![]() When reactants predominate, the solutio n looks pink and when products predominate, the solution looks blue. The reactants are of a different color (pink) than the products (blue). With a K eq of 1.7 x 10 -3 the equilibrium favors the reactants but some products are also present. The instructor will have to interpret and narrate the demonstration as the changing equilibrium of cobalt ion complexes in solution is difficult to follow. Is the reaction, as written left to right, endothermic or exothermic Cooling will shift the products towards the hydrated complex, which is more pink. If heat is added, the equilibrium will shift towards the cobalt chloride complex, which is blue in color. A change in temperature or concentration of the ions will shift the equilibrium. The tube placed in cold water will turn more pink. ![]() The tube placed in hot water will turn blue. Test tubes containing a pink solution of cobalt and chloride ions are placed in hot water and cold water. Add water, however, and the equilibrium will shift back towards the pink hydrated species. For example, when hydrochloric acid is added, the added chloride ions shift the equilibrium position in favour of blue 2- ions and water. If the chloride or cobalt concentrations increase, the equilibrium will also shift towards the blue anhydrous cobalt chloride. Initially, a beaker contains a red-pink solution of cobalt (II) chloride, present as 2+ ions and chloride ions. The equilibrium equation representing the system is ![]() An equilibrium exists between a hydrated cobalt species and anhydrous cobalt chloride, both Co ions have an oxidation state of 2+. ![]()
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