An analytical chemist is titrating 84.6mL of a 0.5800M solution of ethyl amine C2H5NH2 with a 0.7400M solution of HNO3. The pKb of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 10.6mL 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.
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An analytical chemist is titrating 84.6mL of a 0.5800M solution of ethyl amine C2H5NH2 with a...