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When chloroform and acetone are mixed, they form a non-ideal solution. Which of the following statements correctly describes this mixture?

Options

  1. AThe intermolecular attractive forces between chloroform and acetone are stronger than those in the pure liquid
  2. BThe intermolecular attractive forces between chloroform and acetone are weaker than those in the pure liquids,
  3. CThe mixture exhibits a positive deviation from Raoult's law, and _ mix H > 0 .
  4. DThe intermolecular attractive forces remain unchanged upon mixing, and _ mix V = 0 .

Correct answer

A. The intermolecular attractive forces between chloroform and acetone are stronger than those in the pure liquid

Step-by-step solution

When chloroform and acetone are mixed, a hydrogen bond is formed between the hydrogen atom of chloroform and the oxygen atom of acetone. This new intermolecular interaction (solute-solvent) is stronger than the interactions present in the pure liquids (solute-solute and solvent-solvent). As a result, the escaping tendency of the molecules decreases, leading to a lower vapour pressure than expected from Raoult's law. This is termed a negative deviation. For solutions showing a negative deviation from Raoult's law, t

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