posted by Sandy
In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar.
A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the student refilled the buret with NaOH to titrate the acetic acid, the remaining pellets dissolved. Will the molarity of acetic acid in the vinegar solution be too high or low?
Will the concentration of the acetic acid in the vinegar solution will be larger because it takes less NaOH than it should to titrate the acetic acid, meaning the volume of NaOH was small that was required to titrate the acetic acid making the concentration of acetic acid to be larger?