19) Calculate the pH of a solution (aq., 25 °C) prepared by dissolving 48.026 g of ammonium nitrate (MM = 80.043 g/mol) in 2.00 L of 0.225 M ammonia solution. The Kb of ammonia is 1.79 × 10-5. a) 9.85 10.4 b) 6.82 e) 7.52 c) 4.87 f) 9.13 d)

19) Calculate the pH of a solution (aq., 25 °C) prepared by dissolving 48.026 g of ammonium nitrate (MM = 80.043 g/mol) in 2.00 L of 0.225 M ammonia solution. The Kb of ammonia is 1.79 × 10-5. a) 9.85 10.4 b) 6.82 e) 7.52 c) 4.87 f) 9.13 d)

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.

Question

19) Calculate the pH of a solution (aq., 25 °C) prepared by
dissolving 48.026 g of ammonium nitrate (MM = 80.043
g/mol) in 2.00 L of 0.225 M ammonia solution. The Kb of
ammonia is 1.79 × 10-5.
a) 9.85
10.4
b) 6.82
e) 7.52
c) 4.87
f) 9.13
d)

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