Molar concentration
Common symbols
c, [chemical symbol or formula]
SI unitmol/m3
Other units
Derivations from
other quantities
c = n/V

Molar concentration (also called molarity, amount concentration or substance concentration) is a measure of the concentration of a chemical species, in particular, of a solute in a solution, in terms of amount of substance per unit volume of solution. In chemistry, the most commonly used unit for molarity is the number of moles per liter, having the unit symbol mol/L or mol/dm3 in SI units. A solution with a concentration of 1 mol/L is said to be 1 molar, commonly designated as 1 M or 1 M. Molarity is often depicted with square brackets around the substance of interest; for example, the molarity of the hydrogen ion is depicted as [H+].


Molar concentration or molarity is most commonly expressed in units of moles of solute per litre of solution.[1] For use in broader applications, it is defined as amount of substance of solute per unit volume of solution, or per unit volume available to the species, represented by lowercase :[2]

Here, is the amount of the solute in moles,[3] is the number of constituent particles present in volume (in litres) of the solution, and is the Avogadro constant, since 2019 defined as exactly 6.02214076×1023 mol−1. The ratio is the number density .

In thermodynamics the use of molar concentration is often not convenient because the volume of most solutions slightly depends on temperature due to thermal expansion. This problem is usually resolved by introducing temperature correction factors, or by using a temperature-independent measure of concentration such as molality.[3]

The reciprocal quantity represents the dilution (volume) which can appear in Ostwald's law of dilution.

Formality or analytical concentration

If a molecular entity dissociates in solution, the concentration refers to the original chemical formula in solution, the molar concentration is sometimes called formal concentration or formality (FA) or analytical concentration (cA). For example, if a sodium carbonate solution (Na2CO3) has a formal concentration of c(Na2CO3) = 1 mol/L, the molar concentrations are c(Na+) = 2 mol/L and c(CO2−3) = 1 mol/L because the salt dissociates into these ions.[4]


In the International System of Units (SI), the coherent unit for molar concentration is mol/m3. However, most chemical literature traditionally uses mol/dm3, which is the same as mol/L. This traditional unit is often called a molar and denoted by the letter M, for example:

1 mol/m3 = 10−3 mol/dm3 = 10−3 mol/L = 10−3 M = 1 mM = 1 mmol/L.

The SI prefix "mega" (symbol M) has the same symbol. However, the prefix is never used alone, so "M" unambiguously denotes molar. Sub-multiples, such as "millimolar" (mM) and "nanomolar" (nM), consist of the unit preceded by an SI prefix:

Name Abbreviation Concentration
(mol/L) (mol/m3)
millimolar mM 10−3 100=1
micromolar μM 10−6 10−3
nanomolar nM 10−9 10−6
picomolar pM 10−12 10−9
femtomolar fM 10−15 10−12
attomolar aM 10−18 10−15
zeptomolar zM 10−21 10−18
yoctomolar yM 10−24
(6 particles per 10 L)
rontomolar rM 10−27 10−24
quectomolar qM 10−30 10−27

Related quantities

Number concentration

The conversion to number concentration is given by

where is the Avogadro constant.

Mass concentration

The conversion to mass concentration is given by

where is the molar mass of constituent .

Mole fraction

The conversion to mole fraction is given by

where is the average molar mass of the solution, is the density of the solution.

A simpler relation can be obtained by considering the total molar concentration, namely, the sum of molar concentrations of all the components of the mixture:

Mass fraction

The conversion to mass fraction is given by


For binary mixtures, the conversion to molality is

where the solvent is substance 1, and the solute is substance 2.

For solutions with more than one solute, the conversion is


Sum of molar concentrations – normalizing relations

The sum of molar concentrations gives the total molar concentration, namely the density of the mixture divided by the molar mass of the mixture or by another name the reciprocal of the molar volume of the mixture. In an ionic solution, ionic strength is proportional to the sum of the molar concentration of salts.

Sum of products of molar concentrations and partial molar volumes

The sum of products between these quantities equals one:

Dependence on volume

The molar concentration depends on the variation of the volume of the solution due mainly to thermal expansion. On small intervals of temperature, the dependence is

where is the molar concentration at a reference temperature, is the thermal expansion coefficient of the mixture.


See also


  1. ^ Tro, Nivaldo J. (6 January 2014). Introductory chemistry essentials (Fifth ed.). Boston. p. 457. ISBN 9780321919052. OCLC 857356651.((cite book)): CS1 maint: location missing publisher (link)
  2. ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "amount concentration, c". doi:10.1351/goldbook.A00295
  3. ^ a b Kaufman, Myron (2002). Principles of thermodynamics. CRC Press. p. 213. ISBN 0-8247-0692-7.
  4. ^ Harvey, David (2020-06-15). "2.2: Concentration". Chemistry LibreTexts. Retrieved 2021-12-15.