Titration Calculator
Instantly calculate unknown concentration, volume, or moles in acid-base titrations using precise stoichiometric formulas.
Calculate Unknown Concentration or Volume
Enter your known titration values and stoichiometric ratio to instantly solve for the unknown molarity or volume.
Titration Solver
Solve M₁V₁/n₁ = M₂V₂/n₂ with step-by-step breakdown.
How it Works
Understanding titration calculations
Choose Target
Select whether you need to find the unknown concentration (Molarity) or the unknown volume.
Enter Knowns
Input the concentration and volume of your known solution (titrant), and the volume or concentration of the unknown (analyte).
Set Stoichiometry
Enter the mole ratio (n₁ and n₂) derived directly from the balanced chemical equation.
Get Results
Instantly see the unknown value, moles of each substance, and the exact formula breakdown.
Common Acid-Base Titration Ratios
Standard stoichiometric ratios (n₁ : n₂) for frequently encountered laboratory titration reactions.
| Acid (Analyte / n₁) | Base (Titrant / n₂) | Balanced Equation Snippet | Ratio (n₁ : n₂) |
|---|---|---|---|
| Hydrochloric Acid | NaOH (Sodium Hydroxide) | HCl + NaOH → NaCl + H₂O | 1 : 1 |
| Nitric Acid | KOH (Potassium Hydroxide) | HNO₃ + KOH → KNO₃ + H₂O | 1 : 1 |
| Sulfuric Acid | NaOH (Sodium Hydroxide) | H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O | 1 : 2 |
| Phosphoric Acid | NaOH (Sodium Hydroxide) | H₃PO₄ + 3NaOH → Na₃PO₄ + 3H₂O | 1 : 3 |
| Ethanoic (Acetic) Acid | NaOH (Sodium Hydroxide) | CH₃COOH + NaOH → CH₃COONa + H₂O | 1 : 1 |
| Hydrochloric Acid | Ca(OH)₂ (Calcium Hydroxide) | 2HCl + Ca(OH)₂ → CaCl₂ + 2H₂O | 2 : 1 |
Titration Calculator FAQ
Answers to the most frequently asked questions about acid-base titrations, stoichiometry, and molarity calculations.
The standard titration formula is M₁V₁/n₁ = M₂V₂/n₂, where M is molarity (concentration in mol/L), V is volume (in mL or L), and n is the stoichiometric coefficient (number of moles) from the balanced chemical equation for the known (1) and unknown (2) substances.
The equivalence point is the theoretical point in a titration where the moles of titrant exactly equal the moles of analyte according to the stoichiometric ratio. The endpoint is the experimental point where the indicator changes color, which should be as close to the equivalence point as possible.
You must first write the balanced chemical equation for the acid-base reaction. The stoichiometric coefficients of the reactants in the balanced equation are your n₁ and n₂ values. For example, in HCl + NaOH → NaCl + H₂O, the ratio is 1:1. In H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O, the ratio is 1:2.
As long as you use the same volume unit for both V₁ and V₂, the units will cancel out in the M₁V₁/n₁ = M₂V₂/n₂ formula. Milliliters (mL) are most commonly used in laboratory titrations for convenience, as burette readings are typically in mL.