Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added.
(a) 0.0 mL (i've tried this 3 times and have gotten 8.48, 9.26, 13)
(b) 20.0 mL
(c) 25.0 mL
(d) 40.0 mL
(e) 50.0 mL
(f) 100.0 mL
A 25.0 mL sample of 0.100 M pyridine (Kb for pyridine is 1.7 10-9) is titrated with 0.100 M HCl solution. Calculate the pH after the addition of the following amounts of HCl.
0.0 mL (i've tried this 3 times and have gotten 3.12, 2.61, 10.885)
4.0 mL
8.0 mL
12.5 mL
20.0 mL
24.0 mL
24.5 mL
25.0 mL
26.0 mL
28.0 mL
30.0 mL
I don't even know where to start. Please help.