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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