An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.148QP
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![An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid
is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added.
Round your answer to 2 decimal places.
pH = ||](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2932a05-99f3-41c1-989e-7dbca32c3377%2Fa42fed2a-dc9e-4096-a453-d8ea6b884fed%2Fn0yoveue_processed.png&w=3840&q=75)
Transcribed Image Text:An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid
is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 mL of the KOH solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added.
Round your answer to 2 decimal places.
pH = ||
Expert Solution
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Step 1
Given that:
Concentration of butanoic acid = 0.5300 M
Concentration of KOH base = 0.8200 M
Volume of the butanoic acid = 225.8 mL
pKa of the butanoic acid = 4.82
To find: pH of the solution when 40.67 mL of the KOH is added to the solution.
Step 2
Calculate number of moles of butanoic acid and KOH.
Step 3
KOH is a strong base and butanoic acid is a weak acid. Here KOH is in smaller amount. It reacts with butanoic acid in equal amounts to give salt of butanoic acid and water.
CH3CH2CH2COOH + KOH → CH3CH2CH2COO- K+ + H2O
KOH neutralize 0.0333494 moles of butanoic acid to give 0.0333494 moles of salt
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