![]() The quantum mechanics of complex ion formation The result is a solution with both pink and blue complex ions present, and a lavender color. If we add a sufficient amount of water to the blue solution dominated by the blue tetrachloro cobalt(II) complex ion, we can convert some of the tetrachloro cobalt(II) complex ion to hexaaqua cobalt(II) complex ion. The addition of chloride ion pushes the equilibrium to the right favoring the formation of the blue tetrachloro cobalt species product.Īddition of water to the solution pushes the equilibrium to the left favoring the pink hexaaqua cobalt species reactant. Using our understanding of LeChatelier's Principle, we can push this equilibrium to the right, by the addition of more reactant, or the left, by the addition of more product. The addition of chloride ion drives the formation of the tetrachloro cobalt(II) complex ion. The addition of hydrochloric acid to the solution provides a high concentration of chloride ion. The color is due to the presence of the pink hexaaqua cobalt(II) complex ion. Add water to the solution and observe transformation in color of solution.Ī solution of cobalt(II)chloride is a lovely pink color. Add hydrochloric acid to the solution and observe change in color.ģ. Prepare a solution of cobalt chloride in 98% ethyl alcohol.Ģ. Ingredients: cobalt chloride, hydrochloric acid, waterġ. A light pink solution turns blue, and then turns pinkish-blue.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |