A solution of `CHCl_3 ​ +CH3 ​ COCH3` shows negative deviation from Raoults law.

Explanation

To solve the question regarding the solution of CHCl₃ (chloroform) and CH₃COCH₃ (acetone) showing negative deviation from Raoult's law, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Raoult's Law**:
Raoult's law states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent in the solution. It can be expressed as:
\[ P_{solution} = X_{solvent} \cdot P^0_{solvent} \]
where \( P_{solution} \) is the vapor pressure of the solution, \( X_{solvent} \) is the mole fraction of the solvent, and \( P^0_{solvent} \) is the vapor pressure of the pure solvent.

2. **Identifying the Components**:
In this case, the components of the solution are chloroform (CHCl₃) and acetone (CH₃COCH₃).

3. **Analyzing the Interaction**:
When chloroform and acetone are mixed, they interact with each other. Specifically, acetone can form hydrogen bonds with chloroform. This interaction leads to an increase in intermolecular forces between the molecules.

4. **Effect on Vapor Pressure**:
The formation of hydrogen bonds between chloroform and acetone results in stronger intermolecular attractions compared to the attractions in the pure components. As a result, the molecules are held more tightly together, which reduces the tendency of the molecules to escape into the vapor phase.

5. **Conclusion on Deviation**:
Due to the increased intermolecular attraction, the vapor pressure of the solution is lower than what would be predicted by Raoult's law. This is termed a negative deviation from Raoult's law.

6. **Final Statement**:
Therefore, the statement that a solution of CHCl₃ and CH₃COCH₃ shows negative deviation from Raoult's law is true.