How would each of the folowing affect the accuracy of the calculated neutralizing power of the antacid (too high, too low, no effect)? Explain why.

a) Titration flask was wet with distilled water
b) The burette was initally not rinsed with 0.10M NaOH and some water was left in the tip by the previous student
c) The flask was not heated before the titration and when the solution turned pink, there was powder floating on the suface of the solution.

Thanks!

You haven't described the procedure you used; therefore, I don't know if you titrated the antacid tablet(s) directly or if you used a back titration procedure.

Perhaps I can get you started.
a) Titration flask was wet with distilled water will have no effect. Students often say to me, "But the water will dilute the mixture before titration." That is true BUT you dilute everything by the same amount. The CHEMISTRY reason is that you are titrating moles and the water adds no moles of either antacid or base.
b)Not rinsing the buret with NaOH and adding NaOH to a wet buret means you have diluted NaOH. Therefore, you will add more from the buret, it will read higher, the apparent volume of the NaOH will be increased and that will mean moles NaOH is too high. How that affects the results depends upon what kind of procedure was used.
c) I can't comment on c since I don't know the procedure.

No effect

too high
too low

a) If the titration flask was wet with distilled water, it would have no effect on the accuracy of the calculated neutralizing power of the antacid. This is because distilled water does not react with the antacid or affect the concentration of the solution being titrated.

b) If the burette was initially not rinsed with 0.10M NaOH and some water was left in the tip by the previous student, it would affect the accuracy of the calculated neutralizing power of the antacid. Water left in the tip could dilute the NaOH solution, leading to a lower concentration of NaOH than intended. This would result in an underestimation of the neutralizing power of the antacid.

c) If the flask was not heated before the titration and there was powder floating on the surface of the solution when it turned pink, it would also affect the accuracy of the calculated neutralizing power of the antacid. The presence of powder floating on the surface indicates that the reaction may not have gone to completion. This could be due to the antacid particles not fully dissolving or reacting with the acid. As a result, the measured volume of NaOH required for neutralization would be higher than the actual value, leading to an overestimation of the neutralizing power of the antacid.

In summary:
a) No effect
b) Too low
c) Too high