(Eq. 4) CuCO,(s) + 2 H* (aq) + 4 Ct (aq) → CuCl, 2 (aq) + CO(g) + H;0 6- Add 1.5 g of copper ribbon to the solution and cover with a watch glass (Eq. 5) CuCl, 2 (aq) + Cu(s) + 4 Ct (aq) → 2 CuCl, (ag) 7- Boil the solution and then allow it to simmer at low heat (keep the watch glass on top) until the solution turns amber in co 8- Wilke waiting for the color to turn amber -Place 150 mL deionized water in a clean 600 mL beaker -Place 20 mL of Acetone in a 50 mL beaker -Place 25 mL deionized water and 5 drops of 6 M HCl in another 50 ml beaker (acidified water) Place all 3 beakers in an ice bath When the color of the solution in part 7 is amber -> light yellow -carefully decant the solution (do not transfer any solid) into the 600 mL beaker which is in the ice bath. -Allow the solution to cool down, and after several minutes, you will see white crystals of CuCl form. 9- (Eq. 6) CuCl, (aq) → Cucl(s) + 3 CI (aq) 10- Filter your white crystals Wash solid with % of the acidic water (from part 8) with the vacuum on Add the other half of acidic water before the solid dries Turn vacuum off before the solid dries AN A. 508 words o Type here to search
(Eq. 4) CuCO,(s) + 2 H* (aq) + 4 Ct (aq) → CuCl, 2 (aq) + CO(g) + H;0 6- Add 1.5 g of copper ribbon to the solution and cover with a watch glass (Eq. 5) CuCl, 2 (aq) + Cu(s) + 4 Ct (aq) → 2 CuCl, (ag) 7- Boil the solution and then allow it to simmer at low heat (keep the watch glass on top) until the solution turns amber in co 8- Wilke waiting for the color to turn amber -Place 150 mL deionized water in a clean 600 mL beaker -Place 20 mL of Acetone in a 50 mL beaker -Place 25 mL deionized water and 5 drops of 6 M HCl in another 50 ml beaker (acidified water) Place all 3 beakers in an ice bath When the color of the solution in part 7 is amber -> light yellow -carefully decant the solution (do not transfer any solid) into the 600 mL beaker which is in the ice bath. -Allow the solution to cool down, and after several minutes, you will see white crystals of CuCl form. 9- (Eq. 6) CuCl, (aq) → Cucl(s) + 3 CI (aq) 10- Filter your white crystals Wash solid with % of the acidic water (from part 8) with the vacuum on Add the other half of acidic water before the solid dries Turn vacuum off before the solid dries AN A. 508 words o Type here to search
(Eq. 4) CuCO,(s) + 2 H* (aq) + 4 Ct (aq) → CuCl, 2 (aq) + CO(g) + H;0 6- Add 1.5 g of copper ribbon to the solution and cover with a watch glass (Eq. 5) CuCl, 2 (aq) + Cu(s) + 4 Ct (aq) → 2 CuCl, (ag) 7- Boil the solution and then allow it to simmer at low heat (keep the watch glass on top) until the solution turns amber in co 8- Wilke waiting for the color to turn amber -Place 150 mL deionized water in a clean 600 mL beaker -Place 20 mL of Acetone in a 50 mL beaker -Place 25 mL deionized water and 5 drops of 6 M HCl in another 50 ml beaker (acidified water) Place all 3 beakers in an ice bath When the color of the solution in part 7 is amber -> light yellow -carefully decant the solution (do not transfer any solid) into the 600 mL beaker which is in the ice bath. -Allow the solution to cool down, and after several minutes, you will see white crystals of CuCl form. 9- (Eq. 6) CuCl, (aq) → Cucl(s) + 3 CI (aq) 10- Filter your white crystals Wash solid with % of the acidic water (from part 8) with the vacuum on Add the other half of acidic water before the solid dries Turn vacuum off before the solid dries AN A. 508 words o Type here to search
In each redox reaction indicated in equations 4-6, indicate which species is oxidized and which species is reduced.
Transcribed Image Text:### Chemistry Experiment Instructions
#### Steps 6-10: Synthesis and Crystallization of CuCl
**Step 6:**
- Add 1.5 g of copper ribbon to the solution and cover it with a watch glass.
**Equation 5:**
\[
\text{CuCl}_4^{2-} (\text{aq}) + \text{Cu(s)} + 4 \text{Cl}^- (\text{aq}) \rightarrow 2 \text{CuCl}_2^{3-} (\text{aq})
\]
**Step 7:**
- Boil the solution and then let it simmer at low heat (keep the watch glass on top) until the solution turns amber in color.
**Step 8: While waiting for the color to turn amber:**
- Place 150 mL of deionized water in a clean 600 mL beaker.
- Place 20 mL of acetone in a 50 mL beaker.
- Place 25 mL of deionized water and 5 drops of 6 M HCl in another 50 mL beaker (acidified water).
- Place all three beakers in an ice bath.
**Step 9:**
- Once the color of the solution turns amber – or light yellow – carefully decant the solution (do not transfer any solid) into the 600 mL beaker which is in the ice bath.
- Allow the solution to cool down, and after several minutes, you will see white crystals of CuCl form.
**Equation 6:**
\[
\text{CuCl}_2^{3-} (\text{aq}) \rightarrow \text{CuCl(s)} + 3 \text{Cl}^- (\text{aq})
\]
**Step 10: Filter your white crystals:**
- Wash the solid with half of the acidic water (from step 8) with the vacuum on.
- Add the other half of the acidic water before the solid dries.
- Turn the vacuum off before the solid dries completely.
- Collect the purified crystals of CuCl.
These instructions describe a series of chemical reactions and physical changes involved in the preparation and crystallization of copper(I) chloride, CuCl. The process emphasizes careful temperature control and the use of various solutions to achieve the desired chemical transformation.
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
Expert Solution
Step 1
In a redox reaction if oxidation number of a species increase then that will undergo oxidation and if oxidation number of a species decreases then that will undergo reduction.
Here in the given reactions we have to find out which species undergo oxidation and which species undergo reduction.
![### Chemistry Experiment Instructions
#### Steps 6-10: Synthesis and Crystallization of CuCl
**Step 6:**
- Add 1.5 g of copper ribbon to the solution and cover it with a watch glass.
**Equation 5:**
\[
\text{CuCl}_4^{2-} (\text{aq}) + \text{Cu(s)} + 4 \text{Cl}^- (\text{aq}) \rightarrow 2 \text{CuCl}_2^{3-} (\text{aq})
\]
**Step 7:**
- Boil the solution and then let it simmer at low heat (keep the watch glass on top) until the solution turns amber in color.
**Step 8: While waiting for the color to turn amber:**
- Place 150 mL of deionized water in a clean 600 mL beaker.
- Place 20 mL of acetone in a 50 mL beaker.
- Place 25 mL of deionized water and 5 drops of 6 M HCl in another 50 mL beaker (acidified water).
- Place all three beakers in an ice bath.
**Step 9:**
- Once the color of the solution turns amber – or light yellow – carefully decant the solution (do not transfer any solid) into the 600 mL beaker which is in the ice bath.
- Allow the solution to cool down, and after several minutes, you will see white crystals of CuCl form.
**Equation 6:**
\[
\text{CuCl}_2^{3-} (\text{aq}) \rightarrow \text{CuCl(s)} + 3 \text{Cl}^- (\text{aq})
\]
**Step 10: Filter your white crystals:**
- Wash the solid with half of the acidic water (from step 8) with the vacuum on.
- Add the other half of the acidic water before the solid dries.
- Turn the vacuum off before the solid dries completely.
- Collect the purified crystals of CuCl.
These instructions describe a series of chemical reactions and physical changes involved in the preparation and crystallization of copper(I) chloride, CuCl. The process emphasizes careful temperature control and the use of various solutions to achieve the desired chemical transformation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb732abbc-b634-4376-a3f1-15affc6eeba5%2F07430917-7914-42bd-bc9a-ae2ea73bc109%2F8pb0f4d_processed.jpeg&w=3840&q=75)
