What is electromagnetic radiation? radiation moving at the speed of light.
Spectrophotometry I.Electromagnetic Radiation = Light A.What is Light? 1.Visible light is a...
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Transcript of Spectrophotometry I.Electromagnetic Radiation = Light A.What is Light? 1.Visible light is a...
Spectrophotometry
I. Electromagnetic Radiation = LightA. What is Light?
1. Visible light is a particular kind of electromagnetic radiation
2. X-rays, UV, Infrared, Microwaves, and Radio waves are all light forms
3. Light is a form of Energy
4. All light travels in waves at “the speed of light” = c = 3 x 108 m/s
B. Characteristics of Light
1. Wavelength = distance between two peaks in a wave
a. (lambda) is the symbol
b. Meters = m is the unit
2. Frequency = number of complete waves passing a given point per second
a. (nu) is the symbol
b. Hertz = Hz = s-1 is the unit
3. Amplitude = A = measure of the intensity of the wave, “brightness”
4. The speed of light is constant: c = x a. and are inversely proportional
b. If one increases, the other decreases
c. Their product is always the speed of light = c = x = 3 x 108 m/s
II. Spectroscopy = using light to investigate a compoundA. How the experiment works
B. What color do we see?
a) What we see as the color of a compound is the complementary color to what the compound absorbs
b) Example: Absorbs red, we see green
III. Beer’s LawA. Absorbance tells us how much light is absorbed by the molecule
B. A = lc (y = mx + b) describes the absorption of light in a solution
l = the length of the cell containing the solution, usual 1 cm
c = concentration in mol/L = M
= Molar extinction coefficient = constant for a given molecule at a given wavelength of light = how well the molecule absorbs light
%Tlog2%T
100%logA
100% x I
I%T
I
IlogA
0
0
Percent T
0 10 25 50 75 100
2.0 1.0 0.6 0.3 0.1 0Absorbance
Absorbance
Concentration (mol/L)
1.0
0.5
0.00 0.00001 0.00002 0.00003 0.00004 0.00005
Slope = l [L/mol∙cm][cm]
≈ 18,000 for our red dye
IV. Today’s ExperimentA. Make a Beer’s Law Calibration Curve using a Stock Solution
1. Calculating the concentration of your stock solution: (Ex: 0.0788g/L)
2. Calculations for the calibration curve samples: M1V1 = M2V2
3. An Excel Template is available at faculty.swosu.edu/tim.hubin in the “Shared Folder” link called “Spectrophotometry Lab Excel sheet”
Sample # 1 2 3 4 5 6
mL DyeStock Soln
0.50 1.00 1.50 2.00 2.50 3.00
mL Water 9.50 9.00 8.50 8.00 7.50 7.00
Molarity
Lmolxg
mol
L
g/1059.1
44.496
10788.0 4
LmolxL
LLmolx
L
mol
LL
molL
L
molx
/100.8010.0
00050.01059.1
X
010.0 X
00050.01059.1
6
4
4
B. Find the concentration of an unknown sample of the red dye
1. We will give you an unknown amount of the stock solution
2. Dilute it to 25 ml in a volumetric flask
3. Calculate the absorbance (from %T) on the Spec. 20
4. Use your spreadsheet to calculate the concentration from the absorbance
5. Example Calculation: %T = 15% for your diluted unknown
C. Make 100ml of a solution of a known concentration (2.5 x 10-5 M)
LmolxcmcmmolL
/1057.4)1)(/000,18(
0.824AccA
824.015log2%Tlog2A
5
solutionstock of 7.150157.0
1059.1
100.0 105.2
X
100.0 105.2
X1059.1
VMVM
4
5
54
2211
mlL
Lmolx
LLmolx
L
LL
molxL
L
molx
%100% xA
CAError
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