Standard # | Volume of 0.00020 M FeCl3 (mL) | Volume of 2 M HCL (mL) |
Blank | 0 | 10.00 |
1 | 0.20 | 9.80 |
2 | 0.40 | 9.60 |
3 | 1.00 | 9.00 |
4 | 2.00 | 8.00 |
5 | 3.00 | 7.00 |
Using the table, calculate the concentration of [Fe(SCN)6]^3– in each of the standard solutions you will prepare. Show all of your work, including units, for the calculation of the concentration of standard #1. (For standards 2-5, you may simply list the concentrations with units without showing your work.)
You have not given the amount of SCN- added to each solution , the volume of SCN- added has to be considered to determine the concentration of [Fe(SCN)6]^3– in the final solution.
The reaction is:
Fe3+ + 6SCN- = [Fe(SCN)6]3-
Let y mL of (m) molar SCN- solution is added to each solution.
For the solution 1:
Total volume = 0.2 + 9.8 + y = 10 + y mL
Concentration of Fe3+ after mixing the solutions = 0.2 mL * 0.0002 M / (10 + y mL)
=[ 0.00004 /(10 + y mL)] M
According to the reaction, 1 M Fe3+ reacts to give 1 M [Fe(SCN)6]3-
So concentration of [Fe(SCN)6]3- in the solution =[ 0.00004 /(10 + y mL)] M
Do the same for the rest of the solutions.
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