Lab 6 -Determination of the Dye Concentration in a Powerade Drink

Lab 6 – Determination of the Dye Concentration in A Powerade Drink CHM 2045L – Dr. Yavuz Petrowski The statement is: “I certify that this is my own work and I understand that if I am found to be in violation of the honor code, I will be subject to the highest penalty” Name: Merline Michelin Znumber: Z23690996 PRELAB Background: Please complete the following sections. Purpose of the experiment: In your own words, the purpose of the experiment including a brief description of the lab and the reason for doing the experiment (what we are trying to determine and how we will go about determining it). Explain the concepts we are investigating; explain why and how they are useful, and how those concepts apply to the experiment; show relevant equations if you need to. The purpose of this experiment is to determine the concentration of the in a PowerAde drink. We will go about determining this by using spectrophotometry and Beer’s Law. Spectrophotometry is a technique used to measure the intensity of light absorbed by a sample because substances absorb light at different wavelengths, this allows us to identify and quantify unknown substances. Beer-Lambert Law or Beer’s Law describes the relationship between a substances absorbency of light and concentration. These concepts apply to this experiment because by determining the unknown solution absorbency to light we can determine its concentration. By using a spectrophotometer, we cab measure the absorbency of different concentrations of different colored substances to determine the relationship betweeacubveentration and absorbency. Flow Chart: Complete the experimental procedure for this experiment by using the information provided in the power point and 360 experimental videos in a flow diagram format. A flow chart indicates the procedure of how the experiment is performed. The flow chart must be written in the correct flow chart format (box and arrow). Handwritten flow charts are not accepted. See the example of the flow chart in the canvas module. Set up and prepare equipment’s like beakers, pipette, and solutions to be used in lab. Calibrate scale, and weigh about 9.99g CuSO4 on scale. Pour into beaker and try to dissolve CuSO4 in water. Using a pipette pour the designated mL into each labelled 10mL volumetric flask. Then fill water into each flask to equal up to 10mL. Tilt each volumetric flask to mx solution with water. Pour CuSO4 solution into a 100 male volumetric flask. Clean beakers with water and pour remaining solution into flask and add more water up to line in flask. Prepare and label 4 different volumetric flask with different mL of CuSO4 (2mL, 4mL, 6mL, and 8mL). Pour some solution into a beakers and using a pipette pour 10mL into a beaker. Using a small pipette, pour some solution from the beakers into the cuvette. You will do the same for the four 10mL volumetric flask. Calibrate set the spectrophotometer wavelength to 630 nm. Insert each cuvette into the spectrophotometer to obtain the absorbency and record. Clean area and dispose of chemicals properly. Using a pipette, put some of the PowerAde drink into a cuvette and measure and record absorbency. Calculate molarity/concentration and using excel make a standard graph absorbance vs concentration e Waste Collection: Type out the chemicals used in this experiment, their hazards if applicable, and any other safety concerns associated with this experiment. You can search for the Materials Safety Data Sheet document on the internet to list hazards and safety concerns. You can add an extra row if you need extra space. Chemicals Safety Hazard water (H2O) Non-hazardous copper (II) sulfate (CuSO4) Gastrointestinal issues if ingested; skin an eye irritation; respiratory issues if inhaled DATA PROCESS Table: Fill out the following table by using the data collected through virtual 360 Lab. The concentration of unknown solution must be calculated by using Beer-Lambert calibration curve and equation of line. Solution Volume of CuSO4 Solution, mL Volume of DI Water, mL Absorbance (at 630 nm) Concentration in M 1 2.00 mL 8.00 mL 0.222 0.0800 M 2 4.00 mL 6.00 mL 0.383 0.160 M 3 6.00 mL 4.00 mL 0.527 0.240 M 4 8.00 mL 2.00 mL 0.709 0.320 M 5 0.00 mL 10.00 mL 0.400 M 0.838 From equation of line Powerade Solution 0.556 0.466 M Calibration Curve R2= 0.998 Data Processing 1. Calculate the molar concentrations of the diluted solutions and record them on your data sheet. Please use dilution formula for this calculation: M1 xV1 =M2 x V2 (concentration of the CuSO4 stock solution is 0.400 M) 2. Using Excel prepare a plot of the absorbance versus CuSO 4 concentration. Pay attention to the graphing rules. 3. Determination of the unknown concentration: a. Determine the concentration of the Powerade solution from the excel graph by using equation of line. b. Determine the concentration of the Powerade solution by using calibration curve. By using the absorbance of the unknown and marking a straight line from the y-axis to the curve then a straight line from the curve to the x-axis. 4. Complete discussion questions. CALCULATIONS: Show (type in the table) your calculations for molarity. YOU MUST SHOW ALL YOUR CALCULATIONS TO RECEIVE CREDIT FOR THEM! Proper use of significant figures and units is part of the grading. Calculations: Show Your Calculations in Table Provided: Solution Volume of CuSO4 Solution, mL 1 Volume of DI Water, mL Concentration Calculations, M M1V1=M2V2 8.00 mL (0.400 M)(2.00 mL) = M2 × 10.00 mL M2= (0.400 M)(2.00 mL)/ 10.00mL M2 = 0.0800 M (0.400 M)(4.00 mL) = M2 × 10.00 mL M2= (0.400 M)(4.00 mL)/ 10.00mL M2 = 0.160 M (0.400 M)(6.00 mL) = M2 × 10.00 mL M2= (0.400 M)(6.00 mL)/ 10.00mL M2 = 0.240 M (0.400 M)(8.00 mL) = M2 × 10.00 mL M2= (0.400 M)(8.00 mL)/ 10.00mL M2 = 0.320 (0.400 M)(10.00 mL) = M2 × 10.00 mL M2= (0.400 M)(10.00 mL)/ 10.00mL M2 = 0.400 M 2.00 2 6.00 mL 4.00 3 4.00 mL 6.00 4 2.00 mL 8.00 5 0.00 mL 10.00 Powerade Solution From Equation of Line: y=1.8x From Calibration Curve: y= 1.9475x +0.0684 Excel Graph: Directions for Excel Graph 1. Use your data table and type concentration and absorbance data into an Excel document, only type numbers, and do not include units in the data area of your excel table. Start typing concentration into cell A1, absorbance into cell B1, and so on. Start tying the numerical data into the second row and continue until the entire data is copied. 2. Select all data by clicking on the cell, and then dragging over and down to the last cell that data is written. 3. On the Excel window, find the menu item titled “insert” and in the “Charts” area click on the “Insert Scatter (X, Y)” button. A basic graph with data set should appear. 4. Edit your graph so that it contains the correct formatting components, you need a title describes the study under and labels for your x- and y- axes together with units such as unit for x axis. o To add chart components such as x and y labels, click on the top right corner of the graph, then click the menu item in the Windows ribbon titled “Chart Design”. In that menu, click on the “Add Chart Element” and select “Chart Title” and both options under “Axis Titles. You can edit the text by clicking or doubleclicking on the text in the graph and typing. 5. Right click on any of the data points and select “add trend line”. The “Format Trend line” menu that appears to the right of the window, make sure “Linear” is selected. In this same menu, click on “Set Intercept to = 0” and click on “Display equation on chart” 6. Find the concentration from equation of line. 7. Find the concentration from excel graph, mark on the graph. 8. Do not forget to save your Excel sheet and copy a screenshot of your graph into the space given. GRAPH CONSIDERATION FOR DISCUSSION & CONCLUSION As you write your discussion and conclusion paragraphs for the discussion assay, here are some tips and questions you should answer. These are in addition to the "Guidelines for a good discussion and conclusion" document in the introduction module. • Purpose of the experiment. • What is a spectrophotometer, and how is it utilized in this experiment? • What is the Beer-Lambert Law, and how is it related to absorbance and concentration? • What is dilution, and why CuSO4 solution need to be diluted? • How is the concentration calculated from absorbance readings using the Beer-Lambert Law? • What is the process for plotting a standard curve, and how is it used to analyze unknown solution? • Conclusion statement: Was this a good experiment to use to support your purpose and why? DISCUSSION & CONCLUSION ASSAY The purpose of this experiment was to determine the concentration of CuSO4and an unknown sample using spectrophotometry and Beer’s Law. A spectrophotometer is an instrument that is used to measure light absorbance and was used in this lab to quantify the absorbance of CuSO4 solution their maximum absorbance wavelength. The Beer-Lambert Law states that there is a correlation between light absorbance and concentration, providing the basis to find concentrations for unknown substances. Dilution is the process of reducing the concentration of a solution. CuSO4 solutions were diluted to ensure measurements fell within a linear range of the Beer Law and created standards for calibration. The calculations for absorbance readings is made by using the equation of the standard curve and BeerLambert Law. A standard curve is plotted by graphing absorbance as the y-axis and concentration as the x-axis. This is used to determine the concentration of an unknown solution from its absorbance. This was a good experiment to use to support my purpose. The methods used helped to determine unknown concentrations in a clear way.