Not to be confused with Adsorption.
Laboratory absorber. 1a): CO2 inlet; 1b): H2O inlet; 2): outlet; 3): absorption column; 4): packing.

In chemistry, absorption is a physical or chemical phenomenon or a process in which atoms, molecules or ions enter some bulk phase – gas, liquid or solid material. This is a different process from adsorption, since molecules undergoing absorption are taken up by the volume, not by the surface (as in the case for adsorption). A more general term is sorption, which covers absorption, adsorption, and ion exchange. Absorption is a condition in which something takes in another substance.[1]

In many processes important in technology, the chemical absorption is used in place of the physical process, e.g., absorption of carbon dioxide by sodium hydroxide – such acid-base processes do not follow the Nernst partition law.

For some examples of this effect, see liquid-liquid extraction. It is possible to extract from one liquid phase to another a solute without a chemical reaction. Examples of such solutes are noble gases and osmium tetroxide.[1]

The process of absorption means that a substance captures and transforms energy. The absorbent distributes the material it captures throughout whole and adsorbent only distributes it through the surface.

Contents

EquationEdit

If absorption is a physical process not accompanied by any other physical or chemical process, it usually follows the Nernst distribution law:

"the ratio of concentrations of some solute species in two bulk phases when it is equilibrium and in contact is constant for a given solute and bulk phases":
 

The value of constant KN depends on temperature and is called partition coefficient. This equation is valid if concentrations are not too large and if the species "x" does not change its form in any of the two phases "1" or "2". If such molecule undergoes association or dissociation then this equation still describes the equilibrium between "x" in both phases, but only for the same form – concentrations of all remaining forms must be calculated by taking into account all the other equilibria.[1]

In the case of gas absorption, one may calculate its concentration by using, e.g., the Ideal gas law, c = p/RT. In alternative fashion, one may use partial pressures instead of concentrations.

Types of absorptionEdit

Absorption is a process that may be chemical (reactive) or physical (non-reactive).

Chemical absorptionEdit

Chemical absorption or reactive absorption is a chemical reaction between the absorbed and the absorbing substances. Sometimes it combines with physical absorption. This type of absorption depends upon the stoichiometry of the reaction and the concentration of its reactants.[2]

ReferencesEdit

  1. ^ a b c McMurry, John (2003). Fundamentals of Organic Chemistry (Fifth ed.). Agnus McDonald. p. 409. ISBN 0-534-39573-2. 
  2. ^ Leiviskä, Tiina; Gehör, Seppo; Eijärvi, Erkki; Sarpola, Arja; Tanskanen, Juha (10 April 2012). "Characteristics and potential applications of coarse clay fractions from Puolanka, Finland". Central European Journal of Engineering. 2 (2): 239–247. doi:10.2478/s13531-011-0067-9.