Measurement and Correlation of Solubilities of 4-Amino-3,6-dichloropyridazine in Ethanol + Water Mixtures from (303.15 to 323.15) K

Wang³

et al. 2014

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The solid−liquid equilibria of 4-amino-3,6-dichloropyridazine (ADCP) in seven pure organic solvents including methanol, acetone, ethanol, dichloromethane, ethyl acetate, 1,4-dioxane, and tetrahydrofuran were determined with the synthetic method from (278.15 to 333.15) K at atmospheric pressure using a laser monitoring observation technique. The measured solubility data increased with the rise of temperature. These solubility data were correlated with two models: the modified Apelblat and λh (Buchowski) equation. The relative deviation of the modified Apelblat equation was no more than 2.1 %, while that of λh equation was less than 4.5 %. Better correlation results were obtained in most solvents with modified Apelblat equation. Furthermore, using van't Hoff plot, the calculation was performed to obtain the apparent dissolution enthalpy and entropy of the solution of ADCP in these solvents, based on which the apparent dissolution Gibbs free energy change was deduced.

“…The solubility of urea in water was measured and the result showed great agreement with reported values . The results had been published in our previous work …”

Section: Resultssupporting

confidence: 83%

Section: Introductionmentioning

confidence: 99%

Section: ■ Introductionmentioning

confidence: 99%

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4-Amino-3,6-dichloropyridazine Solubility Measurement and Correlation in Seven Pure Organic Solvents from (278.15 to 333.15) K

Wang³

et al. 2014

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“…The solubility of 2-oxindole in different solvents was measured with the synthetic method, which has been described in detail previously. ,,− A brief description follows. There are five parts in our solubility measurement system: a thermostat (to establish a constant temperature), a jacketed glass vessel (50 mL), a magnetic stirrer (to accelerate the dissolution process), a thermometer (to measure the inner temperature, ±0.05 K), and a laser beam system (to monitor the dissolution process).…”

Section: Experimental Partmentioning

confidence: 99%

Solubility Measurement and Correlation of 2-Oxindole in 12 Pure Organic Solvents

Ji²,

Gao

et al. 2019

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The solubilities of 2-oxindole in 12 pure organic solvents including acetonitrile (MeCN), dichloromethane, 1,4-dioxane, ethyl acetate (EtOAc), acetone, toluene, methanol, ethanol, 2-propanol, tetrahydrofuran, 1-butanol, and 1-propanol were experimentally measured from (283.15 to 358.15) K at normal pressure p = 0.1 MPa by employing the synthetic method. The measured solubilities of 2-oxindole in these pure organic solvents were found to increase with the rise of temperature. The experimental solubilities of 2-oxindole were correlated with several thermodynamic models including the modified Apelblat equation, λh (Buchowski) equation, Wilson equation, and nonrandom two-liquid equation. These data could be applied for the large-scale synthesis of 2-oxindole with high purity.

“…The synthetic method is employed to measure the solubility of isatin. Our co-workers have described the detailed procedure previously − and we made little improvement in this study. Following is a concise description.…”

Section: Experimental Partmentioning

confidence: 99%

Solubility and Thermodynamic Functions of Isatin in Pure Solvents

Chen

2014

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The solubility of isatin in eight pure solvents including dichloromethane, toluene, acetone, ethyl acetate, 1,4-dioxane, N,N-dimethylformamide, tetrahydrofuran, and acetonitrile were determined from (278.15 to 333.15) K at atmospheric pressure using the synthetic method. The solubility was determined by a laser monitoring observation technique and found to increase with the rise of temperature. The experimental solubilities were correlated by four models including the ideal solution model, the modified Apelblat equation, λh (Buchowski) equation, and Wilson models with the overall average percentage deviations less than 0.52% in all cases. Thermodynamic functions of the solution of isatin in these solvents including apparent standard enthalpy and entropy of solution were obtained by van’t Hoff plot, and the apparent standard Gibbs energy change of solution was also calculated.