How does the endpoint of a titration differ from the equivalence point?

The point at which the indicator simply changes color is the titration's endpoint.

When the ratio of the reactants is within the amounts given by the equation, this is known as the equivalency point.

It would be ideal for these points to line up.

The final solution is neutral at pH 7 for strong acids and bases, such as NaOH and HCl:

The majority of indicators can be used in a titration because they will change color at the equivalency point.

However, this isn't always the case; for example, the final solution won't be neutral if a strong acid is used to neutralize a weak base.

The slightly acidic nature of the ammonium ion explains this:

The same issue arises when a weak acid neutralizes a strong base, resulting in a slightly alkaline salt.

The term "salt hydrolysis" refers to this.

The indicator you select must also change color at the equivalency point; in this example, methyl orange works well, but phenolphthalein does not.

You can search for "theory of indicators" to learn more.

The point of equivalency is reached when there are exactly the same amounts of base and acid that have been combined.

The point at which the indicator used in this kind of reaction changes color is known as the end point.

Equivalency point and end point are not always 100% identical because in an acid-base titration, the indicator color change is frequently not observed AT the equivalency point but rather after the equivalency point has been exceeded (i.e., once there is an imbalance of acid or base).

The endpoint of a titration is the point at which the indicator changes color or another signal indicates that the reaction has reached its conclusion. The equivalence point, on the other hand, is the point at which the stoichiometrically equivalent amounts of the reactants have reacted completely, regardless of whether an indicator is used or not.