What do you observe in the above picture? Why?
Answer: Ice floating in water; Density
Density is a physical property that relates the mass of a substance to its volume. Density is defined as mass per unit volume of a substance. Density is reported as g/ml or g/cc. The mathematical form of density d= m/v. Physical meaning of density refers to the compactness of the substance.
Density of a substance depends on temperature. Specially for liquids and gases, when temperature increases, volume expands and therefore density decreases. For most substances solid state is denser than liquid and liquid is more dense than gas. Water is an exception. Ice is less dense than liquid water. A less dense substance floats on a denser liquid.
Density also depends on pressure. An allotrope of carbon Diamond can be converted to graphite at a very high pressure. Although they contain the same atoms of carbon but they do not share the same density.
If two liquids are mixed together and they are immiscible, liquid with lower density is always on top of liquid with higher density. In other words, substance with higher density always sinks in substance with lower density and vice versa.
Densities of Common Substances
Material | Density (gm/cm^3) |
|
Liquids | ||
Water at 4 C | 1.0000 | |
Water at 20 C | 0.998 | |
Gasoline | 0.70 | |
Mercury | 13.6 | |
Milk | 1.03 | |
Material | Density (gm/cm^3) |
|
Solids | ||
Magnesium | 1.7 | |
Aluminum | 2.7 | |
Copper | 8.3-9.0 | |
Gold | 19.3 | |
Iron | 7.8 | |
Lead | 11.3 | |
Platinum | 21.4 | |
Uranium | 18.7 | |
Osmium | 22.5 | |
Ice at 0 C | 0.92 | |
Material | Density (gm/cm^3) |
|
Gases at STP | ||
Air | 0.001293 | |
Carbon dioxide | .001977 | |
Carbon monoxide | 0.00125 | |
Hydrogen | 0.00009 | |
Helium | 0.000178 | |
Nitrogen | 0.001251 |
There are two different ways density can be determined in Lab. 1) dimensional method and 2) displacement method.
In dimensional method, volume of the regularly shaped object is determined applying the standard formula. Mass of the object is determined using analytical balance. Then mass is divided by volume to determine the density.
Example: Determine the density of a unknown metal cube that has side length 3.00cmand mass is 310.672g.
Volume of the metal cube 3.00*3.00*3.00= 27.0 cm3
Density of the metal= 310.671/27.0= 11.5 g/cm3
In displacement method some water is taken in the graduated cylinder and then the irregular shaped object is dropped in the cylinder. Volume of water in the cylinder rises. The difference in volume between initial and final volume of graduated cylinder is the volume of the cylinder.
In the above example, volume of the liquid (96.0-90.0)ml =6.0 ml.
If the mass of the sample 16.9050g, the density of the sample = 16.9050/6.0 ml= 2.8 g/ml.
https://gpb.pbslearningmedia.org/resource/arct15-sci-densitylab/density-lab/
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TRY THIS OUT!
Block#1: Styrofoam
Block#2: Wood
Block#3: Ice
Block#4: Aluminum
Block#5: Brick
Activity:
Ans: 1) Wood m= 2.00kg, v= 5.00L; d= 0.400kg/L, Brick = 10.00/5.00=2.00kg/L, Ice 4.60/5.00 kg/L, Aluminum= 13.50/5.00= 2.70 Kg/L
2) density of my block 13.50/5.00= 2.70 Kg/L
3) same
4) Some sink and some float
5) Yes, if the mass/volume ratio>1 , sinks, if the ratio<1, float
6) Yes. Ethanol has different density than water. Less dense object floats, denser object sinks.
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Example problem:
D= m/v= 13.4958/4.98= 2.71 g/cm3
Density can be written as conversion factor.
8.90 g/1 ml or 1 ml/8.90 g Since we have to determine volume, volume will be the numerator of the ratio.
1 ml/8.90 g * 25 g = 2.8 ml (lowest sig fig 2)
Click on the right hand side of the screen and mystery metal. Find the mass and volume of the sample by displacement method, determine the density. Can you identify which metal is this?
Watch the following video:
Dimensional method:
Displacement method
1) The given beaker contains 100 ml of water. Draw an illustration for what would be observed in each circumstances when the following liquids were added. a) Hexane 50.0ml d= 0.65 g/ml b) dichloromethane 50.0ml d=1.33 g/ml.
3. Which one has higher mass? 100 ml of water or 100 ml of Hg?
4. which substance has higher volume? 100 g of gold or 100 f of Copper? Explain. ( Use the density chart above to answerthe question.
Ans: 1.hexane sinks and dichloromethane floats
Combined Dimensional Analysis Practice Problems
7.13 g Zinc=1 mL Zinc 7.13 g Zinc = 1 = 1 mL Zinc
1 mL Zinc 7.13 g Zinc
a) What is the volume, in cm3, of a 5.00 g piece of zinc?
b) What is the mass of a 45.6 L block of zinc?
b) What would be the mass of 15.0 of cm3 iron?
c) What would be the volume of 1000. grams of iron?
Ans: 1. 3550ml
Specific Gravity
Relative density, or specific gravity,[1][2] is the ratio of the density (mass of a unit volume) of a substance to the density of a given reference material. Specific gravity for liquids is nearly always measured with respect to water at its densest (at 4 °C or 39.2 °F); for gases, the reference is air at room temperature (20 °C or 68 °F). The term “relative density” is often preferred in scientific usage.
If a substance’s relative density is less than 1 then it is less dense than the reference; if greater than 1 then it is denser than the reference. If the relative density is exactly 1 then the densities are equal; that is, equal volumes of the two substances have the same mass. If the reference material is water, then a substance with a relative density (or specific gravity) less than 1 will float in water. For example, an ice cube, with a relative density of about 0.91, will float. A substance with a relative density greater than 1 will sink.
Temperature and pressure must be specified for both the sample and the reference. Pressure is nearly always 1 atm (101.325 kPa). Where it is not, it is more usual to specify the density directly. Temperatures for both sample and reference vary from industry to industry. In British brewing practice, the specific gravity, as specified above, is multiplied by 1000.[3] Specific gravity is commonly used in industry as a simple means of obtaining information about the concentration of solutions of various materials such as brines, sugar solutions (syrups, juices, honeys, brewers wort, must, etc.) and acids.