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You prepare a standard solution of ferrous ammonium sulfate that is 50.0 ppm in Fe. You pipette aliquots of 0.50 mL, 1.00 mL, 2.00 mL, 4.00 mL, 8.00 mL, and 10.00 mL into 100-mL volumetric flasks, add 1 mL of hydroxylamine solution, 3 mL of o-phenanthroline solution, and sufficient citrate to adjust to pH 3-4 as described in your laboratory instructions. After diluting each sample to the 100 mL mark, and allowing time for the color to develop, you record the absorbances shown in the table. The data is a bit scattered. Looks like your pipetting ability could use some improvement. However, you can still use this data as a calibration curve. Plot the data in Excel, obtain a trendline and the equation for the linear regression line. Print the graph with the equation and turn in to your laboratory instructor with your name and section printed at the top. Fe Conc. Absorbance (ppm) 0.50 1.0 2.0 3.0 4.0 5.0 0.210 0.258 0.355 0.492 0.659 0.856 Use this graph to answer the following questions: The equation for the line is in the form "y= mx + b", where m is the slope, and b is the intercept. What is the slope of the line? (Neglect units). What is the intercept of the line? (Neglect units). 40 You next add 50 mL of your unknown sample to a 100 mL volumetric flask, treat it with hydroxylamine, o-phenanthroline, and citrate as described above, dilute to the mark, and determine the absorbance of the diluted sample to be 0.722 What is the concentration of Fe in your unknown?

You prepare a standard solution of ferrous ammonium sulfate that is 50.0 ppm in Fe. You pipette aliquots of 0.50 mL, 1.00 mL, 2.00 mL, 4.00 mL, 8.00 mL, and 10.00 mL into 100-mL volumetric flasks, add 1 mL of hydroxylamine solution, 3 mL of o-phenanthroline solution, and sufficient citrate to adjust to pH 3-4 as described in your laboratory instructions. After diluting each sample to the 100 mL mark, and allowing time for the color to develop, you record the absorbances shown in the table. The data is a bit scattered. Looks like your pipetting ability could use some improvement. However, you can still use this data as a calibration curve. Plot the data in Excel, obtain a trendline and the equation for the linear regression line. Print the graph with the equation and turn in to your laboratory instructor with your name and section printed at the top. Fe Conc. Absorbance (ppm) 0.50 1.0 2.0 3.0 4.0 5.0 0.210 0.258 0.355 0.492 0.659 0.856 Use this graph to answer the following questions: The equation for the line is in the form "y= mx + b", where m is the slope, and b is the intercept. What is the slope of the line? (Neglect units). What is the intercept of the line? (Neglect units). 40 You next add 50 mL of your unknown sample to a 100 mL volumetric flask, treat it with hydroxylamine, o-phenanthroline, and citrate as described above, dilute to the mark, and determine the absorbance of the diluted sample to be 0.722 What is the concentration of Fe in your unknown?

Chemistry
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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You prepare a standard solution of ferrous ammonium sulfate that is 50.0 ppm in Fe. You pipette aliquots of 0.50 mL, 1.00 mL, 2.00 mL, 4.00 mL, 8.00 mL, and 10.00 mL into 100-mL volumetric flasks, add 1 mL of hydroxylamine solution, 3 mL of o-phenanthroline solution, and sufficient citrate to adjust to pH 3-4 as described in your laboratory instructions. After diluting each sample to the 100 mL mark, and allowing time for the color to develop, you record the absorbances shown in the table. The data is a bit scattered. Looks like your pipetting ability could use some improvement. However, you can still use this data as a calibration curve. Plot the data in Excel, obtain a trendline and the equation for the linear regression line. Print the graph with the equation and turn in to your laboratory instructor with your name and section printed at the top. Fe Conc. Absorbance (ppm) 0.50 1.0 2.0 3.0 4.0 5.0 0.210 0.258 0.355 0.492 0.659 0.856 Use this graph to answer the following questions: The equation for the line is in the form "y = mx + b", where m is the slope, and b is the intercept. What the slope of the line? (Neglect units). What is the intercept of the line? (Neglect units). You next add 50 mL of your unknown sample to a 100 mL volumetric flask, treat it with hydroxylamine, o-phenanthroline, and citrate as described above, dilute to the mark, and determine the absorbance of the diluted sample to be 0.722 What is the concentration of Fe in your unknown?
Transcribed Image Text:You prepare a standard solution of ferrous ammonium sulfate that is 50.0 ppm in Fe. You pipette aliquots of 0.50 mL, 1.00 mL, 2.00 mL, 4.00 mL, 8.00 mL, and 10.00 mL into 100-mL volumetric flasks, add 1 mL of hydroxylamine solution, 3 mL of o-phenanthroline solution, and sufficient citrate to adjust to pH 3-4 as described in your laboratory instructions. After diluting each sample to the 100 mL mark, and allowing time for the color to develop, you record the absorbances shown in the table. The data is a bit scattered. Looks like your pipetting ability could use some improvement. However, you can still use this data as a calibration curve. Plot the data in Excel, obtain a trendline and the equation for the linear regression line. Print the graph with the equation and turn in to your laboratory instructor with your name and section printed at the top. Fe Conc. Absorbance (ppm) 0.50 1.0 2.0 3.0 4.0 5.0 0.210 0.258 0.355 0.492 0.659 0.856 Use this graph to answer the following questions: The equation for the line is in the form "y = mx + b", where m is the slope, and b is the intercept. What the slope of the line? (Neglect units). What is the intercept of the line? (Neglect units). You next add 50 mL of your unknown sample to a 100 mL volumetric flask, treat it with hydroxylamine, o-phenanthroline, and citrate as described above, dilute to the mark, and determine the absorbance of the diluted sample to be 0.722 What is the concentration of Fe in your unknown?
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