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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- (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 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.

Chemistry
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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  • 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.

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