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A Redox Titration " Determining the percentage of iron in an iron ore

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Introduction

Experiment 2 (25-9-08) A Redox Titration - Determining the percentage of iron in an iron ore Objective To determine the percentage of iron in a spathic iron ore using manganate (VII) solution. Theory Aqueous solution of the iron ore (Solution 'B') can be prepared by dissolving it into dilute sulphuric acid. FeCO3 (s) + H2SO4(aq) � Fe2+(aq) + SO42-(aq) + H2O(l) + CO2 (g) Molar concentration of manganate(VII) solution can be determined by titrated it with a standard solution of iron(II) sulphate. 5Fe2+(aq) + MnO4-(aq) + 8H+(aq) � 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) Molar concentration of iron(II) ion in Solution 'B' can be determined by titrated it with standardized diluted manganate(VII) solution. 5Fe2+(aq) + MnO4-(aq) + 8H+(aq) � 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) Procedures 1. Preparation of solution of a spathic iron ore ( done by teacher) a. Dissolve 8.501g of a spathic iron ore in diluted sulphuric acid. b. Boil the resulting solution to remove carbon dioxide. c. Cool the solution. d. Dilute the solution into 1.0 dm3. e. Label it as 'B'. 2. Preparation of a standard solution of iron(II) sulphate a. Record the mass of iron(II) sulphate crystal given by the teacher. b. ...read more.

Middle

e. Add 25.0 cm3 of 1 M sulphuric acid into the flask. f. Run the solution from the burette into the conical flask, swirling the flask all the time. g. Stop the titration when the colour of solution in the conical flask just changes from colourless to pink. h. Record the final burette reading. i. Repeat steps(c)-(h) three more times. Results and Calculations 1a. Mass of iron(II) sulphate crystals = 5.000g 1b. No. of moles of iron(II) sulphate = = 0.01800 mol Molar concentration of iron(II) sulphate in 'Standard' = = 0.07199 M 2a. Titration results from Procedure 3: Burette reading Trial 1st 2nd 3rd Final burette reading / cm3 9.30 17.90 26.70 35.50 Initial burette reading / cm3 0.40 9.30 17.90 26.70 Volume of diluted manganate(VII) solution added / cm3 8.90 8.60 8.80 8.80 Mean volume = = 8.733 cm3 2b. By equation, no of moles of Fe2+ : MnO4- = 5 : 1 ? no. of moles of MnO4- = = mol Molar concentration of MnO4- ion in the diluted 'Titrant' = = 0.04122 M 3a. Titration results from Procedure 4: Burette reading Trial 1st 2nd 3rd Final burette reading / cm3 39.40 25.20 38.30 37.60 Initial burette reading / cm3 25.90 12.20 25.20 24.80 Volume of diluted manganate(VII) ...read more.

Conclusion

4a. Apparatus used: a beaker, glass rod, 250.0 cm3 of volumetric flask and filter funnel. Steps: 1. Dissolve the crystal with about 100 cm3 of 1 M sulphuric acid in a beaker. 2. Stir the solution with a glass rod until all the crystal is dissolved. 3. Pour the solution into a 250.0 cm3 of volumetric flask through a filter funnel. 4. Rinse the beaker and glass rod with about 30 cm3 of 1 M sulphuric acid. 5. Pour the washing though the funnel into the volumetric flask. 6. Add 1 M sulphuric acid upto the graduated mark of the volumetric flask. 7. Stopper the flask and invert it several times in order to mix the contents well. 8. Label the flask as 'Standard'. 4b. Apparatus used: a pipette, pipette filler and 250.0 cm3 of volumetric flask. Steps: 1. Wash a 25.0 cm3 pipette with distilled water and then with manganate(VII) solution. 2. Pipette 25.0 cm3 of manganate(VII) solution into a 250.0 cm3 of volumetric flask. 3. Repeat step(b) again. 4. Add deionized water upto the graduated mark of the volumetric flask. 5. Stopper the flask and invert it several times in order to mix the contents well. 6. Label the flask as 'Titrant'. Practical Report (Experiment 2) F.6A Angel Chan (4) Page 1 of 5 ...read more.

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