The titration calculator determines the volume of titrant needed to reach the equivalence point in acid-base titrations. Enter the analyte's molarity and volume, the titrant molarity, and the stoichiometric ratio from the balanced equation.
Titration Calculator
Coefficient in balanced eq.
Coefficient in balanced eq.
Results
Step-by-Step
Common Titration Pairs
| Acid | Base | Ratio | pH at EP |
|---|---|---|---|
| HCl | NaOH | 1:1 | 7.0 |
| H₂SO₄ | NaOH | 1:2 | 7.0 |
| CH₃COOH | NaOH | 1:1 | ~8.7 |
| HCl | NH₃ | 1:1 | ~5.1 |
How to Use the Titration Calculator
Acid-base titration determines concentration by reacting a known-concentration solution (titrant) with an unknown-concentration solution (analyte) until the equivalence point is reached. This calculator finds the titrant volume needed.
Step 1: Enter Analyte Information
Enter the analyte's molarity (if known) and volume in mL. If solving for analyte concentration, enter the volume and then work backward from the titrant volume used.
Step 2: Enter Titrant Molarity
Enter the known concentration of your titrant (the solution in the burette). For standard titrations, this is typically a primary standard like oxalic acid or a standardized NaOH/HCl solution.
Example: HCl vs NaOH (1:1)
Analyte: 25.00 mL of 0.1 M HCl. Titrant: 0.1 M NaOH. Stoichiometry: 1:1. Moles HCl = 0.025 × 0.1 = 0.0025 mol. Volume NaOH = 0.0025 / 0.1 = 0.025 L = 25.00 mL. Equivalence point pH = 7.0.
Stoichiometry for Polyprotic Acids
For H₂SO₄ titrated with NaOH: H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O. Set analyte stoichiometry = 1, titrant stoichiometry = 2. This doubles the volume of NaOH needed compared to a 1:1 titration.
FAQ
What is a titration?
Titration is a technique to determine the concentration of a solution (analyte) by reacting it with a solution of known concentration (titrant). At the equivalence point, the moles of titrant exactly neutralize the moles of analyte according to the stoichiometric ratio.
How is the equivalence point volume calculated?
Using the formula: V_titrant = (n_analyte × V_analyte × M_analyte) / (n_titrant × M_titrant), where n_analyte and n_titrant are the stoichiometric coefficients from the balanced equation.
What is the pH at the equivalence point?
For strong acid–strong base titrations, the equivalence point is at pH 7. For weak acid–strong base, it is slightly basic (pH > 7) because the conjugate base hydrolyzes water. For strong acid–weak base, pH < 7 at the equivalence point.
Is this calculator free?
Yes, completely free with no signup required. All calculations run in your browser.
What is the difference between equivalence point and endpoint?
The equivalence point is when stoichiometrically equal moles have reacted — a theoretical concept. The endpoint is when the indicator changes color, which an experimenter observes. These are close but not identical; indicator choice aims to make them coincide.