The
solubility of 5,5-dimethylhydantoin (DMH) in 12 pure solvents
including water, methanol, ethanol, 1-propanol, isopropyl alcohol,
1-butanol, isobutyl alcohol, 2-butanol, 1-pentanol, ethyl acetate,
propyl acetate, and acetonitrile was measured at temperatures from
283.15 to 323.15 K under atmospheric pressure by a gravimetric method.
The values of the mole fraction solubility of DMH in these solvents
increase with increasing temperature and present the following order
at a fixed temperature: methanol > ethanol > 2-butanol >
isopropyl
alcohol > 1-propanol > isobutyl alcohol (1-butanol) > 1-pentanol
>
water > acetonitrile > ethyl acetate > propyl acetate. They
were mathematically
correlated by the modified Apelblat equation, van’t Hoff equation,
λh equation, and the Wilson model. The results showed a satisfactory
correlation for each model.
The
solid–liquid equilibrium solubility of isatoic anhydride
in 12 pure solvents (methanol, ethanol, 1-propanol, isopropyl alcohol,
methyl acetate, ethyl acetate, propyl acetate, isopropyl acetate,
acetone, 2-butanone, acetonitrile, and 1,4-dioxane) at T = 288.15 to 328.15 K was measured by the gravimetric method under
atmospheric pressure. Experimental results demonstrate that the mole
fraction solubility of isatoic anhydride in these selected solvents
increased with the increase of temperature, and the dissolution behavior
is affected by multiple factors like polarity, H-bond interaction,
cohesive energy density, etc. The modified Apelblat model, the van’t
Hoff model, the nonrandom two-liquid model, and the λh model were used to correlate the experimental solubility
data. The maximum values of the relative average deviation and root-mean-square
deviation were no more than 4.23 × 10–2 and
5.31 × 10–4, respectively. Furthermore, the
thermodynamic properties including the mixing Gibbs energy, mixing
enthalpy, and mixing entropy were calculated, which indicates that
the dissolution of isatoic anhydride was a spontaneous and entropy-favorable
process.
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