For part A we have to use dried Na2C2O4 and dissolve in the H2SO4 solution

For part a we have to use dried na2c2o4 and dissolve

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a known amount of another substance. For part A, we have to use dried Na2C2O4 and dissolve in the H2SO4 solution. After heat the solution, we have to maintain the temperature to 60 . Next, we have to titrate using KMnO4 solution. The colour of solution before starting titration is colourless. After the titration is done, the colour will turn to pale pink solution. We have to repeat this experiment for 2 times. So that, the average of the volume KMnO4 is 9.40ml. Aqueous solution of permanganate ion is not stable over a long period of time. Thus, the exact concentration of KMnO 4 must be determined by titration with a known amount of odium oxalate, Na 2 C 2 O 4. From part A, we have to determine the molarity of KMnO4. From the equation, the exact molarity of KMnO4 is 0.3350 M . The unbalanced equation of the reaction is as follow: MnO 4 - (aq) + C 2 O 4 2- aq) Mn 2+ aq) + CO 2 (g) For part B, we have to use previous product in experiment 3, 4 and 5. The product for experiment 3 which is K 3 [Cr(C 2 O 4 ) 3 . 3H 2 O, we have to determine the oxalate content in the product. The colour of the product is dark green. The product is solid. We have to dissolve the solid in the H2SO4 solution. After that we have to boil the solution. After the solution boiled, we have to allow the solution to cool until the temperature drop to the 60 . After that, we have to titrate the solution using KMnO4 solution as a titrant. The colour of solution is dark green. After the titration reach end point, the colour of solution turn to dark purple. We have to beware to the end point because the colour can turn to the brown solution. It is because there is some error while titrate the solution. We have to repeat this part for 2 times. The average volume of KMnO4 solution is 4.30mL. For this part, we have to find the molarity using the part A. The molarity of KMnO4 is 0.0670M. The percent of oxalate in this part is 31.32%. The percentage purity of the complex in this part is 57.82%. The product for experiment 4 which is K 2 [Cu(C 2 O 4 ) 2 (H 2 O) 2 ], we have to determine the oxalate content in the product. The colour of the pr oduct is light blue . The product is solid. We have to dissolve the solid in the H2SO4 solution. After that we have to boil the solution. After the solution boiled, we have to allow the solution to cool until the temperature drop to the 60 . After that, we have to titrate the solution using KMnO4 solution as a titrant. The colour of solution is light blue. After the titration reach end point, the colour of solution turn to pale pink . We have to beware to the end point because the colour ca n turn to the purple solution. It is because there is some error while
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titrate the solution. We have to repeat this part for 2 times. The average volume of KMnO4 solution is 7.05 mL. For this part, we have to find the molarity using the part A. The molarity of KMnO4 is 0.0670M. The percent of oxalate in this part is 49.74 %. The percentage purity of the complex in this part is 91.82 %. The percentage purity is very high. It is good for experiment. For the last part, we have to use the product form experiment 5 which is K 3 [Fe(C 2 O 4 ) 3 ].3H 2 O. We also have to determine the oxalate content in the product. The colour of the product is light green. The product is solid. We have to dissolve the solid in the H2SO4 solution. After that we have to boil the solution. After the solution boiled, we
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  • Fall '15
  • Potassium permanganate

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