doesn't change anything or compromise the data. 6. A titration may be done on any reactive pair of compounds where a balanced equation is known and concentration information on one of the compounds is available. Below is an example of a titration with a Redox reaction between permanganate and iron(II). 1.5203 grams of potassium permanganate (a primary standard) was dissolved in enough water to make 500.0 mL of solution. a. What is molarity of the potassium permanganate solution? b. This permanganate solution is used as a standard to titrate a compound known to known contain iron(II) according to the following net ionic equation: MnO4 + 8H+ + 5Fe²+ Mn²+ + 4H₂O + 5Fe³+ It required 41.10 mL of the permanganate solution to titrate 1.5495 grams of the compound. Identify the iron(II)-containing compound from the list below: ● FeCl₂-4H₂O • Fe(C₂O4)2 2H₂O Fe(NH4)2(SO4)2 6H₂O ● FeSO4.7H₂O

doesn't change anything or compromise the data. 6. A titration may be done on any reactive pair of compounds where a balanced equation is known and concentration information on one of the compounds is available. Below is an example of a titration with a Redox reaction between permanganate and iron(II). 1.5203 grams of potassium permanganate (a primary standard) was dissolved in enough water to make 500.0 mL of solution. a. What is molarity of the potassium permanganate solution? b. This permanganate solution is used as a standard to titrate a compound known to known contain iron(II) according to the following net ionic equation: MnO4 + 8H+ + 5Fe²+ Mn²+ + 4H₂O + 5Fe³+ It required 41.10 mL of the permanganate solution to titrate 1.5495 grams of the compound. Identify the iron(II)-containing compound from the list below: ● FeCl₂-4H₂O • Fe(C₂O4)2 2H₂O Fe(NH4)2(SO4)2 6H₂O ● FeSO4.7H₂O

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 58QAP: The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing...

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A solution contains both iron(II) and iron(III) ions. A sample Of the solution is titrated with 35.0 ml, of M KMnO4, which oxidizes Fe2+ to Fe3+. The permanganate ion is reduced to manganese(ll) ion. The equation for this reaction is MnO4(aq)+8 H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+ +4H2OAnother 50.00-mL sample of the solution is treated with zinc, which reduces all the Fe3+ to Fe2+. The equation for this reaction is 2Fe3+(aq)+Zn(s)2Fe2+(aq)+Zn2+(aq)The resulting solution is again titrated with 0.0280 M KMnO4; this time 48.0 ml, is required. What are the concentrations of Fe2+ and Fe3+ in the solution?
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