Ideal and non ideal solution and it's type

Here is a detailed and comprehensive description of Ideal and Non-Ideal solutions in English, keeping it simple and free of formulas or angle brackets. ​1. Ideal Solutions ​An Ideal Solution is a perfect mixture that strictly obeys Raoult's Law across all ranges of concentrations and temperatures. In simple terms, it is a solution where the component liquids behave exactly the same way after mixing as they did when they were pure. ​Key Characteristics: ​Identical Intermolecular Forces: Suppose you mix Liquid A and Liquid B. In an ideal solution, the attractive forces between the molecules of A and B (A-B interactions) are exactly equal to the forces that existed between A-A molecules and B-B molecules before mixing. No new behavior is introduced. ​No Change in Volume: If you mix 50 mL of Liquid A and 50 mL of Liquid B, the total volume of the resulting solution will be exactly 100 mL. The molecules do not pull closer together or push farther apart. ​No Heat Change (No Thermal Effects): When the two liquids are mixed, no heat is evolved or absorbed. The container will neither feel warm nor cold. The energy required to break old bonds is exactly equal to the energy released during the formation of new bonds. ​Examples: A mixture of Benzene and Toluene, or n-Hexane and n-Heptane. These pairs behave almost ideally because their molecular sizes and structures are very similar. ​2. Non-Ideal Solutions ​In reality, perfectly ideal solutions are rare. Most real-world mixtures are Non-Ideal Solutions. These solutions do not obey Raoult's Law. When Liquid A and Liquid B are mixed, their molecules interact differently than they did in their pure states, causing deviations in vapor pressure, volume, and temperature. ​Non-ideal solutions are classified into two categories based on how they deviate: ​A) Non-Ideal Solutions Showing Positive Deviation ​In this type of solution, the new attractive forces between A and B molecules after mixing are weaker than the original forces between the pure molecules (A-A and B-B). Because the molecules do not hold onto each other tightly, they escape into the air easily. ​Vapor Pressure: The total vapor pressure of the solution is higher than expected. ​Volume Change: Since the molecules repel or don't attract each other strongly, they stay slightly farther apart. As a result, the total volume increases (e.g., 50 mL + 50 mL becomes slightly more than 100 mL). ​Temperature Change: This process absorbs heat from the surroundings. Therefore, the mixing process is endothermic, and the solution becomes cold. ​Example: Ethanol and Acetone mixture. ​B) Non-Ideal Solutions Showing Negative Deviation ​In this type of solution, the new attractive forces between A and B molecules after mixing are stronger than the original forces in the pure liquids. The molecules cling to each other tightly, making it harder for them to escape as vapor. ​Vapor Pressure: The total vapor pressure of the solution is lower than expected. ​Volume Change: Because of the stronger grip between different molecules, they pull closer together. This causes the total volume to decrease (e.g., 50 mL + 50 mL becomes slightly less than 100 mL). ​Temperature Change: This process releases energy as new, stronger bonds are formed. The mixing process is exothermic, and the solution becomes warm. ​Example: Chloroform and Acetone mixture, or Water and Nitric Acid mixture. ​Quick Comparison Summary