9. You prepare a mixture to use to measure the equilibrium constant of the reaction of...
9. You prepare a mixture to use to measure the equilibrium constant of the reaction of Fe3+ and SCN- ions. You mix these things in a 25.00 mL volumetric flask and then diluting to the volume of the flask. 3.00 mL 0.00400 M KSCN 5.00 mL 2 M HNO3 10.00 mL 0.00400 M Fe(NO3)3 How many millimoles of SCN- are there in this mixture initially?
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9. You prepare a mixture to use to measure the equilibrium
constant of the reaction of...
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by...
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by mixing these things in a 25.00 mL volumetric flask and then diluting to the volume of the flask with 0.3 M HNO3. 5.00 mL 0.00200 M NaSCN 10.00 mL 0.30 M Fe(NO3)3 What is the concentration of FeSCN2+ in this mixture? [Pay attention to the values to determine which reactant is being driven to completely react...] 2. You prepare a mixture to use to...
Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...
Calculate the initial concentration of iron(III) in
solution #1, #2, #3.
Beaker (mL) Table 1. Reagent Solutions Provided by the Stockroom Solution Name Reagent [Reagent] (M) Volume (mL) Standard iron Fe(NO3)3 2.50 x 10 in 0.10 M HNO3 nitric acid HNO3 0.10 120 35 50 250 conc. SCN KSCN 0.50 30 50 dilute SCN KSCN 2.50 x 10-3 30 50 Worksheet 1 #1 5.00 #2 10.00 #3 15.00 Dilute iron (mL) [Fe**] (M) [Fe(SCN)?*] (M) %T 480 58.9 35.8 21.5...
Show all work to receive full credit. Express answers to the correct number of significant figures. Note: Complete...
Show all work to receive full credit. Express answers to the correct number of significant figures. Note: Complete the table below by calculating the initial SCN and equilibrium Fe(SCN)2+ concentrations for each of the five standard solutions. In addition to the volume of KSCN indicated in the table below each solution contains 5.00 mL of Fe(NO,)a and sufficient 0.050 M HNO3 to produce a total volume of 25.00 mL of solution. 1. Fe3+ +SCN Fe(SCN)2+ 0.00200 M Molarity of KSCN...
As described in part A of the lab, you are preparing a solution by adding 2.00...
As described in part A of the lab, you are preparing a solution by adding 2.00 mL of 0.00200 M KSCN in HNO3 and 25.00 mL of 0.200 M Fe(NO3)3 in HNO3 into a clean, labeled 100.00 mL volumetric flask and diluting to the 100.00 mL mark with 0.25 M HNO3. Calculate the final concentration of KSCN in HNO3. 0.00200 M 0.000400 M 0.0000400 M 0.0000315 M 0.0500 M
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you...
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
DO ALL PARTS OF QUESTION AND USE SIGNIFICANT FIGURES!!!!!!!!! IF YOU DO NOT DO THIS I...
DO ALL PARTS OF QUESTION AND USE SIGNIFICANT FIGURES!!!!!!!!! IF
YOU DO NOT DO THIS I WILL DOWNVOTE YOU
HERE ARE THE QUESTIONS:
INFORMATION TO USE FOR CALCULATING QUESTIONS:
QUESTION 1 For all of the samples, [Fe3+10 = _M QUESTION 2 For sample 1, [SCN lo = _M. QUESTION 3 For sample 2, [SCN lo = _M For the prelaboratory assignment, you will need to calculate the initial concentrations of [Fe3+10 and [SCN-10 for samples 1-5 that you will use...
Ferric Thiocyanate Standard Solution In Part A of this experiment you are instructed to prepare a...
Ferric Thiocyanate Standard Solution In Part A of this experiment you are instructed to prepare a solution as follows Pipette 10.00 mL of 0.150 M Fe3 solution, and 5.00 mL of 5.00x 10-4 M SCN solution in a 25.00 mL volumetric flask. Dilute to the mark with 0.100 M HNO3 and mix well. Calculate and enter the concentration of FeSCN2+ in this solution and, also, write it in your notebook. (It will be required for your Report sheet.) [FesCN2+1 6M...
3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium...
3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium molar con- centration of FeNCS is assumed to equal the initial molar concentration of the SCN in the reaction mixture. Why is this assumption valid? A. A Set of Standard Solutions to Establish a The set of standard solutions is used to determine the absorbance of known molar con- centrations of FeNCS2. A plot of the data, known as a calibration curve, is used...
Standard solutions of [Fe(SCN)2-] were prepared and their absorbance measured in order to study the Keq...
Standard solutions of [Fe(SCN)2-] were prepared and their absorbance measured in order to study the Keq for the reaction Fe3+ + SCN- <=> FeNCS2+ A plot of absorbance verses concentration of [Fe(SCN)2-] is shown below. To determine the Keq for the above reaction, 10.00 mL of 0.00200 M Fe(NO3)3 solution is mixed with 5.00 mL of 0.0020 M KSCN and diluted with 5.0 mL 0f 0.10 M HNO3. The absorbance of this red solution is found to be 0.322....
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x...
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C.
A student mixes 5.12 mL of 4.02 x 10...
Calculate the initial concentration of iron(III) in
solution #1, #2, #3.
Beaker (mL) Table 1. Reagent Solutions Provided by the Stockroom Solution Name Reagent [Reagent] (M) Volume (mL) Standard iron Fe(NO3)3 2.50 x 10 in 0.10 M HNO3 nitric acid HNO3 0.10 120 35 50 250 conc. SCN KSCN 0.50 30 50 dilute SCN KSCN 2.50 x 10-3 30 50 Worksheet 1 #1 5.00 #2 10.00 #3 15.00 Dilute iron (mL) [Fe**] (M) [Fe(SCN)?*] (M) %T 480 58.9 35.8 21.5...
Show all work to receive full credit. Express answers to the correct number of significant figures. Note: Complete the table below by calculating the initial SCN and equilibrium Fe(SCN)2+ concentrations for each of the five standard solutions. In addition to the volume of KSCN indicated in the table below each solution contains 5.00 mL of Fe(NO,)a and sufficient 0.050 M HNO3 to produce a total volume of 25.00 mL of solution. 1. Fe3+ +SCN Fe(SCN)2+ 0.00200 M Molarity of KSCN...
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
DO ALL PARTS OF QUESTION AND USE SIGNIFICANT FIGURES!!!!!!!!! IF
YOU DO NOT DO THIS I WILL DOWNVOTE YOU
HERE ARE THE QUESTIONS:
INFORMATION TO USE FOR CALCULATING QUESTIONS:
QUESTION 1 For all of the samples, [Fe3+10 = _M QUESTION 2 For sample 1, [SCN lo = _M. QUESTION 3 For sample 2, [SCN lo = _M For the prelaboratory assignment, you will need to calculate the initial concentrations of [Fe3+10 and [SCN-10 for samples 1-5 that you will use...
Ferric Thiocyanate Standard Solution In Part A of this experiment you are instructed to prepare a solution as follows Pipette 10.00 mL of 0.150 M Fe3 solution, and 5.00 mL of 5.00x 10-4 M SCN solution in a 25.00 mL volumetric flask. Dilute to the mark with 0.100 M HNO3 and mix well. Calculate and enter the concentration of FeSCN2+ in this solution and, also, write it in your notebook. (It will be required for your Report sheet.) [FesCN2+1 6M...
3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium molar con- centration of FeNCS is assumed to equal the initial molar concentration of the SCN in the reaction mixture. Why is this assumption valid? A. A Set of Standard Solutions to Establish a The set of standard solutions is used to determine the absorbance of known molar con- centrations of FeNCS2. A plot of the data, known as a calibration curve, is used...
A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C.
A student mixes 5.12 mL of 4.02 x 10...
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