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![I Fe3+ + SCN FESC N2+ For every mor of Fest and sent same mor of FESCN2t will be formed. [Fe3+] = 0.150M volume of Fe3+= 10.0](http://img.homeworklib.com/questions/541c73d0-71b8-11ea-9055-43badcfee8c5.png?x-oss-process=image/resize,w_560)
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Ferric Thiocyanate Standard Solution In Part A of this experiment you are instructed to prepare a...
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...
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?
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...
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...
5. In this experiment, you will prepare a standard solution for a calibration curve for the...
5. In this experiment, you will prepare a standard solution for a calibration curve for the formation of FeSCN2 complex by reaction different volumes of 0.2 M Fe(NO,), and 0.002 M NaSCN. You will use 0.05M HNO, for all dilutions. Using the table, Calculate the equilibrium concentrations of FeSCN2 Vol of Fe Vol of SCN 0.1 M HNO Equilibrium concentration Fe[SCN]2' (mL) (mL.) (mL) 10.00 0.00 10.00 10.00 1.00 9.00 10.00 2.00 8.00 10.00 3.00 7.00 10.00 4.00 6.00 10.00...
3. In this experiment, you will determine the [FeSCNP at equilibrium by measuring its absorbance at...
3. In this experiment, you will determine the [FeSCNP at equilibrium by measuring its absorbance at - 450 nm. This is possible due to which of the following statements? Fe+ (aq) + SCN (aq) FeSCN2+ (aq) a. Fe and SCN do not absorb significantly at 450 nm. b. At equilibrium, only FeSCN* is present in the solution. c. [Fe] and [SCN) are too small to absorb light. d. The equilibrium constant, Keq, is small. 4. Give the names for the...
In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN−) to form a dark...
In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN−) to form a dark red complex: [Fe(H2O)6]3+ + SCN− ⇌ H2O + [Fe(H2O)5NCS]2+ The equilibrium concentration of [Fe(H2O)5NCS]2+ may be determined by how dark the colored solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO3)3 was mixed with 1.0 mL of 9.2 ×10−3M KSCN and 8.0 mL of dilute HNO3. The color of the solution quantitively indicated that the [Fe(H2O)5NCS]2+ concentration was...
For Part A of the Equilibrium experiment, you will be preparing several standard solutions for the...
For Part A of the Equilibrium experiment, you will be preparing several standard solutions for the Beer's Law plot Using the information given in the Worksheet for Equilibrium Lab , answer the following questions. (a) What is the initial Fe3+ concentration of all of the solutions? 1.00 xM (b) What is the initial SCN1-concentrations of Solutions #1A - #5A? Solution #1A 1#1A | 1.00 Solution #2A 1.50 Solution #3A 2.00 Solution #4A2.50 Solution #41 2.50 M Solution #54 3,00 xM...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
A student made solution #3 using the experimental method in this lab, and measured an absorbance of 0.559. The starting...
A student made solution #3 using the experimental method in this
lab, and measured an absorbance of 0.559. The starting reagents are
2.00 x 10-3 M Fe(NO3)3 and 2.00 x
10-3 M KSCN.
The amount of absorption is proportional to the concentration
of
FeSCN2+. This relationship – true for many solutions – is called
“Beer’s Law”, and has the simple equation:
A = bc
where “A” is the absorption, “b” is 5174.6 for FeSCN2+ and “c”
is molarity
Make Five...
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...
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...
5. In this experiment, you will prepare a standard solution for a calibration curve for the formation of FeSCN2 complex by reaction different volumes of 0.2 M Fe(NO,), and 0.002 M NaSCN. You will use 0.05M HNO, for all dilutions. Using the table, Calculate the equilibrium concentrations of FeSCN2 Vol of Fe Vol of SCN 0.1 M HNO Equilibrium concentration Fe[SCN]2' (mL) (mL.) (mL) 10.00 0.00 10.00 10.00 1.00 9.00 10.00 2.00 8.00 10.00 3.00 7.00 10.00 4.00 6.00 10.00...
3. In this experiment, you will determine the [FeSCNP at equilibrium by measuring its absorbance at - 450 nm. This is possible due to which of the following statements? Fe+ (aq) + SCN (aq) FeSCN2+ (aq) a. Fe and SCN do not absorb significantly at 450 nm. b. At equilibrium, only FeSCN* is present in the solution. c. [Fe] and [SCN) are too small to absorb light. d. The equilibrium constant, Keq, is small. 4. Give the names for the...
For Part A of the Equilibrium experiment, you will be preparing several standard solutions for the Beer's Law plot Using the information given in the Worksheet for Equilibrium Lab , answer the following questions. (a) What is the initial Fe3+ concentration of all of the solutions? 1.00 xM (b) What is the initial SCN1-concentrations of Solutions #1A - #5A? Solution #1A 1#1A | 1.00 Solution #2A 1.50 Solution #3A 2.00 Solution #4A2.50 Solution #41 2.50 M Solution #54 3,00 xM...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
A student made solution #3 using the experimental method in this
lab, and measured an absorbance of 0.559. The starting reagents are
2.00 x 10-3 M Fe(NO3)3 and 2.00 x
10-3 M KSCN.
The amount of absorption is proportional to the concentration
of
FeSCN2+. This relationship – true for many solutions – is called
“Beer’s Law”, and has the simple equation:
A = bc
where “A” is the absorption, “b” is 5174.6 for FeSCN2+ and “c”
is molarity
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