NEET Chemistry Solution And Colligative Properties Revision Notes

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Solution And Colligative Properties Notes Full Course Solution and Colligative Properties

Type of Solutions

Vapour Pressure:

Raoult’s Law:

“The partial vapour pressure of any component in the solution is directly proportional to its mole fraction”.

For a binary solution of two components A and B,

P_A = X_A

P_B = X_B

Where

P⁰_A = vapour pressure of component A in pure state.

P_A = vapour pressure of component A in the solution.

P⁰_B = vapour pressure of component B in pure state.

P_B = vapour pressure of component B in the solution

Limitations of Raoult’s Law

• Raoult’s law is applicable only to very dilute solutions.

• It is applicable to solutions containing non-volatile solute only.

• It is not applicable to solutes which dissociate or associate in a particular solution

Raoult’s Law in Combination with Dalton’s Law of Partial Pressure:

P_T = X_A P⁰_A + X_B P⁰_B = P⁰_B + (P⁰_A -P⁰_B) X_A

Where

PT = Total Vapour Pressure of the Solution.

Ideal and Non-Ideal Solutions:

• Ideal Solution:

For Ideal Solution:

1. dH_mixing = 0, i.e. no heat should be absorbed or evolved during mixing

2. dV_mixing = 0, i.e. no expansion or contraction on mixing

Examples , Ethyl chloride and ethyl bromide, n–hexane and n–heptane , CCl₄ and SiCl₄

• Non-Ideal Solution:

?These solutions deviate from ideal behaviour and do not obey Raoult’s law over entire range of

composition.

For non ideal solutions,

1. dH_mixing ≠ 0

2. dH_mixing ≠ 0

Here we may have two cases

A) Positive Deviation:

1. P_A > X_A & P_B > X_B

2. dH_mix > 0

3. dV_mix > 0

Example: Cyclohexane and Ethanol

B) Negative Deviation:

1. P_A > X_A & P_B > X_B

2. dH_mix < 0

3. dV_mix < 0

Colligative Properties

Lowering of Vapour Pressure by a Non-Volatile Solute

Elevation of Boiling Point by a Non-Volatile Solute :

Depression of Freezing Point by a Non-Volatile Solute:

Osmosis and Osmotic Pressure:

• Osmosis: The phenomenon of the passage of pure solvent from a region of lower concentration

(of the solution) to a region of its higher concentration through a semi-permeable membrane.

• Osmotic Pressure: Excess pressure which must be applied to a solution in order to prevent flow of solvent into the solution through the semi-permeable membrane.

V = nRT

where

= Osmotic pressure

V = volume of solution

n = no. of moles of solute that is dissolved

R = Gas constant

T = Absolute temperature

Isotonic Solutions: A pair of solutions having same osomotic pressure is called isotonic solutions.

Abnormal Molecular Weight and Van't Hoff Factor:

Van't Hoff Factor:

Van't Hoff, in order to account for all abnormal cases introduced a factor i known as the Van't Hoff

factor, such that

Degree of Association:

Let a be the degree of association, then,

The number of unassociated moles = 1-α

The number of associated moles = α/n

Total number of effective moles = 1- α+ α /n

Obviously, i < 1

Degree of Dissociation

The fraction of the total number of molecules which dissociates in the solution, that is, breaks into simpler molecules or ions.

KCl ↔ K⁺ + Cl^-

1-α α α

Thus, the total number of moles after dissociation = 1-α + α+α = 1+α

Hence, i = (1+α )/1

i = 1+α = 1+ (2–1)

In general, i = 1+ (n–1) α,

Where, n = number of particles ( ions) formed after dissociation

From the above formula, it is clear that i > 1

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