A student dissolved a 0.139 g sample of oxalic acid, H2C2O4, in water in an Erlenmeyer flask. Then the student titrated the H2C2O4 solution in the flask with a solution of KMnO4, which has a dark purple color. The balanced chemical equation for the reaction that occurred during the titration is shown above. a. Identify the species that was reduced in the titration reaction. Justify your answer in terms of oxidation numbers. b.Thestudentuseda50.0mLburettoaddtheKMnO4(aq)to the H2C2O4(aq)until a faint lavender color was observed in the flask, an indication that the end point of the titration had been reached. The initial and final volume readings of the solution in the buret are shown below. Write down the initial reading and the final reading and use them to determine the volume of KMnO4(aq) that was added during the titration. c.Given that the concentration of KMnO4(aq) was 0.0235M,calculate the number of moles of MnO4–ions that completely reacted with theH2C2O4
A student dissolved a 0.139 g sample of oxalic acid, H2C2O4, in water in an Erlenmeyer flask. Then the student titrated the H2C2O4 solution in the flask with a solution of KMnO4, which has a dark purple color. The balanced chemical equation for the reaction that occurred during the titration is shown above. a. Identify the species that was reduced in the titration reaction. Justify your answer in terms of oxidation numbers. b.Thestudentuseda50.0mLburettoaddtheKMnO4(aq)to the H2C2O4(aq)until a faint lavender color was observed in the flask, an indication that the end point of the titration had been reached. The initial and final volume readings of the solution in the buret are shown below. Write down the initial reading and the final reading and use them to determine the volume of KMnO4(aq) that was added during the titration. c.Given that the concentration of KMnO4(aq) was 0.0235M,calculate the number of moles of MnO4–ions that completely reacted with theH2C2O4
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
Chapter1: Introduction To Chemistry
Section: Chapter Questions
Problem 1.85QE: The melting point of sodium chloride, table salt, is 801 C. What is this temperature in degrees...
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A student dissolved a 0.139 g sample of oxalic acid, H2C2O4, in water in an Erlenmeyer flask. Then the student titrated the H2C2O4 solution in the flask with a solution of KMnO4, which has a dark purple color. The balanced chemical equation for the reaction that occurred during the titration is shown above.
a. Identify the species that was reduced in the titration reaction. Justify your answer in terms of oxidation numbers.
b.Thestudentuseda50.0mLburettoaddtheKMnO4(aq)to the
H2C2O4(aq)until a faint lavender color was observed in the flask, an indication that the end point of the titration had been reached. The initial and final volume readings of the solution in the buret are shown below. Write down the initial reading and the final reading and use them to determine the volume of KMnO4(aq) that was added during the titration.
c.Given that the concentration of KMnO4(aq) was 0.0235M,calculate the number of moles of MnO4–ions that completely reacted with theH2C2O4
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