A. The unknown sample was purple in color and was verified to only contain blue and red dyes. Beers law plot data:
Red at 522nm Abs = 1.552 x 105 * Concentration + 0.03418 R2 = 0.9996
Blue at 622nm Abs = 9.868 x 104 * Concentration + 0.006422 R2 = 0.9997
Absorbance obtained of the unknown purple dye:
Red Color Abs = 0.754 Correct
M
Blue Color Abs = 0.224 Incorrect
2.20
×
10
−
6
2.20
×
10
-
6
M
B. Use the data you collected in lab on the previous side to determine how you would make 1 .00 L of the secondary dye that is the same color. The MW of the dyes are:
Red-3 (R-3), erythrosine, C20H6I4Na2O5, MW 879.86 g/mol.
Blue-1 (B-1), brilliant blue, C37H34N2Na2O9S3, MW 792.85 g/mol.
Yellow-5 (Y-5), tartrazine, C16H9N4Na3O9S2, MW 534.3 g/mol.

In order to make more dye, you will need to start with solid materials. So, you must calculate how many grams of the appropriate dyes you need.
Red Dye = Correct g/L
Blue Dye = Correct0.00174 g/L

C. Write a short argumentation paragraph explaining why you know which two dyes to use as well as how you know how much to use. Look at the correlation coefficients (R =) for each of the Beer’s Law plots and discuss how linear each equation is (how good your data is) by how close the value is to 1.000. Attach that paragraph to this sheet to turn in.