An analytical chemist is titrating 78.3 mL of a 0.7900M solution of aniline (C6H5NH₂) with a 0.2500M solution of HIO3. The p K of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 274.6 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. pH = X 00. Ar

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Chapter16: Acid-base Equilibria
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An analytical chemist is titrating 78.3 mL of a 0.7900M solution of aniline (C6H5NH₂) with a 0.2500M solution of HIO3.
The p K of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 274.6 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.
pH =
X
Ś
ol
Ar
Transcribed Image Text:An analytical chemist is titrating 78.3 mL of a 0.7900M solution of aniline (C6H5NH₂) with a 0.2500M solution of HIO3. The p K of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 274.6 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. pH = X Ś ol Ar
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