Answered: Typically, for a weak acid and its…

Typically, for a weak acid and its conjugate base Ka x Kb = 14 Ka / Kb = 1.0 x 10-14 Ka x Kb = 1.0 Ka / Kb = 1.0 Ka x Kb = 1.0 x 10-14

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.3: Equilibrium Constants For Acids And Bases

Problem 5RC

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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

Typically, for a weak acid and its conjugate base

	Ka x Kb = 14
	Ka / Kb = 1.0 x 10-14
	Ka x Kb = 1.0
	Ka / Kb = 1.0
	Ka x Kb = 1.0 x 10-14

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