Calculations:
1.
0
2
4
6
8
10
12
0
2
4
6
8
10
12
R² = 0
Chem Lab Data
Standard Concentration (M)
Absorbance (A)
Standard Concentration (M)
Absorbance (A)
0.500 x 10^5
0.095
1.00 x 10^5
0.134
2.00 x 10^5
0.216
3.00 x 10^5
0.302
4.00 x 10^5
0.505
Slope
9100.78125
YIntercept
0.041082031
My Prepared Iron Solution
1.96 x 10^5 M
0.138 A
2.
Molarity of concentrate x Volume of concentrate = Molarity of dilute x Volume of dilute
(1.96 x10^5 M)x(.100 L) = (molarity after first diluted) x (.010 L)
Molarity after first dilution = (1.96 x10^5 M) x (.100 L)/(.010 L)
Molarity of first dilution = 1.96x10^4 mol/L
(1.96 x10^4 M) x (.100 L) = (Molarity of original solution) x (.005 L)
Molarity for Second Dilution = (1.96x10^4 M)(.100 L)/(.005 L)
Molarity for Second Dilution = 3.92 x10^3 mol/L
Number for Moles of Iron Solution = (Molarity) x (Volume)
Number for Moles of Iron Solution= (3.92x10^3 M)x(.005 L)
Number for Moles= 1.96x10^5 moles of solute
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Grams of solute= (Molar mass of iron solute)x(number of moles of iron solution)
Grams of solute= (55.85 grams/mol iron)x(1.96x10^5 moles iron)
Grams of solute= 1.09 x10^3 grams of iron = 1.09 milligrams of iron
Questions:
1.Can you think of other metals, besides iron, that are essential for human life? Name at least three.
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 Fall '12
 McFadden

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