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Hello, everyone,,kinda have trouble with a challenging chem hwproblem. I dont need A, i just need help in B) and C)....i thinkits just so much information that it threw me off. Please i willonly award points if the person include units and sig figs. Pleaseonly help me if ur sure.

From combining aqueous solutions of copper (II) nitrate and sodium phosphate, you have isolated a blue solid which you believe to be copper (II) phosphate. You perform the following experiment to determine the purity of the solid you isolated. To a 50 mL volumetric flask was added 0.1280 g of copper (II) chloride dihydrate, and the flask was filled to the calibration mark with water to give Solution A. Five 10 mL volumetric flasks were obtained; using a graduated pipet, 1.00 mL of Solution A was added to the first 10 mL volumetric flask, 2.00 mL of Solution A was added to the second volumetric flask, 3.00 mL of Solution A to the third flask, 4.00 mL of Solution A to the fourth flask, and 5.00 mL of Solution A to the fifth flask. To each 10 mL volumetric flask was added 2.5 mL of 0.10 M aqueous solution of ethylenediamine (abbreviated en), and each 10 mL flask was filled to the calibration mark with water to create five Standard Solutions. The absorbance of each Standard Solution was measured at 565 nm; the values are shown in the table below. To a sixth 10 mL volumetric flask was added 0.0110 g of the blue solid thought to be copper (II) phosphate. The solid dissolved on adding 2.5 mL of 0.10 M en to the flask, and the flask was filled to the calibration mark with water to give Solution B. The absorbance of Solution B at 565 nm was 0.457. In each of the five Standard Solutions and in Solution B, the reaction shown by the following net ionic equation occurred: In each Standard Solution and in Solution B, all copper (II) ion was converted to Cu(en) it is absorbance due to Cu(en) in solution that was observed. Using the data provided, use Excel or Matlab to draw a calibration curve of absorbance versus copper (II) ion molar concentration. Include on your plot the equation for the best-fit line and the R: value for that best-fit line. (Note: you are not allowed to use M1V1 = M2V2 in performing the calculations needed to generate the calibration curve.) What is the molar concentration of copper (II) ion in Solution B? Assuming that the only source of copper (II) ion in Solution B is copper (II) phosphate, calculate the percent by mass of copper (II) phosphate in the solid dissolved in creating Solution B.

Show transcribed image text From combining aqueous solutions of copper (II) nitrate and sodium phosphate, you have isolated a blue solid which you believe to be copper (II) phosphate. You perform the following experiment to determine the purity of the solid you isolated. To a 50 mL volumetric flask was added 0.1280 g of copper (II) chloride dihydrate, and the flask was filled to the calibration mark with water to give Solution A. Five 10 mL volumetric flasks were obtained; using a graduated pipet, 1.00 mL of Solution A was added to the first 10 mL volumetric flask, 2.00 mL of Solution A was added to the second volumetric flask, 3.00 mL of Solution A to the third flask, 4.00 mL of Solution A to the fourth flask, and 5.00 mL of Solution A to the fifth flask. To each 10 mL volumetric flask was added 2.5 mL of 0.10 M aqueous solution of ethylenediamine (abbreviated en), and each 10 mL flask was filled to the calibration mark with water to create five Standard Solutions. The absorbance of each Standard Solution was measured at 565 nm; the values are shown in the table below. To a sixth 10 mL volumetric flask was added 0.0110 g of the blue solid thought to be copper (II) phosphate. The solid dissolved on adding 2.5 mL of 0.10 M en to the flask, and the flask was filled to the calibration mark with water to give Solution B. The absorbance of Solution B at 565 nm was 0.457. In each of the five Standard Solutions and in Solution B, the reaction shown by the following net ionic equation occurred: In each Standard Solution and in Solution B, all copper (II) ion was converted to Cu(en) it is absorbance due to Cu(en) in solution that was observed. Using the data provided, use Excel or Matlab to draw a calibration curve of absorbance versus copper (II) ion molar concentration. Include on your plot the equation for the best-fit line and the R: value for that best-fit line. (Note: you are not allowed to use M1V1 = M2V2 in performing the calculations needed to generate the calibration curve.) What is the molar concentration of copper (II) ion in Solution B? Assuming that the only source of copper (II) ion in Solution B is copper (II) phosphate, calculate the percent by mass of copper (II) phosphate in the solid dissolved in creating Solution B.