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Normality to Molarity Formula:
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Normality (N) and molarity (M) are both measures of chemical concentration. Normality is the number of equivalents per liter of solution, while molarity is the number of moles per liter. The conversion between them depends on the number of equivalents per mole (n) for the specific substance.
The calculator uses the simple formula:
Where:
Explanation: The formula converts normality to molarity by accounting for the number of reactive units (equivalents) per mole of substance.
Details: Normality is particularly useful in titration calculations and reactions where the number of reactive units is important, while molarity is more commonly used in general chemical calculations. Converting between them ensures proper stoichiometric calculations.
Tips: Enter normality in eq/L and the number of equivalents (n). The number of equivalents depends on the substance and reaction (e.g., n=1 for HCl in acid-base reactions, n=2 for H₂SO₄ in acid-base reactions, n=number of electrons transferred in redox reactions).
Q1: When should I use normality instead of molarity?
A: Normality is particularly useful in acid-base titrations, redox reactions, and precipitation reactions where the number of reactive units is important.
Q2: How do I determine the number of equivalents (n)?
A: For acids/bases, n is the number of H⁺/OH⁻ ions per molecule. For redox reactions, n is the number of electrons transferred per molecule.
Q3: Is normality always greater than molarity?
A: No, normality can be equal to or greater than molarity, depending on the number of equivalents per mole (n ≥ 1).
Q4: Why is molarity more commonly used than normality?
A: Molarity is simpler as it doesn't depend on reaction context, while normality varies depending on the specific reaction being considered.
Q5: Can I convert molarity to normality using the same formula?
A: Yes, just rearrange the formula: \( N = M \times n \).