Answered: The base protonation constant K of…

The base protonation constant K of ammonia (NH3) is 1.8 × 10¯5. Calculate the pH of a 0.54 M solution of ammonia at 25 °C. Round your answer to 1 decimal place. [1] = Hd

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 42QAP

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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.

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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

The base protonation constant K₁ of ammonia (NH₂) is 1.8 × 10¯5.
Calculate the pH of a 0.54 M solution of ammonia at 25 °C. Round your answer to 1 decimal place.
= 0
pH =
X

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