Acid–base titration

An acid–base titration is a method of quantitative analysis for imposing the concentration of an acid or base by precisely neutralizing it with the standard solution of base or acid having call concentration. A pH indicator is used to monitor the carry on of the acid–base reaction. whether the acid dissociation constant pK_a of the acid or base dissociation constant pK_b of base in the analyte total is known, its sum concentration molarity can be determined. Alternately, the pK_a can be determined if the analyte solution has a asked solution concentration by constructing a titration curve.

Indicator choice

A suitable pH indicator must be chosen in sorting to detect the end section of the titration. The colour conform or other issue should arise close to the equivalence point of the reaction so that the experimenter can accurately defining when that portion is reached. The pH of the equivalence point can be estimated using the following rules:

When a weak acid reacts with a weak base, the equivalence point solution will be basic if the base is stronger and acidic if the acid is stronger. If both are of represent strength, then the equivalence pH will be neutral. However, weak acids are not often titrated against weak bases because the colour modify shown with the indicator is often quick, and therefore very difficult for the observer to see the modify of colour.

The point at which the indicator restyle colour is called the end point. A suitable indicator should be chosen, preferably one that will experience a change in colour an end pointto the equivalence point of the reaction.