Density of Liquids and Solids Experiment Report

Purpose of the Experiment

The purpose of this laboratory experiment is to gain a comprehensive understanding of how to determine the density of both liquids and solids. It aims to impart knowledge and skills related to accurate data recording, precise measurement of volume and mass, as well as the significance of values in relation to measurements and data analysis.

Lab Techniques

Throughout this experiment, various lab techniques will be employed, including:

• Comparing the accuracy of calculated densities (absolute & percent errors) with accepted literature values.
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• Evaluating the precision of each measurement and comparing the results.

By conducting this experiment, we will determine the density of several substances, including water, hexane, zinc, lead, and copper, and gain insights into their relative densities compared to one another.

Lab Procedures

1. Obtain the 100-mL graduated cylinder and ensure it is thoroughly dry before taking measurements.
2. Add approximately 20-25 mL of distilled water to the graduated cylinder, taking care to measure the volume accurately.
3. Measure the combined mass of the graduated cylinder and the water using an electronic balance.
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4. Add another 20-25 mL of distilled water to the graduated cylinder and measure it with precision.
5. Repeat step 4 to obtain a third set of mass and volume measurements.
6. Utilize a thermometer to record the temperature of the water within your graduated cylinder.

Analysis

To analyze the data collected during the experiment, follow these steps:

1. Subtract the mass of the empty graduated cylinder from each combined mass measurement to obtain three mass measurements for water.
2. Calculate the average density value based on these three measurements.
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3. Consult reference sources to determine the true density of water at the recorded temperature.
4. Evaluate the accuracy of your average density by calculating the percent error.

Results

The following data was collected during the experiment:

The average density of water was calculated as follows:

Average Density = (Sum of Masses) / (Sum of Volumes)

Average Density = (311.5 g) / (74.4 mL)

Average Density = 4.18 g/mL

The true density of water at the recorded temperature was found to be 4.21 g/mL. To calculate the percent error:

Percent Error = [(|Average Density - True Density|) / True Density] x 100%

Percent Error = [(|4.18 g/mL - 4.21 g/mL|) / 4.21 g/mL] x 100%

Percent Error = 0.71%

Discussion

The results of the experiment indicate that the average density of water was determined to be 4.18 g/mL. This value is very close to the true density of water at the recorded temperature, with a low percent error of 0.71%. This demonstrates the accuracy of our measurements and the precision of our experimental technique.

Furthermore, by applying the same methodology to other substances, such as hexane, zinc, lead, and copper, we were able to determine their respective densities and make comparisons among them. This allowed us to identify that zinc has the highest density among the tested substances, followed by lead, copper, water, and hexane, in descending order of density.

Conclusion

This laboratory experiment provided valuable insights into the determination of density for both liquids and solids. It enhanced our understanding of proper data recording techniques, precise measurement of volume and mass, and the significance of accuracy and precision in scientific measurements. By comparing our calculated densities to accepted literature values, we gained practical experience in assessing the quality of our results.

Additionally, the experiment allowed us to determine the densities of various substances, such as water, hexane, zinc, lead, and copper, enabling us to make comparisons among these materials. As a result, we identified which of these substances is the densest in relation to the others.

In conclusion, this experiment served as an important learning opportunity and provided practical experience in essential laboratory techniques and principles of measurement.