Procedure: color of the Co(H2O)s 2 solution in your Data Sheet. (Note: You might
ID: 1062337 • Letter: P
Question
Procedure: color of the Co(H2O)s 2 solution in your Data Sheet. (Note: You might want to use a graduated cylinder to measure 2 known as or sometimes plainly as Also, Co(Haoys" is also 2. Using a dropper, carefull add the CooHzos solution concentrated HC1 dropwise into until the reaction changes color (Note: At least 20 drops but no more than 35 drops) Gently mix the contents of test tube by holding the upper portion of the test tube and rotating the test tube in a circular motion. CAUTION: Never out any part Our body in contact with the concentrated acid. Do NOT put ur finger over the test the acid r additio tube to shake it. Watch the instructor demonstra the and the mixing of the contents of the test tube. Record the color of this product in your Data Sheet. Prepare an ice bath by placing about half a handful ofice into a 250 mL beaker. Then a inthe 3. add approximately 50 m distilled into the beaker. Place the test tube previous step into the ice bath until the color changes. Record the color of this solution into the Data Sheet. 4. Remove the test tube from the ice bath, and warm the test tube using the palm of your hand until the color change. Record the color of this solution into the Data 5. Using a wash bottle, slowly add distilled water into the test tube above until the colo change. Record the color of this solution into the Data Sheet. 6. (ftime permits, gently heat the test tube using a Bunsen burner. Instructor will demonstrate the proper technique. Do not point the test tube at anyone. Heat onl upper part of the liquid by passing it over the blue flame back and forth.) Discard all waste into the proper waste container. 7.Explanation / Answer
(1) According to Le-chatlier's principle, increase in temperature favours endothermic reaction. It retanis its pink colour.
(2)
(a) Adding HCl increses the concentration of Cl- ion, so it shifts the equilibrium position towards right side.
(b) Cooling the solution favours the exothermic reaction, hence it shifts the equilibrium position towards left side. SInce backward reaction is exothermic in nature.
(c) Adding heat increse the temperature which favours the endothermic reaction, so it shifts the equilibrium towards right side since forward reaction is endothermic in nature.
(d) Addintion ofwater increse the amount of products so it shifts the equilibrium towards left side.
(3) We get anhydrous cobalt (II) chloride which is colour less.
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