The equivalence point is the point during a titration when there are equal equivalents of acid and base in the solution. Since a strong acid will have more effect on the pH than the same amount of a weak base, we predict that the solution's pH will be acidic at the equivalence point. 5.2 and 1.3 are both acidic, but 1.3 is remarkably acidic considering that there is an equal amount of base in the solution. As a result, 5.2 is a more appropriate answer.

The equivalence point for a strong acid and strong base will be 7.0. When one of the compounds is weak, however, it will dissociate less than its strong counterpart. In our case, the base will dissociate less than the acid. The acid, thus, contributes more to the pH character of the solution.

At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.

Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pK_a.

Since we are adding acid to a base, the pH must decrease. The initial base will have a high pH, while the final acid will have a low pH; the right of the curve must be lower than the left. In addition, the pH does not change very rapidly until the equivalence point is reached, hence the curve must show little initial change followed by a rapid change.

The equivalence point is the point in a titration at which the number of moles of titrant equals the number of moles of analyte. The endpoint in a titration is when the color of the reaction changes to that of the desired (often neutral) pH. However this is not the same as the equivalence point, which is a stoichiometric value. Indicators may change colors several times throughout a neutralization reaction, thus this is not an accurate attribute of the reaction to use as the equivalence point. Furthermore, the concentrations of titrant and the analyte are rarely equivalent, and there could be differing numbers of ionizable groups on each species.

 and  react in a 1:1 mole ratio. Therefore the number of moles of  at the end point of the reaction equals to the number of moles of . We can use the concentration as a conversion factor to determine the number of moles reacted.

 and  react in a 1:1 mole ratio. Therefore the number of moles of  at the end point of the reaction equals to the number of moles of .

Based on the equation given, we know the that  reacts with  in a 1:1 mole ratio. We can use the molar concentration given as a conversion factor to determine the number of moles of  used which will be equal to the number of moles of  used.

To determine the molar concentration of  used, we can simply use the following equation:

We have determined that the concentration of  used is equal to the concentration of  used.

The equivalence point in a titration is the point in which the number of moles of titrant equals to the number of moles of analyte:

We need to determine the number of moles of acetic acid we are dealing with:

Therefore, at the equivalence point there are also 0.0075 moles of  in the solution. In order to determine the number of moles of  in solution, we must use the concentration of  as a conversion factor to determine the volume added to the acetic acid solution.