Iron ores contain iron oxide minerals, which often contain ferric and ferrous ions. Such an ore can be analyzed for its iron content by dissolving it in acidic solution, reducing all the iron to ferrous ions, and then titrating with a standard solution of potassium permanganate. In the resulting solution, permanganate ion is reduced to manganese (II) ion, and ferrous ion is oxidized to ferric ion. A sample of iron ore weighed 0.3500 g. The titration required 41.56 mL of the permanganate solution (1.621 x 10-2 M) to reach the light purple end point. Determine the mass percent of iron in the iron ore.

For questions 1 and 2, consider the following experimental data.hydrogen emission lines were detected at the following wavelengths (in nm): 121.6102.697.395.093.8question 1use the electromagnetic radiation classifications below and figure 1-1 in the introductory information for this lab (in the lab manual) to determine the nf value for the experimental data provided? wavelength, ? (nm) 650 700 550 600 400 450 500 visible spectrum wavelength, ? (m) 11 10 3 10 10 10 8 10 5 10 10 -10 10 9 10 10 10 10 -12 10 microwave radio infrared x-ray ultraviolet gamma 1020 1019 1018 1 1016 015 1014 01 12 109108 frequency, v (hz)a.1b. 2c. 3d. 4e. 5question 2using the data for the emission line with the longest wavelength, the known value of nf (from question 1 in this prelab), and the value of ni (deduced from the ? and nf values) calculate the rydberg constant for hydrogen (rh) in units of m-1.a) 1.097 x 10-11 m-1b) 5.921 x 107 m-1c) 1.097 x 10-2 m-1d) 9.252 x 106 m-1e) 1.097 x 107 m-1