Liquid ammonia (anhydrous NH3(0)) 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 Tries 0/5 Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Estimate [NH2] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.
Liquid ammonia (anhydrous NH3(0)) 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 Tries 0/5 Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C. mol/L Submit Answer Tries 0/5 Estimate [NH2] (mol/L) in a 7.07x10-5 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(0)) 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
Tries 0/5
Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.
mol/L
Submit Answer
Tries 0/5
Estimate [NH2] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F14f6f234-105d-4046-a76a-a0e18732da07%2Fa4665f04-8c70-4224-a5b3-3bfc22e96185%2Fb1lsh1q_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Liquid ammonia (anhydrous NH3(0)) 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
Tries 0/5
Calculate [NH4+] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.
mol/L
Submit Answer
Tries 0/5
Estimate [NH2] (mol/L) in a 7.07x10-5 M solution of acetic acid in liquid ammonia at -50°C.
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