An analytical chemist is titrating 180.7 mL of a 0.5200M solution of piperidine (C5H₁0NH) with a 0.8300M solution of HIO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 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.
An analytical chemist is titrating 180.7 mL of a 0.5200M solution of piperidine (C5H₁0NH) with a 0.8300M solution of HIO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 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.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![An analytical chemist is titrating 180.7 mL of a 0.5200 M solution of piperidine (\( \text{C}_5\text{H}_{10}\text{NH} \)) with a 0.8300 M solution of \( \text{HIO}_3 \). The \( pK_b \) of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 mL of the \( \text{HIO}_3 \) solution to it.
*Note for advanced students:* you may assume the final volume equals the initial volume of the solution plus the volume of \( \text{HIO}_3 \) solution added.
Round your answer to 2 decimal places.
\[ \text{pH} = \]
(Graph icon)
(Math input box)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F321870cf-5f02-4a7a-9bd1-b1bcd10d94da%2Fda8f0d7b-bf77-49c5-9b72-20cf91bc7383%2Fpketxk_processed.png&w=3840&q=75)
Transcribed Image Text:An analytical chemist is titrating 180.7 mL of a 0.5200 M solution of piperidine (\( \text{C}_5\text{H}_{10}\text{NH} \)) with a 0.8300 M solution of \( \text{HIO}_3 \). The \( pK_b \) of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 37.7 mL of the \( \text{HIO}_3 \) solution to it.
*Note for advanced students:* you may assume the final volume equals the initial volume of the solution plus the volume of \( \text{HIO}_3 \) solution added.
Round your answer to 2 decimal places.
\[ \text{pH} = \]
(Graph icon)
(Math input box)
Expert Solution
Step 1
In this , piperidine is a base and HIO3 is an acid , so they will react to give conjunction acid of piperidine.
To calculate the pH, we need to use Henderson Hasselbalch equation.
For this first we calculate moles of both reactants and then draw an ICE table to calculate the equilibrium moles after reaction.
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