Which of the following is correct for an ideal solution? 

Ideal solutions are those that follow Raoult's law across the entire range of concentrations. This means that the partial vapor pressure of each component in the solution is directly proportional to its mole fraction. If you're wondering, "which of the following is an example of ideal solution", common examples include mixtures like benzene and toluene or hexane and heptane.

Key Properties of Ideal Solutions

• Enthalpy of Mixing: The enthalpy change during the mixing of pure components to form the solution is zero (ΔHmix = 0).
• Volume of Mixing: The volume change upon mixing is also zero (ΔVmix = 0).
• Gibbs Free Energy of Mixing: The Gibbs free energy change during mixing is always negative, ensuring that the process is spontaneous.
• Change in Entropy: The entropy of the system increases upon mixing, which is a hallmark of spontaneous processes.

A common question students ask is, "which of the following is an example of ideal solution?" Ideal solutions typically consist of components with similar molecular sizes and intermolecular forces. Examples include pairs like ethanol and methanol or n-hexane and n-heptane.

Why Do Ideal Solutions Follow These Properties?

Ideal solutions exhibit no significant interactions beyond those present in the pure components. This results in no heat being absorbed or released during mixing, and no expansion or contraction occurs. If you are analyzing experimental data and want to identify "which of the following is an example of ideal solution", look for mixtures where these principles hold true.