The solubility of 2-cyanoacetamide (2-CA) was ascertained
by means
of a gravimetric technique in four different kinds of aqueous mixed
solvents, specifically water + (methanol (MeOH), ethanol (EtOH), 1-propanol
(1-PrOH), or 2-propanol (2-PrOH)). The experiment was conducted between
283.15 and 323.15 K in temperature. The findings show that in all
four binary solvent systems, 2-CA becomes more soluble at higher temperatures.
The KAT-LSER model was employed to analyze the impact of solute–solvent
intermolecular interactions on solubility. In order to simulate the
solubility of 2-CA in binary mixed solvents, three thermodynamic models
were used. The low values for the average relative deviation (RAD%)
(≤1.23, ≤2.20, and ≤3.68) show that the experimental
solubility data for 2-CA in the four binary solvent mixtures exhibit
strong agreement with the correlated data utilizing the Jouyban–Acree,
Jouyban–Acree–van’t Hoff, and Apelblat–Jouyban–Acree
models. The thermodynamic properties of the solution were used to
calculate the special solvation variables by the use of inverse Kirkwood–Buff
integrals. The preferential solvation variables for MeOH/EtOH/1-PrOH/2-PrOH
displayed negative values in the MeOH (1) + water (2) mixture, within
the range of 0.31 < x
1 < 1, for
the EtOH (1) + water (2) mixture with compositions falling between
0.24 < x
1 < 1, for the 1-PrOH (1)
+ water (2) mixture with compositions within 0.20 < x
1 < 1, and for the 2-PrOH (1) + water (2) mixture within
the range of 0.20 < x
1 < 1. This
suggests that while alcohol preferentially solvates water molecules
in surroundings rich in alcohol, alcohol molecules preferentially
solvate 2-CA in mixes rich in water.