Equivalence Point
| Formula / Notation | n_acid × V_acid × M_acid = n_base × V_base × M_base |
|---|---|
| Also Known As | Stoichiometric point, neutral point (strong/strong only), equivalence point |
What is Equivalence Point?
The point in a titration at which the moles of titrant added are stoichiometrically equal to the moles of the analyte being titrated. At the equivalence point, the reaction between titrant and analyte is theoretically complete. It differs from the endpoint, which is the observed color change.
Formula & Notation
Other Names / Synonyms: Stoichiometric point, neutral point (strong/strong only), equivalence point
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
The point in a titration at which the moles of titrant added are stoichiometrically equal to the moles of the analyte being titrated. At the equivalence point, the reaction between titrant and analyte is theoretically complete. It differs from the endpoint, which is the observed color change.
Equivalence points are used to determine the concentration of unknown solutions (titrimetric analysis), to determine pKa values (half-equivalence point method), in pharmaceutical analysis (content assay by titration), and in environmental chemistry (alkalinity, hardness determination).
At the equivalence point in an acid-base titration, the solution may be slightly acidic or basic (depending on whether a weak acid or base is involved). Neutralised solutions are generally less hazardous than the starting acid or base, but should still be disposed of properly.
The formula or notation for Equivalence Point is: n_acid × V_acid × M_acid = n_base × V_base × M_base