Simulate titration curves for strong and weak acids/bases. Visualize pH changes, identify equivalence points, and explore buffer regions.
Enter your titration parameters on the left and click "Simulate Titration" to generate a pH vs. volume curve with key points marked.
This simulator supports:
Learn about the principles behind titration curves and how different acid-base combinations produce characteristic pH profiles.
A titration is a quantitative analytical technique where a solution of known concentration (the titrant) is gradually added to a solution of unknown concentration (the analyte) until the reaction is complete.
The point where stoichiometrically equivalent amounts have reacted is called the equivalence point. By measuring the volume of titrant needed, we can calculate the analyte concentration.
A titration curve plots pH against the volume of titrant added. The curve's shape depends on the strengths of the acids and bases involved:
Initial Point
pH before any titrant is added, determined by the analyte alone.
Half-Equivalence Point
For weak acids: pH = pKa (where [HA] = [A⁻]). Maximum buffer capacity.
Equivalence Point
Moles of titrant = moles of analyte. The steepest part of the curve.
Equivalence Volume:
V_eq = (C_a × V_a) / C_t
Henderson-Hasselbalch:
pH = pKa + log([A⁻]/[HA])
Strong Acid pH:
pH = -log[H⁺]
Weak Acid Initial pH:
[H⁺] ≈ √(Ka × C)
Educational Disclaimer: This simulator uses simplified textbook approximations assuming ideal conditions at 25°C. Real laboratory titrations may differ due to ionic strength, temperature variations, impurities, or CO₂ absorption. Always follow proper safety protocols when performing actual titrations.
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