Molarity to Normality Converter

Convert Molarity (M) to Normality (N) by entering the molarity and the equivalence factor (n).

Molarity (M)

Equivalence Factor (n)

Result

--- N

Molarity vs. Normality

Molarity (M) is the number of moles of solute per liter of solution. It is the most common unit of concentration in chemistry.

Normality (N) is the number of gram-equivalent weights of solute per liter of solution. It is often used in acid-base titrations and redox reactions where the focus is on the equivalents of reactive species.

Conversion Formula

Normality (N) = Molarity (M) × n

Where n is the equivalence factor (or valence factor), which depends on the reaction type:

For acids: n = number of replaceable H⁺ ions (e.g., HCl -> 1, H₂SO₄ -> 2).
For bases: n = number of replaceable OH^- ions (e.g., NaOH -> 1, Ca(OH)₂ -> 2).
For redox reactions: n = number of electrons transferred per molecule.

Example

To find the normality of 0.5 M H₂SO₄:

Since H₂SO₄ can donate 2 protons (H⁺), n = 2.

N = 0.5 M × 2 = 1.0 N

Quick FAQs

Is Normality always greater than or equal to Molarity?

Yes, because the equivalence factor (n) is always an integer greater than or equal to 1.

When should I use Normality instead of Molarity?

Normality is particularly useful in titration calculations, as 1 equivalent of any acid will react exactly with 1 equivalent of any base (N1V1 = N2V2).

Does Normality change with temperature?

Yes, like Molarity, Normality is volume-dependent. Since volume changes with temperature, the concentration also changes slightly.