Distribution law-Definition, explanation, and applications

Learning objectives

In this article, the author has explained the following topics

  • Distribution law
  • Distribution coefficient
  • Applications of distribution law
  • limitations of distribution law

Distribution law or partition law

At constant temperature, a solute distributes itself between two immiscible liquids in a constant ratio of concentration, independent of the amount of solute added.

Definition of distribution law

Two important techniques are totally based on the distribution law.

  • Solvent extraction
  • Partition chromatography

Distribution coefficient

At constant temperature, the ratio of the concentration of a substance in two immiscible liquids, present in equilibrium with each other, is called distribution co-efficient.

Definition of distribution coefficient

It is represented by K

If we talk about its mathematical expression then

Mathematical expression of distribution coefficient
Mathematical expression of distribution coefficient

In above equation the organic phase may be a organic solvent such as CCl4 and aqueous phase is water.

Also read: Experimental techniques in chemistry

Examples of distribution law or partition law

Distribution of iodine between CCl4 and water containing KI

Consider the distribution of I2 between two immiscible liquids, CCl4 and water in the presence of Potassium iodide KI.

Iodine is insoluble in water while KI is added into water.

In water, KI ionizes into ions

Ionization of KI
Ionization of KI

Iodine combines with iodide ion to form tri-iodide ion in a reversible reaction.

Formation of tri-iodide ion
Formation of tri-iodide ion

Thus iodine dissolves as I3 ion in water that is aqueous phase

Now if we add CCl4 to an aqueous solution that contains tri-iodide ion. As iodine is more soluble in CCl4 than in water therefore, it moves from aqueous layer to the CCl4 layer that is organic layer.

As a result, the brown color of tri-iodide ion in the aqueous layer fades while the purple color of free iodine appears in CCl4 layer.

This system of CCl4 and H2O is shaken to further increase the area of contact between the two layers. By doing so more and more iodine moves from the aqueous layer to the organic layer.

Distribution law or partition law
Distribution law or partition law

After repeating this process for some time, equilibrium is established between the two layers. At this point, the rate of movement of I2 from H2O to CCl4 becomes equal to the rate of movement of I2 from CCl4 to H2O.

Hence at equilibrium the ration of concentration of I2 in both layers will be constant at constant temperature. This constant is called distribution co-efficient and it is denoted by K.

Distribution co-efficient is represented as

equation for Distribution of coefficient
equation for Distribution of coefficient

Applications of distribution law or partition law

This law is helpful in many ways in industrial chemistry and physics.

  •  It is much helpful in the separation and purification of substances from mixtures such as solvent extraction. 
  • It is useful to determine the extent of hydrolysis
  • It also helps in the confirmation of the formula of the complexes such as CuSO4.4NH3
  • It  is used to find the equilibrium constant for the equilibrium
  • It is used to determine the solubility of the different solutes in a solvent
  • It is used for solvent removal purposes
  • It is also helpful in the separation of high act liquid chromatography
  • It is used to conserve the emulsions and creams
  • It helps in the formation of the solubilized structure
  • Used to determine the solubility of the different drugs in specific solvents

Limitations of distribution or partition law

Although it is very useful law, but also have some limitations

  • It is not functional in variable temperature condition
  • It does not describe the process of dissociation or association in different molecular state
  • The concentrations of the solute can only be noted when the equilibrium is established.

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