What is the Difference Between Half Equivalence Point and Equivalence Point?
🆚 Go to Comparative Table 🆚The difference between the half equivalence point and the equivalence point lies in the extent of the neutralization reaction that occurs during a titration. A titration is an analytical technique in chemistry used to determine the unknown concentration of a substance in a liquid by slowly adding a solution of known concentration, called the titrant, to the sample solution.
- Half Equivalence Point: This point occurs when half of the initial amount of acid has been neutralized by the base. At the half equivalence point, the concentration of the weak acid (HA) is equal to the concentration of its conjugate base (A-). This is also the point at which the pH of the solution is equal to the pKa value of the weak acid. The half equivalence point is considered the midpoint between the starting point and the equivalence point.
- Equivalence Point: This is the point where the amounts of acid and base are equal, resulting in a solution of only salt and water. At the equivalence point, the moles of acid are equal to the moles of base, and the pH of the solution changes dramatically. The equivalence point is the actual point where the desired chemical reaction in the titration is completed.
In summary, the key difference between the half equivalence point and the equivalence point is that the half equivalence point represents the midpoint of the titration reaction, where half of the initial amount of acid has been neutralized, while the equivalence point represents the completion of the neutralization reaction, where the solution is fully neutralized.
Comparative Table: Half Equivalence Point vs Equivalence Point
The difference between the half equivalence point and the equivalence point can be summarized in the following table:
| Feature | Half Equivalence Point | Equivalence Point |
|---|---|---|
| Definition | The point where the concentration of a weak acid equals $$[\ce{HA}] = [\ce{A-}]$$ | The point where the amount of moles of acid and base are equal, resulting in a solution of only salt and water |
| Occurrence | Halfway between the equivalence point and the starting point (origin) | Actual point where the desired chemical reaction in the titration occurs |
| pH Value | Equal to the pKa of the weak acid | Depends on the strength of the acid and the base |
| Concentration | The amount of protonated [HA] and deprotonated [A-] species of the analyte is equal | The reaction between the acid and base is stoichiometrically complete |
In summary, the half equivalence point is the midpoint between the starting point and the equivalence point, where the concentration of a weak acid equals that of its conjugate base. The equivalence point, on the other hand, is the point where the reaction between the acid and base is completed, and the amount of moles of acid and base are equal.
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