In chemistry, concentration is the abundance of a constituent divided by the total volume of a mixture. Several types of mathematical description can be distinguished: mass concentration, molar concentration, number concentration, and volume concentration.^{[1]} The concentration can refer to any kind of chemical mixture, but most frequently refers to solutes and solvents in solutions. The molar (amount) concentration has variants such as normal concentration and osmotic concentration.
The term concentration comes from the word concentrate, from the French concentrer, from con- + center, meaning "to put at the center".
Often in informal, non-technical language, concentration is described in a qualitative way, through the use of adjectives such as "dilute" for solutions of relatively low concentration and "concentrated" for solutions of relatively high concentration. To concentrate a solution, one must add more solute (for example, alcohol), or reduce the amount of solvent (for example, water). By contrast, to dilute a solution, one must add more solvent, or reduce the amount of solute. Unless two substances are miscible, there exists a concentration at which no further solute will dissolve in a solution. At this point, the solution is said to be saturated. If additional solute is added to a saturated solution, it will not dissolve, except in certain circumstances, when supersaturation may occur. Instead, phase separation will occur, leading to coexisting phases, either completely separated or mixed as a suspension. The point of saturation depends on many variables such as ambient temperature and the precise chemical nature of the solvent and solute.
Concentrations are often called levels, reflecting the mental schema of levels on the vertical axis of a graph, which can be high or low (for example, "high serum levels of bilirubin" are concentrations of bilirubin in the blood serum that are greater than normal).
There are four quantities that describe concentration:
The mass concentration is defined as the mass of a constituent divided by the volume of the mixture :
The SI unit is kg/m^{3} (equal to g/L).
The molar concentration is defined as the amount of a constituent (in moles) divided by the volume of the mixture :
The SI unit is mol/m^{3}. However, more commonly the unit mol/L (= mol/dm^{3}) is used.
The number concentration is defined as the number of entities of a constituent in a mixture divided by the volume of the mixture :
The SI unit is 1/m^{3}.
The volume concentration (not to be confused with volume fraction^{[2]}) is defined as the volume of a constituent divided by the volume of the mixture :
Being dimensionless, it is expressed as a number, e.g., 0.18 or 18%; its unit is 1.
There seems to be no standard notation in the English literature. The letter used here is normative in German literature (see Volumenkonzentration).
Several other quantities can be used to describe the composition of a mixture. Note that these should not be called concentrations.^{[1]}
Normality is defined as the molar concentration divided by an equivalence factor . Since the definition of the equivalence factor depends on context (which reaction is being studied), IUPAC and NIST discourage the use of normality.
(Not to be confused with Molarity)
The molality of a solution is defined as the amount of a constituent (in moles) divided by the mass of the solvent (not the mass of the solution):
The SI unit for molality is mol/kg.
The mole fraction is defined as the amount of a constituent (in moles) divided by the total amount of all constituents in a mixture :
The SI unit is mol/mol. However, the deprecated parts-per notation is often used to describe small mole fractions.
The mole ratio is defined as the amount of a constituent divided by the total amount of all other constituents in a mixture:
If is much smaller than , the mole ratio is almost identical to the mole fraction.
The SI unit is mol/mol. However, the deprecated parts-per notation is often used to describe small mole ratios.
The mass fraction is the fraction of one substance with mass to the mass of the total mixture , defined as:
The SI unit is kg/kg. However, the deprecated parts-per notation is often used to describe small mass fractions.
The mass ratio is defined as the mass of a constituent divided by the total mass of all other constituents in a mixture:
If is much smaller than , the mass ratio is almost identical to the mass fraction.
The SI unit is kg/kg. However, the deprecated parts-per notation is often used to describe small mass ratios.
Concentration depends on the variation of the volume of the solution with temperature due mainly to thermal expansion.
Concentration type | Symbol | Definition | SI unit | other unit(s) |
---|---|---|---|---|
mass concentration | or | kg/m^{3} | g/100mL (= g/dL) | |
molar concentration | mol/m^{3} | M (= mol/L) | ||
number concentration | 1/m^{3} | 1/cm^{3} | ||
volume concentration | m^{3}/m^{3} | |||
Related quantities | Symbol | Definition | SI unit | other unit(s) |
normality | mol/m^{3} | N (= mol/L) | ||
molality | mol/kg | |||
mole fraction | mol/mol | ppm, ppb, ppt | ||
mole ratio | mol/mol | ppm, ppb, ppt | ||
mass fraction | kg/kg | ppm, ppb, ppt | ||
mass ratio | kg/kg | ppm, ppb, ppt | ||
volume fraction | m^{3}/m^{3} | ppm, ppb, ppt |