Question

REDOX TITRATED Sol continued Part A Continued So, the average concentration of krn Oy is 0.0167 +0.0182 (M) -0.0349 (H) = 0.01741 (H) (only I run) panitial buret reading (KM) Final buret reading (KM ) || Ome Molar Mass of Fe 120ml 55.85 almol -Mn + Fe + 4 Using the Average molarity in Part A and the balanced equations MnO, F H HO Calculate the milligrams of iron (Fe) in the iron pill with your titration data. Show all ealculations below clearly and completely and include appropriate units. Now, read the pill bottle label to see how many mg of iron they claim to put in, and record it: Calculate the percent error for the Fe in the Iron pill, using your calculated amount as experimental, and the pill label amount as "theoretical". 1. Consider your percent error. Why do you think that the value is high or low? Explain what you could have done to roduce your crror.

Answer 1

Mnog + 5 feta + 8H7 Meta + 5 pets + 4 Heo Imole of Mnoy neutralises 5 moles of feth as shown in equr. Volume of KMnOy lused = 120ml Molarity of KMnly = 0.01745M Moles af kMudy used – Molarity x vol.in litser = 0.01745M X 0.0/22 = 0.0002094 moles km na. Moles of fe must be neutralised = 0.0020948 5 = 0.001047 moles. So, 0.001047 moles of feta are present in tablet/ pill. mass of Eron (fel = molerx motar = 0.20 1047 motes x 55.859 mas mole This = 0.0585g = 58.5mg mass of (Fe) Iron in fill is = 58.5 mg (this is experimental | mags checla on all table for theoreticall mass" (58.5mg) Percent error = theoretical mars - Experimental mass A x100 theoretical mass