Beers Law, A Equilibrium Kf

So lost and do not have any clue, Please help!

ndefined

hentical Equilibrium: Determination of K, for the iron-thiocyanate complex ion est tube #1: add 5 mL of 0.20 M FoNOs), large excess, standard solution Fe(aq) + SCH(aq) = FeSCN"(aq) K-FeSCN [Fe HSCN) FeSCN), obtain from the absorption of visible light est tubes 2.6: add 10.0 mL of 0.20 M Fe(NO.), to the 25 ml graduated cylinder, add deionized water to get 25 mL of solution (0.080 M Ft) Segel [FeSCN1-1.0 x 10+ x 0.426/0.470 = 9.06 x 10'M [Fe] =0.040-9.06 x 10 =0.040 [SCN1ul - 1.0x 104-9.06 x 109 -9.4 x 10 Re (FeSC_9.06 x 10 = 241 [Fe'SCN] (0.040(9.4 x 10) add 5.0 ml of this solution (0.080 M Fel) to test tube #2 discard all but 10.0 mL of the rest of the solution in the graduated cylinder to the 100 ml of remaining solution, add deionized water to get 25.0 mL of solution (0.032 M Fo") Beer's Law, Aele absorbance (molar absorptivity path length concentration) Ancat of maximum absorption note: at appropriate reactants do not absorb light Krexperimental data: add 5.0 ml of this solution to test tube Ni Test Tube Absorbance repeat procedure for test tubes 1,5anul 6. 1. Standard 0.452 cean Optics spectrophotometer c 1 cuvette only for all the solutions (place in holder the same way each time (V mark)) line cuvette with chen wipe (no fingerprints) 2. 0.434 3. 0.398 ist calibrate the spectrophotometer with a blank solution (0.50 M HNO.) not skip warm up set for the lamp 4. 0.298 Fan all six solutions from 390-700 nm (change scanning range) 5. 0.185 6. 0.096 ant to record the absorption at the top of the curve (recorch both the wavelength and the absorption value), to be consistent in recording the absorption for each solution at approximately the same maximum avelength value need A for a known FeSCN1 standard solution all trials, use 2.0 x 10+ M KSCN trial 1: use a large excess of Fe (0.20 M) Le Chatelier's principle: shift the equilibrium to the right, assume all the SCN reacts, So [SCN] - [FeSC (note dilution for concentrations) trials 26 trial1 [FeSCN']. - [FeSCN). A other trials Al trial I (test tube 1) cample: st the WI: 5.0 int. 2.0 x 104 MKSCN mix together 5.0.0.2 M F NO.). rcmenbertitution [KSCN] - 10 x 10+ [Fe**] -0.10M [FeSON ] -1.0 x 100 [Felgul - [Fe] - [TeSCNI. [SCN1.- [SCNJ... [FeSCN), note dilution at 2. A-0.470 for the standard calculate K, for trials 2-6, get the average Ki Procedure: add 5 mL of 2.0 x 10MKSCN to ench of the six test tubes Fe(NO:) solutions, use a disposable pipet and graduated cylinder Note, above reactants already in 0,50 M HNO tube 12: 5.0 mL 2.0 x 10-KSCN 5.0 ML 0.080 M Fe mix Lagether [SCN) - 10 x 10 [Fe] -0,040 M initial concentrations (aller dilution) [FeSCN-[FeSCN]taskere Aurke Acest (#3 Calculations: Equilibrium concentrations 1. Determine the initial concentrations of Fe and SCN upon mixing the solutions together, Remember that there is a dilution factor present for the calculation of the initial concentrations as the solutions were made. Trial (test tube) FeSCNIM Fell (M) (SCN (M) 2 3 Trial (Test Tube) 2 Fet initial (SCN) initial 4 3 3 5 4 4 6 S 3. Calculate K for trials 2-6, and calculate the average Kt for the complex ion equilibrium. 6 K Trial 2 2. Determine the conceutration of FeSCN in the various solutions using the following equation: Trial 3 [FeSCN]... - FSCNX absorbance unknown absorbance standard Trial 4 Average K- Trials Trial where standard refers to the standard solution (test tube 1) and unknown refers to the other 5 test tubes. For test tube 11 ([FeSCN), assume that all the initial chiacyannte ion (SCN) has been converted to the iron.thiocyanate complex ion (FeSCN). 3. Calculate the concentration of Fe" and SCN present at equilibrium in tubes 2 - 6 by subtracting the amount reacted based on the complex ion formed from the initial values in each test tube. [Fe'll [le]enu - (FeSCN) [SCNJ - (SCNaal - [FeSON Show the calculation for one of the trials hentical Equilibrium: Determination of K, for the iron-thiocyanate complex ion est tube #1: add 5 mL of 0.20 M FoNOs), large excess, standard solution Fe(aq) + SCH(aq) = FeSCN"(aq) K-FeSCN [Fe HSCN) FeSCN), obtain from the absorption of visible light est tubes 2.6: add 10.0 mL of 0.20 M Fe(NO.), to the 25 ml graduated cylinder, add deionized water to get 25 mL of solution (0.080 M Ft) Segel [FeSCN1-1.0 x 10+ x 0.426/0.470 = 9.06 x 10'M [Fe] =0.040-9.06 x 10 =0.040 [SCN1ul - 1.0x 104-9.06 x 109 -9.4 x 10 Re (FeSC_9.06 x 10 = 241 [Fe'SCN] (0.040(9.4 x 10) add 5.0 ml of this solution (0.080 M Fel) to test tube #2 discard all but 10.0 mL of the rest of the solution in the graduated cylinder to the 100 ml of remaining solution, add deionized water to get 25.0 mL of solution (0.032 M Fo") Beer's Law, Aele absorbance (molar absorptivity path length concentration) Ancat of maximum absorption note: at appropriate reactants do not absorb light Krexperimental data: add 5.0 ml of this solution to test tube Ni Test Tube Absorbance repeat procedure for test tubes 1,5anul 6. 1. Standard 0.452 cean Optics spectrophotometer c 1 cuvette only for all the solutions (place in holder the same way each time (V mark)) line cuvette with chen wipe (no fingerprints) 2. 0.434 3. 0.398 ist calibrate the spectrophotometer with a blank solution (0.50 M HNO.) not skip warm up set for the lamp 4. 0.298 Fan all six solutions from 390-700 nm (change scanning range) 5. 0.185 6. 0.096 ant to record the absorption at the top of the curve (recorch both the wavelength and the absorption value), to be consistent in recording the absorption for each solution at approximately the same maximum avelength value need A for a known FeSCN1 standard solution all trials, use 2.0 x 10+ M KSCN trial 1: use a large excess of Fe (0.20 M) Le Chatelier's principle: shift the equilibrium to the right, assume all the SCN reacts, So [SCN] - [FeSC (note dilution for concentrations) trials 26 trial1 [FeSCN']. - [FeSCN). A other trials Al trial I (test tube 1) cample: st the WI: 5.0 int. 2.0 x 104 MKSCN mix together 5.0.0.2 M F NO.). rcmenbertitution [KSCN] - 10 x 10+ [Fe**] -0.10M [FeSON ] -1.0 x 100 [Felgul - [Fe] - [TeSCNI. [SCN1.- [SCNJ... [FeSCN), note dilution at 2. A-0.470 for the standard calculate K, for trials 2-6, get the average Ki Procedure: add 5 mL of 2.0 x 10MKSCN to ench of the six test tubes Fe(NO:) solutions, use a disposable pipet and graduated cylinder Note, above reactants already in 0,50 M HNO tube 12: 5.0 mL 2.0 x 10-KSCN 5.0 ML 0.080 M Fe mix Lagether [SCN) - 10 x 10 [Fe] -0,040 M initial concentrations (aller dilution) [FeSCN-[FeSCN]taskere Aurke Acest (#3 Calculations: Equilibrium concentrations 1. Determine the initial concentrations of Fe and SCN upon mixing the solutions together, Remember that there is a dilution factor present for the calculation of the initial concentrations as the solutions were made. Trial (test tube) FeSCNIM Fell (M) (SCN (M) 2 3 Trial (Test Tube) 2 Fet initial (SCN) initial 4 3 3 5 4 4 6 S 3. Calculate K for trials 2-6, and calculate the average Kt for the complex ion equilibrium. 6 K Trial 2 2. Determine the conceutration of FeSCN in the various solutions using the following equation: Trial 3 [FeSCN]... - FSCNX absorbance unknown absorbance standard Trial 4 Average K- Trials Trial where standard refers to the standard solution (test tube 1) and unknown refers to the other 5 test tubes. For test tube 11 ([FeSCN), assume that all the initial chiacyannte ion (SCN) has been converted to the iron.thiocyanate complex ion (FeSCN). 3. Calculate the concentration of Fe" and SCN present at equilibrium in tubes 2 - 6 by subtracting the amount reacted based on the complex ion formed from the initial values in each test tube. [Fe'll [le]enu - (FeSCN) [SCNJ - (SCNaal - [FeSON Show the calculation for one of the trials