of An analytical chemist is titrating 74.2 mL of a 0.8800 M solution of trimethylamine ((CH3)N) with a 0.8800M solution of HNO. The pK, o trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 46.1 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places