Question

A solution is formed by mixing chloroform (CHCl3) and acetone (CH3COCH3).
Which of the following is true regarding the nature of this solution?

• A. It shows positive deviation from Raoult’s law due to weak intermolecular forces
• B. It shows negative deviation due to strong dipole-dipole interactions
• C. It obeys Raoult’s law over the entire range of composition
• D. It forms an ideal solution with no enthalpy change

Hint:

In solutions with strong dipole-dipole interactions, expect a negative deviation from Raoult's law, where the solution exhibits a lower vapor pressure than predicted.

Answer 1

The Correct Option is B

Mixing chloroform (CHCl3) and acetone (CH3COCH3) results in intermolecular forces between the mixture's molecules that are stronger than those within the individual components. Consequently, the solution exhibits a negative deviation from Raoult’s law. In solutions where dipole-dipole interactions are substantial, a negative deviation from Raoult’s law occurs, indicating that the solution's vapor pressure is lower than predicted by the mole fractions of the individual components. This phenomenon arises because the intermolecular interactions between the solute and solvent are more potent than those present in the pure substances.