An analytical chemist is titrating 53.9 mL of a 0.6000 M solution of trimethylamine ((CH,),N) with a 0.7900 M solution of HNO3. The p K, of 3. trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 46.9 mL of the HNO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0 Ar