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lab 6.docx - Calculations 1 R = 0 Chem Lab Data 12 10 8...

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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 Y-Intercept 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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