From the following data find the percentage of Fe in a sample of crude ferric chloride weighing 1.00 g. The lz liberated by the reaction: 2 FeCl3. + 2HI → 2HCI + 2 FeCl, + 21; is reduced by the addition of 50.00 ml of sodium thiosulfate solution, and the excess thiosulfate is titrated with standard I2 , requiring 7.85 ml. 45.00 ml s 45.95 ml Na2S2O3; 45 mL arsenite solution = 45.27 ml 12 ; I ml arsenite contains 0.005160 g As203.
From the following data find the percentage of Fe in a sample of crude ferric chloride weighing 1.00 g. The lz liberated by the reaction: 2 FeCl3. + 2HI → 2HCI + 2 FeCl, + 21; is reduced by the addition of 50.00 ml of sodium thiosulfate solution, and the excess thiosulfate is titrated with standard I2 , requiring 7.85 ml. 45.00 ml s 45.95 ml Na2S2O3; 45 mL arsenite solution = 45.27 ml 12 ; I ml arsenite contains 0.005160 g As203.
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
Transcribed Image Text:From the following data find the percentage of Fe in a sample of crude ferric chloride weighing 1.00 g.
The Iz liberated by the reaction: 2 FeCl3. + 2HI → 2HCI + 2 FeCl, + 212 is reduced by the addition of 50.00
ml of sodium thiosulfate solution, and the excess thiosulfate is titrated with standard Iz , requiring 7.85
ml. 45.00 ml 45.95 ml NazSzO3; 45 ml arsenite solution = 45.27 ml 2 ; I ml arsenite contains
0.005160 g As203.
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