QUESTION 10If you know Kb for ammonia, NH 3, you can calculate the equilibrium constant, Ka, for the following reaction:NH4* + H20 =NH3 + HgO*using the equation:O Ka = Kb/ KywO Ka = Kw/ KbO Ka = Kw × KbO Ka=1/KbClick Save and Submit to save and submit. Click Save All Answers to save all answers.MacBook Air00020F7F8F4F5F6F2F3C@%24&.%232358.

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QUESTION 10 If you know Kb for ammonia, NH 3, you can calculate the equilibrium constant, Ka, for the following reaction: NH4 + H20 NH3 + H30 using the equation: O Ka = Kb/ Kw O Ka = Kw/ Kb O Ka = Kw x Kb Ka =1/ Kb

QUESTION 10 If you know Kb for ammonia, NH 3, you can calculate the equilibrium constant, Ka, for the following reaction: NH4 + H20 NH3 + H30 using the equation: O Ka = Kb/ Kw O Ka = Kw/ Kb O Ka = Kw x Kb Ka =1/ Kb

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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.

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