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.

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter3: Mechanisms

Section: Chapter Questions

Problem 31EQ: The reaction just described is reversible. Deprotonation of the conjugate acid of an organic base by...

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