TY - JOUR
T1 - Solubility of Bis(salicylidene)-trans-1,2-cyclo-hexanediamine
T2 - Determination, Modeling, and Simulation Study
AU - Ni, Congjian
AU - Ma, Xiaoli
AU - Pang, Ziyuan
AU - Yang, Zhi
N1 - Publisher Copyright:
© 2024 American Chemical Society.
PY - 2024/11/14
Y1 - 2024/11/14
N2 - The solubility of bis(salicylidene)-trans-1,2-cyclohexanediamine (compound 1) in 12 pure solvents was determined by gravimetric analysis in the temperature range of 273.15 to 313.15 K. 1H NMR, 13C NMR, and high-resolution mass spectrometry characterized the structure of compound 1. The melting point and fusion enthalpy of compound 1 were obtained by TG-DSC. The molecular electrostatic potential quantified the electrostatic potential energy of the surface. The intermolecular interaction of compound 1 was described by Hirshfeld surface analysis. The order of solubility was tetrahydrofuran > dichloromethane > 1,2-dichloroethane > toluene > acetone > ethyl acetate > methyl acetate > acetonitrile > 1-propanol > ethanol > n-hexane > methanol. The KAT-LSER model demonstrated the influence of various factors between solvents and the solute on the solubility. Moreover, seven thermodynamic models were used to correlate the solubility data. The NRTL model was determined to be the most appropriate by comparing the average relative deviation and the root mean squared deviation. The findings of this study substantially support the isolation and crystallization of such compounds.
AB - The solubility of bis(salicylidene)-trans-1,2-cyclohexanediamine (compound 1) in 12 pure solvents was determined by gravimetric analysis in the temperature range of 273.15 to 313.15 K. 1H NMR, 13C NMR, and high-resolution mass spectrometry characterized the structure of compound 1. The melting point and fusion enthalpy of compound 1 were obtained by TG-DSC. The molecular electrostatic potential quantified the electrostatic potential energy of the surface. The intermolecular interaction of compound 1 was described by Hirshfeld surface analysis. The order of solubility was tetrahydrofuran > dichloromethane > 1,2-dichloroethane > toluene > acetone > ethyl acetate > methyl acetate > acetonitrile > 1-propanol > ethanol > n-hexane > methanol. The KAT-LSER model demonstrated the influence of various factors between solvents and the solute on the solubility. Moreover, seven thermodynamic models were used to correlate the solubility data. The NRTL model was determined to be the most appropriate by comparing the average relative deviation and the root mean squared deviation. The findings of this study substantially support the isolation and crystallization of such compounds.
UR - http://www.scopus.com/inward/record.url?scp=85207626070&partnerID=8YFLogxK
U2 - 10.1021/acs.jced.4c00384
DO - 10.1021/acs.jced.4c00384
M3 - Article
AN - SCOPUS:85207626070
SN - 0021-9568
VL - 69
SP - 4127
EP - 4137
JO - Journal of Chemical and Engineering Data
JF - Journal of Chemical and Engineering Data
IS - 11
ER -