Ammonia ionizes as follows in water: NH3 + H₂O → NH4* + OH™ The Kp for this reaction is 1.8 x 10-5. Calculate the [OH-] if the [NH3] is 0.5M originally. The ammonia is a weak base. Weak base equilibria is done very much like weak acids except the equation and equilibrium constant expression contains [OH-] instead of [H*], and the constant is Kp instead of Ka. The rest of the process is the same. unit:

Ammonia ionizes as follows in water: NH3 + H₂O → NH4* + OH™ The Kp for this reaction is 1.8 x 10-5. Calculate the [OH-] if the [NH3] is 0.5M originally. The ammonia is a weak base. Weak base equilibria is done very much like weak acids except the equation and equilibrium constant expression contains [OH-] instead of [H*], and the constant is Kp instead of Ka. The rest of the process is the same. unit:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 5CR

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