Determine an unknown volume or concentration using an oxidation-reduction titration.The concentration of a Fe2+ solution is determined by titrating it with a 0.1261 M solution of permanganate. The balanced net ionicequation for the reaction is shown below.MnO, (aq) + 5 Fe2*(aq)+8 H30*(aq) Mn2*(aq) + 5 Fe*(aq)+12 H20()In one experiment, 23.92 mL of the 0.1261 M MnO solution is required to react completely with 20.00 mL of the Fe2+ solution.Calculate the concentration of the Fe2+ solution.MCheck & Submit AnswerShow Approachétvhulu

First calculate the number of moles of MnO4– used for the titration. By using these moles, we can…

The concentration of a Fe2 solution is determined by titrating it with a 0.1261 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. MnO4 (aq) + 5 Fe2*(aq)+8 H30*(aq) Mn2*(aq) + 5 Fe*(aq)+12 H,0(1) In one experiment, 23.92 mL of the 0.1261 M MnO4 solution is required to react completely with 20.00 mL of the Fe2 solution. Calculate the concentration of the Fe2+ solution. M

The concentration of a Fe2 solution is determined by titrating it with a 0.1261 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. MnO4 (aq) + 5 Fe2(aq)+8 H30(aq) Mn2(aq) + 5 Fe(aq)+12 H,0(1) In one experiment, 23.92 mL of the 0.1261 M MnO4 solution is required to react completely with 20.00 mL of the Fe2 solution. Calculate the concentration of the Fe2+ solution. M

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.103QE

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Potassium permanganate solutions used in oxidation-reduction titrations are often standardized against sodium oxalate, Na₂C₂O₄, used as a primary standard. The reaction involved is 5C₂O₄²⁻(aq) + 2MnO₄⁻(aq) + 16 H⁺(aq) → 2Mn²⁺(aq) + 8H₂O(l) + 10CO₂(g) A 0.2452 g sample of sodium oxalate is dissolved in 100 mL of acid solution, and the permanganate solution is added slowly from a buret. The endpoint is reached when 15.85 mL of the permanganate solution has been added. The molar mass of sodium oxalate is 134.00 g/mol. Calculate [MnO₄⁻], the molar concentration of the permanganate solution.
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