Make a mass determination for 10. 00 cm3 of each solution, using an analytical balance and your burette. Be certain to record the temperature for each solution as you test Its density. . Make a mass determination for 10. 0 cm3 of the unknown solution, again recording the temperature for each solution as you test the density. B. Data Processing 1 . Your raw data should be organized In a table designed by you In your lab report (Have this ready before entering the classroom). KCI solution percentages by mass Mass determination for 10. 00 cm3 Temperature (oc) 5 10 20 Unknown Solution percentages by mass (%) 15 2. Your processed data should be entered in a different table also designed by you before coming to class. 3. Using this data, construct a graph of the density of your olutions of the known concentration versus the percentage of KCI the solution contains.
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Number of Trials If there were to be more trials, then the average number would be more precise, and closer to the one of the theoretical value. We can eliminate the incorrect results by trying more times, minimizing the random error. Beaker Number Although the beakers had the same measuring capacity, their mass may be different, making the measurements of the uncertainties, density, and the percentage error different. The way to minimize this error is to use the same beaker throughout the whole experiment Eyesight Our eyesight may have measured a number that was incorrect.
The precision of the lab is put into consideration. By measuring, or weighing the amount of liquid poured into the beaker, we are sure that it is the correct value. Errors: With the table that was found online, we can come to the conclusion of the Percentage Error, which has the equation of:. The reference for the table is listed in the Bibliography. 5% of Solution: 10% of Solution: 15% of Solution: 20% of Solution: Uncertainty of Volume: Uncertainty of Beaker (mass): Uncertainty of the Whole Experiment: Conclusion: The objective of this lab was to find out that when the composition (Percentageof
Page 2 Density of Solutions Lab Essay
Solution) increases, so does the density, and vice-versa. This was what was supposed to happen, but it didn’t happen. What happened was that the results came out very irrational, they didn’t make much sense. In the graph that was created, there was a trend line to demonstrate the supposedgrowth of the density when the composition and then grew again with the unknown solution. By looking to the uncertainty of the beaker and the volume added together, it was only В±0. 5% negligible, which is basically nothing. What went wrong in this experiment was what was in the solutions.See More on Measurement