The concentration of iron(III) can be determined by adding excess thiocyanate (S

Question

The concentration of iron(III) can be determined by adding excess thiocyanate (SCN-) to an aqueous solution. This results in the formation of the highly colored FeSCN2+ complex ion. To do this analysis, a standard solution containing 5.00x10^-5 M Fe3+ was prepared. After addition of excess SCN-, the absorption of the standard solution =0.363 at 580 nm.

To determine [Fe3+] in an unknown solution, 1.00 mL of the solution was diluted to 50.0 mL. After addition of excess SCN-, the absorption of the standard solution =0.193 at 580 nm. What is the [Fe3+] in the ORIGINAL (UNDILUTED) solution?

Explanation / Answer

formation of FeSCN2+. In dilute solution, iron(III) nitrate, Fe(NO3)3(aq) and potassium thiocyanate ... excess of Fe3+ insures that essentially all of the SCN- is converted to FeSCN2+ (equilibrium concentration

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