For an ideal solution of two components A & B, which of the following is true?

For an ideal solution of two components A and B, we need to determine which statement is true among the given options. Let's recall the definition of an ideal solution.

An ideal solution is one where the intermolecular forces between the different components are identical to the intermolecular forces within the same components. This means that the A-B interactions (between molecules of A and B) are equal in strength to the A-A interactions (between molecules of A) and the B-B interactions (between molecules of B).

Now, consider the enthalpy change during mixing, denoted as $$\Delta H_{\text{mixing}}$$. Enthalpy change is related to the energy changes in breaking and forming intermolecular bonds. In an ideal solution, since the A-B interactions are the same as A-A and B-B interactions, there is no net energy change when the components mix. Breaking some A-A and B-B bonds requires energy, but forming A-B bonds releases the same amount of energy. Therefore, the net enthalpy change is zero:

$$\Delta H_{\text{mixing}} = 0$$

Now, let's evaluate each option:

Option A states: $$\Delta H_{\text{mixing}} > 0$$ (zero). This means the enthalpy of mixing is greater than zero, implying an endothermic process. However, for an ideal solution, $$\Delta H_{\text{mixing}} = 0$$, not greater than zero. So, this option is incorrect.

Option B states: A-B interaction is stronger than A-A and B-B interactions. If A-B interactions were stronger, then forming A-B bonds would release more energy than breaking A-A and B-B bonds requires. This would make $$\Delta H_{\text{mixing}} < 0$$ (negative). But in an ideal solution, $$\Delta H_{\text{mixing}} = 0$$, so the interactions must be equal, not stronger. Thus, this option is false.

Option C states: A-A, B-B, and A-B interactions are identical. This means the strength of the interactions between A-A, B-B, and A-B are the same. This aligns perfectly with the definition of an ideal solution, where the intermolecular forces are uniform. Therefore, this option is correct.

Option D states: $$\Delta H_{\text{mixing}} < 0$$ (zero). This means the enthalpy of mixing is less than zero, implying an exothermic process. However, for an ideal solution, $$\Delta H_{\text{mixing}} = 0$$, not less than zero. So, this option is incorrect.

Hence, the correct answer is Option C.