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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 useful for acid-base and redox reactions.
The calculator uses the normality formula:
Where:
Explanation: The equation converts molar concentration to normal concentration by accounting for the number of reactive units (equivalents) in each mole of solute.
Details: Normality is particularly important in titration calculations and when dealing with reactions where the number of reactive species matters (like acids/bases with multiple protons or redox reactions).
Tips: Enter molarity in mol/L and the number of equivalents per mole (n). For acids, n is the number of H+ ions; for bases, it's the number of OH- ions; for redox reactions, it's the number of electrons transferred.
Q1: When should I use normality instead of molarity?
A: Use normality for acid-base titrations, redox reactions, or any situation where the number of reactive units is important.
Q2: How do I determine the value of n?
A: For acids, n equals the number of H+ ions; for bases, OH- ions; for salts, the charge on cation/anion; for redox, electrons transferred per molecule.
Q3: What's the difference between molarity and normality?
A: Molarity counts molecules, normality counts reactive units. For monoprotic acids (like HCl), M = N, but for diprotic acids (like H2SO4), N = 2M.
Q4: Is normality always greater than molarity?
A: No, normality can be equal to or greater than molarity, depending on the value of n (which is always ≥1).
Q5: Why is normality less commonly used today?
A: While useful for specific applications, molarity is more versatile for general chemistry calculations, as it doesn't depend on reaction context.