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:
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![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 K, instead of Ka. The rest of the
process is the same.
unit:
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