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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![This table provides data for an experiment involving lead(II) ions (\( \text{Pb}^{2+} \)) and iodide ions (\( \text{I}^- \)). The table is divided into sections for various calculations across four test tubes.
**Table Columns:**
- Tube Number: 1, 2, 3, 4 (columns for data entry)
**Rows for Data Entry:**
1. Initial moles of \( \text{Pb}^{2+} \) (\( \times 10^{-5} \))
2. Initial moles of \( \text{I}^- \) (\( \times 10^{-5} \))
3. Equilibrium moles of \( \text{I}^- \) (\( \times 10^{-5} \))
4. Precipitated moles of \( \text{I}^- \) (\( \times 10^{-5} \))
5. Precipitated moles of \( \text{Pb}^{2+} \) (\( \times 10^{-5} \))
6. Equilibrium moles of \( \text{Pb}^{2+} \) (\( \times 10^{-5} \))
**Equilibrium Calculations:**
- \([ \text{Pb}^{2+} ]\) at equilibrium: Space to calculate concentration
- \( K_{sp} \, \text{PbI}_2 \): Space to calculate the solubility product
- Average \( K_{sp} \, \text{PbI}_2 \): Space to find the average solubility product across all tubes
This table aids in understanding the equilibrium dynamics of lead(II) iodide precipitation and dissolution in a controlled experimental setting.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fddc1ec45-98e4-4675-b97b-277ce49cbbd0%2F29fc214d-0624-4d1f-94f4-c881a2db0154%2Fl39b9df_processed.jpeg&w=3840&q=75)
Transcribed Image Text:This table provides data for an experiment involving lead(II) ions (\( \text{Pb}^{2+} \)) and iodide ions (\( \text{I}^- \)). The table is divided into sections for various calculations across four test tubes.
**Table Columns:**
- Tube Number: 1, 2, 3, 4 (columns for data entry)
**Rows for Data Entry:**
1. Initial moles of \( \text{Pb}^{2+} \) (\( \times 10^{-5} \))
2. Initial moles of \( \text{I}^- \) (\( \times 10^{-5} \))
3. Equilibrium moles of \( \text{I}^- \) (\( \times 10^{-5} \))
4. Precipitated moles of \( \text{I}^- \) (\( \times 10^{-5} \))
5. Precipitated moles of \( \text{Pb}^{2+} \) (\( \times 10^{-5} \))
6. Equilibrium moles of \( \text{Pb}^{2+} \) (\( \times 10^{-5} \))
**Equilibrium Calculations:**
- \([ \text{Pb}^{2+} ]\) at equilibrium: Space to calculate concentration
- \( K_{sp} \, \text{PbI}_2 \): Space to calculate the solubility product
- Average \( K_{sp} \, \text{PbI}_2 \): Space to find the average solubility product across all tubes
This table aids in understanding the equilibrium dynamics of lead(II) iodide precipitation and dissolution in a controlled experimental setting.
![The table below summarizes the data collected from a series of experiments involving varying volumes of Pb(NO₃)₂, KI, and KNO₃ solutions. The goal is to observe the absorbance of each solution and determine the iodide ion concentration ([I⁻]) at equilibrium.
| Tube # | mL 0.0120 M Pb(NO₃)₂ | mL 0.0300 M KI | mL 0.20 M KNO₃ | Total vol. (mL) | Absorbance of soln. | [I⁻] at equilibrium (M) |
|--------|----------------------|---------------|----------------|-----------------|--------------------|------------------------|
| 1 | 5.00 | 2.00 | 3.00 | 10.00 | 0.381 | |
| 2 | 5.00 | 3.00 | 2.00 | 10.00 | 0.420 | |
| 3 | 5.00 | 4.00 | 1.00 | 10.00 | 0.470 | |
| 4 | 5.00 | 5.00 | 0.00 | 10.00 | 0.542 | |
**Details:**
- **Columns:**
- "Tube #" is the identifier for each sample mixture.
- "mL 0.0120 M Pb(NO₃)₂," "mL 0.0300 M KI," and "mL 0.20 M KNO₃" represent the volumes of each respective solution used in milliliters.
- "Total vol. (mL)" indicates the total volume of the mixture.
- "Absorbance of soln." measures how much light the solution absorbs, indicating the concentration of the solution.
- "[I⁻] at equilibrium (M)" would represent the concentration of iodide ions at equilibrium, though this column is not filled in the table.
This setup is typically used to study the effect of varying concentrations on the absorbance and equilibrium concentration of ions in the solution. The experiments demonstrate how the increase in KI concentration correlates with higher absorbance values, suggesting a change in ion concentration.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fddc1ec45-98e4-4675-b97b-277ce49cbbd0%2F29fc214d-0624-4d1f-94f4-c881a2db0154%2Fdl0qies_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The table below summarizes the data collected from a series of experiments involving varying volumes of Pb(NO₃)₂, KI, and KNO₃ solutions. The goal is to observe the absorbance of each solution and determine the iodide ion concentration ([I⁻]) at equilibrium.
| Tube # | mL 0.0120 M Pb(NO₃)₂ | mL 0.0300 M KI | mL 0.20 M KNO₃ | Total vol. (mL) | Absorbance of soln. | [I⁻] at equilibrium (M) |
|--------|----------------------|---------------|----------------|-----------------|--------------------|------------------------|
| 1 | 5.00 | 2.00 | 3.00 | 10.00 | 0.381 | |
| 2 | 5.00 | 3.00 | 2.00 | 10.00 | 0.420 | |
| 3 | 5.00 | 4.00 | 1.00 | 10.00 | 0.470 | |
| 4 | 5.00 | 5.00 | 0.00 | 10.00 | 0.542 | |
**Details:**
- **Columns:**
- "Tube #" is the identifier for each sample mixture.
- "mL 0.0120 M Pb(NO₃)₂," "mL 0.0300 M KI," and "mL 0.20 M KNO₃" represent the volumes of each respective solution used in milliliters.
- "Total vol. (mL)" indicates the total volume of the mixture.
- "Absorbance of soln." measures how much light the solution absorbs, indicating the concentration of the solution.
- "[I⁻] at equilibrium (M)" would represent the concentration of iodide ions at equilibrium, though this column is not filled in the table.
This setup is typically used to study the effect of varying concentrations on the absorbance and equilibrium concentration of ions in the solution. The experiments demonstrate how the increase in KI concentration correlates with higher absorbance values, suggesting a change in ion concentration.
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