Amount of substance concentration
|Surname||Amount of substance concentration|
|Usual unit: 1 mol / l = 1 mol / dm 3 = 1000 mol / m 3|
The molar concentration ( symbol : c ), outdated also known as molarity , is a so-called content quantity according to DIN 1310 , i.e. a physical-chemical quantity for the quantitative description of the composition of substance mixtures / mixed phases (e.g. solutions ). Here the amount of substance of a considered mixture component is related to the total volume of the mixed phase .
Definition and characteristics
As an alternative to the index notation used here, a notation is also used in which the mixture component i considered is placed in brackets after the symbol c , using the example of sulfuric acid : c (H 2 SO 4 ). A notation that used to be common in the past consisted in putting the mixture component under consideration in square brackets: [H 2 SO 4 ].
The " particles " i on which the concept of the amount of substance is based must be specified; they can be material elementary objects such as atoms , molecules , ions or formula units . Here it is often assumed that the mixture component i considered is present exclusively in the form of these particles. B. an equilibrium concentration established in a solution by dissociation or reaction with the solvent , unless this is explicitly considered. In addition to specifying the species i, a complete specification of the molar concentration also includes the specification of the temperature and possibly the pressure (see below), in the case of solutions also the solvent (if no solvent is specified in the case of solutions, it is usually an aqueous solution ).
V is the actual total volume of the mixing phase after the mixing process, see the explanations under volume concentration .
If the mixture of substances is not homogeneous , the above definition only provides an average concentration of the substance amount; deviating values can then occur in partial volumes of the mixture of substances.
The derived SI unit of the molar concentration is mol / m 3 , in practice the unit mol / l (= mol / dm 3 ) is common, if necessary the molar unit part is also combined with decimal prefixes ( e.g. mmol / l ).
If the mixture component i is not present in the substance mixture (i.e. if n i = 0 mol), the minimum value c i = 0 mol / m 3 results . If component i is present as an unmixed pure substance , a molar concentration c i can also be specified for this , see the example below for water.
The total amount of substance concentration of the substance mixture is obtained by adding up the substance concentrations of all individual mixture components.
The DIN 1310 standard does not recommend shortening the term “substance concentration” for size c to the word “concentration” . Nor should the designations of the other concentration quantities mass concentration β , particle number concentration C and volume concentration σ be shortened to the word concentration.
The terms “molarity” (not to be confused with the independent content quantity molality !), “Molar concentration” or “molar concentration” for the substance concentration and the term “molar” or the symbol “ᴍ” (to be distinguished from the symbol M for the SI -Decimal prefix "Mega" and the symbol M for the molar mass !) For the unit mol / l do not conform to the standard, but are still frequently used. "Molar" should be avoided in this context because, on the one hand, an adjective as a unit designation falls outside the scope of the SI and, on the other hand, according to the general rule, a molar quantity is a quantity related to the amount of substance , i.e. a size quotient in which the quantity of substance is Denominator is (for example molar mass, molar volume , molar enthalpy of reaction , molar heat capacity ). In the case of the amount of substance concentration, however, the amount of substance is in the numerator, rather it is a volume-related quantity. Instead of obsolete forms of representation such as B. in the case of hydrochloric acid ( aqueous solution of hydrogen chloride HCl) the spelling "2.5 molar hydrochloric acid" or "2.5 ᴍ HCl" should indicate the molar concentration using an equation such as "hydrochloric acid, c HCl = 2.5 mol / l "or using a corresponding short form such as" HCl, 2.5 mol / l ".
Temperature and pressure dependency
The substance concentrations for a substance mixture of a given composition are - like all volume-related quantities ( concentrations , volume fraction , volume ratio ) - dependent on the temperature , in the case of gas mixtures also on the pressure (in the case of liquid and solid mixed phases, the pressure dependence can generally be neglected), so that a clear one Therefore, the specification of the associated temperature (possibly also the pressure) should be included. As a rule, an increase in temperature causes an increase in the total volume V of the mixed phase ( thermal expansion ), which leads to a reduction in the molar concentrations of the mixture components if the amounts of substance remain the same. Conversely, cooling usually causes a volume contraction of the mixed phase and thus an increase in the molar concentrations of the mixture components.
Since the change from room temperature to refrigerator temperature or vice versa can falsify the molar concentration of a solution, the temperature influence on the molar concentration should be taken into account in laboratory practice, as the effect is not negligible with regard to the desired accuracy. The extent depends on the one hand on the size of the temperature difference to be considered and on the other hand on the size of the spatial expansion coefficient γ of the mixed phase (the latter is significantly greater with solvents such as acetone , ethanol or methanol than with water ). An exact correction calculation for the temperature dependency of the substance concentration is usually not carried out, since the spatial expansion coefficient γ of the mixed phase with its own temperature dependency must be known exactly. However, a rough estimate can e.g. B. for dilute solutions and not too great differences between reference temperature T 1 and comparison temperature T 2 can be carried out as follows (use of the temperature-independent coefficient of expansion γ of the solvent):
From this it follows, for example, that when a dilute solution of the substance i cools down from 30 ° C to 10 ° C, its molar concentration c i is only about 0.5% for the solvent water or about 2-3% for the solvents acetone, Ethanol or methanol increases. By maintaining a constant temperature when working with solutions, the problem can be avoided in the first place. If this cannot be guaranteed, if there are high demands on accuracy, mass-related content values such as B. the specific partial substance amount can be avoided.
For mixtures of ideal gases it can be derived from the general gas equation that the molar concentration c i of a mixture component i is proportional to its partial pressure p i and inversely proportional to the absolute temperature T ( R = universal gas constant ):
Relationships with other salary levels
The following table shows the relationships between the molar concentration c i and the other content values defined in DIN 1310 in the form of size equations . The formula symbols M and ρ provided with an index stand for the molar mass or density (at the same pressure and temperature as in the substance mixture) of the respective pure substance identified by the index . The symbol ρ without an index represents the density of the mixed phase. The index z serves as a general index for the sums (consideration of a general mixture of substances from a total of Z components) and includes i . N A is Avogadro's constant ( N A ≈ 6.022 · 10 23 mol −1 ).
|Masses - ...||Amount of substance - ...||Particle number - ...||Volume - ...|
|... - share||Mass fraction w||Amount of substance fraction x||Particle number fraction X||Volume fraction φ|
|… - concentration||Mass concentration β||Molar concentration c||Particle number concentration C||Volume concentration σ|
|... - ratio||Mass ratio ζ||Molar ratio r||Particle number ratio R||Volume ratio ψ|
amount of substance / mass
|specific amount of partial substances q|
In the table above in the equations in the mole fraction x and Teilchenzahlanteil X occurring denominator - Terme are equal to the average molar mass of the material mixture and can be replaced in accordance with:
Dilute sulfuric acid
Given is a dilute aqueous solution of sulfuric acid H 2 SO 4 at 20 ° C. which, in a volume V of 3 liters, contains a mass m of pure sulfuric acid of 235.392 grams. From this information, the mass concentration β of the sulfuric acid can first be calculated:
With the help of the molar mass M of sulfuric acid (98.08 g / mol), it follows that the solution has a molar concentration of H 2 SO 4 of 0.8 mol / l (non-standard specification: “0.8 molar (0 , 8 ᴍ) aqueous sulfuric acid solution "):
Cane sugar solution
A dilute aqueous solution of cane sugar ( sucrose C 12 H 22 O 11 ) at 20 ° C. with a particle number N of sucrose molecules of 3.6132 · 10 18 in a solution volume V of 2 cubic centimeters (milliliters) is given. From this information, the particle number concentration C of the sucrose can first be calculated:
Using Avogadro's constant N A , it follows that the solution has a molar concentration of sucrose of 0.003 mol / l (non-standard specification: "3 millimolar (3 mᴍ) aqueous sucrose solution"):
A substance concentration c can also be assigned to a pure substance such as pure water H 2 O. Since the mass fraction w in this case is 1 = 100%, with the known density ρ of water at 20 ° C and the molar mass M of water (18.015 g / mol) for the molar concentration c of water at 20 ° C:
- Standard DIN 1310 : Composition of mixed phases (gas mixtures, solutions, mixed crystals); Terms, symbols. February 1984. p. 2, sections 3 and 7.
- Standard DIN 32625: sizes and units in chemistry; Amount of substance and quantities derived from it; Terms and definitions. December 1989 (withdrawn without replacement by the German Institute for Standardization in April 2006, because no need for this standard was assumed due to a lack of further cooperation and feedback from industry, science, research and other circles).
- Standard DIN EN ISO 80000-9 : Sizes and units. Part 9: Physical Chemistry and Molecular Physics. August 2013. Section 3: Terms, symbols and definitions. Table entry No. 9-13; Section 0.5: Special Notes.
- P. Kurzweil: The Vieweg unit lexicon: terms, formulas and constants from natural sciences, technology and medicine . 2nd Edition. Springer Vieweg, 2013, ISBN 978-3-322-83212-2 , p. 68, 224, 225, 253, 280, 281, 377 , doi : 10.1007 / 978-3-322-83211-5 ( limited preview in the Google book search - softcover reprint of the 2nd edition 2000). - ( Lexical part PDF; 71.3 MB).
- G. Jander, KF Jahr, R. Martens-Menzel, G. Schulze, J. Simon: Measure analysis: theory and practice of titrations with chemical and physical indications . 18th edition. De Gruyter, Berlin / Boston 2012, ISBN 978-3-11-024898-2 , pp. 54 ff ., doi : 10.1515 / 9783110248999 ( limited preview in Google Book Search).
- entry on amount concentration . In: IUPAC Compendium of Chemical Terminology (the “Gold Book”) . doi : 10.1351 / goldbook.A00295 Version: 2.3.3.
- ER Cohen, T. Cvitas, JG Frey, B. Holmström, K. Kuchitsu, R. Marquardt, I. Mills, F. Pavese, M. Quack, J. Stohner, HL Strauss, M. Takami, AJ Thor: Quantities, Units and Symbols in Physical Chemistry ( IUPAC Green Book) . second corrected print 2008. 3rd edition. IUPAC & RSC Publishing, Cambridge 2007, ISBN 978-0-85404-433-7 , pp. 6, 48 ( iupac.org [PDF; 2.5 MB ; accessed on August 3, 2015]). iupac.org ( Memento of the original dated February 11, 2014 in the Internet Archive ) Info: The archive link was inserted automatically and has not yet been checked. Please check the original and archive link according to the instructions and then remove this notice. or as a limited preview in Google Book Search.