Apparent molar property

An apparent molar property of a solution component is the change in the corresponding solution property (for example, volume) when all of that component is added to the solution, per mole of component added. It is described as apparent because it appears to represent the molar property of that component in solution, provided that the properties of the other solution components are assumed to remain constant during the addition. However this assumption is often not justified, since the values of apparent molar properties of a component may be quite different from its molar properties in the pure state.

For instance, the volume of a solution containing two components identified^[1] as solvent and solute is given by

V=V_0 + {}^\phi{V}_1 \ =\tilde{V}_{0} n_{0} + {}^\phi\tilde{V}_1 n_1 \,

where V₀ is the volume of the pure solvent before adding the solute and $\tilde{V}_{0}$ its molar volume (at the same temperature and pressure as the solution), n₀ is the number of moles of solvent, ${}^\phi\tilde{V}_1\,$ is the apparent molar volume of the solute, and n₁ is the number of moles of the solute in the solution.

This equation serves as the definition of ${}^\phi\tilde{V}_1\,$ . The first term is equal to the volume of the same quantity of solvent with no solute, and the second term is the change of volume on addition of the solute. ${}^\phi\tilde{V}_1\,$ may then be considered as the molar volume of the solute if it is assumed that the molar volume of the solvent is unchanged by the addition of solute. However this assumption must often be considered unrealistic as shown in the Examples below, so that ${}^\phi\tilde{V}_1\,$ is described only as an apparent value.

An apparent molar quantity can be similarly defined for the component identified as solvent ${}^\phi\tilde{V}_0\,$ . Some authors have reported apparent molar volumes of both components of the same solution.^[2]^[3]

Apparent quantities can also be expressed using mass instead of number of moles. This expression produces apparent specific quantities, like the apparent specific volume.

V=V_0 + {}^\phi{V}_1 \ =v_0 m_0 + {}^\phi{v}_1 m_1 \,

where the specific quantities are denoted with small letters.

Apparent (molar) properties are not constants (even at a given temperature), but are functions of the composition. At infinite dilution, an apparent molar property and the corresponding partial molar property become equal.

Some apparent molar properties that are commonly used are apparent molar enthalpy, apparent molar heat capacity, and apparent molar volume.

Relation to molality

The apparent (molar) volume of a solute can be expressed as a function of the molality b of that solute (and of the densities of the solution and solvent). The volume of solution per mole of solute is

\frac{1}{\rho}\left( \frac{1}{b}+M_1\right).

Subtracting the volume of pure solvent per mole of solute gives the apparent molar volume:

{}^\phi\tilde{V}_1 = \frac{1}{b}\left( \frac{1}{\rho} - \frac{1}{\rho_0^0}\right) + \frac{M_1}{\rho}

Relation to partial (molar) quantities

The relation between partial molar properties and the apparent ones can be derived from the definition of the apparent quantities and of the molality.

\bar{V_1}={}^\phi\tilde{V}_1 + b \frac{\partial {}^\phi\tilde{V}_1}{\partial b}.

Multicomponent mixtures/solutions

For multicomponent solutions, there is no unambiguous definition of apparent molar properties. With two solutes for example, there is still only one equation $(V=\tilde{V}_{0} n_{0} + {}^\phi\tilde{V}_1 n_1+ {}^\phi\tilde{V}_2 n_2)$ , which is insufficient to determine the two apparent volumes. (This is in contrast to partial molar properties, which are intrinsic properties of the materials and therefore unambiguously defined in multicomponent systems.)

There are situations when there is no rigorous way to define which is solvent and which is solute like in the case of liquid mixtures (say water and ethanol) that can dissolve or not a solid like sugar or salt. In these cases apparent molar properties can and must be ascribed to all components of the mixture.

Examples

Electrolytes

The apparent molar volume of a salt is usually less than the molar volume of the solid salt. For instance, solid NaCl has a volume of 27 cm³ per mole, but the apparent molar volume at low concentrations is only 16.6 cc/mole. In fact, some aqueous electrolytes have negative apparent molar volumes: NaOH -6.7, LiOH -6.0, and Na₂CO₃ -6.7 cm³/mole.^[4] This means that their solutions in a given amount of water have a smaller volume than the same amount of pure water. (The effect is small however.) The physical reason is that nearby water molecules are strongly attracted to the ions so that they occupy less space.

Alcohol

Excess volume of a mixture of ethanol and water

Another example of the apparent molar volume of the second component being less than its molar volume as a pure substance is the case of ethanol in water. For example, at 20 mass-percent ethanol, the solution has a volume of 1.0326 litres per kg at 20 °C, while pure water is 1.0018 L/kg (1.0018 cc/g).^[5] The apparent volume of the added ethanol is 1.0326 L - 0.8 kg x 1.0018 L/kg = 0.2317 L. The number of moles of ethanol is 0.2 kg / (0.04607 kg/mol) = 4.341 mol, so that the apparent molar volume is 0.2317 L / 4.341 mol = 0.0532 L / mol = 53.2 cc/mole (1.16 cc/g). However pure ethanol has a molar volume at this temperature of 58.4 cc/mole (1.27 cc/g). The nonideality of the solution is reflected by a slight decrease (roughly 2.2%, 1.0326 rather than 1.055 L/kg) in the volume of the combined system upon mixing. As the percent ethanol goes up toward 100%, the apparent molar volume rises to the molar volume of pure ethanol.

Electrolyte - non-electrolyte systems

Apparent quantities can underline interactions in electrolyte - non-electrolyte systems which show interactions like salting in and salting out.

References

↑ This labelling is arbitrary. For mixtures of two liquids either may be described as solvent. For mixtures of a liquid and a solid, the liquid is usually identified as the solvent and the solid as the solute, but the theory is still valid if the labels are reversed.
↑ Rock, Peter A., Chemical Thermodynamics, MacMillan 1969, p.227-230 for water-ethanol mixtures.
↑ H. H. Ghazoyan and Sh. A. Markarian (2014) DENSITIES, EXCESS MOLAR AND PARTIAL MOLAR VOLUMES FOR DIETHYLSULFOXIDE WITH METHANOL OR ETHANOL BINARY SYSTEMS AT TEMPERATURE RANGE 298.15 – 323.15 K PROCEEDINGS OF THE YEREVAN STATE UNIVERSITY no.2, p.17-25. See Table 4.
↑ Herbert Harned and Benton Owen, The Physical Chemistry of Electrolytic Solutions, 1950, p. 253.
↑ Calculated from data in the CRC Handbook of Chemistry and Physics, 49th edition.

External links

This article is issued from Wikipedia - version of the Friday, March 18, 2016. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.