🧬 N = Mass ÷ (Eq. Wt. × Volume)

Normality Calculator

Calculate the normality of a solution by entering mass of solute, equivalent weight, and volume. Essential for titrations and analytical chemistry.

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1.0000N
40 g ÷ (40 g/eq × 1 L) = 1.0000 N
Common Solutes:
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Visualize Solution Concentration

See how normality changes with mass and volume

1.0 N

📐 Formula

N = mass ÷ (Eq. Wt. × V)

🔬 Gram Equivalents

1.000 eq

Understanding Normality

Normality (N) measures solution concentration in terms of gram equivalents per liter. It is widely used in acid-base titrations, redox reactions, and precipitation reactions.

The Formula

N = Mass of Solute (g) ÷ (Equivalent Weight × Volume in L)

Step-by-Step Example

Finding the normality of a solution with 49 g of H₂SO₄ in 500 mL:

  1. Mass of solute: 49 g
  2. Equivalent weight of H₂SO₄: 49 g/eq (98 ÷ 2)
  3. Volume in liters: 500 mL = 0.5 L
  4. N = 49 ÷ (49 × 0.5) = 2.0 N

Normality vs Molarity

  • Molarity (M) = moles of solute per liter of solution.
  • Normality (N) = gram equivalents per liter of solution.
  • N = M × n (where n = number of H⁺, OH⁻, or electrons transferred).
  • For HCl (monoprotic): N = M. For H₂SO₄ (diprotic): N = 2M.

🔑 Key Points

  • N = equivalents ÷ volume (L)
  • Eq. Wt. = Molar Mass ÷ n-factor
  • n-factor depends on reaction type
  • Used in titration calculations
  • 1 N HCl neutralizes 1 N NaOH

📌 Common Eq. Weights

  • HCl — 36.5 g/eq
  • NaOH — 40.0 g/eq
  • H₂SO₄ — 49.0 g/eq
  • HNO₃ — 63.0 g/eq
  • KMnO₄ — 31.6 g/eq

Conversion Tools

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Example: 100 g ÷ 100 mL = 1.0 g/mL
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Normality Calculator

Calculate normality (N) from molarity, equivalent weight, and volume for chemistry.

Example: 0.5 M × 2 eq = 1.0 N
❓ Frequently Asked Questions

Normality Calculator FAQ

Common questions about calculating normality.

Normality (N) is a measure of concentration equal to the gram equivalents of solute per liter of solution. It accounts for the reactive capacity of a solute in a specific reaction.

Equivalent weight = Molar mass ÷ n-factor. The n-factor is the number of H⁺ ions (acids), OH⁻ ions (bases), or electrons transferred (redox). For H₂SO₄ (molar mass 98, donates 2 H⁺): Eq. Wt. = 98 ÷ 2 = 49.

Molarity counts moles of solute per liter; normality counts equivalents. For monoprotic acids (HCl), N = M. For diprotic acids (H₂SO₄), N = 2M. Normality is reaction-specific.

Use normality for titration calculations (N₁V₁ = N₂V₂), acid-base neutralization, and redox stoichiometry where the number of reactive units matters.

Yes. Normality = Molarity × n-factor. When n > 1 (polyprotic acids, polyvalent ions), normality is greater than molarity. For example, 1 M H₂SO₄ = 2 N.