Assertion: A solution of phenol and aniline will show negative deviations from Raoult's law.Reason: In case of negative deviations from Raoult's law, A-B forces are stronger than A-A and B-B forcesA. Both assertion and reason are correct and reason is correct explanation for assertion.B. Both assertion and reason are correct and reason is not the correct explanation for assertion.C. Assertion is correct but reason is incorrect.D. Assertion as well as reason are both incorrect.

The correct answer is C. Assertion is correct but reason is incorrect.

Explanation:
Negative deviations from Raoult's law occur when the intermolecular forces between the components in the mixture are weaker than the forces between like molecules (A-A and B-B), leading to a higher vapor pressure than predicted by Raoult's law. In other words, the molecules in the mixture tend to escape the liquid phase more easily than predicted by their individual vapor pressures.

In the case of a solution of phenol and aniline, both molecules have similar types of intermolecular forces, specifically hydrogen bonding. Phenol has a hydroxyl (-OH) group that can form hydrogen bonds, and aniline has an amino (-NH2) group that can also form hydrogen bonds. These hydrogen bonds are relatively strong intermolecular forces.

The reason provided, stating that "In case of negative deviations from Raoult's law, A-B forces are stronger than A-A and B-B forces," is not accurate. Negative deviations occur due to the formation of strong intermolecular interactions (such as hydrogen bonding) between the components of the mixture. It's not about A-B forces being stronger than A-A and B-B forces.

Therefore, the assertion that a solution of phenol and aniline will show negative deviations from Raoult's law is correct, but the reason provided is not a correct explanation for the assertion.