The mass density or density of a material is its mass per unit volume. The symbol most often used for density is (the lower case Greek letter rho). Mathematically, density is defined as mass divided by volume:
 \rho = \frac{m}{V},
where is the density, m is the mass, and V is the volume. In some cases (for instance, in the United States oil and gas industry), density is also defined as its weight per unit volume,^{[1]} although this quantity is more properly called specific weight.
Different materials usually have different densities, so density is an important concept regarding buoyancy, purity and packaging. Osmium and iridium are the densest known elements at standard conditions for temperature and pressure but not the densest materials.
Less dense fluids float on more dense fluids if they do not mix. This concept can be extended, with some care, to less dense solids floating on more dense fluids. If the average density (including any air below the waterline) of an object is less than water it will float in water and if it is more than water's it will sink in water.
In some cases density is expressed as the dimensionless quantities specific gravity or relative density, in which case it is expressed in multiples of the density of some other standard material, usually water or air/gas. (For example, a specific gravity less than one means that the substance floats in water.)
The mass density of a material varies with temperature and pressure. (The variance is typically small for solids and liquids and much greater for gasses.) Increasing the pressure on an object decreases the volume of the object and therefore increase its density. Increasing the temperature of a substance (with some exceptions) decreases its density by increasing the volume of that substance. In most materials, heating the bottom of a fluid results in convection of the heat from bottom to top of the fluid due to the decrease of the density of the heated fluid. This causes it to rise relative to more dense unheated material.
The reciprocal of the density of a substance is called its specific volume, a representation commonly used in thermodynamics. Density is an intensive property in that increasing the amount of a substance does not increase its density; rather it increases its mass.
History
In a wellknown but probably apocryphal tale, Archimedes was given the task of determining whether King Hiero's goldsmith was embezzling gold during the manufacture of a golden wreath dedicated to the gods and replacing it with another, cheaper alloy.^{[2]} Archimedes knew that the irregularly shaped wreath could be crushed into a cube whose volume could be calculated easily and compared with the mass; but the king did not approve of this. Baffled, Archimedes took a relaxing immersion bath and observed from the rise of the water upon entering that he could calculate the volume of the gold wreath through the displacement of the water. Upon this discovery, he leaped from his bath and went running naked through the streets shouting, "Eureka! Eureka!" ( ! Greek "I found it"). As a result, the term "eureka" entered common parlance and is used today to indicate a moment of enlightenment.
The story first appeared in written form in Vitruvius' books of architecture, two centuries after it supposedly took place.^{[3]} Some scholars have doubted the accuracy of this tale, saying among other things that the method would have required precise measurements that would have been difficult to make at the time.^{[4]}^{[5]}
From the equation for density ( = m / V), mass density must have units of a unit of mass per unit of volume. As there are many units of mass and volume covering many different magnitudes there are a large number of units for mass density in use. The SI unit of kilogram per cubic metre (kg/m^{3}) and the cgs unit of gram per cubic centimetre (g/cm^{3}) are probably the most common used units for density. (The cubic centimeter can be alternately called a millilitre or a cc.) equals one g/cm^{3}. In industry, other larger or smaller units of mass and or volume are often more practical and US customary units may be used. See below for a list of some of the most common units of density. Further, density may be expressed in terms of weight density (the weight of the material per unit volume) or as a ratio of the density with the density of a common material such as air or water.
Measurement of density
The density at any point of a homogeneous object equals its total mass divided by its total volume. The mass is normally measured with an appropriate scale or balance; the volume may be measured directly (from the geometry of the object) or by the displacement of a fluid. For determining the density of a liquid or a gas, a hydrometer or dasymeter may be used, respectively. Similarly, hydrostatic weighing uses the displacement of water due to a submerged object to determine the density of the object.
If the body is not homogeneous, then the density is a function of the position. In that case the density around any given location is determined by calculating the density of a small volume around that location. In the limit of an infinitesimal volume the density of an inhomogeneous object at a point becomes: , where is an elementary volume at position . The mass of the body then can be expressed as
 m = \int_V \rho(\mathbf{r})\,dV.
The density of granular material can be ambiguous, depending on exactly how its volume is defined, and this may cause confusion in measurement. A common example is sand: if it is gently poured into a container, the density will be low; if the same sand is then compacted, it will occupy less volume and consequently exhibit a greater density. This is because sand, like all powders and granular solids, contains a lot of air space in between individual grains. The density of the material including the air spaces is the bulk density, which differs significantly from the density of an individual grain of sand with no air included.
Changes of density
In general, density can be changed by changing either the pressure or the temperature. Increasing the pressure always increases the density of a material. Increasing the temperature generally decreases the density, but there are notable exceptions to this generalization. For example, the density of water increases between its melting point at 0 C and 4 C; similar behavior is observed in silicon at low temperatures.
The effect of pressure and temperature on the densities of liquids and solids is small. The compressibility for a typical liquid or solid is 10 ^{6} bar ^{1} (1 bar = 0.1 MPa) and a typical thermal expansivity is 10 ^{5} K ^{1}. This roughly translates into needing around ten thousand times atmospheric pressure to reduce the volume of a substance by one percent. (Although the pressures needed may be around a thousand times smaller for sandy soil and some clays.) A one percent expansion of volume typically requires a temperature increase on the order of thousands of degrees Celsius.
In contrast, the density of gases is strongly affected by pressure. The density of an ideal gas is
 \rho = \frac {MP}{RT}, \,
where is the molar mass, is the pressure, is the universal gas constant, and is the absolute temperature. This means that the density of an ideal gas can be doubled by doubling the pressure, or by halving the absolute temperature.
In the case of volumic thermal expansion at constant pressure and small intervals of temperature the dependence of temperature of density is :
 \rho = \frac }
where \rho_{T_0} is the density at a reference temperature, \alpha is the thermal expansion coefficient of the material.
Density of water (at 1 atm)
Temp ( C) 
Density (kg/m^{3}) 
100 
958.4 
80 
971.8 
60 
983.2 
40 
992.2 
30 
995.6502 
25 
997.0479 
22 
997.7735 
20 
998.2071 
15 
999.1026 
10 
999.7026 
4 
999.9720 
0 
999.8395 
10 
998.117 
20 
993.547 
30 
983.854 
The values below 0 C refer to supercooled water. 
Density of air (at 1 atm)
Density vs. temperature
T ( C) 
(kg/m^{3}) 
25 
1.423 
20 
1.395 
15 
1.368 
10 
1.342 
5 
1.316 
0 
1.293 
5 
1.269 
10 
1.247 
15 
1.225 
20 
1.204 
25 
1.184 
30 
1.164 
35 
1.146 
Density of solutions
The density of a solution is the sum of mass (massic) concentrations of the components of that solution.
Mass (massic) concentration of each given component _{i} in a solution sums to density of the solution.
 \rho = \sum_i \varrho_i \,
Expressed as a function of the densities of pure components of the mixture and their volume participation, it reads:
 \rho = \sum_i \rho_i \frac{V_i}{V}.\,
Densities of various materials
Unless otherwise noted, all densities given are at standard conditions for temperature and pressure.
Material 
(kg/m^{3}) 
Notes 
Air 
1.2 
At sea level 
Aerographite 
0.2 

Metallic microlattice 
0.9 
* 
Aerogel 
1.0 
* 
Styrofoam 
75 
Approx.^{[8]}

liquid hydrogen 
70 
At ~ 255 C 
Cork 
240 
Approx.^{[8]}

Lithium 
535 

Potassium 
860 
^{[9]} 
Sodium 
970 

Ice 
916.7 
At temperature

Water (fresh) 
1,000 

Water (salt) 
1,030 
Plastics 
1,175 
Approx.; for polypropylene and PETE/PVC 
Tetrachloroethene 
1,622 
Magnesium 
1,740 

Beryllium 
1,850 

Glycerol 
1,261 
^{[10]} 
Silicon 
2,330 

Aluminium 
2,700 

Diiodomethane 
3,325 
liquid at room temperature 
Diamond 
3,500 

Titanium 
4,540 

Selenium 
4,800 

Vanadium 
6,100 

Antimony 
6,690 

Zinc 
7,000 

Chromium 
7,200 

Manganese 
7,325 
Approx. 
Tin 
7,310 

Iron 
7,870 

Niobium 
8,570 

Cadmium 
8,650 

Cobalt 
8,900 

Nickel 
8,900 

Copper 
8,940 

Bismuth 
9,750 

Molybdenum 
10,220 

Silver 
10,500 

Lead 
11,340 

Thorium 
11,700 

Rhodium 
12,410 

Mercury 
13,546 

Tantalum 
16,600 

Uranium 
18,800 

Tungsten 
19,300 

Gold 
19,320 

Plutonium 
19,840 

Platinum 
21,450 

Iridium 
22,420 

Osmium 
22,570 

 Air excluded when calculating density
Other densities
Entity 
(kg/m^{3}) 
Notes 
Interstellar medium 
10E20 
Assuming 90% H, 10% He; variable T 
The Earth 
5,515.3 
Mean density 
The Inner Core of the Earth 
13,000 
Approx.; as listed in Earth 
White dwarf star 
10E+8 
Approx.^{[11]}

Neutron star 
10E+17 
Atomic nuclei 
2.3E+17 
Does not depend strongly on size of nucleus^{[12]}

Black hole 
4E+17 
Mean density inside the Schwarzschild radius of an Earthmass black hole (theoretical) 
Other common units
The SI unit for density is:
 kilograms per cubic metre (kg/m^{3})
Litres and metric tons are not part of the SI, but are acceptable for use with it, leading to the following units:
 kilograms per litre (kg/L)
 grams per millilitre (g/mL)
 metric tons per cubic metre (t/m^{3})
Densities using the following metric units all have exactly the same numerical value, one thousandth of the value in (kg/m^{3}). Liquid water has a density of about 1 kg/dm^{3}, making any of these SI units numerically convenient to use as most solids and liquids have densities between 0.1 and 20 kg/dm^{3}.
 kilograms per cubic decimetre (kg/dm^{3})
 grams per cubic centimetre (g/cc, gm/cc or g/cm^{3})
 1 gram/cm^{3} = 1000 kg/m^{3}
 megagrams (metric tons) per cubic metre (Mg/m^{3})
In US customary units density can be stated in:
 Avoirdupois ounces per cubic inch (oz/cu in)
 Avoirdupois pounds per cubic inch (lb/cu in)
 pounds per cubic foot (lb/cu ft)
 pounds per cubic yard (lb/cu yd)
 pounds per US liquid gallon (lb/gal)
 pounds per US bushel (lb/bu)
 slugs per cubic foot
Imperial units differing from the above (as the Imperial gallon and bushel differ from the US units) in practice are rarely used, though found in older documents. The density of precious metals could conceivably be based on Troy ounces and pounds, a possible cause of confusion.
See also
 List of elements by density
 Charge density
 Buoyancy
 Bulk density
 Dord
 Energy density
 Lighter than air
 Number density
 Orthobaric density
 Specific weight
 Spice (oceanography)
 Standard temperature and pressure
 Orders of magnitude (density)
 Density prediction by the Girolami method
References
External links
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