Molarity, Normality, And Relationship in between them

What Is Molarity?
Molarity is the most commonly used measure of concentration. It is expressed as the number of moles of solute per liter
of solution.
For example, a 1 M solution of H2SO4 contains 1 mole of H2SO4 per liter of solution. H2SO4 dissociates into H+ and
SO4- ions in water. For every mole of H2SO4 that dissociates in solution, 2 moles of H+ and 1 mole of SO4- ions are
formed. This is where normality is generally used.
What Is Normality?
Normality is a measure of concentration that is equal to the gram equivalent weight per liter of solution. Gram equivalent
weight is a measure of the reactive capacity of a molecule. The solution's role in the reaction determines the solution's
normality.
For acid reactions, a 1 M H2SO4 solution will have normality (N) of 2 N because 2 moles of H+ ions are present per liter
of solution. For sulfide precipitation reactions, where the SO4- ion is the most significant factor, the same 1 M H2SO4
solution will have a normality of 1 N.
Converting From Molarity to Normality
You can convert from molarity (M) to normality (N) using the following equation:
N = M*n, where n is the number of equivalents
Note that for some chemical species, N and M are the same (n is 1). The conversion only matters when ionization changes
the number of equivalents.