Question

1. Answer the following questions in detail.

a) Given 25mL of 0.10 M HCl and 25 mL of 0.10 M acetic acid, will the amount of 0.10 M NaOH required to reach the equivalence point for each solution be the same, more, or less?

b) Again, using 0.10 M NaOH, will the pH at the equivalence point of 25 mL 0.10 M HCl be the same, more, or less as the pH at the equivalence points for 25 mL of 0.10 M acetic acid?

c) Given 25 mL of 0.10 M acetic acid and 25 mL of 0.010 M acetic acid:

i) Will the amount of 0.10 M NaOH required to neutralize each solution be the same, more, or less? Explain.
ii) Will the pH at the equivalence point be the same, more, or less? Explain.

d) The following parts are about the shape of a pH titration graph.

i) How can the steep part of the curve be used to determine the unknown concentration of a known substance? Explain.

ii) Explain why the graph of a weak acid (conical) vs a strong base (burette) is relatively flat halfway to the equivalence point.

iii) Explain how a "half-titration value" determined from the graph in part ii) can be used to determine the K_a of a weak acid.

Answer 1