An analytical chemist is titrating 93.1 mL of a 0.8600 M solution of butanoic acid (HC,H,CO,) with a 1.100M solution of KOH. The p K of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 83.4 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 93.1 mL of a 0.8600 M solution of butanoic acid (HC,H,CO,) with a 1.100M solution of KOH. The p K of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 83.4 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.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 112CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)...

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

An analytical chemist is titrating 93.1 mL of a 0.8600 M solution of butanoic acid (HC,H,CO,) with a 1.100 M solution of KOH. The p K, of butanoic
a
acid is 4.82. Calculate the pH of the acid solution after the chemist has added 83.4 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 =

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