A 0.1362g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as...
An iron ore sample weighing 0.5562 g is dissolved HCl (aq), and the iron is obtained as Fe2+ in solution. This solution is then titrated with 28.72 mL of 0.04021 M K2Cr2O7 (aq). What is the percent by mass iron in the ore sample? How do I get to the equation 6Fe^2+ + 14H^+ + Cr2O7^2- ----> 6Fe^3+ + 2Cr^3+ + 7H2O ??? I am just generally confused on how to start this and how to do this step by...
A sample of iron ore weighing 0.6428g is dissolved in acid, the iron is reduced to Fe2+, and the solution is titrated with 36.30 mL of 0.01753 M K2Cr2O7 solution. The reaction is 6Fe2+ + Cr2O72- +14H+ à 6Fe3+ + 2Cr3+ + 7H2O What is the Percentage of iron (55.85g/mol) in the sample?
In a potentiometric titration of iron with cerium, the reaction is Fe2+ + Ce4+ --> Ce3+ + Fe3+. After collecting data it was found that 0.8925 grams of iron could be titrated with 20.95 milliliters of 0.04945 Molarity cerium(IV) to reach an end point with a potential of 0.806 Volts. Using the Nernst equation [Ecell = {E^o (Fe) - 0.0592 log {(21.05 - Volume added)/Volume added}} - Eref], calculate values of formal electrode potentials for reduction of iron...
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,...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an end point with 24.80 mL of 0.629 M Cr2O72−. The following redox reaction takes place: Cr2O72− (aq) + Fe2+ (aq) ⟶ Cr3+ (aq) + Fe3+ (aq) a. balance the reaction b. what % of the ore sample if FeBr2 (molar mass = 215.65 g/mol)
A sample of copper ore with a mass of 0.4225 g was dissolved in acid. A solution of potassium iodide was added, which caused the reaction: 2Cu2+(aq) + 5I– (aq) → I3–(aq ) + 2CuI(s) The I3– that formed reacted quantitatively with exactly 29.96 mL of 0.02100 M Na2S2O3 according to the following equation: I3– (aq) + 2S2O32– (aq) → 3I– (aq ) + S4O62–(aq ) What was the percentage by mass of copper in the ore? If the ore...
3 attempts left Check my work Enter your answer in the provided box. A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Feat in acid and then titrating the Fe?* with MnO4 A 1.0986-g sample was dissolved in acid and then titrated with 31.36 mL of 0.04891 M KMnO4. The balanced equation is 8 H*(aq) + 5 Fe2+ (aq)+ Mno, (aq) → 5 Fe3+(aq) + Mn²+(aq) + 4 H20(1) Calculate the...
3. A 3.33g rock sample containing iron was dissolved in sulfuric acid with the formation of a solution of FeSO4. This solution of FeSO4 was then titrated with 16.9mL of a 0.250M K2Cr207 solution. + K2SO4 (aq) 6FESO4 (aq) + K2Cr2O7 (aq) + 7H2SO4 (aq) 3Fe2(SO4)3 (aq) + Cr2(SO4)3 (aq)+7H20 (D) Calculate the percentage of iron (Fe) in the 3.33g rock sample.
23. The iron present in a sample of iron ore is converted to Fe2+ and titrated with dichromate on 420 +6Fe2+ +14H-20** +6F99 +7H20. If 17.6 mL of 0.125 M dichromate ion is required to titrate a 25.0 mL sample of Fe2+ solution, a) what is the molarity of the Fe2+ b) what mass of iron is present in the 25.0 mL sample?
HUW/ L ecLhtml ork-Week 7 0 Saved Check my work Enter your answer in the provided box. A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Feat in acid and then titrating the Fe with MnO,- A1.2056 g sample was dissolved in acid and then titrated with 36.29 mL of 0.01441 M KMnO The balanced equation is ST*(aq) +5 Fe2(aq)+ MnO, (aq) + 5 Fe(aq) + Mn?" (aq) + 4 H...