Question

Consider the titration of 80.0 mL of 0.0200 M C5H5N (a weak base; Kb = 1.70e-09) with 0.100 M HNO3.

Calculate the pH after the following volumes of titrant have been added:

(a) 0.0 mL pH =

(b) 4.0 mL pH =

(c) 8.0 mL pH =

(d) 12.0 mL pH =

(e) 16.0 mL pH =

(f) 25.6 mL pH =

PART TWO:

A buffer solution contains 0.14 mol of ascorbic acid (HC₆H₇O₆) and 0.84 mol of sodium ascorbate (NaC₆H₇O₆) in 2.80 L.
The K_a of ascorbic acid (HC₆H₇O₆) is K_a = 8e-05.



(a) What is the pH of this buffer?

pH =


(b) What is the pH of the buffer after the addition of 0.07 mol of NaOH? (assume no volume change)

pH =


(c) What is the pH of the original buffer after the addition of 0.21 mol of HI? (assume no volume change)

pH =