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5. Calculate the initial concentration of Fe³+ and HSCN in each solution. a. Calculate the initial concentration of Fe3+ using M1V1=M2V2. M1 = 2.00x10-³ M (Table 2) Vi = 5.00 mL V2= 10.00 mL 0.001 M b. Calculate the initial concentration of HSCN for each solution. M1 = 2.00x10-3 M HSCN V2 = 10.00 mL Vị is given in Table 2 Find M2 for each. Answers will have 3 significant figures. 0.0002 0.0004 0.0006 Solution 1: Solution 2: Solution 3: 0.0008 Solution 4:

5. Calculate the initial concentration of Fe³+ and HSCN in each solution. a. Calculate the initial concentration of Fe3+ using M1V1=M2V2. M1 = 2.00x10-³ M (Table 2) Vi = 5.00 mL V2= 10.00 mL 0.001 M b. Calculate the initial concentration of HSCN for each solution. M1 = 2.00x10-3 M HSCN V2 = 10.00 mL Vị is given in Table 2 Find M2 for each. Answers will have 3 significant figures. 0.0002 0.0004 0.0006 Solution 1: Solution 2: Solution 3: 0.0008 Solution 4:

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’m not sure if question 5a and 5b are right or not
3. Plot the absorbance versus the [FESCN²+1. Calculate the slope of the linear regression line. Graphical Analysis would make this easier. Equilibrium solutions and Determination of the Equilibrium Constant 4. Using the absorbance values and your Beer's Law plot, determine the equilibrium concentration of FeSCN²+. This is easily calculated from the slope and y-intercept values. 5. Calculate the initial concentration of Fe3+ and HSCN in each solution. a. Calculate the initial concentration of Fe3+ using M1V1=M2V2. M1 = 2.00x10-3 M (Table 2) Vi = 5.00 mL V2= 10.00 mL 0.001 M b. Calculate the initial concentration of HSCN for each solution. M1 = 2.00x10-³ M HSCN V2 = 10.00 mL Vị is given in Table 2 Find M2 for each. Answers will have 3 significant figures. a del O.0002 Solution 1: 0.0004 0.0006 0.0008 Solution 2: Solution 3: Solution 4: 6. Calculate the equilibrium [Fe³*] and [HSCN] in each solution, using an equilibrium table. Calculate the [H*] at equilibrium. Is the additional H* produced in the reaction significant compared to the initial 0.5 M H* concentration? 7.
Transcribed Image Text:3. Plot the absorbance versus the [FESCN²+1. Calculate the slope of the linear regression line. Graphical Analysis would make this easier. Equilibrium solutions and Determination of the Equilibrium Constant 4. Using the absorbance values and your Beer's Law plot, determine the equilibrium concentration of FeSCN²+. This is easily calculated from the slope and y-intercept values. 5. Calculate the initial concentration of Fe3+ and HSCN in each solution. a. Calculate the initial concentration of Fe3+ using M1V1=M2V2. M1 = 2.00x10-3 M (Table 2) Vi = 5.00 mL V2= 10.00 mL 0.001 M b. Calculate the initial concentration of HSCN for each solution. M1 = 2.00x10-³ M HSCN V2 = 10.00 mL Vị is given in Table 2 Find M2 for each. Answers will have 3 significant figures. a del O.0002 Solution 1: 0.0004 0.0006 0.0008 Solution 2: Solution 3: Solution 4: 6. Calculate the equilibrium [Fe³*] and [HSCN] in each solution, using an equilibrium table. Calculate the [H*] at equilibrium. Is the additional H* produced in the reaction significant compared to the initial 0.5 M H* concentration? 7.
. Determination of FeSCN²* at equilibrium Label four clean 10.00 mL volumetric flasks #1-4. Using pipets, carefully prepare the four couilibrium solutions described in Table 2 below. Transfer 5.00 mL of the 2.00 X 10³ M iron nitrate solution (record the exact molarity shown) to a 10 mL volumetric flask. Add the appropriate volume of your freshly prepared HSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitric acid. Mix the solutions thoroughly. Measure the absorbance of each solution at the wavelength of maximum absorbance, 447 nm, in the spectrophotometer. Use the same instrument you used in Part B. Note that the concentration of the Fe(NO3)3 is 100 times less concentrated than that used in Part B. 1- D. 138 20. asI 3= 0.397 4=0.481 Table 2. Equilibrium Solutions Solution No. 2.00 X 10-3 M Fe(NO3)3 2.00 X 10-3 M HSCN 0.5 M HNO3 5.00 mL 5.00 mL 1.00 mL 2.00 mL 3.00 mL 1 Dilute to the mark! 3 5.00 mL 4. 5.00 mL 4.00 mL Calculations: Plan to work on these calculations in lab and organize your results in the tables that follow. Standard Solutions Calculate the molarity of HSCN for each solution using M¡V1 = M2V2. 1. M1 = 2.00x10-³ M HSCN V2 = 25.00 mL Vị is given in Table 1 Find M2 for each. Answers will have 3 significant figures. 4.00x10 M 800x10M 144x10 4 2.00x10 Solution 1: Solution 2: -4 M. 54 Solution 3: Solution 4: 2. Calculate the molarity of FESCN2* in each of the standard solutions, assuming that the initial concentration of HSCN is equivalent to the concentration of the complex, FESCN²+. 1- 2x10-4M 2= 4x 104 M 3-6x10 -4 M 45 4=8x104M
Transcribed Image Text:. Determination of FeSCN²* at equilibrium Label four clean 10.00 mL volumetric flasks #1-4. Using pipets, carefully prepare the four couilibrium solutions described in Table 2 below. Transfer 5.00 mL of the 2.00 X 10³ M iron nitrate solution (record the exact molarity shown) to a 10 mL volumetric flask. Add the appropriate volume of your freshly prepared HSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitric acid. Mix the solutions thoroughly. Measure the absorbance of each solution at the wavelength of maximum absorbance, 447 nm, in the spectrophotometer. Use the same instrument you used in Part B. Note that the concentration of the Fe(NO3)3 is 100 times less concentrated than that used in Part B. 1- D. 138 20. asI 3= 0.397 4=0.481 Table 2. Equilibrium Solutions Solution No. 2.00 X 10-3 M Fe(NO3)3 2.00 X 10-3 M HSCN 0.5 M HNO3 5.00 mL 5.00 mL 1.00 mL 2.00 mL 3.00 mL 1 Dilute to the mark! 3 5.00 mL 4. 5.00 mL 4.00 mL Calculations: Plan to work on these calculations in lab and organize your results in the tables that follow. Standard Solutions Calculate the molarity of HSCN for each solution using M¡V1 = M2V2. 1. M1 = 2.00x10-³ M HSCN V2 = 25.00 mL Vị is given in Table 1 Find M2 for each. Answers will have 3 significant figures. 4.00x10 M 800x10M 144x10 4 2.00x10 Solution 1: Solution 2: -4 M. 54 Solution 3: Solution 4: 2. Calculate the molarity of FESCN2* in each of the standard solutions, assuming that the initial concentration of HSCN is equivalent to the concentration of the complex, FESCN²+. 1- 2x10-4M 2= 4x 104 M 3-6x10 -4 M 45 4=8x104M
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