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Titration of Iron (II) ammonium sulphate

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Titration of Iron (II) ammonium sulphate Aim: To find the concentration of Fe (II) in (NH4)2SO4 Fe SO4.6H2O Method: 1. A weighing bottle was accurately weighed and approximately 5g of Iron (II) ammonium sulphate was then added to the bottle, after which the total mass of bottle + Iron (II) ammonium sulphate was weighed and recorded. ALL of the crystals were then tipped into a 100cm3 beaker. The bottle was carefully rinsed out 3 or so times with 1 mol dm-3 of sulphuric acid (whilst taking care not to let the acid come into contact with skin as it is irritant), transferring the rinsings to the beaker each time. Care was taken to ensure that all of the crystals were transferred to the beaker. 2. A further 25cm3 of acid was then added to the beaker but the beaker was not filled to more than half its volume. The acid and solid were then stirred together in the beaker with a glass rod until it was clear that all of the solid was dissolved. ...read more.


(Process 1) 6. Potassium Manganate (VII) was then added to a clean 100cm3 beaker and transferred to a clean burette. A small amount of the solution was allowed to run through the jet to make sure it was full of solution. (Process 2) 7. The volume reading on the burette before titration was recorded in a table to the nearest 0.05cm3. (Process 3) 8. Potassium Manganate was then added in small volumes to the solution in the conical flask, and after each addition the flask was swirled. The purple colour of the Manganate ions disappeared as they reacted with the iron ions. When a faint purple colour began to emerge in the solution this was the end point of the titration. (Process 4) 9. The final burette reading was recorded and the volume of solution run out into the flask was calculated. (Process 5) 10. Processes 1,2,3,4 and 5 were repeated until at least three titration volumes agreed to within 0.1cm3 Raw Results: Mass of weighing bottle and solid 6.85g Mass ...read more.


ammonium sulphate compound was quite pure (only a small amount of the Iron (II) in the compound has been oxidised). Evaluation: Percentage error = error x 100 reading Quantity measured % error Mass of iron compound weighed on balance 0.1 250cm3 solution made up in volumetric flask 0.08 25cm3 solution delivered by pipette 0.24 average titre 0.2 Percentage error of graph: 0.07% (5/70) Error Identification- The first stage in the procedure, which could have led to errors, is transferring the iron (II) ammonium sulphate to the clean beaker. This would have led to a lower titration result. The second stage in the procedure, which could have led to errors, is the transfer of the solution to the volumetric flask. This would also have led to a lower titration result. The third stage in the procedure, which could have led to errors, is the dropping of potassium manganate (VII) solution into the iron (II) solution. This error would have led to a higher titration result. The final error, which was identified, would have the most impact on the overall titration result. James Holman ...read more.

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