The equivalence point of a titration marks the exact moment when the amount of acid equals the amount of base in the solution. At this point, the number of moles of hydrogen ions, H+, from the acid, matches the number of moles of hydroxide ions, OH-, from the base, resulting in a neutral solution — at least theoretically. It's the target that chemists aim for in a titration, and it can be confirmed by the indicator’s color change or by monitoring the solution's pH.
In practice, the equivalence point is where the titration curve shows the steepest rise or fall in pH. It's important to understand that the equivalence point and the end point (where the indicator changes color) might not be exactly the same due to the properties of the indicator used. Therefore, selecting an appropriate indicator, whose pH range of color change flanks the pH of the equivalence point, is critical for accurate titration results.
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