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.

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.

A pH indicator added to a solution causes a color change which is an indication that a reaction has reached the equivalence point. The equivalence point is when the number of moles of titrant equals the number of moles of analyte. The end point is an approximation of this in a titration.

At the equivalence point:

The number of moles of NaOH at equivalence point is calculated as follows:

Assuming we were trying to convert the number of grams of the monoprotic acid to moles, the equation would be set up as follows:

Let's plug the values we have into this equation and give the molar mass a value of :

Rearranging this equation to solve for the molar mass gives:

The equivalence point is the point in a titration at which the number of moles of titrant species equals the number of moles of analyte. For a polyprotic acid there are multiple equivalence points because there are more than one acidic proton in one molecule of the acid. A titration curve has as many equivalence points as the number of protons that may be neutralized by the interaction with a base. In this titration curve there are two equivalence points. The equivalence points occur when the graph has a very steep slope, and involve very large changes in pH with additions of small amounts of base. For this graph, the equivalence points occur at about pH 3.5 and 10.

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.

We must first calculate the molecular weight of :

We can calculate the grams of using the molecular weight calculated as a conversion factor:

Finally, we can calculate the percent mass using the total grams of vinegar solution:

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 = pKa.

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 .

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.