Important Definitions from "Volumetric Analysis" : HSEB Chemistry (Grade-XII)

1. MOLARITY (M)
The number of moles (gram molecular weight) of solute present in 1 litre of solution is known as molarity of solution and the solution prepared is known as molar solution.

2. DECIMOLAR SOLUTION (M/10)
A solution containing 1/10th mole of solute dissolved in one litre of solution is known as decimolar solution.

3. NORMALITY (N)
The number of gram equivalent of solute present in one litre of solution is known as normality of solution.

4. NORMALITY FACTOR (f)
The normality factor is defined as the ratio of actual weight of substance taken to the theoritical weight of substance to be taken.

5. TITRATION
The process of determining the strength of unknown solution by finding the exact volume of it required to react completely with given volume of standard solution is called titration. Titration can be classified into following types :
I) Acid-base or neutralization titration
II) Oxidation-reduction or redox titration
III) Precipitation titration
IV) Complexometric titration

6. END POINT
The stage during the titration which shows the completion of the reaction or shows that the reaction is just completed as indicated by indicator is known as end point.

7. EQUIVALENCE POINT (THEORITICAL END POINT)
The stage during the titration at which exactly equivalent amount of titrant is added to titrand to get end point is known as equivalence point. But in practice, small difference occurs between equivalent point and end point which is known as titration error.

8. ACIDITY OF BASE
The number of replacable hydroxyl ion present in one mole of base is called acidity of base.

9. BASICITY OF ACID
The number of replacable hydrogen ion present in one mole of acid is called basicity of acid.

10. REDOX TITRATION
A titration which involves the oxidation and reduction reaction i.e. redox reaction is called redox titration.