A 1.389 g sample containing some iron(II) in it was dissolved in 1 M H2SO4, then...
A 1.389 g sample containing some iron(II) in it was dissolved in 1 M H2SO4, then titrated with 0.0292 permanganate until the reaction solution was a pale yellow. 6.8 mL of 7.9 M H3PO4 were added to the reaction solution to form a colorless complex with the Fe3+ reaction product. The titration was finished when the pale pink of excess permanganate was visible in the reaction flask. The initial buret reading was 2.4 mL. The final buret reading was 40.1 mL. Question: What is the mass % iron in the sample?
Homework Answers
To solve this problem use the following steps
1.calculate volume of permanganate used from burette readings.
2.Calculate moles of permanganate used by multiplying it's molarity with volume used.
3.Write balanced equation between iron II and permanganate ion.
4.Use unitary method to determine the moles of iron II reacting with moles of permanganate used(calculated in step 2)
5.convert moles of Fe II into mass by multiplying with its molar mass.
6.Calculate mass % by dividing mass of iron × 100 by mass of sample.
The solution is as follows
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A 1.389 g sample containing some iron(II) in it was dissolved in
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BACKGROUND: Synthesis of Potassium Iron
(III) Oxalate Hydrate Salt
The iron(II) ions from
Fe(NH4)2(SO4)2•6H2O
will be precipitated as iron(II) oxalate.
Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s)
The supernatant liquid, containing the ammonium and sulfate
ions, as well as excess oxalate ions and oxalic acid will be
decanted and discarded. The solid will then be re-dissolved and the
iron(II) ions will be oxidized to iron(III) ions by reaction with
hydrogen peroxide.
2Fe^2+(aq) + H2O2(aq) --> 2Fe^3+(aq) +2 OH^ - (aq)
The...
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in the data table correct, and if not, how do I calculate it. Also,
the questions below the data table in the second picture. How are
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In this experiment you will use an oxidation - reduction titration to determine the percent of oxalate ion, CO2 in an unknown sample containing oxalate ion. Potassium permanganate (KMnO.) will be titrated against the oxalic acid (C2H:08) as shown by the following oxidation-reduction reaction: +3 +7 5C,044 2MnO4 + 16H* → 10CO, 8H0 + 2Mn2 +4 + + Mno. Mn? is the reduction process C2042 → CO2 is the oxidation process The underlying principle behind a titration is that an...
used to titrate a solution of iron(II) ions., with which it reacts according to Cerium(IV) sulfate Ce4(aq)Fe2 (aq)>Ce3*(aq) + Fe3 (aq) A cerium(IV) sulfate solution is prepared by dissolving 40.47 g of Ce(SO42 in water and diluting to a total volume of 1.000 L. A total of 19.41 mL of this solution is required to reach the endpoint in a titration of a 100.0-mL sample containing Fe(aq). Determine the concentration of Fe2 in the original solution It is desired precipitate,...
The Fe2+ (55.845 g/mol) content of a 2.264 g steel sample dissolved in 50.00 mL of an acidic solution was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 44.82 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel Mn2+5 Fe34 H20 + 5 Fe2+ MnO8 H concentration g Fe/g steel A 1.969 g...
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BACKGROUND: Synthesis of Potassium Iron
(III) Oxalate Hydrate Salt
The iron(II) ions from
Fe(NH4)2(SO4)2•6H2O
will be precipitated as iron(II) oxalate.
Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s)
The supernatant liquid, containing the ammonium and sulfate
ions, as well as excess oxalate ions and oxalic acid will be
decanted and discarded. The solid will then be re-dissolved and the
iron(II) ions will be oxidized to iron(III) ions by reaction with
hydrogen peroxide.
2Fe^2+(aq) + H2O2(aq) --> 2Fe^3+(aq) +2 OH^ - (aq)
The...
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