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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Question
Determine the equilibrium [FeSCN2+] for each of the solutions 1-5. Equation of the best fit line: y=3385.7x-0.0072
![**Data Analysis**
1. From the data in Table 15.2, prepare an appropriate labeled calibration curve of absorbance vs. [FeSCN²⁺] as an x-y scatter plot using Excel or another spreadsheet software (see Appendix 1). Determine the equation for the best-fit line through the data.
2. Using the equation of the best-fit line from the calibration curve, determine the equilibrium [FeSCN²⁺] for each of Solutions 1-5, and report the average. You may find it helpful to use an ICE (initial-change-equilibrium) table to set up the calculations.
**ICE Table:**
\[ \text{Fe}^{3+} (aq) + \text{SCN}^- (aq) \rightleftharpoons \text{FeSCN}^{2+} (aq) \]
| | Initial | Change | Equilibrium |
|-------|---------|--------|-------------|
| \[\text{Fe}^{3+} \] (aq) | | | |
| \[\text{SCN}^- \] (aq) | | | |
| \[\text{FeSCN}^{2+} \] (aq) | | | |
**For Your Consideration**
- What color light, and in what wavelength range of the visible spectrum, is absorbed by a violet solution?
- How will mistakenly using Solution 1 to calibrate the spectrophotometer, instead of the blank, affect the following?
- The measured absorbance for Solution 2.
- The calculated concentration of FeSCN²⁺ at equilibrium.
- The calculated concentrations of Fe³⁺ and SCN uncomplexed at equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0000f46-99cd-4ff7-a4f7-2945716c158c%2F6ecae692-e4cf-442a-852d-ae18392bc198%2Fc9gjae.jpeg&w=3840&q=75)
Transcribed Image Text:**Data Analysis**
1. From the data in Table 15.2, prepare an appropriate labeled calibration curve of absorbance vs. [FeSCN²⁺] as an x-y scatter plot using Excel or another spreadsheet software (see Appendix 1). Determine the equation for the best-fit line through the data.
2. Using the equation of the best-fit line from the calibration curve, determine the equilibrium [FeSCN²⁺] for each of Solutions 1-5, and report the average. You may find it helpful to use an ICE (initial-change-equilibrium) table to set up the calculations.
**ICE Table:**
\[ \text{Fe}^{3+} (aq) + \text{SCN}^- (aq) \rightleftharpoons \text{FeSCN}^{2+} (aq) \]
| | Initial | Change | Equilibrium |
|-------|---------|--------|-------------|
| \[\text{Fe}^{3+} \] (aq) | | | |
| \[\text{SCN}^- \] (aq) | | | |
| \[\text{FeSCN}^{2+} \] (aq) | | | |
**For Your Consideration**
- What color light, and in what wavelength range of the visible spectrum, is absorbed by a violet solution?
- How will mistakenly using Solution 1 to calibrate the spectrophotometer, instead of the blank, affect the following?
- The measured absorbance for Solution 2.
- The calculated concentration of FeSCN²⁺ at equilibrium.
- The calculated concentrations of Fe³⁺ and SCN uncomplexed at equilibrium.
Transcribed Image Text:**Graph or Data Table Explanation:**
This image contains handwritten data typically used in an educational setting to show absorbance values of various solutions.
---
**Transcription of Text:**
---
**Light blue**
A = 0.036
**A**
- **Blank:** -0.001
- **Solution 1:** 0.033
- **Solution 2:** 0.070
- **Solution 3:** 0.080
- **Solution 4:** 0.106
- **Solution 5:** 0.129
---
**Explanation:**
This data represents absorbance (A) values measured for a series of solutions, where “Blank” refers to the baseline or control measurement with an absorbance of -0.001. The absorbance values for Solutions 1 through 5 range from 0.033 to 0.129. These measurements could be used to assess the concentration of a substance in each solution.
The term "Light blue" at the top likely indicates the color of the solution or the result after a reaction occurred, which correlates with the absorbance value provided (A = 0.036).
This setup might be used in a chemistry lab for experiments involving spectroscopy or to demonstrate the principles of Beer's Law, illustrating how absorbance is related to concentration.
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