Introduction
Experiment five was a two-part experiment meant to have us practice our skills and then use those skills in actual data collection and analysis. In part one we used a sample of sodium saccharinate combined with a sample of a metal halide salt, our group used copper(II) chloride. The combination of these two samples allowed for the synthesis of a metal complex. In part two of the experiment we used a procedure similar to part one in order to collect phosphorus out of a sample of fertilizer. This sample was then compared to the amount of phosphorus which was present in the NPK ratio for that fertilizer. Part one of the experiment was based entirely on the collection of the total mass for the end product metal complex compared to …show more content…
The end product mass of our metal complex was 0.61 grams which gave us a percent yield of 117.30%, this is due to the fact that theoretically our end product mass should have been 0.52 grams. The reasoning behind our error in mass for this part of the experiment could be because we did not allow the water to completely filter out of our product. The added water weight could account for our high percent yield at the end of the experiment, had we allowed our product to filter out for a longer period of time we may have had a more accurate mass. In experiment 2 our group, along with the other groups, ended up with a greater amount of phosphorus than what we should have collected. After calculation, we discovered our percent P was 47.95% when it should have been 35%. The mass of phosphorus we collected from our 2.00-gram sample was 0.959-grams. Our data was similar to two other groups; one of which had the same mass of phosphorus as our group, and the other group had a mass that was slightly smaller than our own. The third group had a mass that was very close to the mass we should have had which was 33.15g actual percent P. The reasoning behind our error in this experiment could be because of inadequate filtration, or incorrect drying time for our product. The error of our experiment could more than likely be adjusted so that we could get a more accurate percent P if we were ever to reconduct the experiment. Overall, the experiments allowed us to realize that our samples can come out much more accurate if we allow ourselves time to filter out and dry our products and if we follow the procedures carefully from the
Experiment five was a two-part experiment meant to have us practice our skills and then use those skills in actual data collection and analysis. In part one we used a sample of sodium saccharinate combined with a sample of a metal halide salt, our group used copper(II) chloride. The combination of these two samples allowed for the synthesis of a metal complex. In part two of the experiment we used a procedure similar to part one in order to collect phosphorus out of a sample of fertilizer. This sample was then compared to the amount of phosphorus which was present in the NPK ratio for that fertilizer. Part one of the experiment was based entirely on the collection of the total mass for the end product metal complex compared to …show more content…
The end product mass of our metal complex was 0.61 grams which gave us a percent yield of 117.30%, this is due to the fact that theoretically our end product mass should have been 0.52 grams. The reasoning behind our error in mass for this part of the experiment could be because we did not allow the water to completely filter out of our product. The added water weight could account for our high percent yield at the end of the experiment, had we allowed our product to filter out for a longer period of time we may have had a more accurate mass. In experiment 2 our group, along with the other groups, ended up with a greater amount of phosphorus than what we should have collected. After calculation, we discovered our percent P was 47.95% when it should have been 35%. The mass of phosphorus we collected from our 2.00-gram sample was 0.959-grams. Our data was similar to two other groups; one of which had the same mass of phosphorus as our group, and the other group had a mass that was slightly smaller than our own. The third group had a mass that was very close to the mass we should have had which was 33.15g actual percent P. The reasoning behind our error in this experiment could be because of inadequate filtration, or incorrect drying time for our product. The error of our experiment could more than likely be adjusted so that we could get a more accurate percent P if we were ever to reconduct the experiment. Overall, the experiments allowed us to realize that our samples can come out much more accurate if we allow ourselves time to filter out and dry our products and if we follow the procedures carefully from the