Colloids 130605050740-phpapp02
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This document discusses colloids, including their definition and classification. Colloids can be classified into different types of mixtures including sols, foams, emulsions, and gels. Sols are solid particles dispersed in a liquid, foams contain gas pockets in a liquid or solid, emulsions involve two immiscible liquids, and gels contain molecules of a liquid dispersed within a solid matrix. The document also provides examples of each type of colloidal mixture and discusses reversible versus irreversible colloid formation.
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Colloids presentation slides
Colloids are substances microscopically dispersed throughout another substance. The dispersed particles range in size from 1-100 nm. Colloids exhibit properties between true solutions and suspensions due to their intermediate particle size. They are able to pass through filters but not semipermeable membranes. Common examples include milk, fog, mayonnaise and paints. Colloids can be classified based on factors like the physical state of the phases, the interaction between the phases, the size and nature of dispersed particles, and the electrical charge on particles. They are purified using techniques like dialysis, electrodialysis, and ultrafiltration which separate colloidal particles from dissolved substances.
Colloids and surface chemistry
This document defines and classifies colloids. Colloids have particle sizes between 1-1000 nm, which are larger than true solutions and smaller than suspensions. Colloids are classified based on the physical state of the dispersed and dispersion medium (solid-liquid, liquid-liquid, etc.), interaction between the phases (lyophobic or lyophilic), and particle type (multimolecular, macromolecular, associated). Common colloids include emulsions, gels, sols, and foams. Properties include the Tyndall effect, Brownian motion, and coagulation with electrolytes. Colloids find applications in products like rubber, soaps, and medicines.
Colloids part 1 general introduction
The document discusses colloids and their classification. It defines colloids as substances that are microscopically dispersed through another substance, with particle sizes between 10-10000 Angstroms. Colloids are classified in several ways, including by particle size (molecular dispersion, colloidal dispersion, coarse dispersion), physical state of phases, type of dispersed particles (multimolecular, macromolecular), appearance (sols, gels), and electrical charge on particles (positive, negative). Common colloidal systems include sols, emulsions, foams and aerosols. Micelle formation in colloids and the critical micelle concentration are also explained.
Colloids
Colloids have particle sizes between 1 nm and 1000 nm. They are classified as lyophilic, lyophobic, or association colloids based on particle interactions with the dispersion medium. Lyophilic colloids readily disperse in the medium while lyophobic colloids do not. Association colloids form micelles above a critical micelle concentration. Colloids demonstrate optical properties like Tyndall effect and can be imaged with electron microscopes. They also exhibit kinetic properties including Brownian motion, diffusion, osmotic pressure, and sedimentation. Colloidal particles are often electrically charged, leading to electrokinetic phenomena like electrophoresis and electroosmosis. Stability is important for preventing
Colloidal state
Colloids are heterogeneous mixtures where small insoluble particles are dispersed throughout a liquid medium. Thomas Graham first classified substances as either crystalloids or colloids based on their ability to pass through a membrane. A colloid has particle sizes between 1-100nm, are not visible under a low power microscope but show Brownian motion. Common examples include blood, milk, and fog. Colloids exhibit properties like Tyndall effect, adsorption, precipitation with electrolytes, and non-dialyzability. They play important roles biologically such as in protoplasm, blood coagulation, and fat digestion.
Colloids - Physical Pharmacy
The document discusses colloids and their properties. It defines colloids as dispersed systems with particle sizes between 1-1000 nm. Colloids can be lyophilic, lyophobic, or association colloids depending on interactions between particles and dispersion medium. Key properties of colloids include optical effects like Tyndall scattering, Brownian motion, diffusion, osmotic pressure, and electrokinetic phenomena that are influenced by particle size, temperature, and viscosity. Colloids find applications in pharmaceuticals for solubilization, increasing bioavailability, and as therapeutic or diagnostic agents.
Lecture colloids
This document discusses colloids and their properties. It defines colloids as dispersed systems with particle diameters between 1 nm and 1000 nm. Colloids have large surface areas and can be classified as lyophilic, lyophobic, or association colloids. Common examples and methods of preparation are provided. The document also discusses optical properties like Tyndall effect and use of electron microscopes to view colloids, as well as comparisons between types of colloids.
Colloidal solutions
Colloidal solutions are heterogeneous mixtures where solute particles are intermediate in size between true solutions and suspensions. Particles in colloids are larger than in solutions but smaller than suspensions, ranging from 1-100 nm. Colloids are classified based on the state of the dispersed and continuous phases, including sols (solid in liquid), emulsions (liquid in liquid), and aerosols (solid or liquid in gas). Key properties are that colloids appear homogeneous but are heterogeneous, particles do not separate on settling and scatter light, known as the Tyndall effect. Common examples include milk, fog, paints, and soap solutions.
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Colloids presentation slides
Colloids are substances microscopically dispersed throughout another substance. The dispersed particles range in size from 1-100 nm. Colloids exhibit properties between true solutions and suspensions due to their intermediate particle size. They are able to pass through filters but not semipermeable membranes. Common examples include milk, fog, mayonnaise and paints. Colloids can be classified based on factors like the physical state of the phases, the interaction between the phases, the size and nature of dispersed particles, and the electrical charge on particles. They are purified using techniques like dialysis, electrodialysis, and ultrafiltration which separate colloidal particles from dissolved substances.
Colloids and surface chemistry
This document defines and classifies colloids. Colloids have particle sizes between 1-1000 nm, which are larger than true solutions and smaller than suspensions. Colloids are classified based on the physical state of the dispersed and dispersion medium (solid-liquid, liquid-liquid, etc.), interaction between the phases (lyophobic or lyophilic), and particle type (multimolecular, macromolecular, associated). Common colloids include emulsions, gels, sols, and foams. Properties include the Tyndall effect, Brownian motion, and coagulation with electrolytes. Colloids find applications in products like rubber, soaps, and medicines.
Colloids part 1 general introduction
The document discusses colloids and their classification. It defines colloids as substances that are microscopically dispersed through another substance, with particle sizes between 10-10000 Angstroms. Colloids are classified in several ways, including by particle size (molecular dispersion, colloidal dispersion, coarse dispersion), physical state of phases, type of dispersed particles (multimolecular, macromolecular), appearance (sols, gels), and electrical charge on particles (positive, negative). Common colloidal systems include sols, emulsions, foams and aerosols. Micelle formation in colloids and the critical micelle concentration are also explained.
Colloids
Colloids have particle sizes between 1 nm and 1000 nm. They are classified as lyophilic, lyophobic, or association colloids based on particle interactions with the dispersion medium. Lyophilic colloids readily disperse in the medium while lyophobic colloids do not. Association colloids form micelles above a critical micelle concentration. Colloids demonstrate optical properties like Tyndall effect and can be imaged with electron microscopes. They also exhibit kinetic properties including Brownian motion, diffusion, osmotic pressure, and sedimentation. Colloidal particles are often electrically charged, leading to electrokinetic phenomena like electrophoresis and electroosmosis. Stability is important for preventing
Colloidal state
Colloids are heterogeneous mixtures where small insoluble particles are dispersed throughout a liquid medium. Thomas Graham first classified substances as either crystalloids or colloids based on their ability to pass through a membrane. A colloid has particle sizes between 1-100nm, are not visible under a low power microscope but show Brownian motion. Common examples include blood, milk, and fog. Colloids exhibit properties like Tyndall effect, adsorption, precipitation with electrolytes, and non-dialyzability. They play important roles biologically such as in protoplasm, blood coagulation, and fat digestion.
Colloids - Physical Pharmacy
The document discusses colloids and their properties. It defines colloids as dispersed systems with particle sizes between 1-1000 nm. Colloids can be lyophilic, lyophobic, or association colloids depending on interactions between particles and dispersion medium. Key properties of colloids include optical effects like Tyndall scattering, Brownian motion, diffusion, osmotic pressure, and electrokinetic phenomena that are influenced by particle size, temperature, and viscosity. Colloids find applications in pharmaceuticals for solubilization, increasing bioavailability, and as therapeutic or diagnostic agents.
Lecture colloids
This document discusses colloids and their properties. It defines colloids as dispersed systems with particle diameters between 1 nm and 1000 nm. Colloids have large surface areas and can be classified as lyophilic, lyophobic, or association colloids. Common examples and methods of preparation are provided. The document also discusses optical properties like Tyndall effect and use of electron microscopes to view colloids, as well as comparisons between types of colloids.
Colloidal solutions
Colloidal solutions are heterogeneous mixtures where solute particles are intermediate in size between true solutions and suspensions. Particles in colloids are larger than in solutions but smaller than suspensions, ranging from 1-100 nm. Colloids are classified based on the state of the dispersed and continuous phases, including sols (solid in liquid), emulsions (liquid in liquid), and aerosols (solid or liquid in gas). Key properties are that colloids appear homogeneous but are heterogeneous, particles do not separate on settling and scatter light, known as the Tyndall effect. Common examples include milk, fog, paints, and soap solutions.
Colloid chemistry
Here almost full every topics interrelated with colloid chemistry has been discussed.The slides have been made showing question pattern taking Begum Rokeya University Chemistry Department previous year questions to appear the slides easy towards the viewers.Stay join with me.Thank you.
The colloidal state
This document provides an overview of colloids, including:
1) What colloids are and the difference between lyophobic and lyophilic colloids
2) Methods for preparing colloidal solutions, including dispersion and condensation methods
3) Properties of colloidal systems like optical properties related to light scattering and the electrical double layer
Colloids
The document discusses colloids, defining them as heterogeneous mixtures with dispersed particles between 1-100 nm. It classifies different types of colloids based on the state of the dispersed and continuous phases, such as emulsions, foams, sols, and gels. The document also examines the unique properties of colloids, including the Tyndall effect, Brownian motion, and their ability to adsorb other substances.
Colloids
Definition
Application
Difference between molecular and Colloidal dispersion
Characteristics of dispersed phase
Classification of colloidal dispersion
Purification of colloidal dispersion
colloidal dispersion
This document summarizes a seminar on colloidal dispersions presented by Sayani Saha. It defines colloidal dispersions as systems with a dispersed particle phase and continuous dispersion medium between 1-1000 nm. Dispersions are classified by size as molecular, colloidal, or coarse dispersions. The properties of colloidal sols are discussed, including how they are lyophilic or lyophobic, how particles are solvated, how they are prepared, and how they are affected by electrolytes. Various shapes of colloidal particles and classifications based on dispersion medium and phase are also summarized. The document concludes with brief discussions of coacervation and peptization processes.
Colloids By Sitwat Rafi
Colloids are mixtures where one substance is microscopically dispersed throughout another. They consist of two phases - a dispersed phase made of very tiny particles 1nm to 1um in size suspended in a continuous dispersion medium. Common examples are milk, fog, and blood. Colloids can be classified based on the physical state of the phases and the interactions between them. Preparation methods include mechanical grinding, electrical dispersion, peptization of precipitates, and condensation by changes in conditions. The interactions between colloidal particles, such as excluded volume repulsion, electrostatic forces, van der Waals forces, and steric effects influence colloid stability and properties.
Lecture- 'Colloid'
This document discusses different types of colloids classified based on the state of the dispersed and continuous phases. The main types are aerosols, foams, emulsions, sols, and gels. It provides examples like fog and smoke as aerosols, whipped cream as a foam, mayonnaise as an emulsion, and paints as sols. The document also discusses classification based on interaction between phases and nature of particles, and methods for preparing and purifying colloidal solutions.
Unit 2, Lesson 2.5 - Suspensions and Colloids
Unit 2, Lesson 2.5 - Suspensions and Colloids
Lesson Outline:
1. Suspensions
2. Colloids
3. Properties of Colloids
4. Summary: Solution, Suspension, Colloid
Colloid
1) Colloids are heterogeneous mixtures where one substance is dispersed evenly throughout another. They can exist as solid aerosols, foams, emulsions, sols, or solid foams.
2) Colloids exhibit unique optical properties like the Tyndall effect where light is scattered by colloidal particles. They also display random Brownian motion from bombardment by the dispersion medium.
3) Colloids can be classified and prepared through various processes like condensation, dispersion, or using emulsifying agents. Their stability is important and they may undergo destabilization through phenomena like sedimentation or flocculation.
Nature of stability of Colloidal Systems
This document provides an overview of colloidal systems and their classification. It begins by defining colloids as mixtures where one substance is dispersed as minute particles throughout another substance. Colloids are classified based on the state of the dispersed and dispersion mediums, which can be solid, liquid or gas. This results in different types of colloids including sols, emulsions, gels and aerosols. The document also discusses factors that influence the stability of colloids such as electrical forces, interaction with the dispersion medium, and stabilization methods.
Lab colloid chemistry & turbidity
This document outlines objectives and concepts related to colloids and their importance in environmental engineering. It discusses the electrical double layer theory of colloidal surface charge and how colloids can be destabilized through processes like increasing ionic strength or adjusting pH. It also addresses turbidity in water supplies and its environmental significance.
Kinetic properties of colloids
Dispersed systems consist of particulate matter dispersed in a continuous medium and are classified based on particle size as molecular dispersions, colloidal dispersions, or coarse dispersions. Colloidal dispersions have particle sizes between 1-1000 nm that are not visible under an ordinary microscope but can be seen under an electron microscope. Colloidal dispersions exhibit Brownian motion, diffusion, sedimentation, osmotic pressure, viscosity, and optical properties. The document then provides details on these various properties of colloidal dispersions.
colloidal chemistry in foods
The document discusses different types of colloidal systems including emulsions, sols, gels, and foams. It provides examples of each type in foods such as salad dressing as an emulsion, gravy as a sol, baked custard as a gel, and egg white foam as a foam. It also describes key properties of colloids like small particle size visible only under microscope and Brownian motion. Common colloidal systems in foods, properties of each type, and methods of formation and stabilization are summarized.
Colloidal disp[1] ppt [compatibility mode]
Colloids can be classified based on particle size as molecular, colloidal, or coarse dispersions. Colloidal dispersions have particle sizes between 1-500 nm. Colloids can also be classified as lyophilic, lyophobic, or association colloids based on particle interactions. Lyophilic particles are solvent-loving, lyophobic are solvent-hating, and association colloids form micelles. Purification of colloids can be done using dialysis, which separates colloidal particles from dissolved impurities based on size, or electrodialysis, which uses an electric field to enhance impurity removal.
2 colloidal system
Colloids have many important applications in pharmaceuticals, food, and industry. Pharmaceutical applications include using colloids for drug delivery and therapy, as well as coating tablets for protection and controlled release. Colloids are also important in food products like milk, butter, and ice cream. Industrial uses involve non-drip paints, sewage treatment, clarifying water, and in artificial kidney machines.
UNIT 01/PART 01: BP 403T_PHYSICAL PHARMACEUTICS: INTRODUCTION
This presentation deals with the Introduction of Colloidal Dispersion (Unit 1) of syllabus of AKTU, Lucknow and PCI, New Delhi. In this ppt I have discussed the basics of Colloidal Dispersion and how various factors helps in the dispersion formation or destruction.
Colloids (2)
The document discusses colloids, which are heterogeneous mixtures with one substance dispersed evenly throughout another. Colloids are distinguished from true solutions by their ability to scatter visible light via the Tyndall effect. Colloidal particles range in size from 1-1000 nm and can be suspended in gases, liquids, or solids. Colloids are stabilized by electrostatic repulsion between particles coated with layers of ions of the same charge. Colloids can be destroyed through coagulation by heating, which increases particle velocities, or by adding electrolytes to neutralize the stabilizing ion layers.
Colloids
This document discusses colloids, including their definition and classification. Colloids can be classified into different types of mixtures including sols, foams, emulsions, and gels. Sols are solid particles dispersed in a liquid, foams contain gas pockets in a liquid or solid, emulsions involve two immiscible liquids, and gels contain molecules of a liquid dispersed within a solid matrix. The document also provides examples of each type of colloidal mixture and discusses reversible versus irreversible colloid formation.
Methdos of preparation colloids
The document discusses four methods of dispersion for preparing colloids: 1) Mechanical dispersion uses grinding to break large particles into smaller colloidal particles, 2) Electrical dispersion applies an electric arc to vaporize and disperse metal particles, 3) Peptization dispersion converts a precipitate into a colloidal sol using an electrolyte, and 4) Homogenization emulsifies substances like milk or cream to form a stable colloid.
Colloid
A colloid is a mixture where one substance is dispersed evenly throughout another. Unlike solutions, colloidal particles are larger and do not completely dissolve. Colloids can be solid, liquid, or gaseous mixtures. Common examples include fog, milk, and blood. Colloidal particles scatter light and exhibit Brownian motion. They cannot be separated by filtration due to their small but suspended particle size.
Ppt colloidsppt 21
This document provides information about colloids. It defines a colloid as a substance microscopically dispersed throughout another substance. Colloidal solutions contain insoluble particles ranging from 1-1000 nm in size suspended in another substance. Colloids can be classified based on physical state, interaction type, particle size, appearance, or electrical charge. Common examples of colloids include milk, blood, fog and smoke. Colloids can be separated via mechanical dispersion, electrical methods, peptization, or condensation. Properties of colloids depend on whether they are gels, foams, emulsions or aerosols.
Colloidal dispersion.pptx
Colloidal dispersions are heterogeneous systems where one substance is divided into small particles, between 1 nm and 1 μm, dispersed throughout a second substance. They can be classified based on the dispersed and dispersion medium, such as sols where the medium is a liquid. Colloidal particles exhibit properties like Brownian motion, diffusion, and Tyndall effect. Their size, shape, and surface charge affect characteristics like stability, flowability, and pharmacological effects. Purification methods remove electrolytes and impurities through dialysis, ultrafiltration, or electrodialysis.
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Colloid chemistry
Here almost full every topics interrelated with colloid chemistry has been discussed.The slides have been made showing question pattern taking Begum Rokeya University Chemistry Department previous year questions to appear the slides easy towards the viewers.Stay join with me.Thank you.
The colloidal state
This document provides an overview of colloids, including:
1) What colloids are and the difference between lyophobic and lyophilic colloids
2) Methods for preparing colloidal solutions, including dispersion and condensation methods
3) Properties of colloidal systems like optical properties related to light scattering and the electrical double layer
Colloids
The document discusses colloids, defining them as heterogeneous mixtures with dispersed particles between 1-100 nm. It classifies different types of colloids based on the state of the dispersed and continuous phases, such as emulsions, foams, sols, and gels. The document also examines the unique properties of colloids, including the Tyndall effect, Brownian motion, and their ability to adsorb other substances.
Colloids
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This document summarizes a seminar on colloidal dispersions presented by Sayani Saha. It defines colloidal dispersions as systems with a dispersed particle phase and continuous dispersion medium between 1-1000 nm. Dispersions are classified by size as molecular, colloidal, or coarse dispersions. The properties of colloidal sols are discussed, including how they are lyophilic or lyophobic, how particles are solvated, how they are prepared, and how they are affected by electrolytes. Various shapes of colloidal particles and classifications based on dispersion medium and phase are also summarized. The document concludes with brief discussions of coacervation and peptization processes.
Colloids By Sitwat Rafi
Colloids are mixtures where one substance is microscopically dispersed throughout another. They consist of two phases - a dispersed phase made of very tiny particles 1nm to 1um in size suspended in a continuous dispersion medium. Common examples are milk, fog, and blood. Colloids can be classified based on the physical state of the phases and the interactions between them. Preparation methods include mechanical grinding, electrical dispersion, peptization of precipitates, and condensation by changes in conditions. The interactions between colloidal particles, such as excluded volume repulsion, electrostatic forces, van der Waals forces, and steric effects influence colloid stability and properties.
Lecture- 'Colloid'
This document discusses different types of colloids classified based on the state of the dispersed and continuous phases. The main types are aerosols, foams, emulsions, sols, and gels. It provides examples like fog and smoke as aerosols, whipped cream as a foam, mayonnaise as an emulsion, and paints as sols. The document also discusses classification based on interaction between phases and nature of particles, and methods for preparing and purifying colloidal solutions.
Unit 2, Lesson 2.5 - Suspensions and Colloids
Unit 2, Lesson 2.5 - Suspensions and Colloids
Lesson Outline:
1. Suspensions
2. Colloids
3. Properties of Colloids
4. Summary: Solution, Suspension, Colloid
Colloid
1) Colloids are heterogeneous mixtures where one substance is dispersed evenly throughout another. They can exist as solid aerosols, foams, emulsions, sols, or solid foams.
2) Colloids exhibit unique optical properties like the Tyndall effect where light is scattered by colloidal particles. They also display random Brownian motion from bombardment by the dispersion medium.
3) Colloids can be classified and prepared through various processes like condensation, dispersion, or using emulsifying agents. Their stability is important and they may undergo destabilization through phenomena like sedimentation or flocculation.
Nature of stability of Colloidal Systems
This document provides an overview of colloidal systems and their classification. It begins by defining colloids as mixtures where one substance is dispersed as minute particles throughout another substance. Colloids are classified based on the state of the dispersed and dispersion mediums, which can be solid, liquid or gas. This results in different types of colloids including sols, emulsions, gels and aerosols. The document also discusses factors that influence the stability of colloids such as electrical forces, interaction with the dispersion medium, and stabilization methods.
Lab colloid chemistry & turbidity
This document outlines objectives and concepts related to colloids and their importance in environmental engineering. It discusses the electrical double layer theory of colloidal surface charge and how colloids can be destabilized through processes like increasing ionic strength or adjusting pH. It also addresses turbidity in water supplies and its environmental significance.
Kinetic properties of colloids
Dispersed systems consist of particulate matter dispersed in a continuous medium and are classified based on particle size as molecular dispersions, colloidal dispersions, or coarse dispersions. Colloidal dispersions have particle sizes between 1-1000 nm that are not visible under an ordinary microscope but can be seen under an electron microscope. Colloidal dispersions exhibit Brownian motion, diffusion, sedimentation, osmotic pressure, viscosity, and optical properties. The document then provides details on these various properties of colloidal dispersions.
colloidal chemistry in foods
The document discusses different types of colloidal systems including emulsions, sols, gels, and foams. It provides examples of each type in foods such as salad dressing as an emulsion, gravy as a sol, baked custard as a gel, and egg white foam as a foam. It also describes key properties of colloids like small particle size visible only under microscope and Brownian motion. Common colloidal systems in foods, properties of each type, and methods of formation and stabilization are summarized.
Colloidal disp[1] ppt [compatibility mode]
Colloids can be classified based on particle size as molecular, colloidal, or coarse dispersions. Colloidal dispersions have particle sizes between 1-500 nm. Colloids can also be classified as lyophilic, lyophobic, or association colloids based on particle interactions. Lyophilic particles are solvent-loving, lyophobic are solvent-hating, and association colloids form micelles. Purification of colloids can be done using dialysis, which separates colloidal particles from dissolved impurities based on size, or electrodialysis, which uses an electric field to enhance impurity removal.
2 colloidal system
Colloids have many important applications in pharmaceuticals, food, and industry. Pharmaceutical applications include using colloids for drug delivery and therapy, as well as coating tablets for protection and controlled release. Colloids are also important in food products like milk, butter, and ice cream. Industrial uses involve non-drip paints, sewage treatment, clarifying water, and in artificial kidney machines.
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This presentation deals with the Introduction of Colloidal Dispersion (Unit 1) of syllabus of AKTU, Lucknow and PCI, New Delhi. In this ppt I have discussed the basics of Colloidal Dispersion and how various factors helps in the dispersion formation or destruction.
Colloids (2)
The document discusses colloids, which are heterogeneous mixtures with one substance dispersed evenly throughout another. Colloids are distinguished from true solutions by their ability to scatter visible light via the Tyndall effect. Colloidal particles range in size from 1-1000 nm and can be suspended in gases, liquids, or solids. Colloids are stabilized by electrostatic repulsion between particles coated with layers of ions of the same charge. Colloids can be destroyed through coagulation by heating, which increases particle velocities, or by adding electrolytes to neutralize the stabilizing ion layers.
Colloids
This document discusses colloids, including their definition and classification. Colloids can be classified into different types of mixtures including sols, foams, emulsions, and gels. Sols are solid particles dispersed in a liquid, foams contain gas pockets in a liquid or solid, emulsions involve two immiscible liquids, and gels contain molecules of a liquid dispersed within a solid matrix. The document also provides examples of each type of colloidal mixture and discusses reversible versus irreversible colloid formation.
Methdos of preparation colloids
The document discusses four methods of dispersion for preparing colloids: 1) Mechanical dispersion uses grinding to break large particles into smaller colloidal particles, 2) Electrical dispersion applies an electric arc to vaporize and disperse metal particles, 3) Peptization dispersion converts a precipitate into a colloidal sol using an electrolyte, and 4) Homogenization emulsifies substances like milk or cream to form a stable colloid.
Colloid
A colloid is a mixture where one substance is dispersed evenly throughout another. Unlike solutions, colloidal particles are larger and do not completely dissolve. Colloids can be solid, liquid, or gaseous mixtures. Common examples include fog, milk, and blood. Colloidal particles scatter light and exhibit Brownian motion. They cannot be separated by filtration due to their small but suspended particle size.
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UNIT 01/PART 01: BP 403T_PHYSICAL PHARMACEUTICS: INTRODUCTION
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This document provides information about colloids. It defines a colloid as a substance microscopically dispersed throughout another substance. Colloidal solutions contain insoluble particles ranging from 1-1000 nm in size suspended in another substance. Colloids can be classified based on physical state, interaction type, particle size, appearance, or electrical charge. Common examples of colloids include milk, blood, fog and smoke. Colloids can be separated via mechanical dispersion, electrical methods, peptization, or condensation. Properties of colloids depend on whether they are gels, foams, emulsions or aerosols.
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Colloidal dispersions are heterogeneous systems where one substance is divided into small particles, between 1 nm and 1 μm, dispersed throughout a second substance. They can be classified based on the dispersed and dispersion medium, such as sols where the medium is a liquid. Colloidal particles exhibit properties like Brownian motion, diffusion, and Tyndall effect. Their size, shape, and surface charge affect characteristics like stability, flowability, and pharmacological effects. Purification methods remove electrolytes and impurities through dialysis, ultrafiltration, or electrodialysis.
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This document provides information about colloidal dispersions. It defines colloids as mixtures where one substance is dispersed as very small particles (1-1000 nm) throughout another substance. Colloids are classified based on properties of the dispersed and continuous phases. Key characteristics include particle size, shape, surface area, and charge. Colloids exhibit optical properties like Tyndall effect and kinetic properties such as Brownian motion and electrophoresis. The stability of colloids can be impacted by the addition of electrolytes or other charged particles/colloids.
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Here are the steps to make mayonnaise:
1. Place the egg yolks in a small clear jar. Beat the yolks lightly with a fork or whisk.
2. Add 1/4 cup vinegar to the beaten yolks and mix well.
3. Add 1/4 cup oil, one drop at a time, beating vigorously after each addition. Continue adding oil in this slow, dropwise manner until it is all incorporated and the mayonnaise is thickened.
4. If the mayonnaise becomes too thick, thin it with a few drops of water.
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In
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- 1. Colloids
- 2. -To know the definition of colloids -To determine the classification of colloids -To distinguish the common and some examples of colloids according to their classification -To know how colloids are classified. Objectives:
- 3. Colloids The word "Colloid" was derived from the Greek, "kolla" for glue, as some of the original organic colloidal solutions were glues.
- 4. The mixture is also called a colloidal solution, colloidal system, or colloidal dispersion. Colloidal systems can be any combination of these states. Colloid formation can be classified in two systems, namely reversible and irreversible. In an irreversible system, the products are so stable or removed so well that the original reactants cannot be reproduced.
- 5. Find words associated with colloids. Motivation
- 7. Sols Foams Emulsions Gel Connect each mixture with their specific classification. Activity 1
- 10. A foam is a substance that is formed by trapping pockets of gas in a liquid or solid. In most foams, the volume of gas is large, with thin films of liquid or solid separating the regions of gas. foam
- 11. An emulsion is a mixture of two or more liquids that are normally immiscible (nonmixable or unblendable). Emulsions are part of a more general class of two-phase systems of matter called colloids. emulsion
- 12. __________________________________ __________________________________ __________________________________ Tell whether the picture is an emulsion or not. Activity 2
- 13. A sol is a colloidal suspension of very small solid particles in a continuous liquid medium. They are quite stable and show the Tyndall effect. Examples include blood, pigmented ink, and paint. Artificial sols may be prepared by dispersion or condensation. Dispersion techniques include grinding solids to colloidal dimensions byball milling and Bredig's arc method. The stability of sols may be maintained by using dispersing agents. Sols are commonly used in preparing sol-gels.
- 15. A gel (from the lat. gelu— freezing, cold, ice or gelatus— frozen, immobile) is a solid, jelly- like material that can have properties ranging from soft and weak to hard and tough. It is the crosslinking within the fluid that give a gel its structure (hardness) and contribute to the adhesive stick (tack). In this way gels are a dispersion of molecules of a liquid within a solid in which the solid is the continuous phase and the liquid is the discontinuous phase. gel
- 16. 1. GSLE is a solid, jelly-like material that can have properties ranging from soft and weak to hard and tough. In this way gels are a dispersion of molecules of a liquid within a solid in which the solid is the ____2______ and the liquid is the_____3____. 2. coouinntus pahes 3. dsincouintuos pshae It is _____4________ the within the fluid that give a gel its structure (hardness) and contribute to the _____5____ (tack). 4.conkinsslirg 5. ahvdeesi sktic Activity 3
- 17. 1-2. The term colloid comes from the Greek words “kolla” and “oidos” . What are the meaning of KOLLA and OIDOS a. milk, acid b. glue, appearance c. glue, phase 3-4.Colloidal system is composed of two phase. What are these phase? a. continuous phase and dispersed phase b. continuous phase and dispersion medium c. discontinuous phase and dispersed phase 5-6. Colloidal system can be classified according to their _____________and _______________. a. Internal phase and dispersed phase b. dispersion medium and continuous phase c.dispersion medium and dispersed phase QUIZ
- 18. 7. what is the suspension of liquid or solid particles in gas? A. gel b. foams c. aerosols 8. these are the colloidal dispersion of gas bubbles in liquid or solids. a. gel b. foams c. aerosols 9. What is the colloidal dispersion of liquid in either a liquid or solid? A. emulsion b. sols c. aerosols 10. it is a solid dispersed in either a solid or a liquid. A. emulsion b. sols c. aerosols
- 19. 11. What are the colloidal system in which the dispersed phase consist of fibrous, interwoven particles? A. emulsion b. sols c. gels 12. what is the interwoven particles which exert marked effect on the physical properties of the dispersing medium? A. fiber b. fibrils c. fibroins 13. who is the father of colloid chemistry? A. Robert Brown b. Thomas Graham c. john Tyndall 14. Which of the following is NOT a colloidal system? A. marshmallow b. seawater c. mayonnaise 15. which of the following is an aerosol? A. milk B. fog C. cream
- 20. 1. Gel 2. continuous phase 3. discontinuous phase 4. Crosslinking 5. adhesive stick 1-2.b 3-4.b 5-6.a 7.c 8.b 9.a 10.b 11.c 12.b 13.b 14.b 15.b Answer key: