Which of the following is true when components forming an ideal solution are mixed?

Options

A. `DeltaH_m=DeltaV_m=0`
B. `DeltaH_m gt DeltaV_m`
C. `DeltaH_m lt DeltaV_m`
D. `DeltaH_m=DeltaV_m=1`

Answer

To determine which statement is true when components forming an ideal solution are mixed, we need to analyze the characteristics of ideal solutions.

### Step-by-Step Solution:

1. **Understanding Ideal Solutions**:
An ideal solution is one where the interactions between the different components are similar to the interactions between the molecules of each component. This means that when they are mixed, there are no significant changes in energy or volume.

2. **Enthalpy Change (ΔH_mix)**:
For an ideal solution, the enthalpy change upon mixing (ΔH_mix) is zero. This indicates that no heat is absorbed or released during the mixing process. The intermolecular forces between the different components are similar to those in the pure components.

3. **Volume Change (ΔV_mix)**:
Similarly, the change in volume upon mixing (ΔV_mix) is also zero for an ideal solution. This means that the total volume of the solution after mixing is equal to the sum of the volumes of the individual components before mixing.

4. **Conclusion**:
Based on the characteristics of ideal solutions, we can conclude that both ΔH_mix = 0 and ΔV_mix = 0 when components forming an ideal solution are mixed. Therefore, the correct option is that both enthalpy change and volume change are zero.

### Final Answer:
The correct statement when components forming an ideal solution are mixed is:
- ΔH_mix = 0 and ΔV_mix = 0.