Question

Mention any two differences between ideal and non ideal solution.

Answer 1

Hint: In order to answer this question you need to recall the concept of Raoult’s law.
You should know that the mole fraction is directly proportional to its partial pressure.

Complete step by step answer:
Raulot’s law is a law of thermodynamics established by French chemist in 1887
Generally for a particular solution,
Raoult's law states that the vapor pressure of a solution is equal to the sum of the vapor pressures of each volatile component if it were purely multiplied by the mole fraction of that component in the solution. Raoult's law can be used to calculate the molecular mass of an unknown solute. In simple words it is stated as the relative lowering of vapor pressure of a dilute solution containing nonvolatile solute is equal to the mole fraction of solute in the solution.

Generally based on Raoult's law, liquid-liquid solutions can be of two types. They are
* Ideal solutions
* Non idea solutions

Let’s differentiate between ideal and non ideal solutions.

Ideal solution	Non ideal solution
Any solution which obeys Raoult’s law at all conditions of concentration and temperature is called the ideal solution	Any solution which does not explain Raoult’s law is called a non-ideal solution.
Basically, a solution where the interactions between all the molecules are identical is called an ideal solution	Non ideal solution is a solution that has differences between the molecules of different components in the solution.
The change in enthalpy when an ideal solution forms is approximately zero.	The change in enthalpy when a non ideal solution forms is either a positive or negative value.
The activity of each component is equal to its mole fraction under all conditions.	The activity of each component is not equal to its mole fraction under any conditions.
Generally, highly dilute solutions can behave as ideal solutions.	Concentrated solutions behave as non ideal solutions.

Note: You should know that Raoult’s law is generally applicable to solutions containing non-volatile solute only. It is not applicable to solutes which dissociate in the particular solution.