CoCl42-(aq) + 6H2O(l) >< Co(H2O)62+(aq) + 4Cl-(aq) 1) What was the original color of the cobalt solution? 2) What color did you observe after adding the concentrated HCl solution? 3) What color did you observe after adding the DI water? 4) Assume that the dynamic equilibrium represented in the equation is present in the original solution you placed in the test tube. Based on LeChatelier’s Principle, as stated above, you will interpret your observations in 2, above. a) When hydrochloric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be favored? b) Assume that the system rapidly returns to equilibrium. At this new position of equilibrium, is there more or less Co(H2O)62+present after the addition of the acid? Based on this, what happened to the amount of CoCl42-?
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.
CoCl42-(aq) + 6H2O(l) >< Co(H2O)62+(aq) + 4Cl-(aq)
1) What was the original color of the cobalt solution?
2) What color did you observe after adding the concentrated HCl solution?
3) What color did you observe after adding the DI water?
4) Assume that the dynamic equilibrium represented in the equation is present in the original solution you placed in the test tube.
Based on LeChatelier’s Principle, as stated above, you will interpret your observations in 2, above.
a) When hydrochloric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be favored?
b) Assume that the system rapidly returns to equilibrium. At this new position of equilibrium, is there more or less Co(H2O)62+present after the addition of the acid? Based on this, what happened to the amount of CoCl42-?
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