Answered: What is the [CH3CH2CO2−] in a solution…

What is the [CH3CH2CO2−] in a solution which is 0.1416 M in CH3CH2CO2H and 0.1929 M in HNO3? CH3CH2CO2H(aq) + H2O(l) → CH3CH2CO2−(aq) + H3O+(aq) Ka = 1.3000e-5

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.85QE

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Concept explainers

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.

Arrhenius Acid

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

What is the [CH₃CH₂CO₂⁻] in a solution which is 0.1416 M in CH₃CH₂CO₂H and 0.1929 M in HNO₃?

CH₃CH₂CO₂H(aq) + H₂O(l) → CH₃CH₂CO₂⁻(aq) + H₃O⁺(aq)

K_a = 1.3000e-5

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