When non-ideal solution was prepared by mixing 30 mL chloroform and 50 mL acetone. The volume of mixture will be

Options

A. `gt 80` ml
B. `lt 80` ml
C. = 80 ml
D. `ge 80` ml

Answer

To solve the problem of determining the volume of a non-ideal solution formed by mixing 30 mL of chloroform and 50 mL of acetone, we can follow these steps:

### Step 1: Understand the Components
Identify the components being mixed:
- Chloroform (A) = 30 mL
- Acetone (B) = 50 mL

### Step 2: Calculate the Total Volume
Calculate the expected total volume if there were no interactions between the components:
\[ \text{Total Volume} = \text{Volume of Chloroform} + \text{Volume of Acetone} = 30 \, \text{mL} + 50 \, \text{mL} = 80 \, \text{mL} \]

### Step 3: Consider Non-Ideal Behavior
Since the solution is described as non-ideal, we need to consider the effects of negative deviation from Raoult's law. In a non-ideal solution, the interactions between different molecules (AB) are stronger than the interactions between like molecules (AA and BB). This results in a volume contraction.

### Step 4: Determine the Volume Change
In the case of negative deviation, the volume of the mixture (V_mixture) will be less than the expected total volume:
\[ \Delta V = V_mixture - \text{Total Volume} \]
Since we know that the volume of the mixture is less than the total volume, we can express this as:
\[ V_mixture < 80 \, \text{mL} \]

### Step 5: Conclusion
Although we cannot determine the exact volume without experimental data, we can conclude that the volume of the mixture will be less than 80 mL due to the negative deviation.

### Final Answer
The volume of the mixture will be less than 80 mL.

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