In the empirical data above the mean percentage of water in the iron salt crystal was 6.27%. The mean percentage of the potassium ion was determined to be 17.81%. For the iron ion the mean percentage was 12.20% and the average percent for oxalate was 57.20%. The total percentage of the mean adds up to 97.28%. The empirical formula using the means provided created the formula K2Fe(C2O4)3*2H2O. The total molar mass in this equations is 434.05 grams. The percent yield of iron salt using the actual yield of 8.71 grams with a theoretical yield of 17.8 grams is 49%.
Discussion:
The percent yield calculated in this experiment was 49% that indicates errors occurred during this lab. Possible sources of error could have arisen in the decantation and recrystallization of the crystals. This process in the lab was difficult and was not
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During this process the solvent was suppose to be used to create more crystals. Without this step it lessened our actual yield of crystals created in reaction. Furthermore, measuring the total mass of crystals was not done with the correct number of significant figures. Another process of the lab that may have caused errors was during the dehydration process. As seen in the data, the mass of the crystals did not change significantly after being heated. The hydrate was suppose to lose water from evaporation but the crystals did not lose that much mass after being heated. This led to a very high relative range, 79.34%, that is above the other components in the iron salt lab. Also in this stage of the lab we did not evenly distribute the crystals between the beakers and did not put more grams in each container when we had extra grams to spare. To lower the errors during this process we could of put iron crystals under the heat stove longer and used more crystals in each trial. Likewise, errors occurred during the titration