Density, defined as a substance’s mass per unit volume, is an important physical property for characterizing a material or chemical system.

Mathematically, density is calculated as a substance’s mass per the volume it occupies. The Greek symbol “ρ” is normally used to denote density in the physical sciences. To obtain the density of a substance, its mass and volume are determined by measurement.

This video will introduce the principles of density determination, the procedures for calculating the density of both solid and liquid substances, and some applications of density in scientific research.

All matter has mass, and that mass occupies a specific volume.

However, the volume of space occupied by the same mass is different for different substances, depending on their respective density. For example, a ton of bricks has the same mass as a ton of feathers, but occupies considerably less volume. Density is obtained by dividing mass by volume. . Mass can be measured with scales or balances, and is expressed in grams or kilograms.

By convention, the volume of liquids and gases is often expressed in units of liters or milliliters, measured with glassware. The dimensions of regularly shaped solids can be measured directly with rulers or calipers, which have linear units, giving volumes in units such as cubic centimeters. One milliliter is equivalent to one cubic centimeter.

The dimensions of irregularly shaped solid samples cannot be easily measured. Instead, their volumes can be determined by submerging the solid in a liquid. The volume of the submerged solid is equal to the volume of liquid displaced.

Now that you understand the concept of density, let’s take a look at two protocols for accurately determining the density of a liquid and a solid.

To begin this procedure, place a clean and dry 50-mL volumetric flask on an analytical balance. After the measurement has stabilized, tare the balance. The balance should read zero. Use a funnel to add approximately 45 mL of liquid to the flask. Do not fill to the calibration mark. Use a Pasteur pipette to carefully add the final 5 mL of liquid, just until the bottom of the liquid’s meniscus touches the line on the flask. Weigh the flask again and record the mass of the liquid. Repeat the measurements at least twice to obtain additional values to calculate an average density. The results are shown in this table. The average measured density was 0.789 g/mL, matching the literature value for ethanol.

To determine the density of an irregular solid in pellet form, add approximately 40 mL of water to a clean and dry 100-mL graduated cylinder. Record the exact volume. Place the cylinder on an analytical balance and tare. Add approximately 10 pellets, and record the new volume after the addition. Weigh the cylinder, water, and pellets. The mass is only the pellets, as the rest have been tared. Make at least two additional sets of mass and volume measurements to calculate an average value of the density. The density for zinc was measured for three different samples. It was found to be 6.3 g/mL. Note that, since the measurements were made in a graduated cylinder, which is less precise than a volumetric flask, the density has lower degree of precision.

Let’s now look at several different applications of density to different field of scientific research.

Density is useful for identifying or validating pure materials, such as elements or other species of known purity. For example, because gold has a higher density than many other cheaper metals, calculating the density of a gold coin is a quick and inexpensive way to test for its purity. If the density does not match that of gold, the coin is not pure. Here, a gold coin was found to have a mass of 27.55 g and a volume of 1.84 cm3, giving a density of 14.97 g/cm3, which is significantly less than gold’s density of 19.3 g/cm3, indicating that the coin is not made of pure gold.

Density measurements can also be used to identify an unknown substance if a list of possible reference densities is available, and can be used to distinguish between metals similar in appearance. In this example, the scientist is trying to identify two samples of shiny silver metal, which could be either aluminum or zinc. While the two samples have the same mass, their volumes are considerably different. The densities were determined to be 2.7 and 7.1 g/cm3 respectively, confirming their identities as aluminum and zinc.

Finally, differences in density are useful for separating components of a complex mixture. In a method called density gradient centrifugation, decreasing concentrations of sucrose or polymers are layered to create a gradient. The sample is then added on top. This mixture is then subjected to centrifugation — the spinning of the mixture at high speed to generate a “centrifugal force” that will lead to the formation of a concentration gradient of the molecule. Components of the mixture will migrate to a point along this gradient with which its density is comparable.

In this example, a specific type of lipid droplets, or small drops of fat molecules, was isolated from cells. A homogenized mixture was first obtained by breaking the cells open. By centrifuging the mixture in a sucrose density gradient, the droplets were successfully separated from other cellular components that are made of lipids, such as the cells’ membranes. 

You’ve just watched JoVE’s introduction the determination of the density of a liquid and a solid. You should now understand mass, volume, and density, as well as having a good idea of how to measure these quantities.

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