Understanding the conversion between normality (N) and molarity (M) is essential for accurate chemical calculations. Normality measures the concentration of equivalents, while molarity measures the concentration of moles per liter. This distinction is crucial in various chemical applications, such as titrations and reaction stoichiometry.

### Definition and Relationship

Normality and molarity are related through the equivalent factor, which depends on the chemical reaction. Normality is the number of equivalents of a solute per liter of solution, while molarity is the number of moles of solute per liter of solution. To convert normality to molarity, divide normality by the equivalent factor.

### Conversion Formula

The conversion formula is M = N / n, where n is the number of equivalents per mole of solute. For example, for a diprotic acid like sulfuric acid (H2SO4), n equals 2. Hence, if the normality of the sulfuric acid solution is 2 N, the molarity would be 1 M.

### Practical Applications

Understanding this conversion is crucial for accurate chemical preparation and reactions. It ensures that the concentration used in calculations aligns with the actual chemical behavior, particularly in reactions involving multiple equivalents.

In summary, the conversion between normality and molarity is vital for precise chemical work. By understanding and applying the correct conversion formulas, accurate measurements and reactions can be achieved.