Final answer:
Over-titration in the standardization of NaOH would result in an underestimation of the acidity of lemon-lime soda in subsequent trials, as the NaOH would be less concentrated than assumed, requiring more solution to reach the equivalence point, indicating a higher acidity.
Step-by-step explanation:
If each trial in the standardization of NaOH were over-titrated to a similar degree, this would indicate that more NaOH than necessary was added to reach the equivalence point. Since the amount of NaOH necessary for standardization is inflated, when the same over-titrated NaOH solution is used for further titrations, such as those with lemon-lime soda, it would lead to the underestimation of the acidity in these subsequent trials. Because the titrant (NaOH) concentration would effectively be less than assumed, it would require more titrant to reach the equivalence point, suggesting that the soda is more acidic than it actually is.
The relationship can be understood by considering the titration of a strong acid (like HCl) with a strong base (NaOH). The pH changes only gradually until the equivalence point, at which most H+ ions have been consumed, and then the pH increases rapidly.