Liquid ammonia (anhydrous NH3(1)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 = NH4+ + NH2" K = 1x10-33 at -50°C Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia. Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. mol/L Submit Answer Calculate [NH4*] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Estimate [NH2"] (mol/L) in a 7.07x105 M solution of acetic acid in liquid ammonia at -50°C.
Liquid ammonia (anhydrous NH3(1)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 = NH4+ + NH2" K = 1x10-33 at -50°C Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia. Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. mol/L Submit Answer Calculate [NH4*] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Estimate [NH2"] (mol/L) in a 7.07x105 M solution of acetic acid in liquid ammonia at -50°C.
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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![Liquid ammonia (anhydrous NH3(1)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton:
2NH3 = NH4+ + NH2"
K = 1x10-33 at -50°C
Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia.
Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C.
mol/L
Submit Answer
Calculate [NH4*] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.
mol/L
Submit Answer
Estimate [NH2"] (mol/L) in a 7.07x105 M solution of acetic acid in liquid ammonia at -50°C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F26eb10a4-9023-4150-a307-859edc2786be%2F399244a6-676e-45e0-b703-761eb096efb2%2Fmt8f7i8_processed.png&w=3840&q=75)
Transcribed Image Text:Liquid ammonia (anhydrous NH3(1)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton:
2NH3 = NH4+ + NH2"
K = 1x10-33 at -50°C
Since ammonia is better proton acceptor than water, the ionization of acids is relatively enhanced in liquid ammonia. For example, acetic acid is a strong acid in liquid ammonia.
Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C.
mol/L
Submit Answer
Calculate [NH4*] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.
mol/L
Submit Answer
Estimate [NH2"] (mol/L) in a 7.07x105 M solution of acetic acid in liquid ammonia at -50°C.
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