The [FeSCN2+] will serve as your x-axis in the Beer’s Law plot. We will assume that all the SCN– ions react and that it functions as the limiting reagent. This means that in Part I of the experiment, mol of SCN– = mol of FeSCN2+. Based on this relationship, record the values for [FeSCN2+] so that you have your x-axis values for when you create your Beer’s Law plot. Required Calculations 1. Create an absorbance vs. concentration plot of your known standard solutions. Apply a linear fit to obtain the linear regression equation. 2. Use the linear regression equation from your plot of known solutions to determine the unknown equilibrium concentration of FeSCN2+ for each of your mixtures. 3. Use the given amounts and concentrations from Table 2 in the procedure to calculate the initial concentrations of Fe3+ and SCN- in each of your unknowns. 4. Use the values you calculated in the previous two steps to construct ICE tables to determine Keq for each unknown solution, including the one at elevated temperature. You should have a total of 6 ICE tables and 6 Keq values. You should not create an ICE table for E1 which is your blank. 5. Determine the average Keq for the room temperature unknowns.
The [FeSCN2+] will serve as your x-axis in the Beer’s Law plot. We will assume that all the SCN– ions react and that it functions as the limiting reagent. This means that in Part I of the experiment, mol of SCN– = mol of FeSCN2+. Based on this relationship, record the values for [FeSCN2+] so that you have your x-axis values for when you create your Beer’s Law plot. Required Calculations 1. Create an absorbance vs. concentration plot of your known standard solutions. Apply a linear fit to obtain the linear regression equation. 2. Use the linear regression equation from your plot of known solutions to determine the unknown equilibrium concentration of FeSCN2+ for each of your mixtures. 3. Use the given amounts and concentrations from Table 2 in the procedure to calculate the initial concentrations of Fe3+ and SCN- in each of your unknowns. 4. Use the values you calculated in the previous two steps to construct ICE tables to determine Keq for each unknown solution, including the one at elevated temperature. You should have a total of 6 ICE tables and 6 Keq values. You should not create an ICE table for E1 which is your blank. 5. Determine the average Keq for the room temperature unknowns.
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Mark S. Cracolice, Ed Peters
Chapter16: Solutions
Section: Chapter Questions
Problem 16.3TC
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The [FeSCN2+] will serve as your x-axis in the Beer’s Law plot. We will assume that all the SCN– ions react and that it functions as the limiting reagent. This means that in Part I of the experiment, mol of SCN– = mol of FeSCN2+. Based on this relationship, record the values for [FeSCN2+] so that you have your x-axis values for when you create your Beer’s Law plot. Required Calculations 1. Create an absorbance vs. concentration plot of your known standard solutions. Apply a linear fit to obtain the linear regression equation. 2. Use the linear regression equation from your plot of known solutions to determine the unknown equilibrium concentration of FeSCN2+ for each of your mixtures. 3. Use the given amounts and concentrations from Table 2 in the procedure to calculate the initial concentrations of Fe3+ and SCN- in each of your unknowns. 4. Use the values you calculated in the previous two steps to construct ICE tables to determine Keq for each unknown solution, including the one at elevated temperature. You should have a total of 6 ICE tables and 6 Keq values. You should not create an ICE table for E1 which is your blank. 5. Determine the average Keq for the room temperature unknowns.
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