An analytical chemist is titrating 245.6 mL of a 0.6400 M solution of ethylamine (C2H_NH,) with a 0.9000 M solution of HNO3. The pK, of ethylamine is
3.19. Calculate the pH of the base solution after the chemist has added 17.7 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 HNO, solution added.
Round your answer to 2 decimal places.
pH ?
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An analytical chemist is titrating 245.6 mL of a 0.6400 M solution of ethylamine (C2H_NH,) with a 0....
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