PART 4 Co(H2O)62++ 4 Cl-1 (aq) CoC14-2 (aq) + 6 H2O (1) 1. Place a few crystals
ID: 939010 • Letter: P
Question
PART 4 Co(H2O)62++ 4 Cl-1 (aq) CoC14-2 (aq) + 6 H2O (1) 1. Place a few crystals of CoCl2 6H20 into each of three test tubes. Label your test tubes Tube 1, Tube 2 and Tube 3 2. Add 2 mL of water to Tube 1. Stir the crystals to dissolve them into solution. Record these observations: What is the color of this solution? What is the dominant species of cobalt in this solution? Explain your observations with a chemical equation. 3. Add 2 mL of 12 M HCI to Tube 2. Tube 2 will be used steps 3-6. . Stir the crystals to dissolve them into solution. Record these observations: What is the color of this solution? What is the dominant species of cobalt in this solution? 4. Slowly add distilled or deionized water drop by drop with stirring, until no further color change occurs. Record these observations: What is the color of the solution? What is the dominant species of cobalt in this solution? Explain your observations using a chemical equation. 5. Now put Tube 2 into a hot-water bath and observe the color of the solution. Record these observations: What is the color of the solution at room temperature? What is the color of the solution in the hot-water bath? What is the dominant species of cobalt in the hot water bath? 6. Take Tube 2 out of the hot-water bath and place it in an ice bath. Observe the color of the solution. Record these observations: What is the color of the solution in the ice bath? What is the dominant species of cobalt in this solution? Explain your observations using the ideas presented in the Discussion sectionExplanation / Answer
If we add sodium chloride to the system it would release the Cl- ions in the sysem,
[Co(H2O)6] +2 (alc) + 4 Cl-1 (alc)<——> [CoCl4] -2 (alc) + 6 H2O (alc)
if we increase the Cl- ions concentration the system would try to decrease it and thus the equilibrium would shift towards the right.
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