Figure 4c analysis of oxalate in k 3 fec 2 o 4 3 3h 2

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Figure 4c – Analysis of Oxalate in K 3 Fe(C 2 O 4 ) 3 ·3H 2 O Total Volume of Solution A 0.100L Moles of Oxalate 0.00493moles Molecular Weight of Oxalate 88.018 g/mol Mass of Oxalate in Solution A 0.434 grams Mass of K 3 Fe(C 2 O 4 ) 3 ·3H 2 O 1.00 grams Weight Percentage of Oxalate in Sample 43.4% Theoretical Weight Percentage of Oxalate 53.75% Percent Error 19.25% Discussion
The percent yield of the experiment was 60.9% meaning that although the majority of the product was collected but just under 40% of the product was lost. This could be because of many different reasons. One of which being while decanting the liquid in the first stage of the experiment, synthesis, there was no filtration system. This caused many problems because the solid may have been discarded in the draining of the liquid and some liquid may have stayed in the solid. Another possibility is an incomplete reaction while heating. If the reaction was not fully reacted during the heating process it could have left some, (NH 4 ) 2 Fe(SO 4 ) 2 ·6H 2 O , in the solution which would change the total yield of the synthesis process. The second part of the synthesis is another place error could have occurred. As in the first part of the synthesis a mistake in the heating process could occur and affect the total yield .a solution of iron oxalate and potassium oxalate was heated to 40 o C.Unlike an oven a Bunsen burner cannot be set a temperature and be trusted to get to that exact temperature ,the Bunsen burner has a capacity of 800 o C this means that the solution could very easily have been over heated and caused side reactions in the solution. Another possible outcome is if the thermometer was left to touch the bottom it could have read much hotter than the actual temperature of the substance it may have not reached 40 o C and been too cold for the full reaction to occur. While collecting the crystals formed the in the synthesis portion, they were put through a simple filtration system and rinsed with DI water. The crystals were very fragile, and some could have dissolved while being rinsed. They were also moved several times from the beaker to filter paper to blotting paper and finally to weighing paper so there could have been some loss in crystals in any part of the transferring of the crystals. The iron analysis produced a 34.56% error from the theoretical percentage of iron in K 3 Fe(C 2 O 4 ) 3 ·3H 2 O.A contributing factor to the higher than expected percent of iron in the solution could be because of residue left behind in the volumetric flask .Although it was rinsed with DI water prior to starting the experiment the shape of the flask made it very difficult to effectively clean and dry the flask. The oxalate analysis produced a 19.25% error. The oxalate analysis produced a number lower than the theoretical value expected. This could be a result of the transferring to many different containers and having some product lost along the way. While titrating the solution for a very brief second in a few different instances the solution turned a burnt orange color. This is an

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