Equations describing the various stages of a titration provide a mathematical framework to quantify changes in pH of a solution, effectively illustrating the transition from the start point to the endpoint of the titration.
In summary, the pH curve of a strong base to weak acid titration can be described by the following simplified equations in place of a complex complete pH titration equation:
| Start point | |
| After start point but before stoichiometric point | |
| Maximum buffer capacity point | |
| Stoichiometric point | |
| Beyond stoichiometric point |
The diagram below shows the plot of the above equations on a single graph for the titration of 10 cm3 of 0.200 M of CH3COOH (Ka = 1.75 x 10-5) with 0.100 M of NaOH:
A complementary set of equations can be derived using the same logic mentioned in the earlier articles to describe a strong acid to weak base titration.