Which of the following is true for ideal solution :-

Options

A. `Delta H_(("mix"))=0`
B. `Delta S_(("mix"))=0`
C. `Delta G_(("mix"))=0`
D. `Delta A_(("mix"))=0`

Answer

To determine which statement is true for an ideal solution, we need to analyze the properties of ideal solutions. Here’s a step-by-step breakdown:

### Step 1: Understand the Characteristics of Ideal Solutions
An ideal solution is one that follows Raoult's Law throughout its composition. This means that the interactions between the molecules of the different components are similar to the interactions between the molecules of the same component.

### Step 2: Evaluate the Given Options
The options provided are:
1. ΔH_mix = 0
2. ΔS_mix = 0
3. ΔG_mix = 0
4. ΔA_mix = 0

### Step 3: Analyze Each Option
- **ΔH_mix = 0**: This indicates that there is no heat absorbed or released during the mixing of the two components. This is a characteristic of ideal solutions, as the enthalpy change upon mixing is zero.

- **ΔS_mix = 0**: This would imply that there is no change in entropy when the two components are mixed. However, for an ideal solution, there is typically an increase in entropy due to the mixing of different molecules, so this statement is not true.

- **ΔG_mix = 0**: This would mean that there is no change in Gibbs free energy upon mixing, which is not the case for ideal solutions. The Gibbs free energy change is generally negative for mixing, indicating spontaneity.

- **ΔA_mix = 0**: This refers to the Helmholtz free energy change, which is also not zero for mixing in ideal solutions.

### Step 4: Conclusion
From the analysis, the only statement that holds true for an ideal solution is:
**ΔH_mix = 0**.

### Final Answer
The correct answer is: **ΔH_mix = 0**.

---