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This page contains tables of azeotrope data for various binary and ternary mixtures of solvents. The data include the composition of a mixture by weight (in binary azeotropes, when only one fraction is given, it is the fraction of the second component), the boiling point (b.p.) of a component, the boiling point of a mixture, and the specific gravity of the mixture.
Vapor-liquid Equilibrium for Benzene/Ethanol [5] P = 760 mm Hg BP Temp. °C ... Vapor-liquid Equilibrium for Benzene/Acetone [5] P = 101.325 kPa BP Temp. °C
The ionization equilibrium of an acid or a base is affected by a solvent change. ... Benzene: 14.7 Ethanol: 5.8 Dichloromethane: 4.2 Water: 0.23 Effects on reaction rates
The best known example is adding benzene or cyclohexane to the water/ethanol azeotrope. With cyclohexane as the entrainer, the ternary azeotrope is 7% water, 17% ethanol, and 76% cyclohexane, and boils at 62.1 °C. [23] Just enough cyclohexane is added to the water/ethanol azeotrope to engage all of the water into the ternary azeotrope.
The addition of a material separation agent, such as benzene to an ethanol/water mixture, changes the molecular interactions and eliminates the azeotrope. Added in the liquid phase, the new component can alter the activity coefficient of various compounds in different ways thus altering a mixture's relative volatility.
An equilibrium of dissolved substance distributed between a hydrophobic phase and a hydrophilic phase is established in special glassware such as this separatory funnel that allows shaking and sampling, from which the log P is determined. Here, the green substance has a greater solubility in the lower layer than in the upper layer.
A particular problem in the area of liquid-state thermodynamics is the sourcing of reliable thermodynamic constants. These constants are necessary for the successful prediction of the free energy state of the system; without this information it is impossible to model the equilibrium phases of the system.
The Van Laar equation is a thermodynamic activity model, which was developed by Johannes van Laar in 1910-1913, to describe phase equilibria of liquid mixtures. The equation was derived from the Van der Waals equation.