Liquid ammonia (anhydrous NH3(l)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 NH4+ + NH2- K = 1×10-33 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. a) Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. b) Calculate [NH4+] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C. c) Estimate [NH2-] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C.
Liquid ammonia (anhydrous NH3(l)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton: 2NH3 NH4+ + NH2- K = 1×10-33 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. a) Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C. b) Calculate [NH4+] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C. c) Estimate [NH2-] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C.
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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Liquid ammonia (anhydrous NH3(l)) is often used as a solvent. Like water, ammonia undergoes autoionization by the transfer of a proton:
2NH3 NH4+ + NH2- K = 1×10-33 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.
a) Estimate [NH4+] (mol/L) in pure (i.e. neutral) liquid ammonia at -50°C.
b) Calculate [NH4+] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C.
c) Estimate [NH2-] (mol/L) in a 6.29×10-2 M solution of acetic acid in liquid ammonia at -50°C.
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