I have done the first page and have graphed but confuse ok concentration on second page

can someone please help me

Attachment 1

Attachment 2

ReportData AnalysisData for Standard SolutionsFirst, we must construct the Beer’s Law plot that you will use to find the concentration of the aspirinin your unknown samples.Mass of empty Erlenmeyer flask:Mass of Erlenmeyer flask plus standard sample:Mass of standard sample:You diluted your sample to make 250 mL of solution. What is the concentrationof this solution in mg/L:Next, pipetted portions of the above solution were transferred to a 50-mL flask to give the finalconcentration. Use the dilution formula to get the concentrations of solutions A-E:CIV1 = C2V2(10-2)The left hand side represents the initial concentration and volume, and the right hand siderepresents the final concentration and volume, respectively. Use this relationship to calculate theconcentration of each of your solutions, and record them in the table below.DATASolutionConcentration (mg/L)AbsorbanceA1600 701/4 X2 .5 X10 4) /(50×1874) – 80 7 9%6 . 812B1600 9% X2.0x 10 1) / ( Sox (o’) – 64 mg/0 – 643C(160omglix I. S xlot) / (50 Koz)- 48 mg/0. 499D(160or19/ Xt. 6xtot)/box (o’2) – 32 mg/0. 340E(1600/ X 6.SK1o’ L) /So Mo’ ) – 16 mg/L0.178Prepare a graph of the Absorbance (y-axis) vs. the concentration in mg/ mL (x-axis). Fitstraight line to the points in the graph in accordance with Beer’s Law, which states that the absorbance should be proportional to the concentration. Graph paper is provided at the end of this experiment, though you may use Excel or a similar computer program to create your graph.