To a 125 mL Erlenmeyer flask were added 1.220 g of solid copper (II) nitrate trihydrate, 10.0 mL of water, and a magnetic stirring bar. To the stirred solution was added, in small portions, a total of 2.000 g of sodium carbonate decahydrate. The blue solid that formed was isolated by vacuum filtration, partially dried, and placed in a second 125 mL Erlenmeyer flask. To the flask was added 2.0 mL of 12 M hydrochloric acid. To the resultant yellow solution was added 0.500 g of solid copper; the mixture was heated until the solution became colorless. After cooling the solution to room temperature, addition of 10.0 mL of water caused white, solid copper (I) chloride to separate from the solution. Isolated by vacuum filtration was 0.705 g of solid copper (I) chloride. Calculate the percent yield of copper (I) chloride. The equations for the reactions performed are shown below

Cu2+(aq) + CO32-(aq) â CuCO3(s)

CuCO3(aq) + 2H+(aq) + 4Cl-(aq) â CuCl42-(aq) + H2O(l) + CO2(g)

CuCl42-(aq) +Cu(s) â 2CuCl(s) + 2Cl-(aq)

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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.

A 2.9 g sample of a caffeine/binder mixture was added to a 125mL Erlenmeyer flask and 50mL of water was added. The suspension was heated to boiling and the insoluble solid was removed by filtration. The aqueous filtrate was cooled and extracted with two 15 mL portions of dichloromethane. The combined organic layers were washed with 15 mL of a saturated sodium chloride solution and dried over anhydrous magnesium sulfate. The magnesium sulfate was removed by filtration and the organic layer was evaporated under reduced pressure to give 1.72g of white solid. The density of aqueous sodium chloride is 1g/mL and the density of dichloromethane is 1.3 gmL.

What was the percent composition of the original mixture? (Please show me the steps to get the answer. I already know the answer I just don't understand how to get to the answer)

Caffeine % = ???

Binder % = ???

In IR and NMR spectra, how would you know if unreacted benzaldehyde was a contaminate in your product?