The Colloidal State Preparation and Purification

A colloid is an intermediate state between true solution and suspension. In a true solution, the size of the particles is < 1nm. The particles do not settle down under the influence of gravity or by any method and they cannot be filtered by a filter paper.

Colloids are heterogeneous systems containing two phases – the dispersed phase and the dispersion medium.

Dispersed Phase: The phase which is dispersed in the other (medium) is called the Dispersed Phase or internal phase, or discontinuous phase.
Dispersion Medium: The phase or medium in which the dispersion is made is called dispersion medium or external phase or continuous phase.

Classification colloids
(i) Based on the physical state of the dispersed phase and the dispersion medium:
Depending upon the physical state of the dispersed phase and the dispersion medium, there are eight types of colloidal systems.

Dispersed Phase Dispersion medium Type of colloid Examples
Solid Solid Solid sol Some coloured glasses, gems stones
Solid Liquid Sol Paints, muddy water, cell fluids
Solid Gas Aerosol Smoke, dust
Liquid Solid Gel Cheese, butter, jellies
Liquid Liquid Emulsion Milk, hair cream
Liquid Gas Aerosol Fog, mist, cloud, insecticide sprays
Gas Solid Solid foam Pumice stone, foam rubber
Gas Liquid Foam Froth, whipped cream, soap lather

 

(ii) Based on the nature of the dispersion medium:

Dispersion medium Name of colloid (Sol)
Air Aerosol
Water Hydrosol
Alcohol Alcosol
Benzene Benzosol

Based on the attraction between the dispersed phase and the dispersion medium:

On the basis of the nature of the interaction of the dispersed phase and the dispersion medium colloids are of two types: lyophilic (solvent loving) and lyophobic (solvent hating). If the force of attraction between the dispersed phase and dispersion medium is strong, it is called lyophilic sol e.g. gum, gelatin, starch, rubber etc in a suitable dispersion medium.

If the force of attraction between the dispersed phase and dispersion medium is weak, it is called a lyophobic sol. e.g. Arsenic sulphide (As2S3) sol, Sulpher sol and metal sols like gold sol, silver sol etc.

Difference Between Lyophilic and Lyophobic Sols:

Properties Lyophilic sol Lyophobic sol
Force of attraction Strong Weak
  Preparation Can be easily prepared by mixing the dispersed phase with the dispersion medium Some special methods are used for the
Reversibility Reversible (i.e. they can be easily separated and remixed. Irreversible
Stability Self-Stabilized Less stable and requires some stabilizing agent
Coagulation a large amount of electrolyte is required for coagulation Only a small amount of electrolyte is required.

 

Based on Nature of Particles:
On this basis, the colloids are classified into three types namely Multimolecular colloids, Macromolecular colloids and Associated colloids.
Multimolecular colloids. They are formed by the aggregation of a large number of atoms or molecules which generally have a diameter less than 1nm, e.g., sols of gold, sulphur etc. Their atoms or molecules are held together by weak van der Waals forces and their molecular masses are not high.
Macromolecular colloids. They are molecules of large size, e.g., polymers like rubber, nylon, polythene, starch, cellulose, proteins, enzymes, etc. These substances when dissolved in a suitable liquid, directly from the colloidal solution. They have high molecular masses and have lyophobic character.
Associated colloids: The substances which when dissolved in a medium at low concentration behave as normal strong electrolytes but at higher concentration exhibit colloidal state properties due to the formation of aggregated particles are called associated colloids. The aggregated particles thus formed are called micelles.
Micelle formation takes place above a particular temperature called Kraft temperature (Tk) and above a particular concentration called Critical Micelle Concentration (CMC). These molecules contain both lyophilic and lyophobic groups.

Mechanism of micelle formation:
An example of the micelle is a soap solution. Soap is sodium or potassium salt of higher fatty acid and may be represented as RCOONa+. When dissolved in water, it dissociates into RCOO and Na+ ions. The RCOO ions consist of two parts – a long hydrocarbon chain R (also called non-polar ‘tail’) which is hydrophobic (water-repelling), and a polar group COO (also called polar-ionic ‘head’), which is hydrophilic (water-loving).
The RCOO ions are present on the surface with their COO groups in water and the hydrocarbon chains (R) at the surface. But at critical micelle concentration, the anions are pulled into the bulk of the solution and aggregate to form a spherical shape. Thus, a micelle is formed.

Cleansing Action of Soaps: The cleansing action of soap is due to micelle formation. The soap molecules form micelle around the oil droplet in such a way that hydrophobic part is in the oil droplet and hydrophilic part projects out. Since the polar groups (hydrophilic end) can interact with water, the oil droplets are pulled in water and removed from the dirty surface. Thus, soap helps in emulsification and washing away of oils and fats.

 The Colloidal State Preparation and Purification

Preparation of colloids:
Some of the methods used for the preparation of colloids are:
Preparation of lyophilic sols: Prepared by dissolving these substances (e.g. starch, gelatine, glue etc.) in water either in cold or warm. Solutions of colloidal electrolytes (e.g. soaps, dyes) are also prepared in a similar manner.

Preparation of lyophobic sols: To obtain a substance in the colloidal form either the substance in bulk is broken down into particles of colloidal dimension (1nm to 1000nm) or the size of molecular particles is increased to colloidal dimensions. In some cases, another substance is added to increase the stability of sol. Such substances are known as a stabilizer. Thus, there are two ways by which lyophobic sols can be prepared.

(i) Chemical methods: Colloidal solutions can be prepared by chemical reactions like oxidation, reduction, double decomposition, hydrolysis etc.

  • Oxidation: Sulphur sol can be prepared by passing H2S gas through an aqueous solution of sulphur dioxide. SO2 + 2H2S → 3S(sol) + 2H2
  • Reduction: Sols of metals like silver, gold and platinum are obtained by the reduction of their salts with reducing agents like formaldehyde, stannous chloride etc.

2AuCl3 + 3HCHO + 3H2O     →    2Au(sol) + 3HCOOH + 6HCl

  • Hydrolysis: Ferric hydroxide sol is obtained when the concentrated solution of ferric chloride is added drop-wise to hot water.

FeCl3 + 3H2O  →  Fe(OH)3 (sol) + 3HCl

  • Double Decomposition: A colloidal solution of arsenic sulphide is formed by passing H2S through a dilute solution of arsenious oxide in water.

As2O3 + 3H2S  →  As2S3(sol) + 3H2O

(ii) Electrical disintegration (Bredig’s arc method): This method is used for the preparation of metal sols like Ag, Au, Pt etc. The metal whose sol is to be prepared is taken in the form of two rods and it is kept in a suitable dispersion medium containing a small amount of electrolyte. The whole arrangement is kept in an ice bath. When high voltage is passed through the metal, the intense heat produced vapourises the metal, which then condensed to form particles of colloidal dimension.

(iii) Peptisation: It is the process of converting a freshly precipitated substance into colloidal particles by shaking with a suitable electrolyte, e.g., Fe(OH)3 ppt with FeCl3 solution, AgI ppt with AgNO3 or KI solution and Al(OH)3 ppt . with an insufficient quantity of very dil. HCl solution. During peptization, the precipitate adsorbs one of the ions of the electrolyte on its surface resulting in the development of positive or negative charge on the precipitate, which ultimately breaks into particles of colloidal dimensions.

The Colloidal State Preparation and Purification

Purification of Colloids:
The colloidal solution prepared contains an excess amount of electrolyte and some other soluble impurities. Even though a small amount of electrolyte is required for the stability of colloid, a large amount may cause precipitation. The process of reducing the concentration of electrolyte and other impurities is known as the purification of colloids. Some methods used for purification are:
(i) Dialysis: The process of removing the impurities from a sol by means of diffusion through a semi-permeable membrane is called dialysis.

(ii) Electrodialysis: When the dialysis process is accelerated by the application of a potential difference across the membrane, so ions migrate faster than the colloids.

(iii) Ultra-filtration: Purification of colloidal solution using special filter paper called ultrafilters (filter paper which is impregnated with gelatin or collodion followed by hardening in formaldehyde). Collodion is a 4% nitrocellulose soln in alcohol and ether.

 

The Colloidal State Preparation and Purification

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