1. Characteristics, Types, Colligative properties
Solution:
Characteristics, Types,
Colligative properties
Dr. N.K. Shukla
Associate Professor
Mahatma Gandhi P.G. College
Gorakhpur

2. Solution
A solution is a homogeneous mixture of two or more substances. A solution may exist in any phase.
A solution consists of a solute and a solvent.
The solute is the substance that is dissolved in the solvent.
The amount of solute that can be dissolved in solvent is called its solubility.
For example, in a saline solution, salt is the solute dissolved in water as the solvent.
For solutions with components in the same phase, the substances present in lower concentration are solutes, while the substance present in highest abundance is the solvent.
A dilute solution has a low concentration of the solute compared to the solvent. The opposite of a dilute solution is a concentrated solution, which has high levels of solute in the mixture.

3. Ideal Solution
An ideal solution or ideal mixture is a solution in which the enthalpy of solution (ΔHsolution=0) is zero; with the closer to zero the enthalpy of solution, the more "ideal" the behavior of the solution becomes.
The vapor pressure of the solution obeys Raoult's law, and the activity coefficient of each component (which measures deviation from ideality) is equal to one.

4. Characteristics of a Solution
A chemical solution exhibits several properties:
A solution consists of a homogeneous mixture.
A solution is composed of one phase (e.g., solid, liquid, gas).
Particles in a solution are not visible to the naked eye.
A solution does not scatter a light beam.
Components of a solution cannot be separated using simple mechanical filtration.

5. Hydrogen Gas In Palladium Metal Mercury Dental Amalgam
Types of Solution
Solution Type
Example
Gas-gas
Air
Gas-liquid
Carbon Dioxide In Soda
Gas-solid
Hydrogen Gas In Palladium Metal
Liquid-liquid
Gasoline
Solid-liquid
Sugar In Water
Liquid-solid
Mercury Dental Amalgam
Solid-solid
Sterling Silver

6. Units of Concentration
Percent volume
% volume = volume solute (ml) x 100
volume solution (ml)
Percent mass
% mass = mass solute (g) x 100
mass solution (g)
Solution = solvent + solute

7. Measures of Concentration
s = solute ; A = solvent; V = Tot. Vol. of solution.
Weight %:
Mole Fraction:
Molarity:
Molality:
Different Composition Equations for different Laws

8. Colligative Properties
Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions, but not upon the identity of the solute.
Colligative properties include: 
vapor pressure lowering, 
boiling point elevation, 
freezing point depression,
and osmotic pressure.

9. Colligative Properties
Elevation in Boiling-Point : Molal boiling-point-elevation constant, Kb, expresses how much Tb changes with molality, mS:
Decrease in freezing point (Tf) is directly proportional to molality (Kf is the molal freezing-point-depression constant):

11. Freezing Point Depression ( T vs. conc’n )
Kf = molal freezing point constant, all properties of the solvent A [ units = K kg mol-1 ]
Similar equation for Tb

12. Colligative Properties
Osmosis
movement of a solvent from low solute concentration to high solute concentration across a semipermeable membrane.

13. Colligative Properties
Osmosis
Osmotic pressure, , is the pressure required to stop osmosis:

14. References Physical Chemistry- P.W. Atkins
Physical Chemistry- B.S. Bahl, A. Bahl & G.D. Tuli
Essentials of Physical Chemistry- Pui, Sharma & Pathania