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Aim; 1)To prepare a standard potassium dichromate solution 2)To standardize the ammonium iron(II) sulphate solution 3)To determine the given unknown potassium permanganate solution 4)To estimate the concentration of hydrogen peroxide

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Course Code: 13554/Y1 Student Name: Chow Man Chung Lam Kwok Kei Lee Long Sing Chan Ka Chun Date performed: 29th September, 2010 Experiment 4: Reduction Titration I Objective: 1) To prepare a standard potassium dichromate solution 2) To standardize the ammonium iron(II) sulphate solution 3) To determine the given unknown potassium permanganate solution 4) To estimate the concentration of hydrogen peroxide Apparatus & equipments used: 1) Burette, 50mL capacity 2) Bulb pipette, 25mL capacity 3) Volumetric flask, 250mL capacity Chemicals used: 1) Potassium dichromate solid 2) Potassium permanganate solution, 0.02M 3) Dilute sulphuric acid solution, 2.5M 4) Hydrogen peroxide sample solution 5) Fe2+ Solution, approx. 0.1M 6) N-phenylanthranilic acid indicator 7) Barium diphenylamine sulphonate indicator, 1% aq. Results and Data Treatment: Weighting Data: Mass of vial: 6.3545g Mass of vial and Potassium dichromate: 7.5975g Mass of Potassium dichromate: 1.2430g Resulting Potassium dichromate solution made up to: 250.0cm3 Titration I: Standardization of iron(II) ...read more.


2 3 4 Final burette reading (cm3) 24.45 24.20 48.40 24.30 Initial burette reading (cm3) 0.00 0.00 24.20 0.00 Volume of titrant used (cm3) 24.45 24.20 24.20 24.30 Average volume: 24.23 cm3 Calculation: ? due to last titration I's calculation ?Number of mole of Fe2+ = 0.002535 Molarity of Fe2+ solution = 0.002535 / (24.23/1000) = 0.1046 ~ 0.10M Titration II: Determination of the potassium permanganate solution Titrant (in burette): Potassium Permanganate Solution Titrate (in Conical flask): 25.0cm3 of Fe2+ Solution Indicator used: Potassium Permanganate Solution Colour of indicator changed from: Green to Pink Titration No. 1(trial) 2 3 4 Final burette reading (cm3) 24.90 49.50 24.70 49.30 Initial burette reading (cm3) 0.15 24.90 0.00 24.70 Volume of titrant used (cm3) 24.75 24.60 24.70 24.60 Average volume: 24.63 cm3 Calculation: Number of mole of Fe2+ = (0.1046)(25.0/1000) ...read more.


(100%) = 7.6656 ~ 7.67% Volume concentration of H2O2 = (7.67/6.8)(22.4) = 25.26588 volume ~ 25.27 volume Discussion: 1. Deep colour of potassium permanganate solution will show out two meniscuses but according to burette using, we are try to measure the volume by different. Therefore if we technically use the same meniscuses in the all reading, it will be fine for the experiment. 2. Store the dilute hydrogen peroxide in a cool, dry and well-ventilated area. Also put it in a steel or glass and opaque container. On the other hand, keep away from heat, flame and light. Conclusion: In titration I, we standardize the iron(II) solution is 0.10M with N-phenylanthranilic acid indicator and Barium diphenylamine sulphonate indicator. In titration II, we determined the potassium permanganate solution is 0.02M. In titration III, we estimated the dilute hydrogen peroxide is 0.038g and we found out the molarity of it is 0.045M. And for the original hydrogen peroxide's percentage is 7.67%(w/v) and volume concentration is 25.27 volume. ?? ?? ?? ?? ...read more.

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