**Relationship between Normality and Molarity**

Molarity and normality are two important concepts in chemistry that are used to express the concentration of a solution. While molarity is based on the number of moles of solute per liter of solution, normality is based on the number of equivalents of solute per liter of solution. Let's understand the relationship between these two concepts in detail.

**Molarity (M)**:
Molarity, also known as molar concentration, is defined as the number of moles of solute present in one liter of solution. It is expressed in moles per liter (mol/L or M).

Mathematically, molarity can be calculated using the formula:
Molarity (M) = Moles of solute / Volume of solution (in liters)

For example, if we dissolve 0.1 moles of sodium chloride (NaCl) in 1 liter of water, the molarity of the solution would be 0.1 M.

**Normality (N)**:
Normality is a measure of concentration that takes into account the chemical reactivity of a solute. It is defined as the number of equivalents of solute present in one liter of solution. An equivalent is the amount of solute that can donate or accept one mole of electrons.

Mathematically, normality can be calculated using the formula:
Normality (N) = Equivalents of solute / Volume of solution (in liters)

The number of equivalents of a solute depends on the reaction it undergoes. For example, in an acid-base reaction, the number of equivalents is equal to the number of moles of hydrogen ions (H+) or hydroxide ions (OH-) produced or consumed by one mole of the acid or base.

**Relationship between Molarity and Normality**:
The relationship between molarity and normality depends on the reaction stoichiometry. In most cases, the molarity and normality of a solution are equivalent, meaning that one mole of solute is equivalent to one liter of solution.

However, in certain reactions where multiple ions are involved, the molarity and normality may not be equal. In such cases, the normality can be calculated by multiplying the molarity by the reaction stoichiometry.

For example, if we have a solution of sulfuric acid (H2SO4) with a molarity of 0.1 M, the normality would be 0.2 N because each mole of sulfuric acid produces 2 moles of hydrogen ions (H+).

In summary, molarity and normality are related concepts that express the concentration of a solution. While molarity is based on the number of moles of solute per liter of solution, normality takes into account the chemical reactivity of the solute and is based on the number of equivalents per liter of solution. The relationship between molarity and normality depends on the reaction stoichiometry and can be calculated using appropriate conversion factors.

N = n × M where n = H+ and OH- ions