Ideal and non ideal solution

On the basis of Raoult's law liquid-liquid solution can be classified into ideal solution and non ideal solution.

What are ideal solution?

• Ideal solution can be define as the type solution which obey Raoult's law over entire range of concentration are known as Ideal solution.

• In Ideal solution total pressure over solution in the container will be equal to the sum of the partial pressure of components of the solution.

p₁ = p_i1n₂    p₂ = p_i2n₂

p_total = p_i1 + (p_i2 - p_i1) n₂

Component A + Component B = Solution AB

• The force of attraction between ion on the Solution A-B are exact by same as force of attraction between A-A and B-B. [F_A-A = F_B-B = F_A-B].

• 

• On mixing there is no enthalpy and volume change.

ΔH_mix = 0  ΔV_mix = 0

Exmple of ideal solution: n-Hexane and n-Heptane Bromoethane and chloroethane and Benzene and

Tolesene.

What are non-ideal solution?

• Non ideal solution is a type of solution which does not obey Raoult's law over entire range of concentration, then it is called Non-ideal solution.

• In Non-ideal solution total pressure over solution in the container will be not equal to the sum of the partial pressure of components of the solution.

p₁ ≠ p_i1n₂    p₂ ≠ p_i2n₂

p_total ≠ p_i1 + (p_i2 - p_i1) n₂

Component A + Component B = Solution AB

• The force of attraction between ion on the Solution A-B are not exact by same as force of attraction between A-A and B-B. [F_A-A ≠ F_B-B ≠ F_A-B].

• Enthalpy and volume  both are change on mixing.

ΔH_mix ≠ 0  ΔV_mix ≠ 0

Example of non-ideal solution: H₂O and ethanol, H₂O and CH₃COOH, CHCL₃ and CCL₄