Experiment 5 Titration of a Strong Acid with a Strong Base

Part I:

The purpose of this experiment was to prepare an aqueous solution of NaOH, and to determine the concentration of the secondary standard NaOH solution by titrating it with a solute of primary standard, KHP. Another objective of this experiment was to learn how to plot a 2nd derivative graph using LoggerPro, and determining the concentration of the secondary standard from the 2nd derivative data. The primary standard was KHP and the secondary standard was NaOH. The difference between the 2 types of standards is that the primary standard is a has powerful reactants and isn't sensitive to the the environment and the secondary standard is something that is determined will react with a highly pure primary standard that can be standardized. It was necessary to standardize the NaOH solution because NaOH absorbs moisture from the air, making the compound not 100% NaOH, so to obtain precise concentrations, the NaOH needed to be standardized with KHP. The molarity of the NaOH solution was determined by dividing the average number of moles of NaOH (determined by taking the moles of KHP and using the 1:1 ratio) and diving it by the average volume (number of L) at the indicator point. The difference between the equivalence point and the indicator point is that the indicator point is where the indicator changes color, and the equivalent point is the place in a titration where the amount of indicator added neutralizes the solution. Yes the calculated molarities of NaOH for the indicator method and 2nd derivative plot method were within a reasonable range of each other. The molarities calculated for each method were the same (0.5138M) The actual molarity of the NaOH solution was 0.5138, which is in the the 15% range. To determine the molarity of NaOH, the 2nd derivative method was used because it is