Titration Lab
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Introduction
Chemistry Lab Report Kevin Schulze 11th IB SL Chemistry 10/11/10 Redox Titration with Potassium Permanganate Research Question How much amount is needed to titrate redox with potassium permanganate? Background Theory An acidified solution of manganate or permanganate ions are both strong oxidising chemical agents. Hypothesis/Predictions My hypothesis is that it will take approximately 10-15 drops of redox in order titrate redox with potassium permanganate. Key Variables Independent: Titration of potassium permanganate. Dependent: Amount of redox to titrate the potassium permanganate. Controlled: Amount of potassium permanganate, amount of force put in, temperature of the liquids. Apparatus AR ammonium iron (II) sulphate Crystals Sulphuric Acid Weight Scale Volumetric Flask/Conical Flask Distilled Water Pipette Method for Control of Variables 1. In order to control the titration of potassium permanganate, we used the pipette to make the titration constant. We also used the same amount of chemical solutions, with the same flasks, to make the titration as constant as possible. 2. To control the amount of redox in the experiment, we have used the pipette to keep on putting the same amount of drop every time. ...read more.
Middle
4. I have used the pipette to pipette 10cm� of the solution into a conical flask and added about an equal volume of distilled water. 5. I titrated this with 0.0200mol dm-� potassium manganate (VII) solution to a faint pink color. 6. I repeated the titration for at least 2 times for accuracy in the data and recorded all the results. Table of Raw Results Table Showing Volume of KMnO4 Used to React With the Solution Initial Reading Final Reading Volume of KMnO4 Trial 1 0.00 10.00 10.00 Trial 2 10.00 20.00 10.00 Trial 3 20.00 30.00 10.00 Trial 4 30.00 41.00 11.00 Trial 5 41.00 51.00 10.00 Trial 6 0.00 10.00 10.00 Table of Processed Results Table Showing Volume of KMnO4 Used to React With the Solution in cm��0.05cm� Initial Reading/cm��0.05cm� Final Reading/cm��0.05cm� Volume of KMnO4/cm��0.10cm� Trial 1 0.00 10.00 10.00 Trial 2 10.00 20.00 10.00 Trial 3 20.00 30.00 10.00 Trial 4 30.00 41.00 11.00 Trial 5 41.00 51.00 10.00 Trial 6 0.00 10.00 10.00 Average 16.83 27.00 10.17 Standard Deviation 16.62 16.78 0.41 The error or uncertainty of this data is �0.05cm�. ...read more.
Conclusion
The main aim of this experiment, titration of redox with potassium permanganate, was well presented, and overall the experiment was good. Problem Calculation 1. MnO4- + 8H+ + 5Fe- = Mn2+ + 4H2O + Fe3+ 2. 5 moles of Fe2+ is required. 3. 10cm3 = 0.01dm3 0.02 mol dm-3 x 0.01 dm3 = 0.0002 mol 0.0002 moles of KMnO4 is present. 4. MnO4- : Fe2+ 1:5 0.0002 mol : 0.001 mol 0.001 moles of Fe2+ is present in 10cm3 of the solution. 5. 0.001 mol x 10 =0.01 mol 0.01 moles of Fe2+ is present in 100cm3 of the solution. 6. 1 mole of Fe2+ = 56grams 56g x 0.01 mol = 0.56g 0.56 grams of Fe2+ is in the ammonium iron (II) sulfate 7. Number of moles of ammonium iron (II) sulfate = 39 0.56g/(39mol x 0.1) = 14.4% 8. 1 mol of ammonium iron(II) sulfate = (NH4)2Fe(SO4)2 x 6H2O = 2N + 8H+ 1Fe+ 2S + 8O + 12H + 6O = 392 grams 56g/392g = 14.3% 9. My result was 14.4% and it is almost equal to the correct value which is 14.3%. The difference is only 0.1%. 10. The iron (II) salt might evaporate if I heat it, and will affect the result. ?? ?? ?? ?? ...read more.
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