Solubility of 2,2′,4,4′,6,6′-hexanitrostilbene in binary solvent of N,N-dimethylformamide and acetonitrile

Solubility data were measured for omeprazole sulfide in ethanol, 95 mass-% ethanol, ethyl acetate, isopropanol, methanol, acetone, n-butanol and n-propanol in the temperature range from 280.35 to 319.65 K by employing the gravimetric method. The solubilities increase with temperature and they are in good agreement with the calculated solubility of the modified Apelblat equation and the λh equation. The experimental solubility and correlation equation in this work can be used as essential data and model in the purification process of omeprazole sulfide. The thermodynamic properties of the solution process, including the Gibbs energy, enthalpy, and entropy were calculated using the van’t Hoff equation.

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Solubility of Omeprazole Sulfide in Different Solvents at the Range of 280.35–319.65 K

Synthesis of hollow ZnFe2O4/residual carbon from coal gasification fine slag composites for multiband electromagnetic wave absorption

The solubility of veramoss in n-butyl alcohol, ethanol, isopropanol, ethyl acetate, acetone, tetrahydrofuran, isoamyl alcohol, n-amyl alcohol, n-propyl alcohol, and DMF pure solvents and various {ethanol + water} mixtures at T = 283.15–333.15 K and atmospheric pressure was measured by using the dynamic method. The experiment solubility data showed that the solubility of veramoss increased with increasing temperature in all solvents selected and decreased with the rise of mole fraction of water in the binary solvent mixtures of {ethanol + water}. The modified van’t Hoff equation and the Apelblat model were successfully used to correlate the experimental solubility in pure solvents while the modified Apelblat model, the van’t Hoff equation, and the CNIBS/R model were applied to correlate the solubility in binary solvent mixtures, and all of the models provided good fitting to the data. Furthermore, the thermodynamic parameters (dissolving enthalpy, dissolving entropy, and Gibbs free energy) of veramoss in d...

Solubility and Thermodynamic Behavior of Veramoss in Different Pure Solvents and {Ethanol + Water} Mixtures from T = 283.15 to 333.15 K

The solubility of coenzyme Q10 in ethyl acetate, n-hexane, 1-butanol, 1-propanol, 2-propanol and ethanol in the temperature range 270.15–320.15 K, under atmospheric pressure, was measured by a gravimetric method and compared with the data predicted using the conductor like screening model for realistic solvation (COSMO-RS) method. The results show that the solubilities of coenzyme Q10 in the above solvents increase with temperature. The temperature dependences of predicted solubilities were consistent with the experimental data. The experimental data were correlated with the Apelblat equation. At the same temperature, the order of increasing solubility is ethyl acetate > n-hexane > 1-butanol > 1-propanol > 2-propanol > ethanol.

Solubility Measurements and Prediction of Coenzyme Q10 Solubility in Different Solvent Systems

The solubilities of 1,3,3-trinitroazetidine, TNAZ, in pure solvent and mixed solvents were measured using a synthetic method. The laser monitoring technique was used to determine the disappearance of the solid phase in a solid + liquid mixture. All data were measured at atmospheric pressure and temperatures ranging from (293.15 to 323.15) K. The effect of solvent composition and temperature on the solubility was discussed. The experimental data were correlated with an empirical equation.

Jin-Wei Hu

Papers

Solubility of 1,3,3-Trinitroazetidine in Ethanol + Water Systems from (293.15 K to 323.15 K)

Ultrasmall Co-Nip Embedded Into Lantern Shaped Composite Achieved by Coordination Confinement Chosphorization for Overall Water Splitting

Metal-organic framework derived Fe3C nanoparticles coupled single-atomic iron for boosting oxygen reduction reaction.

Unveiling the Relationship between Active Site and Performance of Nickel-Based Photocatalysis for Hydrogen Production

PdIr nanoparticles on NH2-functionalized dendritic mesoporous silica nanospheres for efficient dehydrogenation of formic acid