What is commonly assumed about mixing in an ideal solution?

In an ideal solution, it is commonly assumed that mixing does not result in a change in enthalpy. This is based on the definition of an ideal solution, where the interactions between different components are similar to the interactions between like molecules. As a result, when two substances mix, their enthalpic change is negligible, leading to the conclusion that the process is thermodynamically favorable and does not absorb or release significant energy.

This assumption arises from the ideal gas law principles carried over into solutions, reflecting that the energy of mixing is balanced—a result of similar intermolecular forces at play. Thus, the total energy of the system remains relatively constant, supporting the notion that mixing involves no significant enthalpy change.