An analytical chemist is titrating 51.3 mL of a 0.3500 M solution of ethylamine (C2H5NH2) with a 0.3300 M solution of HIO3. The pkb of ethylamine is 3.19.
Calculate the pH of the base solution after the chemist has added 61.6 mL of the HIO3 solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added.
Round your answer to 2 decimal places.