Final answer:
The equivalence point is where the stoichiometrically correct amount of titrant has been added to react completely with the analyte, while the end point is observed when the indicator signals the completion of the reaction, which may not precisely align with the equivalence point.
Step-by-step explanation:
In the context of titrations in chemistry, there are two critical concepts to understand: the equivalence point and the end point. The equivalence point is reached when the stoichiometric amount of one reactant has been added to react completely with the other reactant, meaning the number of moles of hydrogen ions equals the number of moles of hydroxide ions in an acid-base reaction, or the stoichiometry is fulfilled in other types of reactions. On the other hand, the end point is a practical measure, denoted by the change in color of an indicator or another detectable signal. It indicates when the titration reaction appears to be complete, although this may not coincide exactly with the theoretical equivalence point.
The equivalence point can be accurately found on a titration curve where the ph rapidly changes, often at an inflection point. For a 1:1 reaction, this would be a symmetric equivalence point; however, if the stoichiometry is different, an asymmetric equivalence point might occur, shifting the point on the curve. After the equivalence point, any added titrant will be an excess reactant, which is especially evident in titrations involving strong acids or bases.