CHAPTER 2-SOLUTION

SOLUTION

A solution is a homogeneous mixture of two or more substance whose composition can be varied within certain limits.

SOLVENT AND SOLUTE

A component which is present in the largest quantity in a solution is called a solvent and the component which is present in the lesser quantity is known as solute

TYPES OF SOLUTION 

Depending on the physical state of solute and solvent solution can be classified into 9 types

TYPES OF SOLUTION	SOLUTE	SOLVENT	EXAMPLE
Gaseous	Gas	Gas	O2(g)+N2(g)
	Liquid	Gas	CHCl3 + N2(g)
	Solid	Gas	Camphor + N2(g)
Liquid	Gas	Liquid	O2(g)+ H2o(l)
	Liquid	Liquid	Ethanol+ H2o(l)
	Solid	Liquid	Glucose + H2o(l)
Solid	Gas	Solid	H(aq) +palladium
	Liquid	Solid	Amalgam +mercury
	Solid	Solid	Copper + gold

EXPRESSNG THE CONCENTRATION

MASS % (w/w)

It is the mass of the component in 100g of the solution.

VOLUME % (v/v)

It is represented as the volume of component per 100 parts of solution by volume.

MASS BY VOLUME % (w/v)

It is the mass of solute dissolved in 100 ml of the solution.

PARTS PER MILLION (ppm)

It is the parts of the component per million parts of the solution.

1 liter of the sea water contains 6 X 10^-3g of dissolved oxygen which is equal to 5.8ppm.

MOLARITY (M)

The no of the mole of the solute dissolved per liter of solution.

Molarity changes with change in temperature because volume changes with change in temperature. This is why molality is preferred rather than molarity for expressing the concentration.

MOLALITY (m)

The no of the moles of the solute dissolved per 1kg of the solvent.

MOLE FRACTION

It is the ratio of number of moles of a component to the total no of moles of all components present in the solution.