The vanadium in a sample of ore is converted to VO2+. The VO2+ ion issubsequently titrated with MnO4- in acidic solution to form V(OH)4+ and manganese (II) ion. The unbalanced 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 MMnO4- was required. If themass percent of vanadium in the orewas 58.1%,what was the mass ofthe ore sample? Hint: Balance the titration reaction by the oxidation states method.

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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
subsequently titrated with MnO^4- in acidic solution to form V(OH)⁴⁺ and manganese (II) ion. The unbalanced 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 MMnO₄^- was required. If the
mass percent of vanadium in the orewas 58.1%,what was the mass of
the ore sample? Hint: Balance the titration reaction by the oxidation states method.

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