The vanadium in a sample of ore is converted to VO2+ . The VO2+ ion is subsequentlytitrated with MnO4- in acidic solution to form V(OH)4+ and manganese(II) ion. Theunbalanced titration reaction isMnO4 − (aq) + VO2+ + (aq) +H2O (l) → V(OH)4+ (aq) + Mn2+ (aq) + H+ (aq)To titrate the solution, 26.45 mL of 0.02250 M MnO4- was required. If the mass percent ofvanadium in the ore was 58.1 %, what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.

Answer:- Firstly the given redox reaction is balanced using the oxidation number method then using…

Answered: The vanadium in a sample of ore is…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The vanadium in a sample of ore is converted to VO²⁺ . The VO²⁺ ion is subsequentlytitrated with MnO₄^- in acidic solution to form V(OH)₄⁺ and manganese(II) ion. Theunbalanced titration reaction is

MnO₄ − (aq) + VO²⁺ + (aq) +H₂O (l) → V(OH)₄⁺ (aq) + Mn²⁺ (aq) + H⁺ (aq)

To titrate the solution, 26.45 mL of 0.02250 M MnO₄^- was required. If the mass percent ofvanadium in the ore was 58.1 %, what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.

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