For the prelab today, all solutions were made using the procedure as outlined in your lab manual. When the absorbances of the solutions were measured, the following data were collected: Part 1 Part 2 Solution Absorbance Solution Absorbance 1 0.000 1 0.000 2 0.300 2 0.343 3 0.450 0.498 4 0.600 0.642 0.750 0.777 Use the data given above to calculate the average value of K for the equilibrium: Fe3*(aq) + SCN' (aq) Fe(SCN)2*(aq) Average K = 3. 4)

For the prelab today, all solutions were made using the procedure as outlined in your lab manual. When the absorbances of the solutions were measured, the following data were collected: Part 1 Part 2 Solution Absorbance Solution Absorbance 1 0.000 1 0.000 2 0.300 2 0.343 3 0.450 0.498 4 0.600 0.642 0.750 0.777 Use the data given above to calculate the average value of K for the equilibrium: Fe3(aq) + SCN' (aq) Fe(SCN)2(aq) Average K = 3. 4)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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a. 0.35 b. 0.30 c. 0.010 d. 0.008 e. 0.009
When using a spectrophotometer to measure concentration of a solution, which of the following absorbance readings would indicate the highest concentration? 1. 0.56 2. 0.32 3. 1.34 4. 1.28
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A standard curve of absorbance vs. concentration has a linear trendline of y = 0.56x + 0.987. Use this trendline to calculate the concentration of an unknown sample that has an absorbance of 1.245.
You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.
Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…
A medical lab technician creates a standard solutions of percent hemoglobin in whole blood. The technician measures the absorbance of each solution at 520 nm and creates a standard curve of the absorbance versus percent hemoglobin in whole blood and finds the linear equation below, with an R2 of 0.9985. y= 0.0523x + 0.072 A patient sample has an absorbance of 0.893. Using the standard curve data, calculate the percent hemoglobin in the patient sample.
3
The spectroscopic data in the table is generated with five solutions of known concentration. Concentration (M) Absorbance 0.0170 0.0586 0.0340 0.117 0.0680 0.234 0.136 0.469 0.272 0.937 If the concentration is on the x-axis, what is the slope of the line formed by these points? slope = M-! * TOOLS x10