Acid–Base Titration Simulator
Analyze neutralization curves and stoichiometric equivalence points during strong and weak acid titrations.
Volumetric Stoichiometry & Titration Curves
Titration is a quantitative analytical technique in which a standard solution of known concentration (titrant) is delivered incrementally to an analyte solution until stoichiometric equivalence is attained:
For a strong acid–strong base system, the equivalence pH is exactly 7.00. For a weak acid (e.g., acetic acid CH₃COOH), the conjugate base (acetate CH₃COO⁻) undergoes hydrolysis, producing an equivalence pH in the basic range (typically ~8.7).
Model Assumptions & Experimental Conditions
- Monoprotic acid-base system undergoing 1:1 molar reaction.
- Instantaneous chemical equilibrium and homogeneous mixing.
- Standard laboratory temperature maintained without heat of neutralization distortion.
Frequently Asked Questions
What is an equivalence point?
The equivalence point is the exact point in a titration where chemically equivalent stoichiometric amounts of titrant and analyte have combined.
Why does the pH rise steeply near equivalence?
Near equivalence, almost all analyte acid has been neutralized, so a single fraction of a drop introduces a massive fractional change in [H₃O⁺] concentration.
More from Alok Das
These interactive tools are personal side-projects built for exploration and utility. My primary professional commitment is in M.Sc. Chemistry, analytical research, and laboratory methodology.