When a solution of `CHCl_(3)` is mixed with a solution of `O = C(CH_(3))_(2),DeltaV_(mix)` is

Options

A. Positive
B. Negative
C. Zero
D. Can't be predicted

Answer

To solve the question regarding the volume change (ΔV_mix) when a solution of chloroform (CHCl₃) is mixed with a solution of acetone (O=C(CH₃)₂), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Components**: We have two components in this mixture: chloroform (CHCl₃) and acetone (O=C(CH₃)₂).

2. **Understand the Interaction**: When these two solutions are mixed, they can form hydrogen bonds. Although chloroform does not typically participate in hydrogen bonding due to its structure, the presence of highly electronegative chlorine atoms influences its behavior. The hydrogen atom in chloroform can interact with the oxygen atom in acetone, leading to hydrogen bonding.

3. **Consider the Effect of Hydrogen Bonding**: The formation of hydrogen bonds between chloroform and acetone means that the molecules are more strongly associated in the solution than they are in their pure states. This results in a decrease in the volume of the mixture compared to the sum of the volumes of the individual components.

4. **Apply Raoult's Law**: According to Raoult's Law, the vapor pressure of a solution is directly related to the mole fraction of the components. In this case, the presence of hydrogen bonding leads to a lower vapor pressure than expected, indicating a negative deviation from Raoult's Law.

5. **Determine the Sign of ΔV_mix**: Since the interaction between the two components leads to a more stable solution (due to hydrogen bonding), the overall volume change (ΔV_mix) will be negative. This means that the volume of the mixture is less than the sum of the volumes of the individual components.

6. **Conclusion**: Therefore, the volume change upon mixing, ΔV_mix, is negative.

### Final Answer:
ΔV_mix < 0 (Negative deviation)