ is a criterion of the nonrandomness of the mixtures. The relative deviation (RD) was used as fitting degree between the calculated solubility data and the experimental data.…”

Section: Thermodynamic Modelsmentioning

confidence: 99%

“…As the driving force for the crystallization process, the supersaturation degree of cinnamyl alcohol is dependent on its solubility in different solvents, which is unfortunately not reported. We herein tested the solubility profiles of cinnamyl alcohol in 11 commonly applied solvents (methanol, ethanol, n -propanol, isopropyl alcohol, n -butyl alcohol, isobutyl alcohol, sec -butyl alcohol, acetone, methyl acetate, ethyl acetate, and n -hexane) and two kinds of binary solvents ( n -propanol + n -hexane, n -butyl alcohol + n -hexane) under atmospheric pressure at temperatures ranging from 253.15 K to 293.15 K. , The experimental data were then correlated by the Apelblat model, the λ h model and the nonrandom two-liquid (NRTL) model to calculate the solubility of CA under different conditions. In addition, the mixing thermodynamic properties (Δ mix H , Δ mix G , and Δ mix S ) of the two kinds of binary solvents were modeled by the NRTL function, which provided us a better understanding about the mixing behaviors of cinnamyl alcohol and the selected solvent.…”

Section: Introductionmentioning

confidence: 99%

Determination and Correlation of Solubility and Thermodynamic Properties of trans-Cinnamyl Alcohol in Pure and Binary Solvents from 253.15 K to 293.15 K

Wang

Zhu

et al. 2017

J. Chem. Eng. Data

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The solubility of cinnamyl alcohol in 11 pure solvents (methanol, ethanol, n-propanol, isopropyl alcohol, n-butyl alcohol, isobutyl alcohol, sec-butyl alcohol, acetone, methyl acetate, ethyl acetate and n-hexane) and two binary solvents of n-hexane + (n-propanol, n-butyl alcohol) was measured by a gravimetric method over temperatures from 253.15 K to 293.15 K at atmosphere pressure. From the experimental results, it was found that the solubility increased with the increasing temperature in all these solvents. The Apelblat model, the λh model, and the nonrandom two-liquid (NRTL) model were used to correlate the solubility data of cinnamyl alcohol in pure and mixed solvents. The thermodynamic properties of the mixing process in binary solvents were calculated by the NRTL model. The result indicates that the mixing process of cinnamyl alcohol is endothermic and spontaneous. The experimental solubility provides good guidance for the subsequent study of crystallization design and crystal morphology of cinnamyl alcohol.

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Solubility of Minoxidil in Methanol, Ethanol, 1-Propanol, 2-Propanol, 1-Butanol, and Water from (278.15 to 333.15) K

Cited by 27 publications

References 7 publications

Identification and Molecular Understanding of the Odd–Even Effect of Dicarboxylic Acids Aqueous Solubility

Identification and Molecular Understanding of the Odd–Even Effect of Dicarboxylic Acids Aqueous Solubility

Measurement and Modeling of Solid–Liquid Equilibria of l-Glutamic Acid in Pure Solvents and Aqueous Binary Mixtures

Determination and Correlation of Solubility and Thermodynamic Properties of trans-Cinnamyl Alcohol in Pure and Binary Solvents from 253.15 K to 293.15 K

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