Titration Curve
Add strong base to an acid, strong or weak, and trace pH against volume — see the equivalence point's sharp jump and, for a weak acid, the buffer plateau where pH equals pKa at the half-equivalence point.
What you can adjust
- Acid concentration
- 0.01 – 1 mol/L
- Titrant (base) concentration
- 0.01 – 1 mol/L
- Initial acid volume
- 10 – 100 mL
- Acid type
- 0 – 1
- Acid pKa
- 2 – 8
Concentration of the acid in the flask before any titrant is added.
Concentration of the strong base being added from the burette. A more concentrated titrant reaches the equivalence point in less volume.
Volume of acid solution in the flask at the start of the titration.
Strong acids dissociate completely; weak acids sit in equilibrium with their conjugate base, governed by pKa below — producing the buffer region and the elevated (basic) equivalence-point pH a strong-acid titration never shows.
Only used when the acid type above is 'weak'. At the half-equivalence point, pH equals pKa — this is what sets the height of the buffer plateau. Default 4.76 is acetic acid's real pKa.