Molar concentration

Molar concentration
Common symbols
c
SI unitmol/m3
Other units
mol/L
Derivations from
other quantities
c = n/V
Dimension${\displaystyle {\mathsf {L}}^{-3}{\mathsf {N}}}$

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 unit. A solution with a concentration of 1 mol/L is said to be 1 molar, commonly designated as 1 M.

Definition

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 ${\displaystyle c}$:[2]

${\displaystyle c={\frac {n}{V}}={\frac {N}{N_{\text{A}}\,V}}={\frac {C}{N_{\text{A}}}}.}$

Here, ${\displaystyle n}$ is the amount of the solute in moles,[3] ${\displaystyle N}$ is the number of constituent particles present in volume ${\displaystyle V}$ (in litres) of the solution, and ${\displaystyle N_{\text{A}}}$ is the Avogadro constant, since 2019 defined as exactly 6.02214076×1023 mol−1. The ratio ${\displaystyle {\frac {N}{V}}}$ is the number density ${\displaystyle C}$.

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]

Units

In the International System of Units (SI) the coherent unit for molar concentration is mol/m3. However, this is inconvenient for most laboratory purposes and 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:

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

To avoid confusion with SI prefix mega, which has the same abbreviation, small caps or italicized M are also used in journals and textbooks.[5]

Sub-multiples such as millimolar 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[6] 10−24
(6 particles per 10 L)
10−21

Related quantities

Number concentration

The conversion to number concentration ${\displaystyle C_{i}}$ is given by

${\displaystyle C_{i}=c_{i}N_{\text{A}},}$

where ${\displaystyle N_{\text{A}}}$ is the Avogadro constant.

Mass concentration

The conversion to mass concentration ${\displaystyle \rho _{i}}$ is given by

${\displaystyle \rho _{i}=c_{i}M_{i},}$

where ${\displaystyle M_{i}}$ is the molar mass of constituent ${\displaystyle i}$.

Mole fraction

The conversion to mole fraction ${\displaystyle x_{i}}$ is given by

${\displaystyle x_{i}=c_{i}{\frac {\overline {M}}{\rho }},}$

where ${\displaystyle {\overline {M}}}$ is the average molar mass of the solution, ${\displaystyle \rho }$ 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:

${\displaystyle x_{i}={\frac {c_{i}}{c}}={\frac {c_{i}}{\sum _{j}c_{j}}}.}$

Mass fraction

The conversion to mass fraction ${\displaystyle w_{i}}$ is given by

${\displaystyle w_{i}=c_{i}{\frac {M_{i}}{\rho }}.}$

Molality

For binary mixtures, the conversion to molality ${\displaystyle b_{2}}$ is

${\displaystyle b_{2}={\frac {c_{2}}{\rho -c_{1}M_{1}}},}$

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

For solutions with more than one solute, the conversion is

${\displaystyle b_{i}={\frac {c_{i}}{\rho -\sum _{j\neq i}c_{j}M_{j}}}.}$

Properties

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:

${\displaystyle \sum _{i}c_{i}{\overline {V_{i}}}=1.}$

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

${\displaystyle c_{i}={\frac {c_{i,T_{0}}}{1+\alpha \Delta T}},}$

where ${\displaystyle c_{i,T_{0}}}$ is the molar concentration at a reference temperature, ${\displaystyle \alpha }$ is the thermal expansion coefficient of the mixture.

Examples

• 11.6 g of NaCl is dissolved in 100 g of water. The final mass concentration ρ(NaCl) is
ρ(NaCl) = 11.6 g/11.6 g + 100 g = 0.104 g/g = 10.4 %.

The density of such a solution is 1.07 g/mL, thus its volume is

V = 11.6 g + 100 g/1.07 g/mL = 104.3 mL.

The molar concentration of NaCl in the solution is therefore

c(NaCl) = 11.6 g/58 g/mol / 104.3 mL = 0.00192 mol/mL = 1.92 mol/L.
Here, 58 g/mol is the molar mass of NaCl.
• A typical task in chemistry is the preparation of 100 mL (= 0.1 L) of a 2 mol/L solution of NaCl in water. The mass of salt needed is
m(NaCl) = 2 mol/L × 0.1 L × 58 g/mol = 11.6 g.
To create the solution, 11.6 g NaCl is placed in a volumetric flask, dissolved in some water, then followed by the addition of more water until the total volume reaches 100 mL.
• The density of water is approximately 1000 g/L and its molar mass is 18.02 g/mol (or 1/18.02 = 0.055 mol/g). Therefore, the molar concentration of water is
c(H2O) = 1000 g/L/18.02 g/mol ≈ 55.5 mol/L.
Likewise, the concentration of solid hydrogen (molar mass = 2.02 g/mol) is
c(H2) = 88 g/L/2.02 g/mol = 43.7 mol/L.
The concentration of pure osmium tetroxide (molar mass = 254.23 g/mol) is
c(OsO4) = 5.1 kg/L/254.23 g/mol = 20.1 mol/L.
• A typical protein in bacteria, such as E. coli, may have about 60 copies, and the volume of a bacterium is about 10−15 L. Thus, the number concentration C is
C = 60 / (10−15 L) = 6×1016 L−1.
The molar concentration is
c = C/NA = 6×1016 L−1/6×1023 mol−1 = 10−7 mol/L = 100 nmol/L.
• Reference ranges for blood tests, sorted by molar concentration: