Question

a. A titration enthusiast titrates because he wants to titrate things because that is what good scientists do....they titrate. In this very interesting titration, 50 mL of 0.125M NaOH is added to a 50 mL solution of 0.25M formic acid (HCOOH) at 25 oC. What is the pH after the addition of NaOH? Ka (HCOOH) = 1.7x10−4.

b. How many mL of 0.125M NaOH need to be added to the 50 mL solution of 0.25M formic acid (HCOOH) to reach the equivalence point? What is the pH at the equivalence point? The Ka of HCOOH = 1.7x10−4.

c. A titration enthusiast titrates ANOTHER solution. This time, a 100 mL solution of 0.13M trimethylamine ((CH3)3N) is titrated with 25 mL of 0.31M HCl at 25 oC. What is the pH of the solution AFTER the addition of the HCl? Kb for (CH3)3N = 6.4x10−5.

d. How many mL of 0.31M HCl need to be added to the 100 mL solution of 0.13M trimethylamine ((CH3)3N) to reach the equivalence point? What is the pH at the equivalence point? The Kb for (CH3)3N is 6.4x10−5.

Answer 1