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Consider the titration of a 45.0 mL sample of 0.100 M HN3 with 0.250 M KOH....

Consider the titration of a 45.0 mL sample of 0.100 M HN3 with 0.250 M KOH. (Ka of HN3 = 2.5 x 10-5) Calculate each of the following: (a) How many mL are required to reach the equivalence point?

(b) What is the initial pH of the acid solution?

(c) What is the pH after the addition of 5.00 mL of KOH?

(d) What is the pH after the addition of 9.00 mL of KOH? (e) What is the pH after the addition of 19.00 mL of KOH?

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