As part of the discussion, explain your results from Part 2 within the context of Le Châtelier's Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue? Co(H,O),* + 2CI= CoCl,(H,O)2 + 4H,O II As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)
As part of the discussion, explain your results from Part 2 within the context of Le Châtelier's Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue? Co(H,O),* + 2CI= CoCl,(H,O)2 + 4H,O II As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)
As part of the discussion, explain your results from Part 2 within the context of Le Châtelier's Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue? Co(H,O),* + 2CI= CoCl,(H,O)2 + 4H,O II As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)
The procedure is as follows: Weigh out around 0.3 g of cobalt chloride hexahydrate, CoCl2•6H2O, and place it in a clean, dry
beaker. Dissolve it in 20 mL of 95% ethanol (95% ethanol contains about 5% water). Record your
observations.
Place about 3 mL of the ethanolic cobalt chloride solution in each of five dry test tubes that you have
labeled A-E. Place B in a hot water bath. (See figure and instructions below.) Place C in an ice-water
bath. Wait a few minutes for them to equilibrate to the temperatures of the baths. Compare the tubes
with the control (the ones still at room temperature, i.e. A, D, and E), and record your observations.
Add 5 drops of a saturated aqueous sodium chloride solution to D. Observe the result and compare
with A. NOTE: any clear or white precipitate that forms in the bottom of this test tube is sodium
chloride coming out of solution and is not involved with the chemical reaction that we are studying.
Add 3 drops of distilled water to E. Compare with A and D. Cool E in the ice-water bath and
compare with A and D. Heat E in the hot water bath and compare with A and D. Add an additional
3 drops of distilled water to E. Repeat the cooling/heating process, all the while comparing the
solution to the solutions in A and D. Record all of your observations.
Transcribed Image Text:As part of the discussion, explain your results from Part 2 within the context of Le Châtelier's Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue?
\[ \text{Co(H}_2\text{O)}_6^{2+} + 2\text{Cl}^- \rightleftharpoons \text{CoCl}_2(\text{H}_2\text{O)}_2 + 4\text{H}_2\text{O} \]
I \hspace{90pt} II
As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)
Transcribed Image Text:The image shows a laboratory setup featuring a test tube rack holding eight test tubes. The test tubes are labeled with colored paper (green, orange, yellow, white, and red). Behind the test tubes, a person wearing protective eyewear is visible, ensuring safety in the laboratory environment.
The test tubes contain liquids of varying colors, suggesting different chemical solutions or reactions:
1. **Green-labeled test tube** - Contains a blue liquid.
2. **Orange-labeled test tube** - Appears empty, or with colorless liquid.
3. **Yellow-labeled test tube (labeled "C")** - Appears empty, or with colorless liquid.
4. **White-labeled test tube (labeled "B")** - Appears empty, or with colorless liquid.
5. **Red-labeled test tube** - Contains a purple liquid.
The remaining tubes seem either empty or filled with colorless solutions. The background shows typical laboratory equipment such as a spray bottle and other test instruments, enhancing the authentic lab setting.
This setup may be used for chemical testing or demonstration purposes, emphasizing the importance of labels and careful observation in experimental procedures.
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
![As part of the discussion, explain your results from Part 2 within the context of Le Châtelier's Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue?
\[ \text{Co(H}_2\text{O)}_6^{2+} + 2\text{Cl}^- \rightleftharpoons \text{CoCl}_2(\text{H}_2\text{O)}_2 + 4\text{H}_2\text{O} \]
I \hspace{90pt} II
As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc45a61cd-259f-4034-96ab-adfb5c1cf9d8%2F945f50d5-c462-4815-bcd2-ce1a561aaf74%2Fmpn4vyg_processed.jpeg&w=3840&q=75)
