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Florida Institute of Technology *

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1101

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Chemistry

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Feb 20, 2024

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Laboratory Techniques Lab Report Instructions: For this investigative phenomenon, you will need to determine the densities of an unknown solid and liquid using different methods of measurement to determine if the solid will float on water. Record your observations and test measurements in the lab report below. You will submit your completed report. Lab Help Video Title: Density Measurements Virtual Lab Objective: To determine density of liquid and solids Hypothesis: None Materials: What scientific equipment and tools were used to collect data in the simulation? (Record the materials as you work through the simulation.) Part I Materials Part II Materials liquid, graduated cylinder, scale, beaker digital scaled, irregular shaped solid, cylinder, beaker, string Access the virtual lab and complete Part I and Part II trials of the experiment. List your controlled variables, independent variable, and dependent variable.

Controlled variables: The same measurement tools are used, and the masses of the empty graduated cylinder and the irregular shaped object are the same. Independent variable: Part I—the volume of the unknown liquid Part II—the matter of the solid Dependent variable: Part I—the matter of unknown liquid; Part II—the volume of water after the object is placed into the water Significant Figure Rules Data Type the results of your tests in the data table below. The saved results of your measurements can also be found by selecting the data table button within the virtual lab. Don’t forget to record measurements with the correct number of significant figures. Part I: Density of Unknown Liquid (Trial 3 Student Trial) Trial 1 Trial 2 Trial 3 Mass of empty 10 mL graduated cylinder (grams) 25.80 24.50 25.50 Volume of liquid (milliliters) 8.45 8.50 8.60 Mass of graduated cylinder and liquid (grams) 36.75 35.00 36.50 Part II: Density of Irregular-Shaped Solid Mass of solid (grams) 38.951 42.235 42.891 Volume of water (milliliters) 52.0 50.0 49.5 Volume of water and solid (milliliters) 56.5 55.0 54

Calculations Show your calculations for each property. Be careful to follow significant figure rules in each calculation. Part I: Density of Unknown Liquid · Determine the liquid's mass: mass = (grad. cylinder and liquid) – (empty grad. cylinder) · Determine the density of the liquid: density = mass ÷ volume. Rules for calculations: Addition and Subtraction: line up decimal points and record to the least accurate measurement Multiplication and division: Count the significant figures in each measurement and then use the least accurate for your answer: ex.. o Sample calculation: 10.95 g / 8.45 mL = 1.30 g/mL o 4 sig figs / 3 sig figs = 3 sig figs o (rounded up to show three significant figures) Part I Calculations Trial 1 Trial 2 Trial 3 Mass of liquid 36.75 g – 25.80 g = 10.95 g 35.00 - 24.50 = 10.50 g 36.50-25.50 = 11g Density of liquid 10.95 g / 8.45 mL = 1.30 g/mL 10.50 g / 8.50 mL = 1.23 g/mL 11g/ 8.60mL=1.27g/mL

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Average density of the three trials Part II: Density of Irregular-Shaped Solid · Determine the solid’s volume: volume = (volume of water and solid) – (volume of water) · Determine the density of the solid: density = mass ÷ volume. Part II Calculations Trial 1 Trial 2 Trial 3 Volume of solid 56.5 mL – 52.0 mL = 4.5 mL 55.0mL - 50.0 mL = 5.0 mL 54.0mL -49.5mL= 4.5mL Density of solid 38.951 g ÷ 4.5 mL = 8.7 g/mL 42.235 g / 5.0 mL = 8.5 g mL 42.891g/4.5mL =9.5g/mL Average density of the three trials Conclusion: In conclusion, this lab allowed me to explore and determine the densities of liquids and solids. I learned about the concept of density, how to calculate it for liquids and solids, and the impact of uncertainty in measurements. By understanding these principles and considering the sources of uncertainty, I can strive for more accurate and reliable data in future experiments. Using complete sentences, write a conclusion that addresses the following: ● The purpose of the lab, what you explored, what you learned ● An explanation of how densities were determined for liquids and solids ● A description of how uncertainty in measurements impacted your data collection

Post-Lab Connection Questions Answer questions in complete sentences and support with data from lab. 1. Claim: Density is an intensive (does not depend on sample size) property of matter. Explain how your data supports this claim with examples in your data. To determine if density is an intensive property, we compare the density measurements obtained in the experiment. If the measurements are consistent and similar to each other, it supports the claim that density is an intensive property. For example, if we obtain density values of 1.52 g/mL, 1.49 g/mL, and 1.50 g/mL, these values are close to each other and show that density does not depend on the sample size.On the other hand, if the density measurements vary significantly, it would suggest that density depends on the sample size, which contradicts the claim. For instance, if we obtain density values of 1.40 g/mL, 1.60 g/mL, and 1.55 g/mL, these values are not consistent and indicate that density might be affected by the sample size. 2. Compare the density values for the liquid in Part I. The actual density of our liquid is 1.50 g/mL. 1. Are the density measurements of the liquid precise? Explain your answer. If the density measurements for the liquid in Part I are consistent and similar to each other, they are precise.Precision refers to how close multiple measurements of the same quantity are to each other. If the density measurements for the liquid in Part I are consistent and similar to each other, then they are precise. 2. Are the density measurements of the liquid accurate? Explain your answer. If the average density is close to the actual value of 1.50 g/mL, the measurements are accurate.To assess accuracy, we need to compare the average or mean density measurement to the actual value of 1.50 g/mL. If the average density is close to the actual value, the measurements are accurate. 3. Compare the density values for the solid in Part II. The actual density of our solid is 8.9 g/mL. What are some things you can do in the lab to improve accuracy of data collection? There are alot of things you can do to improve accuracy of data such as repeating measurements, getting someone else's opinion, and being precise. By using these steps you can improve the accuracy of data collection for the density values of the solid in Part II.

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