Normality Calculator
Calculate normality (N), the number of equivalents per liter. Use this for acid-base titrations and redox reactions where equivalents matter.
H⁺ for acids, OH⁻ for bases, charge for salts
What is normality in chemistry?
Normality (N) is a measure of concentration equal to the number of equivalents per liter of solution. It is particularly useful for acid-base reactions and redox reactions where the reactive capacity (equivalents) matters more than the number of molecules.
What is an equivalent weight?
Equivalent weight is the mass of one equivalent of a substance, calculated by dividing molar mass by the number of reactive units (n). For acids, n = number of H⁺ ions; for bases, n = number of OH⁻ ions; for salts, n = total charge. Example: For H₂SO₄ (M = 98 g/mol), equivalent weight = 98/2 = 49 g/eq.
How do I convert between normality and molarity?
Normality = Molarity × n, where n is the number of equivalents per molecule. For H₂SO₄ (n=2): 1 M H₂SO₄ = 2 N. For HCl (n=1): 1 M HCl = 1 N. Conversely, Molarity = Normality ÷ n.
When should I use normality instead of molarity?
Use normality for: acid-base titrations (where equivalents react), redox reactions (electron transfer), and when measuring reactive capacity. It simplifies calculations because equivalents always react 1:1 regardless of molecular weight. Required for standard analytical procedures.
What is the difference between normal and equivalent?
An equivalent is the amount of substance that supplies or reacts with one mole of reactive particles (H⁺, OH⁻, electrons). Normality (N) is equivalents per liter. So 1 liter of 1 N solution contains 1 equivalent of reactive material. A 1 N acid neutralizes 1 equivalent of base.
How do I calculate equivalents for different compound types?
For acids: equivalents = moles × number of H⁺ (HCl = 1, H₂SO₄ = 2, H₃PO₄ = 3). For bases: equivalents = moles × number of OH⁻ (NaOH = 1, Ca(OH)₂ = 2). For salts: equivalents = moles × total positive charge (NaCl = 1, CaCl₂ = 2, Al₂(SO₄)₃ = 6).