For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M) **(Top screenshot is slide 11, and bottom is slide 12)**
For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M) **(Top screenshot is slide 11, and bottom is slide 12)**
For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M) **(Top screenshot is slide 11, and bottom is slide 12)**
For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation.
Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M)
**(Top screenshot is slide 11, and bottom is slide 12)**
Transcribed Image Text:### pH Range of Acid-Base Indicators
This chart illustrates the pH range over which various acid-base indicators change color. Each bar represents an indicator, with the color transitions occurring within specific pH ranges. This visual guide is useful for selecting appropriate indicators for titrations and understanding pH changes in different solutions.
#### Key:
- **Crystal Violet:** Changes color from yellow at pH 0 to blue at pH 2.
- **Thymol Blue:** Orange at lower pH of 2, transitioning to yellow at pH 4.
- **2,4-Dinitrophenol:** Yellow at pH 2, changing to a different shade of yellow-pass at pH 4.
- **Bromophenol Blue:** Yellow to purple transition occurs from pH 3 to 5.
- **Bromocresol Green:** Yellow to blue transition between pH 4 and 6.
- **Methyl Red:** Red at pH 4, turning yellow at pH 6.
- **Alizarin:** Yellow to red transition between pH 5 and 7.
- **Bromthymol Blue:** Transitions from yellow to blue over the pH range of 6 to 8.
- **Phenol Red:** Yellow at pH 6, shifting to red at pH 8.
- **Phenolphthalein:** Colorless in acidic solution, turns pink over pH 8 to 10.
- **Alizarin Yellow R:** Changes from yellow at pH 10 to red at pH 12.
This chart provides a clear representation of how each indicator can be effectively used based on the desired pH range for different chemical analyses and laboratory applications.
Transcribed Image Text:**Buffer Capacity vs. pH Change**
This graph illustrates the relationship between buffer capacity and pH change. The x-axis represents the pH values ranging from 4.7 to 5.1, indicating how the pH changes under different conditions. The initial pH is marked as 4.74.
The y-axis represents the concentration of buffer components, measured in molarity (M), with specific concentrations marked as 1.0 M, 0.30 M, 0.10 M, and 0.030 M.
**Description of the Graph:**
- **1.0 M Buffer**: This buffer solution shows a very slight change in pH, maintaining stability close to the initial pH of 4.74.
- **0.30 M Buffer**: This concentration also maintains stable pH, with only a minor increase in pH value.
- **0.10 M Buffer**: Displays a noticeable but controlled increase in pH.
- **0.030 M Buffer**: This component shows the largest increase in pH, highlighting a limited buffer capacity at lower concentrations.
**Conclusion:**
Higher concentrations of buffer components provide greater resistance to changes in pH, demonstrating increased buffer capacity. As the concentration decreases, the ability of the buffer to maintain the initial pH diminishes.
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.
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