Unit: Measurement
Chemistry, Wilson
Density Lab
Purpose:
To perform an experiment that will determine the density of the following: Wood
Cube, Aluminum Cylinder, Antifreeze, and an odd shaped object.
Theory:
Density equals mass divided by volume.
Procedure:
Part A
Part B
Wood Block
1.
Measure the mass using a triple beam balance scale. Create a Data
Table and record with last digit estimated.
2.
Measure the length, width, and height. Record with last digit estimated.
3.
Calculate the volume showing all of your work. Record in data table.
4.
Calculate the density showing all of your work. Record in data table.
Aluminum Cylinder
Part C
1.
Measure the height and diameter. Record with last digit estimated.
2.
Calculate the volume showing all of your work. Record in data table.
3.
Measure the mass using a triple beam balance scale. Record with last
digit estimated.
4.
Calculate the density showing all of your work. Record in data table.
Antifreeze
1. Measure the mass of a graduated cylinder. Record with last digit estimated.
2. Add some Antifreeze. (It doesn’t matter how much you add.)
3. Measure the new mass of the graduated cylinder.
4. Calculate the mass of Antifreeze added and record.
5. Record the volume of Antifreeze in the graduated cylinder.
6. Calculate the density showing all of your work.
687307093
Unit: Measurement
Chemistry, Wilson
Part D Odd Shaped Object
1. Measure the mass of the odd shaped object. Record with last digit
estimated.
2. Fill a displacement container with water.
3. Hold graduated cylinder under spout and gently place the odd shaped object
in the container. Record the volume of water displaced.
4. Calculate the density showing all of your work.
BELOW IS THE DATA TABLE FOR PROCEDURE A. YOU MUST CREATE PROPER DATA TABLES FOR
PROCEDURES B – D.
Data & Calculation Table:
Wood Block
Mass
Length
Width
Height
Volume
Density
Show Labeled Calculation(s):
g
cm
cm
cm
ml
g/ml
Conclusion: Answer both questions in complete sentences, showing work where
appropriate.
1. The actual density of Antifreeze is 1.109 g/mL. Using the % error equation
in your notes, determine your accuracy.
2. What are two changes could you make in the procedure to increase the
accuracy and precision of your results?
687307093