Question

1)If a Solution absorbed yellow light, what color would the solution appear to be?

2)Calculate the concentration of a solution obtained when 15.00ml of 2.00x10-3 M KMnO4 is measured from a buret into a 50ml volumetric flask which is then filled to the 50.00 ml graduated mark with distilled water

3)A graph of a absorbed vs.concentrated yields a linear standard curve for a set of standard solutions. Use a graphical analysis program to plot the following absorbents (y) vs. concentration (x) data:

Aborbants	Concentration (M)
0.347	6.00x10-4
0.277	4.80x10-4
0.208	3.60x10-4
0.139	2.40x10-4
0.069	1.20x10-4

Hint: the concentration are so tiny that they will show up as zero in the graphical analysis   data table unless you change the display from 3 places after the decimal to 3 significant figures. (recall this can be changed after double-clicking on the column heading.) This will not affect the graph.

What is the slope of the graph?

4) Suppose that an unknown sample is analyzed spectrophotometrically (at the same wavelength as that used for the standard curve measurements) and the absorbance was found to be 0.194. use the standard curve to determine the concentration of the unknown.

Answer 1