3. Unknown Solution Concentration: From the calibration curve, determine the molarity of your unknown solution, not by interpolation on the graph but algebraically from the computer - generated m value in the equation for a straight line, y = mx + b. If b equals zero, then y = mx, where m is the slope of the line, x is the solution concentration and y is the measured absorbance. Since the molar absorptivity & and the path length are constants, this equation is consistent with Beer's law A = ɛbc which becomes A = mc.
3. Unknown Solution Concentration: From the calibration curve, determine the molarity of your unknown solution, not by interpolation on the graph but algebraically from the computer - generated m value in the equation for a straight line, y = mx + b. If b equals zero, then y = mx, where m is the slope of the line, x is the solution concentration and y is the measured absorbance. Since the molar absorptivity & and the path length are constants, this equation is consistent with Beer's law A = ɛbc which becomes A = mc.
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter34: Particle Size Determination
Section: Chapter Questions
Problem 34.6QAP
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Transcribed Image Text:3. Unknown Solution Concentration: From the calibration curve, determine the molarity of your
unknown solution, not by interpolation on the graph but algebraically from the computer-
generated m value in the equation for a straight line, y = mx + b. If b equals zero, then
y = mx, where m is the slope of the line, x is the solution concentration and y is the measured
absorbance. Since the molar absorptivity & and the path length are constants, this equation is
consistent with Beer's law A = ɛbc which becomes A = mc.
%3D
%3D
Transcribed Image Text:Yellow Dye Calibration Curve
y = 254.78x - 0.1414
R? = 0.9792
2.5
1.5
1
0.5
0.002
0.004
0.006
0.008
0.01
0.012
Concentration(M)
3.
2.
Absorbance
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