Conclusion:
Throughout the course of the lab, we utilized an acid-base titration of 10mL of an unknown solution (NaOH) as to determine its molarity. The titration process involved the repetitive dropping of .5 mL of .2M HCl into the unknown solution and the recording of the solution's pH as each drop was added. Initially starting at a pH of 12.5, the NaOH was titrated until 4.762 mL of HCl was added, in which the pH was neutralized at 7. Through the usage of stoichiometry and molarity laws, we were able to determine the concentration of the solution, which was 0.09524M. The theoretical molarity for the solution was calculated to be 0.10M, thus leaving us with a percent error of 4.76%. This was likely due to human error - namely through the inefficient cleaning of the pH probe with distilled water (resulting in inaccuracies in pH readings) and mildly varying amounts of HCl dropped per test (thus making our data points for HCl used disproportional with the given pH at that moment). Had the mL of HCl recorded been a little larger, the molarity of the solution would be larger, whereas if it were smaller, the molarity would be smaller. Thus, it can be inferred that the molarity is proportional to the mL of HCl dropped. From this lab, we proved the validity of the rules of stoichiometry and the molarity formula, while also seeing firsthand the neutralization of a substance through an acid-base reaction.