Density of a Solid Lab
Name_______________________________
Chemistry I 5.0
Period______Date____________________
Purpose: To determine the density of a solid.
Procedure:
1. Mass an empty 100 mL beaker. Record the mass in the data table.
2. Choose 1 metal to analyze. Add a small amount of the metal to your beaker and determine its mass.
3. Fill half of your graduated cylinder up with water. Note the initial volume of the water.
4. Add your metal to the water. Note the final volume of the water.
5. Return the wet metal to the front lab bench for drying.
6. Repeat the procedure 4 times with a different amount of the metal each time. Only use dry metal
in this lab.
Note: Strive for a 1 mL or larger difference between all volume measurements.
.
Data: Name of metal:_______________________________
Trial 1
Trial 2
Trial 3
Trial 4
Trial 5
Mass of empty
beaker
Mass of beaker
and metal
Mass of metal
Initial Volume
Final Volume
Volume of
metal
Density of
metal
Average
density of
metal
Graph:
Prepare a mass vs. volume line graph using your data from the table above. Do not connect the
plotted points. Rather, draw a line of best fit. Remember to follow all previous graphing
instructions.
Calculations
1. Determine the slope of the line. This is the density of your metal. Show all work and include units.
Remember:
y2 – y1
x2 - x1
2. The actual densities of copper, lead and aluminum respectively are 8.96 g/mL, 11.4 g/mL, and 2.70
g/mL. Determine the percent error for your experiment. Use the slope of your graph for your density!
% Error 
Experimental  Accepted
x100
Accepted
3. Examine the results of your experiment. How would they appear if they were precise and accurate?
4. Examine the results of your experiment. How would they appear if they were precise but inaccurate?
5. Using 8.96 g/mL for the density of copper, calculate the volume that a 4.75 g sample would occupy.