Co(H2O)62+(aq) + 4 Cl–(aq)⇄CoCl42–(aq) + 6 H2O What happens to the equilibrium using Le Chateliers principle when DI water is added to this? What about when silver nitrate was added? Any precipitate formed? If so, what is the precipitate?
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.
Given Reaction
Co(H2O)6(aq.) + 4 Cl– (aq.)⇄CoCl42–(aq.) + 6 H2O
What happens to equilibrium using Le Chatelier's principle
Case 1: When DI water is Added
Case 2 : When Silver Nitrate was Added.
Precipitate Formed when Silver Nitrate was added = To be determined
Le Chatelier's principle in chemistry is used to study the effect of Concentration, temperature and pressure on Equilibrium of a reaction
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
