A 1.2516 gram sample of a mixture of CaCO3 and Na2SO4 was analyzed by dissolving the sample and completely precipitating the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid and the resulting H2C2O4 was titrated with a standard KMnO4 solution.(a) Write the balanced equation for the titration reaction, shown unbalanced below: MnO4- + H2C2O4 + H+ ® Mn2+ + CO2 + H2O (i) Indicate which substance is the oxidizing agent and which substance is the reducing agent.(b) The titration of the H2C2O4 obtained required 35.62 milliliters of 0.1092 molar MnO4- solution. Calculate the number of moles of H2C2O4 that reacted with the MnO4-(c) Calculate the number of moles of CaCO3 in the original sample.(d) Calculate the percentage by weight of CaCO3 in the original sample.

(a) From the mixture, CaCO3 is precipitated out as CaC2O4. Thus1 mole of CaC2O4 is precipitated by 1…

Answered: A 1.2516 gram sample of a mixture of…

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter18: Representative Metals, Metalloids, And Nonmetals

Section: Chapter Questions

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A 1.2516 gram sample of a mixture of CaCO3 and Na2SO4 was analyzed by dissolving the sample and completely precipitating the Ca²⁺ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid and the resulting H2C2O4 was titrated with a standard KMnO4 solution.

(a) Write the balanced equation for the titration reaction, shown unbalanced below:

MnO4- + H2C2O4 + H+ ® Mn²⁺ + CO2 + H2O

(i) Indicate which substance is the oxidizing agent and which substance is the reducing agent.

(b) The titration of the H2C2O4 obtained required 35.62 milliliters of 0.1092 molar MnO4- solution. Calculate the number of moles of H2C2O4 that reacted with the MnO4-

(d) Calculate the percentage by weight of CaCO3 in the original sample.

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