A 750.0-mg sample of iron ore was dissolved in acid and treated to oxidize all the iron to ferric ion. After destroying any remaining oxidizing agent, excess KI was added. The liberated I, required 28.50 ml of 0.07500 M Na,S,0, for titration. What is the % w/w Fe in the sample? The reactions involved for this titration are the following: 2Fe* +I→ 2Fe* +1, 1, + 25,0, → 21 + S,0,*
A 750.0-mg sample of iron ore was dissolved in acid and treated to oxidize all the iron to ferric ion. After destroying any remaining oxidizing agent, excess KI was added. The liberated I, required 28.50 ml of 0.07500 M Na,S,0, for titration. What is the % w/w Fe in the sample? The reactions involved for this titration are the following: 2Fe* +I→ 2Fe* +1, 1, + 25,0, → 21 + S,0,*
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 115E: A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of...
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A 750.0-mg sample of iron ore was dissolved in acid and treated to oxidize all the iron to ferric ion. After destroying any remaining oxidizing agent, excess KI was added. The liberated I2 required 28.50 mL of 0.07500 M Na2S2O3 for titration. What is the % w/w Fe in the sample? The reactions involved for this titration are the following:
2Fe3+ + I- ? 2Fe2+ + I2
I2 + 2S2O32- ? 2I- + S4O62-
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