Calculate equilibrium constant for each solution and report to 3 significant figures. Calculate average equilibrium constant and report to 3 significant figures. PHASE 10:Lab Data- XCalculate EquilibriumConstantPrepared solutions, absorbance, and calculated [FESCN²*]Complete the following steps:Solution 1Solution 2Solution 3Solution 4Solution 51Calculate equilibrium constantConcentration iron(III) nitrate[Fe(NO3)3] (M)0.002000.002000.002000.002000.00200for each solution. Record in LabWash/WasteData. Report to 3 significantfiguresConcentration potassium thiocyanate[KSCN] (M)0.002000.002000.002000.002000.002002Calculate average equilibriumVolume Fe(NO3)3 (mL)5.005.005.005.005.00constant. Record in Lab Data.Volume KSCN (mL)5.004.003.002.001.00Report to 3 significant figuresVolume DI water (mL)0.001.002.003.004.00Initial concentration [Fe³+] (M)0.001000.001000.001000.001000.00100Initial concentration [SCN'] (M)0.001000.0008000.0006000.0004000.000200Absorbance0.2690.1920.1540.1040.052Equilibrium [FESCN²*] (M)0.0002120.0001520.0001220.00008210.000041Equilibrium constant KeAverage Ke

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PHASE 10: A Lab Data - X Calculate Equilibrium Constant Prepared solutions, absorbance, and calculated [FESCN2*] Complete the following steps. Solution 1 Solution 2 Solution 3 Solution 4 Solution 5 1 Calculate equilibrium constant Concentration iron(III) nitrate [Fe(NO3)3] (M) 0.00200 0.00200 0.00200 0.00200 0.00200 for each solution. Record in Lab Data. Report to 3 significant figures Wash/Waste Concentration potassium thiocyanate [KSCN] (M) 0.00200 0.00200 0.00200 0.00200 0.00200 Calculate average equilibrium Volume Fe(NO3)3 (mL) 5.00 5.00 5.00 5.00 5.00 constant. Record in Lab Data. Volume KSCN (mL) 5.00 4.00 3.00 2.00 1.00 Report to 3 significant figures Volume DI water (mL) 0.00 1.00 2.00 3.00 4.00 Initial concentration [Fe3+] (M) 0.00100 0.00100 0.00100 0.00100 0.00100 Initial concentration [SCN'] (M) 0.00100 0.000800 0.000600 0.000400 0.000200 Absorbance 0.269 0.192 0.154 0.104 0.052 Equilibrium [FesCN2*] (M) 0.000212 0.000152 0.000122 0.0000821 0.000041 Equilibrium constant K. Average Ke

PHASE 10: A Lab Data - X Calculate Equilibrium Constant Prepared solutions, absorbance, and calculated [FESCN2] Complete the following steps. Solution 1 Solution 2 Solution 3 Solution 4 Solution 5 1 Calculate equilibrium constant Concentration iron(III) nitrate [Fe(NO3)3] (M) 0.00200 0.00200 0.00200 0.00200 0.00200 for each solution. Record in Lab Data. Report to 3 significant figures Wash/Waste Concentration potassium thiocyanate [KSCN] (M) 0.00200 0.00200 0.00200 0.00200 0.00200 Calculate average equilibrium Volume Fe(NO3)3 (mL) 5.00 5.00 5.00 5.00 5.00 constant. Record in Lab Data. Volume KSCN (mL) 5.00 4.00 3.00 2.00 1.00 Report to 3 significant figures Volume DI water (mL) 0.00 1.00 2.00 3.00 4.00 Initial concentration [Fe3+] (M) 0.00100 0.00100 0.00100 0.00100 0.00100 Initial concentration [SCN'] (M) 0.00100 0.000800 0.000600 0.000400 0.000200 Absorbance 0.269 0.192 0.154 0.104 0.052 Equilibrium [FesCN2] (M) 0.000212 0.000152 0.000122 0.0000821 0.000041 Equilibrium constant K. Average Ke

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.23QAP

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EDTA abstracts bismuth(III) from its thiourea complex:Bi1tu2631 1 H2Y22 S BiY2 1 6tu 1 2H1where tu is the thiourea molecule (NH2)2CS. Predict the shape of a photometric titration curve based on thisprocess, given that the Bi(III) or thiourea complex is the only species in the system that absorbs light at 465nm, the wavelength selected for the analysis.
A reaction was carried out with Fe3+ and SCN- to produce FeSCN2+. Two best-fit lines for Absorbance vs [FeSCN-] were obtained. The first line produced: y = 200x + 0.005, r2=0.951 and the second line produced: y= 10,000x + 0.005, r2 = 0.993. Determine the best-fit line of two, and then use the line equation to determine the equilibrium concentration of FeSCN2+ if the absorbance = 0.863.
You want to determine the amount of iron(III) in acomplex salt. You make a 100.0 mL solution of the complex salt by dissolving 0.0670 g of complex salt with water to the mark on a 100.0 mL volumetric flask. You get an absorbance reading for the iron from the spectrometer of 0.334. The molar absorptivity is determined to be 17605 L/mole∙cm and the pathlength is 1.00 cm. Determine the molarity of iron(III) in solution. Determine the mass percentage of iron(III) in the complex salt.
An absorbance versus concentration data for the thiocyanatoiron(III) complex at 510 nm and makes a Beer's law plot.Based on the plot, what [Fe(SCN)2+] would the student report for a solution that has an absorbance of 0.300 at 510 nm? Also select all below closely matches the procedures to be followed in this experiment and why they are being carried out. 1) A Beer's law plot will be used as a means to determine the equilibrium concentration of the thiocyanatoiron(III) complex. 2)A Beer's law plot will be used to confirm known values of the equilibrium constant for the formation of the thiocyanatoiron(III) complex. 3)To make the Beer's law calibration graph, the formation equilibrium for the thiocyanatoiron(III) complex will be flooded with a large excess of thiocyanate ion. 4)To make the Beer's law calibration graph, the formation equilibrium for the thiocyanatoiron(III) complex will be flooded with a large excess of iron(III) ion.
This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of NH3(aq) to test tube #6: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. Explain why the addition of NH3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use chemical reaction in your explanation. Addition of heat/cold to test tube #7 & 8: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is increased? Explain. As a result of the colour…
This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of heat/cold to test tube #7 & 8: As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is increased? Explain. As a result of the colour change, what can be concluded about the [FeSCN2+(aq)] when the temperature is decreased? Explain. What can you conclude about the reaction (i.e. is it endothermic or exothermic) based on the above results?
This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of Na2CO3(s) to test tube #4: d) Explain why the addition of Na2CO3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use a chemical reaction in your explanation. Addition of NaOH(aq) test tube #5: e) As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. f) Explain why the addition of NaOH(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use a chemical reaction in your explanation.
This is the lab with my data sheet and please answer all of them. Thank you and please answer all of them. If you do it would be appreciated My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour Addition of Fe(NO3)3(aq) to test tube #3: a) what can you infer about the system from the colour change of the solution? b)How can this be possible if no additional SCN-(aq) has been introduced? Addition of Na2CO3(s) to test tube #4: c) As a result of the colour change, what can be concluded about the [FeSCN2+(aq)]? Explain. d) Explain why the addition of Na2CO3(aq) affects the [FeSCN2+(aq)] as indicated in (a). Use a chemical reaction in your…
Ammonium iron(II) sulfate crystals have the following formula: (NH4)2SO4.FeSO4.nH2O . In an experiment to determine n 8.492g of the salt were dissolved and made up to 250cm^-3 of solution with distilled water and sulphuric acid. A 25.0cm^-3 portion of the solution was titrated against 0.0150 mol dm^-3 KMnO4. A volume of 22.5cm^-3 was required. Find the value of n
A standard solution was put through appropriate dilutions to give the concentrations of iron shown in the table that follows. The iron(II)-1,10-phenanthroline complex was then formed in 25.0-mL aliquots of these solutions, following which each was diluted to 50.0 mL. The following absorbances (1.00-cm cells) were recorded at 510 nm: Calculate the concentration, in ppm, of a sample with an abosrbance of 0.829. Fe(II) concentration (ppm) A510 4.00 0.160 10.0 0.390 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580
This is the lab with my data sheet and please answer all of them. Thank you My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour What species is responsible for the observed colour change when KSCN(aq) and Fe(NO3)3(aq) are mixed? What can be concluded about the system based on your ~1 minute observation of the mixture. what does the addition of the solid do to the [SCN-(aq)]? What can you infer about the system from the colour change of the solution?  How can this be possible if no additional Fe3+(aq) has been introduced?
This is the lab with my data sheet and please answer all of them. Thank you My data to support answers for questions. The equilibrium is Fe3+ + SCN- <--> [FeSCN]2+. The Fe3+ is a pale yellow colour and the complex ion product is red.Stresses:Add KSCN - turned deep redAdd Fe(NO3)3 - turned deep redAdd Na2CO3 - turned yellow/colourlessAdd NaOH - turned yellow/colourlessAdd NH3 - turned yellow/colourlessHeat - turned lighter orange colourCold - turned darker orange colour question: What can you infer about the system from the colour change of the solution?  How can this be possible if no additional Fe3+(aq) has been introduced? What does the addition of the solution do to the [Fe3+(aq)]?