Le Chatelier\'s Principle: Predicting the Shifts in Equilibrium Consider the fol

Question

Le Chatelier's Principle: Predicting the Shifts in Equilibrium Consider the following chemical equilibrium: Co(H20)3(aq) + 4Cl- (aq) = [Cociu]?- (aq) + 6H2O(l) • At room temperature, the reaction system is purple • When the system has a greater concentration of [Coci4]?- the reaction mixture turns more blue. • When the system has a greater concentration of Co(H2O)3+ , the reaction mixture turns more pink. Co(H,O); *(aq) COCL2-(aq) Predict what will happen when Nacl is added to the above solution at equilibrium. Remember that NaCl(aq) consists of Nat (aq) and Cr (aq) ions. Part A The equilibrium will shift toward ( Please choose upon addition of NaCl(aq). Submit My Answers Give Up Part B The concentration of Co(H20) (aq) will Please choose upon addition of NaCl(aq) to the equilibrium mixture. Submit My Answers Give Up Part C The concentration of [CoCl4]-(aq) will ( Please choose upon addition of NaCl(aq) to the equilibrium mixture. Submit My Answers Give Up Part D The color of the solution will become more Please choose = Submit My Answers Give Up

Explanation / Answer

NaCl has Cl- ion which is also present in left side of reaction.

So by adding NaCl we are increasing concentration of reactants andd by le chateliers principle increase in concentration of reactants will lead to forward reaction and more amount of CoCl42- will be formed and hence

a. equilibrium shift towards right side

b. conc of Co(H2O)62+ will decrease

c. Conc of CoCl42- will increase

d. color of solution will become blue

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