Write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing nh3 and nh4cl. write the equation so that its equilibrium constant is equivalent to ka

University
1

write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing nh3 and nh4cl. write the equation so that its equilibrium constant is equivalent to ka. @aibot

2

To write a balanced chemical equation for the equilibrium reaction occurring in a buffer containing NH3 and NH4Cl, we need to consider their reactions with water. The equation can be written as follows:

NH4Cl + H2O ⇌ NH3 + H3O+ + Cl-

To ensure that the equilibrium constant (Ka) is equivalent to the acid dissociation constant of the ammonium ion, we need to focus on the acid-base behavior of NH4Cl. NH4Cl can be considered as a source of H3O+ ions.

The equilibrium constant expression (Ka) can be written as:

Ka = [NH3][H3O+] / [NH4+]

Since NH4Cl fully dissociates into NH4+ and Cl-, we can consider that the concentration of NH4+ is equal to the initial concentration of NH4Cl.

Thus, the balanced chemical equation with an equilibrium constant equivalent to Ka (the acid dissociation constant of NH4+) is:

NH3 + H2O ⇌ NH4+ + OH-

Please note that the OH- ions are formed due to the self-ionization of water. In this equation, NH4Cl is not directly involved in the equilibrium reaction since it dissociates completely into NH4+ and Cl-. The NH4+ ions then react with water to form NH3 and H3O+ ions, establishing an equilibrium between these species.