Final answer:
The concentration of acetic acid relative to sodium hydroxide cannot be determined without specific volume data from the titration. However, based on the provided molarity, if completely neutralized, acetic acid would have half the molarity of sodium hydroxide.
Step-by-step explanation:
Based on the information provided, when comparing the concentration of acetic acid to that of sodium hydroxide during a titration, it depends on the volumes used to reach the equivalence point. Given that we don't have specific volumes that were used to reach the equivalence point, we cannot determine the exact concentration of acetic acid only based on the initial molarities provided. However, if the titrations mentioned used the stoichiometric point to neutralize the acid completely with the base, we can infer that the concentration of acetic acid is half that of sodium hydroxide based on the molarities used (0.100 M acetic acid and 0.200 M NaOH).
The pH change in the titration of acetic acid compared to that of HCl suggests that acetic acid is a weak acid and does not ionize as completely as HCl, resulting in a less steep curve before the equivalence point and a higher pH at the equivalence point due to the formation of the acetate ion, which is a weak base and raises the pH.
Therefore, without additional volumes from the titration data, the most accurate choice would be that the concentration of the acetic acid solution cannot be determined (option c).