If you add 0.4397 g of benzoic acid to a 100 ml volumetric flask and then add enough water to bring the total volume to 100.00 ml, how many ml of 0.2759 M NaOH solution will be required to completely neutralize the benzoic acid? At the neutralization point, will the solution be somewhat acidic, neutral, or somewhat basic?
If you accidentally overshoot the neutralization point in the experiment described in question 1 and add 0.10 ml too much of the NaOH solution, what will be the final solution pH?
You need to determine both the molar mass and the pKa of your known acid. On which of these experiments will you use the pH meter? (Remember, you can only use the pH meter on one experiment.) Please explain your decision.