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Normality Formula:
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Normality (N) is a measure of concentration equal to the gram equivalent weight per liter of solution. It accounts for the number of reactive units in a chemical compound, making it particularly useful in titration calculations and reactions where the number of reactive sites matters.
The calculator uses the simple formula:
Where:
Explanation: The normality is calculated by multiplying the molar concentration by the number of equivalents the solute contributes to the reaction.
Details: Normality is particularly important in acid-base chemistry (for protons or hydroxide ions), redox reactions (for electrons transferred), and precipitation reactions (for ions participating in the reaction).
Tips: Enter the molar concentration in mol/L and the number of equivalents per mole. The number of equivalents depends on the reaction context (e.g., 1 for HCl in acid-base, 2 for H₂SO₄ in acid-base).
Q1: What's the difference between molarity and normality?
A: Molarity is moles per liter, while normality is equivalents per liter. Normality accounts for reactive capacity in a specific reaction.
Q2: How do I determine the number of equivalents?
A: It depends on the reaction type. For acids, it's the number of H⁺ ions donated. For bases, it's the number of OH⁻ ions donated. For redox, it's electrons transferred.
Q3: When should I use normality instead of molarity?
A: Use normality for titration calculations, precipitation reactions, and when the number of reactive sites is important. Use molarity for general concentration measurements.
Q4: Why is normality less commonly used today?
A: Many modern applications prefer molarity since it's simpler and equivalents can be ambiguous. However, normality remains important in specific applications like titrations.
Q5: Can I convert normality back to molarity?
A: Yes, if you know the number of equivalents: \( M = N / n \).