The ionization constant for NH4+ is K = 5.8 x 10-10 at 25°C. It is in a reversible equilibrium with ammonia and H+. NH4+ --> NH3 + H+ where, H+ + NH3 --> NH4* with a k₁ = 4.000 x 1010 M-1 S-1 A temperature jump from 20°C to 25°C is made on a 0.1 M NH4Cl solution at pH 6. Calculate the relaxation time in microseconds for the reaction, assuming that the mechanism is given by the ionization equation shown. Assume that the pH is buffered.

The ionization constant for NH4+ is K = 5.8 x 10-10 at 25°C. It is in a reversible equilibrium with ammonia and H+. NH4+ --> NH3 + H+ where, H+ + NH3 --> NH4* with a k₁ = 4.000 x 1010 M-1 S-1 A temperature jump from 20°C to 25°C is made on a 0.1 M NH4Cl solution at pH 6. Calculate the relaxation time in microseconds for the reaction, assuming that the mechanism is given by the ionization equation shown. Assume that the pH is buffered.

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 3RQ: Define or illustrate the meaning of the following terms: a. amphoteric b. Kw reaction c. Kw...

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