In this lab you will be titrating a solution of the potassium trioxalatferrate(I

Question

In this lab you will be titrating a solution of the potassium trioxalatferrate(III) trihydrate you synthesized in a prior experiment with a standardized potassium permanganate solution. You will determine the number of oxalate in your sample and Compare it to the expected value. Here are the essential facts: Oxalate ion is oxidized to carbon dioxide by permanganate ion The manganese in the permanganate ion is reduced to manganese(II) ion in the reaction The oxidation reduction reaction occur, in an acidic solution The permanganate km is purple The products are colorless. Therefore the purple of the Permanganate solution disappears during the titration until the endpoint it reached At the endpoint. The slightly pink the lighter the better. The endpoint in a titration occurs when all of the reactant being analyzed has been used up. I millimole (mmol) - 0.001 mole Molarity x L gives moles. molarity x ml. gives mmol. (Molarity = mol l, or mmol ml.) On a separate piece Ol paper to be turned in with your Data Sheet. write a balanced redox reaction for oxalate ion reacting with permanganate ion in an acidic solution to produce manganese (II) ion plus carbon dioxide. Show your work. Weigh two samples of potassium oxalate monohydrate. Each sample should have a mass of 0.1 to 0.11 g. Record the exact masses you weigh to the nearest milligram and place the samples into separate 125 ml. Frlenmeyer flasks. Label the flasks in some way so you can keep track of the two different samples. Add approximately 35 ml. of 1.0 M H_2SO_4 to each flask then add five of six diops of phosphoric acid to each flask. Wear gloves and keep them on for the next steps. Heat the flasks on a hoi plate set at a medium selling. Occasionally swirl the samples to make sure all of the solid dissolves. You will need to heal the solutions until the temperature of the acid solution is 70 degreeC. Proceed with the next steps while you are waiting for the samples to reach the proper temperature. If the solutions reaches 70 degreeC before the buret is set up. turn the hoi plate down Do not let the solutions gel above 80 degreeC. You may want to handle the hot flask using a couple of layers of paper towels.

Explanation / Answer

1.

The reaction between permanganate ion (MnO4-) and oxalate ion (C2O42-) in acidic solution:

MnO4- + C2O42- --> Mn2+(aq) + CO2(g)

To balance this redox reaction using the method of half-reactions, begin by writing the incomplete oxidation and reduction half-reactions:

MnO4- --> Mn2+(aq)

C2O42- --> 2CO2(g)

therefore the balance equation is, MnO4- + C2O42- --> Mn2+(aq) + CO2(g)

Problem 2-4 should be done in your laboratory. Goodluck! :)

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