My professor had to cancel lab last week and just sent us the absorbances for the test tubes to do on our own at home but I don't even know how to go about finding any of this information in the table. I know it's it one question per post but I need the formulas to figure these out.
1 |
2 |
3 |
4 |
|
Initial moles of Fe3+ |
0.006 |
0.006 |
0.006 |
0.006 |
initial moles of SCN- |
0.004 |
0.006 |
0.008 |
0.01 |
equilibrium [FeSCN2+] |
0.178349 |
0.304286 |
0.392242 |
0.49519 |
moles of FeSCN2+ at equilibrium |
0.001783 |
0.003043 |
0.003922 |
0.004952 |
moles of Fe3+ at equilibrium |
0.004217 |
0.002957 |
0.002078 |
0.001048 |
Equilibrium [Fe3+] |
0.421651 |
0.295714 |
0.207758 |
0.10481 |
Moles of SCN- at equilibrium |
0.002217 |
0.002957 |
0.004078 |
0.005048 |
Equilibrium [SCN-] |
0.221651 |
0.295714 |
0.407758 |
0.50481 |
Keq |
1.908299 |
3.479663 |
4.630127 |
9.359292 |
Average Keq |
4.844345 |
|||
standard deviation |
2.779989 |
|||
relative standard deviation |
57.38628 |
My professor had to cancel lab last week and just sent us the absorbances for the...
Lab Report: Determination of Kc for a Complex Ion Formation
tube
2.00e-3 Fe3+ (mL)
2.00E-3M SCN- (mL)
water (mL)
initial conc. Fe3+
initial conc. SCN-
1
5.00
5.00
0
1.00e-3M
1.00E-3M
2
5.00
4.00
1.00
1.00E-3M
8.00E-3M
3
5.00
3.00
2.00
1.00E-3,
6.00E-3M
4
5.00
2.00
3.00
1.00E-3M
4.00E-3M
5
5.00
1.00
4.00
1.00E-3M
2.00E-3M
10ml of 0.200M Fe3+, 2.00ml of 0.00200M SCN-, AND 8.00ml of
water results in an eq. [FeSCN2+] IN Standard
Soln.:2.00E-4M
Could you please explain how...
Could you please help me with calculating the initial
concentrations, and please tell me if I did table 4 correctly. I
would like to see one or two calculations for the second bullet so
I can figure out how to do them all. Thank you!
13. Use a 3.00 mL pipette to deliver 0.0020 M Fe(NO3)3 solution and burettes to deliver the required volumes of KSCN solution and DI water into clean and dry test tubes. Note that this set...
fill out the chart
Lab Notebook Initial concentrations of Feº and SCN KSCN, mL Di water, mL (Fe) Solution Fe(NO3). mL M [SCN] initia M Spectrophotometric determination of (FeSCN) (Calibration curve: A =1269.6c) Solution Measured absorbance Calculated (FeSCN).M alvo Instructions In separate test tubes, make the 5 solutions according to the table below. Then stir each solution. Solution Fe(NO3)3, mL KSCN, mL 2.00 x 10M 2.00 x 10M Dl water, ml 5.0 5.0 0.0 5.0 4.0 1.0 5.0 3.0 2.0...
can you please help me with this
Data and Calculations Trial 0:29 Absorbance 0.378 Je 0.086 Trial 2 0.47 Trial 3 0.632 Trial 4 0.729 0.686 Absorbance of standard Triw. 329 0.6 6 Temperature ke [Fe(SCN) 2+]/([Fe3+] [SCN-]) Ferrag) + SCN Cag) 2 FescN2t (ag) Absorbance of standard (Trial) Temperature 0.3 Ke expression: [Fe] 0.0010 [SCN) 10.00040 [FeSCN? Jeg [Fe [SCN ] Ke value Average of Ke values Percent error (see pg 7): (Discuss this result as part of your...
please do 1 through 4. Thank you.
0 1. Fe 1.SCN Procedure B: 1. Prepare ICE tables for beakers 2 - 6 using the example below as a guideline (you will have 5 different ICE tables). Table 3. Sample "ICE" table. Fe(aq)*3 + SCN(aq) = FeSCN2 Initial: **M calculated **M calculated using your Table 2 using your Table 2 volumes volumes Change: - 1x - 1x Equilibrium: M 1x 1x = concentration calculated from Procedure A slope-intercept equation +1x M...
help with finding the equilibrium of [Fe(SCN)^2+] morality value
Equilibrium Solutions Data 1. Use your "Absorbance of Solution" values and the graph you made above to interpolate the "Equilibrium [Fe(SCN)]" molarity values. 2. Calculate both the "Initial [Fe ]" and the "Initial [SCN']" molarity values using then dilution equation CiVi C2V2. 3. Calculate the "Equilibrium [Fe ]" molarity values by subtracting the "Equilibrium [Fe(SCN) " molarity values from the "Initial [Fe'" molarity values. 4. Calculate the "Equilibrium [SCN']" molarity values...
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...
4 please
in part 1 gires us absorbance values for each sample , changes in concentration and absorbance will cause a curve 1. For each new concentration of FeSCN2+ a new absorbance will be plotted. 4. After completing Part A of this experiment, a student determines the slope of their calibration graph of absorbance versus (FeSCN to be 5140 M". In Part B, a student combines 2.00 mL of a 0.00200 M solution of KSCN with 5.00 mL of a...
What's the concentration of [FeSCN2+] using limiting
reactant theory and equation?
For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
Im
still not understanding how to calculate the molarity of Fe(SCN)^2+
I have the absorbance for them but I dont know what to do from
there.
I would really appreciate the help. please and thank
you.
H115 lab manual_rev2016_MOD19AUG18_JSchesser.pdf (2.82 MB) Page < 65 > of 130 Tortas experiment unless you can measure their absorbance values within one hour 0 - ZOOM + Label 6 screw top test tubes A-F Using pipets, measure the solutions as outlined in the table...