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b. Because of the very high concentration of KSCN used in each test tube, you can assume essentially all of the Fe(NO:)a that has been added has reacted to form FESCN?" (by Equation 2, in the Background). Calculate the molar concentration of Fe(NO3)a in each standard after it is diluted with the other solutions, which equals the concentration of FESCN?* formed in each sample (show your work for at least one of these calculations). These are the concentrations that were used in the standard curve.

b. Because of the very high concentration of KSCN used in each test tube, you can assume essentially all of the Fe(NO:)a that has been added has reacted to form FESCN?" (by Equation 2, in the Background). Calculate the molar concentration of Fe(NO3)a in each standard after it is diluted with the other solutions, which equals the concentration of FESCN?* formed in each sample (show your work for at least one of these calculations). These are the concentrations that were used in the standard curve.

Chemistry
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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I only need help answering the highlighted part b in the first picture attached. The other pictures should contain the information needed :)

Equation 2 Fe*(aq) + SCN'(aq) FESCN*"(aq) Studies of iron(I) thiocyanate 1. Standard solutions of iron(III) thiocyanate have been prepared in the screw-cap vials that are used for the spectrophotometers you used earlier this semester. They were made by mixing aqueous solutions of Fe(NO3)3 (1.0 × 10“ M), KSCN (1.0 M), and HNO3 (0.10 M) as shown in Table 1 in clean, dry vials. Note that the Fe(NO3); stock solution prepared was dissolved in 0.10 M HNO; so that all of your solutions have the same concentration of nitric acid. Table 1 Standard ID Vol. 1.0 x 10“ M Vol. 1.0 M KSCN Vol. 0.10 M ΗΝΟ Fe(NO;)3 A 1.0 mL 5.0 ml 4.0 ml 2.0 ml 5.0 mL 3.0 mL 3.0 ml 5.0 ml 2.0 ml D 4.0 mL 5.0 ml 1.0 mL E 5.0 mL 5.0 mL O0 mL
Transcribed Image Text:Equation 2 Fe*(aq) + SCN'(aq) FESCN*"(aq) Studies of iron(I) thiocyanate 1. Standard solutions of iron(III) thiocyanate have been prepared in the screw-cap vials that are used for the spectrophotometers you used earlier this semester. They were made by mixing aqueous solutions of Fe(NO3)3 (1.0 × 10“ M), KSCN (1.0 M), and HNO3 (0.10 M) as shown in Table 1 in clean, dry vials. Note that the Fe(NO3); stock solution prepared was dissolved in 0.10 M HNO; so that all of your solutions have the same concentration of nitric acid. Table 1 Standard ID Vol. 1.0 x 10“ M Vol. 1.0 M KSCN Vol. 0.10 M ΗΝΟ Fe(NO;)3 A 1.0 mL 5.0 ml 4.0 ml 2.0 ml 5.0 mL 3.0 mL 3.0 ml 5.0 ml 2.0 ml D 4.0 mL 5.0 ml 1.0 mL E 5.0 mL 5.0 mL O0 mL
Studies of iron(II) thiocyanate 1. The standard solutions of iron(II) thiocyanate (solutions of known concentration) were prepared for you by mixing the solutions as shown in Table 1. a. Based on what you learned in last week's lab, if the reaction between Fe?* and SCN" is at equilibrium and more KSCN is added, how does the reaction shift as equilibrium is restored? What happens to the concentration of Fe(NO3);? What happens to the concentration of FESCN?*? b. Because of the very high concentration of KSCN used in each test tube, you can assume essentially all of the Fe(NO:)3 that has been added has reacted to form FeSCN²* (by Equation 2, in the Background). Calculate the molar concentration of Fe(NO3)3 in each standard after it is diluted with the other solutions, which equals the concentration of FESCN?" formed in each sample (show your work for at least one of these calculations). These are the concentrations that were used in the standard curve.
Transcribed Image Text:Studies of iron(II) thiocyanate 1. The standard solutions of iron(II) thiocyanate (solutions of known concentration) were prepared for you by mixing the solutions as shown in Table 1. a. Based on what you learned in last week's lab, if the reaction between Fe?* and SCN" is at equilibrium and more KSCN is added, how does the reaction shift as equilibrium is restored? What happens to the concentration of Fe(NO3);? What happens to the concentration of FESCN?*? b. Because of the very high concentration of KSCN used in each test tube, you can assume essentially all of the Fe(NO:)3 that has been added has reacted to form FeSCN²* (by Equation 2, in the Background). Calculate the molar concentration of Fe(NO3)3 in each standard after it is diluted with the other solutions, which equals the concentration of FESCN?" formed in each sample (show your work for at least one of these calculations). These are the concentrations that were used in the standard curve.
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