The purpose of the experiment was to measure the concentration of acid using acid-base titration and the volumetric method of analysis. To determine the concentration, the molality of NaOH solution was calculated assuming that at the equivalence point, the number of millimoles of NaOH equals the number of millimoles of KHP. Using that law of equivalence, the number of grams of KHP and its concentration has been calculated. However, an error in estimated values should be taken into account. Therefore, for good results, four trials will be performed, and the three determinations should agree within 1,0%.
An acid-base titration is a commonly used method to measure the amount of a solution needed to react with another solution having a known concentration. Even though titration is a valid form of finding the concentration of a solution, errors made by experimenters could change the outcome of the whole experiment. In particular, the readings on the burette when titrating the solution could have been off even by the slightest mark. The burette could have been placed not in a direct vertical position. This would account for a little mistake in the number of millimoles of NaOH used and, consequently, the mass and concentration of KHP.
At the initial stage of the experiment, the standardization of NaOH solution could have been measured not accurately. Also, it was difficult to determine the right time and the right intensity of the pink color to stop the titration. If the volume of titrant delivered were too large, a large final concentration would be obtained. It should be mentioned that temperature can also influence the titration procedure. At lower temperatures, the NaOH solution would turn the entire solution from colorless to pink more slowly. To determine the accuracy of the experiment, the standard deviation of the results has been calculated.