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Binary Solid–Liquid Solubility Determination and Model Correlation of Quizalofop-p-ethyl in Different Pure Solvents

  • Zhudan Jin
    Zhudan Jin
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    More by Zhudan Jin
  • Cunbin Du
    Cunbin Du
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    More by Cunbin Du
  • Ruimei Dong
    Ruimei Dong
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    More by Ruimei Dong
  • Yi Xue
    Yi Xue
    Southeast University—Red Sun Research Center for Intelligent Industry, Nanjing 211189, P. R. C.
    More by Yi Xue
  • Bin Qiao
    Bin Qiao
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    More by Bin Qiao
  • Ying Zhang
    Ying Zhang
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    More by Ying Zhang
  • Tingting Ye
    Tingting Ye
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    More by Tingting Ye
  • , and 
  • Mingliang Wang*
    Mingliang Wang
    School of Chemistry and Chemical Engineering, Southeast University, Nanjing 211189, P. R. C.
    Southeast University—Red Sun Research Center for Intelligent Industry, Nanjing 211189, P. R. C.
    *E-mail: [email protected]
Cite this: J. Chem. Eng. Data 2019, 64, 4, 1611–1621
Publication Date (Web):March 21, 2019
https://doi.org/10.1021/acs.jced.8b01181
Copyright © 2019 American Chemical Society

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    Abstract

    Abstract Image

    The solid–liquid equilibrium for quizalofop-p-ethyl in 12 solvents (methanol, ethanol, 1-propanol, 2-propanol, 1-butanol, N,N-dimethylformamide (DMF), acetone, acetonitrile, ethyl acetate, 1,4-dioxane, toluene, and 1-hexane) was measured by using a static equilibrium method at temperatures T = 273.15–313.15 K under a pressure of 101.2 kPa. The results show that the solubility in those 12 monosolvents increases with increasing temperature. At a given temperature range, they gradually decrease in the following order: 1,4-dioxane > acetonitrile > DMF > toluene > acetone > ethyl acetate > 1-butanol > 1-propanol > 1-hexane > 2-propanol > ethanol > methanol. Moreover, a modified Apelblat model, λh model, Wilson model, and NRTL model were used to correlate the experiment values. Compared with the results of the above models, the calculated values provided good results with the experimental data. Consequently, the values of root-mean-square deviation (RMSD) and relative average deviation (RAD) were no more than 4.57 × 10–4 and 2.29%, respectively. Furthermore, the thermodynamic properties of quizalofop-p-ethyl in monosolvents were calculated. From the analysis results, the dissolution process of quizalofop-p-ethyl was a spontaneous and entropy-driven process. The experimental solubility and the models in this study could be helpful in the application in the field of purification and recrystallization.

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