The solubility of
aspirin in four binary solvents of ethanol + methyl cyclohexane, n-propanol + methyl cyclohexane, acetone + methyl cyclohexane,
and ethyl acetate + methyl cyclohexane was measured by the gravimetric
method at temperatures from T = 283.15 to 323.15
K. The solubility of aspirin in all mixed solvents increased with
the increase of temperature and decreased with the increase of the
mole fraction of methyl cyclohexane. The solubility data of aspirin
was correlated by the CNIBS/R–K model, Jouyban–Acree
model, and nonrandom two-liquid (NRTL) model. Also, the average relative
deviation (ARD) of all models was lower than 5%. The results indicated
that these models fit the solubility data well. Besides, the mixing
thermodynamic properties of aspirin in four binary solvent mixtures
were investigated on the basis of the solubility data and the NRTL
model. The results showed that the
mixing process of aspirin is a spontaneous process and follows the
increase of entropy principle.
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