Is Matter Around Us Pure Notes Class 9th Science Chapter 2


CHAPTER – 2 “Is Matter Around Us Pure”


KEY CONCEPTS : [ *rating as per the significance of concept ]

1. Pure Substance & Mixture


2. Types of Mixtures


3. Methods of Separation of Mixtures


4. Concentration & Types of Solutions


5. Physical & Chemical Changes


6. Alloys


-I- Pre requisites

  • Basic knowledge of particle nature of matter
  • Different states of matter


Conceptual levels of comprehension on the basis of feedback taken from the students




• Pure substance consists of a single type of substance .

• Mixture consists of two or more pure substances.

• Pure substance cannot be

separated into other substances by physical methods.

• Mixture can be separated into its components by physical methods.

• Pure substance has its own definite properties.

• Mixture shows the

properties of its components.

Elements are made up of one kind of atoms only. Compounds are made up of one kind of

1. Pure Substance & mixture |

molecules only.

Difference between Compound &Mixture [ refer NCERT text Book Tab.2.2, page 26]

Q.1 Is air around us a compound or mixture?

Q.2 Water is a compound. Justify.

Q.3 Classify the following as element, compound and mixture: Iron, sea water, Milk Q.4 Are the naturally occurring material in nature chemically pure substances?


Mixtures can also be grouped

  1. on the basis of their physical states:





• Salt and sugar

• Salt and water

• Dust in air


• Mercury and copper

• Alcohol and water

• Clouds


• Hydrogen and palladium

• Oxygen and water

• Air

ii) on the basis of miscibility:

Homogeneous Mixture

Heterogeneous Mixture

  • It consists of single phase.
  • Uniform composition.
  • Example: Sugar dissolved in water
  • It consists of two or more phase.
  • Does not have uniform composition.
  • Example: Air, sand and common salt.

Q.1 Give one example for each of the following mixtures: i) Solid/solid (homogeneous)

  1. Solid/solid (heterogeneous) iii) Liquid/liquid (homogeneous) iv) Liquid/liquid (heterogeneous) v) Gas/liquid (homogeneous)..

Q.2 Classify the following as homogeneous & heterogeneous mixture:

  1. sodium chloride & water ii) glucose & water iii) sand & water iv) air
  2. Separating the components of a mixture |

The components of a heterogeneous mixture can be separated by

  • simple methods like –

hand picking, sieving, & Winnowing

  • special techniques like –
  1. Evaporation : a mixture of salt and water or sugar and water.
  2. Centrifugation : Butter from curd, Fine mud particles suspended in water.
  3. Decantation (Using separating funnel) : Oil from water.
  4. Sublimation : Camphor from salt,
  5. Chromatography : Different pigments from an extract of flower petals.
  6. Distillation and fractional distillation : Separating components of Petroleum viii) Magnetic separation: Iron pins from sand.

Q.1 Name the process you would use to :

  1. recover sugar from an aqueous sugar solution.
  2. separate mixture of salt solution and sand.

Q.2 How will you separate a mixture of sand, water and mustard oil ?

  1. Concentration of Solution |

The amount of solute present in a given amount (mass or volume) of solution.

Amount of solute Amount of solute

Concentration of a solution = OR

Amount of solvent Amount of solution

The concentration of a solution can be expressed as mass by mass percentage or as mass by volume percentage.

Mass of solute

Mass by mass percentage of a solution = x 100

Mass of solution Mass of solute

Mass by volume percentage of a solution = x 100

Volume of solution


a) on the basis of size of solute particles:

True solution

Sol [ Colloid]


• Homogeneous

• Heterogeneous

• Heterogeneous

• Size of solute

particles is less than


1 n m or 10 m .

• Size of solute particles is between 1 nm to 1000 nm.

• Size of solute particles is more than 1000 nm.

• Particles cannot pass through filter paper.

• Particles can pass through filter paper.

• Particles cannot pass thorough filter paper.

• Stable

• Stable and settle only on centrifugation.

• Unstable and settle down on its own.

• Solution of sodium chloride in water, sugar & water.

• Milk , Fog

  • muddy water, chalk & water,
  • smoke in the air.

[ types of colloids : refer NCERT Text Book table 2.1, page 18 ]

Colloidal solution is a heterogeneous mixture. It consists of two phases:-

  1. Dispersed phase : component present in small proportion
  2. Dispersion medium : component present in large proportion

The particles of colloid are large enough to scatter a beam of light passing through it and make its path visible. Thus, they show Tyndall effect.

The colloidal particles are moving at random in a zigzag motion in all directions.

This type of zig-zag motion of colloidal particles is called Brownian movement.

b) on the basis of amount of solute:

Unsaturated solution

Saturated Solution

Supersaturated solution

A solution which has lesser amount of solute that it can dissolve at a given temperature is known as unsaturated solution.

A solution which has maximum amount of solute that it can dissolve at a given temperature is known as saturated solution.

A solution which can dissolve amount of solute by increasing temperature saturated solution is known as supersaturated solution.

c) on the basis of nature of solvent

Aqueous solution

Non-Aqueous solution

The solution in which the solvent is water is known as aqueous solution.

The solution in which the solvent is other than water (ether, alcohol or aceton) known as non-aqueous solution.

Q.1 Classify the following substances into true solutions and colloidal solutions.

Milk , ink , starch dissolved in water.

Q.2 A solution has been prepared by dissolving 5g of urea in 95 g of water. What is the mass percent of urea in the solution?

Q.3 Give an example of an aqueous solution in which gas is dissolved.

  1. Physical & Chemical Changes I

Physical changes – Changes that do not result in the production of a new substance.

  • If you melt a block of ice, you still have H2O at the end of the change.
  • If you break a bottle, you still have glass.

Examples : melting, freezing, condensing, breaking, crushing, cutting, and bending.

Chemical changes – Changes that result in the production of another substance.

  • As in the case of autumn leaves, a change in color is a clue to indicate a chemical change.
  • a half eaten apple that turns brown.

Q.1 Which of the following is an example of physical change?

  1. Mixing baking soda and vinegar together, and this causes bubbles and foam.
  2. A glass cup falls from the counter and shatters on the ground.
  3. Lighting a piece of paper on fire and the paper burns up and leaves ashes.
  4. Baking a birthday cake for your mother.

Q.2. Which of the following is an example of chemical change?

  1. Filling up a balloon with hot air.
  2. Taking a glass of water and freezing it by placing it in the freezer.
  3. A plant collecting sunlight and turning it into food.
  4. Your dog ripping up your homework.
  5. Which change can be easily be reversed?
  6. Chemical Change
  7. Physical Change
  8. Both a physical and chemical change
  9. Neither a physical or chemical change


A material that has metallic properties and is composed of two or more chemical elements of which at least one is a metal .

  • These cannot be separated into their components by physical methods.
  • However, these are considered as mixture because these show the properties of its constituents and can have variable composition.

The benefit of alloys is that you can combine metals that have varying characteristics to create an end product that is stronger, more flexible, or otherwise desirable to manufacturers.

  • Aluminium alloys are extensively used in the production of automotive engine parts.
  • Copper alloys have excellent electrical and thermal performance, good corrosion resistance, high ductility and relatively low cost.
  • Stainless steel alloys are used for many commercial applications such as watch straps, cutlery etc.
  • Titanium alloys have high strength, toughness and stiffness & are used in aerospace structures .

Q,1 Why should we use alloys instead of pure metals? Q.2 State uses of Aluminium & Stainless steel alloys.


  1. Mark Questions:
  2. What is meant by pure substance?
  3. What is meant by mass percentage of solution?
  4. Name the process of separation of miscible liquids.
  5. Arrange the following in decreasing order of size of the particles.

True Solution , Suspension , Colloid.

  1. *Give an example of an aqueous solution in which gas is dissolved.
  2. Name the dispersion medium and dispersed phase in the white material inside an egg.
  3. What happens when hot saturated solution is cooled?
  4. How would you separate a mixture of chalk and water?
  5. *How much water should be added to 15 grams of salt to obtain 15 % salt solution?
  6. What type of mixtures are separated by technique of crystallization ?
  7. Marks Questions:
  8. Which of the following materials fall in the category of a pure substance?

a) Ice b) Milk c) Iron d) Hydrochloric acid

e) Calcium oxide f) Mercury g) Brick h) Wood.

  1. What do you understand by saturated solution and unsaturated solution?
  2. *What do you observe when sunlight passes through a dense forest?
  3. List two points of differences between homogeneous and heterogeneous mixtures.
  4. State the difference between aqueous & non aqueous solution .
  5. Which of the following will show “Tyndal Effect” & Why ?

a) Salt Solution b) Milk c) Copper Sulphate Solution d) Starch Solution

  1. *How can we obtain pure copper sulphate from an impure sample?
  2. Give two differences between compounds and mixtures.
  3. Why is hydrogen considered as element ? Give two reasons.
  4. Why water is a compound and not a mixture?
  5. Marks Questions:
  6. Classify the following into elements, compounds and mixtures:

a) Sodium b) Soil c) Sugar solution d) Silver e) Calcium carbonate f) Tin g) Silicon h) Coal i) Air j) Soap k) Methane l) Carbon dioxide m) Blood.

  1. Give any two applications of centrifugation.
  2. Which of the following is chemical change?

a) Growth of a plant b) Rusting of iron c) Mixing of iron fillings and sand d) Cooking of food e) Digestion of food f) Freezing of water g) Burning of a candle.

  1. *State the difference between simple distillation & fractional distillation.
  2. * A solution contains 40 ml of ethanol mixed with 100 ml of water. Calculate the concentration in terms of volume by volume percentage of the solution.

5 Marks Questions:

  1. *What is meant by Tyndall effect? What is its cause? Illustrate with example.
  2. How would you separate the mixture containing sulphur and sand ?
  3. What is crystallization? Give its two applications.
  4. How are sol, solution and suspension different from each other?
  5. How do we obtain coloured components, i.e. dye from Blue/Black ink ?


  • Types of mixtures.
  • Method of Separation of mixtures.
  • Types of solutions.
  • Concentration terms of solution.
  • Physical and Chemical Change.
  • Significance of alloys.
Previous articleMatter in Our Surroundings Notes Class 9th Science Chapter 1
Next articleAtoms and Molecules Notes Class 9th Science Chapter 3


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