please help within five minutes

timer Asked: Feb 15th, 2015

Question description

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 4.41×10-4 M solution of acetic acid in liquid ammonia at -50°C.

C. Estimate [NH2-] (mol/L) in a 4.41×10-4 M solution of acetic acid in liquid ammonia at -50°C.

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