Equivalence point

The equivalence point at a acid -base titration is the point at which a certain amount of substance is present acid or base with the equivalent amount of base or acid material. The equivalence point therefore applies:

Moreover, there are equivalence points for example redox titrations.

Compared with neutral point

The number of moles of hydroxide ions / oxonium ions is initially undetermined. Only for the combination of strong acid / strong base applies here good approximation:

Titrated to strong acids and bases together so the equivalence point in aqueous solution is equal to the neutral point, the pH is 7 titrated against it different strong acids and bases are to each other, the resulting solution is not neutral at the equivalence point. For example, a weak acid (e.g., acetic acid, CH3COOH ) neutralized with the equivalent amount of a strong base, the pH is eventually in a basic medium. This is because the acetate ion ( CH3COO - ), which form the conjugate base of the weak acid CH3COOH, then itself act as a base, and thus are able to capture the H ions, in other words with H2O to CH3COOH and OH to react. The pH at the equivalence point corresponds here do not necessarily 7

Examples

If you give every 1 mole of hydrochloric acid ( HCl) and sodium hydroxide ( NaOH) together, the result is a neutral saline solution.
If you give every 1 mole of acetic acid ( CH3COOH ) and sodium hydroxide ( NaOH) together, we obtain an alkaline solution of sodium acetate.