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For one of the solutions you make up for this week's experiment, 6.00 mL of 2.0E-3 M iron(III) nitrate solution is mixed with 3.00 mL of 2.0E-3 M...

For one of the solutions you make up for this week's experiment, 6.00 mL of 2.0E-3 M iron(III) nitrate solution is mixed with 3.00 mL of 2.0E-3 M potassium thiocyanate solution, 4.00 mL of 0.500 M nitric acid solution, and 7.00 mL of distilled water for a total volume of 20.00 mL. See line 3 in Table 1.

What is the initial concentration of Fe3+ ions in this solution, in other words, what is the concentration of Fe3+ ions before any reaction with the thiocyanate?

Initial concentration of Fe3+ = M

Calculate the mole fractions of Fe3+ and SCN- in this solution with respect to the total number of moles of Fe3+ and SCN-. This means, of course, that these two mole fractions should add up to 1.00.

Mole fraction of Fe3+ =

Mole fraction of SCN- =

Suppose that the mole fraction of Fe3+ in the iron(II) - thiocyanate solution was plotted against the absorbance of the solution at 450 nm. Suppose also that the maximum absorbance was established at a mole fraction of Fe3+ equal to 0.167 by plotting the two best straight lines through the data points. What is the stoichiometry of the complex formed between the Fe3+ and the thiocyanate?

Enter the answer as a whole number ratio; whole numbers separated by a colon (for example, 2:3, indicating a stoichiometry Fe2(SCN)3).

Stoichiometry of the complex formed between Fe3+ and SCN- =

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