Convert normality (eq/L) to molarity (mol/L) with M = N / n. Presets assume complete acid-base neutralization; select a custom reaction factor for another endpoint or reaction.
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Normality to Molarity Formula
The following formula is used to convert normality to molarity.
Variables:
- M is the molarity in moles per liter
- N is the normality in equivalents per liter
- n is the reaction-specific number of equivalents per mole (eq/mol)
To calculate the molarity, divide the normality by the equivalent factor for the selected acid or base.
What is Normality to Molarity Conversion?
Normality to molarity conversion is used to translate a concentration from equivalents per liter into moles per liter. Normality depends on how many reactive equivalents one mole of a substance provides in a given reaction, while molarity simply measures the number of moles of solute per liter of solution. Because of this, the conversion depends on the solute’s n-factor.
For complete acid-base neutralization, HCl, HNO₃ and NaOH have n = 1; H₂SO₄ and Ca(OH)₂ have n = 2; H₃PO₄ and Al(OH)₃ have n = 3. Partial neutralization or another reaction can require a different factor. The conversion is stoichiometric and does not establish that a concentration is physically achievable or account for solubility.
How to Convert Normality to Molarity?
The following steps outline how to convert normality to molarity.
- First, determine the solution normality (N).
- Next, determine the correct equivalent factor (n-factor) for the acid or base.
- Finally, calculate the molarity using the formula M = N / n.
- After inserting the values and calculating the result, check your answer with the converter above.
Normality to Molarity Conversion Table
The table gives formal stoichiometric conversions from 1 eq/L for complete neutralization. Values for n = 3 are rounded; these examples do not assess solubility or describe a solution-preparation procedure.
| Solute | n-factor | 1 N in M |
|---|---|---|
| Hydrochloric Acid (HCl) | 1 | 1.00 M |
| Nitric Acid (HNO₃) | 1 | 1.00 M |
| Sodium Hydroxide (NaOH) | 1 | 1.00 M |
| Sulfuric Acid (H₂SO₄) | 2 | 0.50 M |
| Phosphoric Acid (H₃PO₄) | 3 | 0.33 M |
| Calcium Hydroxide (Ca(OH)₂) | 2 | 0.50 M |
| Aluminum Hydroxide (Al(OH)₃) | 3 | 0.33 M |
In laboratory work, some references report concentrations in normality while others use molarity. Knowing the correct n-factor for the solute makes it easy to convert between the two concentration units and compare values accurately.
Example Problem :
Use the following variables as an example problem to test your knowledge.
Normality (N) = 2
Solute = Sulfuric Acid (H₂SO₄)
Equivalent Factor (n) = 2
Molarity (M) = 1.0
