Consider the titration of 80.0 mL of 0.0200 M C5H5N (a weakbase; Kb = 1.70e-09) with 0.100 M HNO3.
Calculate the pH after the following volumes of titrant havebeen 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 sodiumascorbate (NaC6H7O6) in 2.80L.
The Ka of ascorbic acid(HC6H7O6) is Ka =8e-05.
(a) What is the pH of this buffer?
pH =Â Â
(b) What is the pH of the buffer after the addition of 0.07 mol ofNaOH? (assume no volume change)
pH =Â Â
(c) What is the pH of the original buffer after the addition of0.21 mol of HI? (assume no volume change)
pH =Â Â
