# 11 calibration graphfall06
TRANSCRIPT
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A Calibration Graph
Experiment 11
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Introduction
Purpose: To build a calibration graph and
use it to determine concentration.
Calibration graph Used to determine
concentration of an unknown solution bymeasuring the absorption of a solution with
a known concentration.
the solution we will be using today isCuSO4
.5H20
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Absorption
Absorption is directly proportional toconcentration.
Absorption Light is passed through a
solution, at a particular wavelength. The instrument used to measure
absorption is a spectrophotometer. The
device measures the intensity of lightafter it has been projected through a
sample.
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Review
Solute Vs. Solvent
Molarity Concentration
M = moles/L of Solution moles= grams/mw
1L = 1000ml
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Review # 2
What would be the concentration if we
placed that .60 mol of NaCl into 1L of
water? M=mol/L = .60moles/1L thus .6M NaCl
Note: does not always have to be 1 L
# moles in 35 grams of NaCl ?
NaClmoles60.NaCl58g
NaCl1mole
1
NaCl35g
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Obtain and crush a small amount of CuSO4.5H20
Measure accurately 0.04grams of CuSO4.5H20
Obtain, clean, and label 4 small beakers A-D
Obtain 1 small graduated cylinder
In beaker A add your CuSO4 and 20 ml of Di. water
Under the hood add 8 drops of NH4OH
Mix Carefully
Making our calibration graph
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In B add 10 ml of cylinder A + 10ml of Di
water plus 8 drops of NH4OH In Cylinder C add 10 ml of cylinder B +
10 ml of water plus 8 drops of NH4OH
In Cylinder D add 10 ml of cylinder C + 10ml of water plus 8 drops of NH4OH
Each cylinder is the concentration of the
previous cylinder. Each cylinder will be a lighter shade of blue.
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Set wavelength to 610nm and follow the
directions on the spec 20.
Transfer a portion of your sample to test
tube one for each cylinder.
Determine the absorbance for each sample.
How to determine absorbance
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My Trial
I Used 0.040g of CuSO4.5H20
so grams / 20 mL = 0.040g
and grams /20 mL X10+2 = 4.0
my second sample is of the CuSO4 from sample #1
thus 0.020 g
my third sample of the CuSO4 from sample # 2 thus1.00X10- 2 g
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Chart on pg 152
G/20 mL. Is asking for how many
grams you used. For my trial 0.040g
G/20 mL.X 10 +2 = 4.0g
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Chart on pg 152 Continued
= 8.0 X10 -3 moles CuSO4/ 1L
For M convert to G/20 mL M/L
249.60g
0.04g CuSO4.5H2O
20 mL 1L
1000mL 1mol CuSO4.5H 2O
= M
M X 103 = 8.0
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1. Type in Data X data first
2. Highlight data
3. Click on Chart Wizard
4. Use X-Y scatter5. Pick type of graph you want to use
6. Click next
7. Add Title and Units for X and Y
8. Add trend line if required.9. Add your name date and section to
the worksheet.
How To make a Graph using Excel
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Independent Vs. Dependent Variables
Independent variable We can change this variable.
Graphed on X axis.
Dependent variable - We cannot change this variable.We measure the dependent variable as the independent
changes. Graphed on Y axis. Title of graph should be Independent Vs. Dependent
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How to place equation of line on graph
1. Right click on line
2. Click on add trend line
3. Click on linear
4. Click on options5. Click on Display equation on chart
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Graph #1
Molarity Vs. Absorbance
y = 0.0325x + 0.0505
0
0.2
0.4
0.6
0 5 10 15
Molarity (mol/L)X10+2
Absorba
nce
Lou Tisone
116-30
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Graph #2
g/20ml Vs. Absorbance
y = 0.0649x + 0.0516
0
0.2
0.4
0.6
0 2 4 6 8
g/20ml X10+2
Absorbance
Lou Tisone
116-30
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If given absorbance (y-axis)
and need concentration solve
for (x)
y=mx +b
xm
b-y
bmxy
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To Determine M X 10 +3 (from graph)
My absorbance = .448
Y= 0.0325X + 0.0505
Put abs in for Y and solve for X
12.20MX
0.0325
0.0505.448
This is M X 10 +3
To determine M simply x10-3 1.22X10-2 M
The equation of graph # 1
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Due Next Week
Calculate mol and M for each sample. Complete chart on page 152 and questions
1a-d
Question # 2 Two computerized graphs are required
(1) Absorbance Vs. Grams/20mL X10+2
(2) Absorbance Vs. Molarity X10+3
Place equation of line on graph