If you were to have a stock solution with a concentration of 1.475 M and performed a serial dilution as shown in Fig. 5.1, what would the concentrations be in flasks A, B, C, and D
If you were to have a stock solution with a concentration of 1.475 M and performed a serial dilution as shown in Fig. 5.1, what would the concentrations be in flasks A, B, C, and D
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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- If you were to have a stock solution with a concentration of 1.475 M and performed a serial
dilution as shown in Fig. 5.1, what would the concentrations be in flasks A, B, C, and D?
Transcribed Image Text:The image represents a serial dilution process involving a stock solution and four beakers labeled A, B, C, and D.
1. **Stock Solution Beaker:**
- Contains the initial stock solution.
2. **Beaker A:**
- 10.00 mL of the stock solution is transferred to Beaker A.
- An additional 10.00 mL of water (H₂O) is added, resulting in a total volume of 20.00 mL.
3. **Beaker B:**
- 10.00 mL from Beaker A is transferred to Beaker B.
- Another 10.00 mL of water (H₂O) is added, resulting in a total volume of 20.00 mL.
4. **Beaker C:**
- 10.00 mL from Beaker B is transferred to Beaker C.
- 10.00 mL of water (H₂O) is added, resulting in a total volume of 20.00 mL.
5. **Beaker D:**
- 10.00 mL from Beaker C is transferred to Beaker D.
- Another 10.00 mL of water (H₂O) is added, resulting in a total volume of 20.00 mL.
**Figure 5.1** demonstrates the dilution steps, showing the gradual decrease in concentration as the solution is diluted through each successive transfer and addition of water.
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