Concentration

For other uses, see Concentration (disambiguation).

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 term concentration can be applied to any kind of chemical mixture, but most frequently it refers to solutes and solvents in solutions. The molar (amount) concentration has variants such as normal concentration and osmotic concentration.

Qualitative description

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 fully 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.

Quantitative notation

There are four quantities that describe concentration:

Mass concentration

Main article: Mass concentration (chemistry)

The mass concentration $\rho_i$ is defined as the mass of a constituent $m_i$ divided by the volume of the mixture $V$ :

\rho_i = \frac {m_i}{V}.

The SI unit is kg/m³ (equal to g/L).

Molar concentration

Main article: Molar concentration

The molar concentration $c_i$ is defined as the amount of a constituent $n_i$ (in moles) divided by the volume of the mixture $V$ :

c_i = \frac {n_i}{V}.

The SI unit is mol/m³. However, more commonly the unit mol/L (= mol/dm³) is used.

Number concentration

The number concentration $C_i$ is defined as the number of entities of a constituent $N_i$ in a mixture divided by the volume of the mixture $V$ :

C_i = \frac{N_i}{V}.

The SI unit is 1/m³.

Volume concentration

The volume concentration $\phi_i$ (do not confuse with volume fraction) is defined^[1] as the volume of a constituent $V_i$ divided by the volume of the mixture $V$ :

\phi_i = \frac {V_i}{V}.

Being dimensionless, it is expressed as a number, e.g., 0.18 or 18%; its unit is 1.

Related quantities

Several other quantities can be used to describe the composition of a mixture. Note that these should not be called concentrations.^[1]

Normality

Normality is defined as the molar concentration $c_i$ divided by an equivalence factor $f_\mathrm{eq}$ . Since the definition of the equivalence factor depends on context (which reaction is being studied), IUPAC and NIST discourage the use of normality.

Molality

Main article: Molality

(Not to be confused with Molarity)

The molality of a solution $b_i$ is defined as the amount of a constituent $n_i$ (in moles) divided by the mass of the solvent $m_\mathrm{solvent}$ (not the mass of the solution):

b_i = \frac{n_i}{m_\mathrm{solvent}}.

The SI unit for molality is mol/kg.

Mole fraction

Main article: Mole fraction

The mole fraction $x_i$ is defined as the amount of a constituent $n_i$ (in moles) divided by the total amount of all constituents in a mixture $n_\mathrm{tot}$ :

x_i = \frac {n_i}{n_\mathrm{tot}}.

The SI unit is mol/mol. However, the deprecated parts-per notation is often used to describe small mole fractions.

Mole ratio

Main article: Mixing ratio

The mole ratio $r_i$ is defined as the amount of a constituent $n_i$ divided by the total amount of all other constituents in a mixture:

r_i = \frac{n_i}{n_\mathrm{tot}-n_i}.

If $n_i$ is much smaller than $n_\mathrm{tot}$ , 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.

Mass fraction

Main article: Mass fraction (chemistry)

The mass fraction $w_i$ is the fraction of one substance with mass $m_i$ to the mass of the total mixture $m_\mathrm{tot}$ , defined as:

w_i = \frac {m_i}{m_\mathrm{tot}}.

The SI unit is kg/kg. However, the deprecated parts-per notation is often used to describe small mass fractions.

Mass ratio

Main article: Mixing ratio

The mass ratio $\zeta_i$ is defined as the mass of a constituent $m_i$ divided by the total mass of all other constituents in a mixture:

\zeta_i = \frac{m_i}{m_\mathrm{tot}-m_i}.

If $m_i$ is much smaller than $m_\mathrm{tot}$ , 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.

Dependence on volume

Concentration depends on the variation of the volume of the solution due mainly to thermal expansion.

Table of concentrations and related quantities

Concentration type	Symbol	Definition	SI unit	other unit(s)
mass concentration	$\rho_i$ or $\gamma_i$	$m_i/V$	kg/m³	g/100mL (= g/dL)
molar concentration	$c_i$	$n_i/V$	mol/m³	M (= mol/L)
number concentration	$C_i$	$N_i/V$	1/m³	1/cm³
volume concentration	$\phi_i$	$V_i/V$	m³/m³
Related quantities	Symbol	Definition	SI unit	other unit(s)
normality		$c_i/f_\mathrm{eq}$	mol/m³	N (= mol/L)
molality	$b_i$	$n_i/m_\mathrm{solvent}$	mol/kg
mole fraction	$x_i$	$n_i/n_\mathrm{tot}$	mol/mol	ppm, ppb, ppt
mole ratio	$r_i$	$n_i/(n_\mathrm{tot}-n_i)$	mol/mol	ppm, ppb, ppt
mass fraction	$w_i$	$m_i/m_\mathrm{tot}$	kg/kg	ppm, ppb, ppt
mass ratio	$\zeta_i$	$m_i/(m_\mathrm{tot}-m_i)$	kg/kg	ppm, ppb, ppt

References

↑ 1.0 1.1 1.2 IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "concentration".

Articles related to solutions

Solution	Ideal solution Aqueous solution Solid solution Buffer solution Flory–Huggins Mixture Suspension Colloid Phase diagram Eutectic point Alloy Saturation Supersaturation Serial dilution Dilution (equation) Apparent molar property Miscibility gap

Concentration and related quantities	Molar concentration Mass concentration Number concentration Volume concentration Normality Percentage solution Molality Mole fraction Mass fraction Isotopic abundance Mixing ratio

Solubility	Solubility equilibrium Total dissolved solids Solvation Solvation shell Enthalpy of solution Lattice energy Raoult's law Henry's law Solubility table (data) Solubility chart

Solvent	(Category) Acid dissociation constant Protic solvent Inorganic nonaqueous solvent Solvation List of boiling and freezing information of solvents Partition coefficient Polarity Hydrophobe Hydrophile Lipophilic Amphiphile