1. A student doing the experiment in this module extended the study of the [CoCl4]2 ion /[Co(H2O)6]2+ ion equilibrium. In one test tube, the student added silver nitrate (AgNO3) to a blue equilibrium mixture prepared from CoCl2. The reaction mixture became pink and cloudy, and a white precipitate settled out leaving a clear, pink solution. The student identified the precipitate as silver chloride, AgCl. a) Briefly explain how these observations are consistent with Le Chatelier's principle. b) In a second test, the student placed a test tube containing a pink equilibrium mixture in a hot-water bath. The solution turned blue, When the student removed the test tube from the hot-water bath and placed it in an ice-water bath, the solution turned pink. c) Is the forward reaction in the [CoCl4]2 ion /[Co(H2O)6]2+ ion equilibrium exothermic or endothermic? d) Briefly explain how the student's observations support your answer to (2). e) Write the net ionic equation for this equilibrium, including heat. 2. The popular antacid, Milk of Magnesia, is a suspension of magnesium hydroxide, Mg(OH)2. In water, Mg(OH)2 undergoes the reaction shown : Mg(OH)2(S,white)Mg2+(aq)+2OH-(aq) a) What would you observe if you add an acid to an equilibrium mixture containing Mg(OH)2 in water? b) Write a chemical equation that accounts for the effect of the added acid. c) Briefly explain how your answer is consistent with Le Chatelier's principle