Part A: 50 mL of 2.0 M acetic acid (CH3COOH) was titrated with 1.0 M NaOH. What is the pH at the equivalence point of this titration? The ionization constant is 1.8 × 10−5.

1. 7.00 2. 9.52 3. 9.28 4. 9.20 5. 10.52 

Part B: A 200 mL sample of 0.5 M N2H4 (hy- drazine) is titrated to its equivalence point with200mLof0.5MHCl. IftheKb ofN2H4 is 2.5 × 10−6, what is the pH of the solution at the equivalence point?

1. 8.5 2. 4.5 3. 1.5 4. 7.0