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States of Matter

Vikasana – Bridge Course 2012

States of Matter

Matter: It is something thatoccupies space possessing

t i H ll thcertain mass. Hence all theSubstances present in thisSubstances present in thisuniverse are matters.

Vikasana – Bridge Course 2012universe are matters.

Li idSubstances which possess definite massLiquid

and volume but indefinite shape are calledliquid. In this state particles are close toeach other and they can move within theirvolume.Ex: water, Benzene,CarbonTetrachloride, Kerosene.

Vikasana – Bridge Course 2012

Gas

Substances which possess definite massbut indefinite volume and shape are calledbut indefinite volume and shape are calledgases. In gases particles are far apart ascompared to solid and liquidcompared to solid and liquid.The particles can move freely from onepoint to another Ex: Nitrogen Oxygenpoint to another. Ex: Nitrogen, Oxygen,Carbon dioxide etc.

Vikasana – Bridge Course 2012

Vikasana – Bridge Course 2012

Classification of matter on the basis of composition:

On the basis of the chemicalcomposition matter can beclassified as fallows.Heterogeneous matterHomogeneous matter

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Heterogeneous matter

A substance is heterogeneous if it exhibitsdifferent properties at its different position.Different types of heterogeneous matter area) Suspensiona) Suspensionb) Colloidc) Hetero mixturec) Hetero mixture

Vikasana – Bridge Course 2012

Vikasana – Bridge Course 2012

Heterogeneous matterMatter

Heterogeneous matter Homogeneous matter

Suspension       colloid      Hetero mixture   

Homogeneous mixture       Pure substanceHomogeneous mixture       Pure substance

Element  Compoundp

M t l               N t l            t ll idMetal               Non‐metal           metalloid

SuspensionSuspensionIt is a heterogeneous matter in which thegsolute particles do not dissolve but remainsuspended throughout the bulk of thep gmedium.Ex: Dirt particles in water, Butter milk.p ,

ColloidColloids are the heterogeneous mixture oftwo components with the size of thepparticle is 1nm to 100nm(or 10 A0 to1000A0).These particles of colloid are) puniformly spread throughout the solution.Ex: Blood,Milk,Butter,Cloud.Ex: Blood,Milk,Butter,Cloud.

HeteromixtureIt is obtained by mixing two or more substancein any ratio. These are possessing the mixed

ti f th bi d b t Thproperties of the combined substance. Thesecan be separated by physical method.

E A i t f d d ltEx: A mixture of sand and common salt.

Homogeneous matterA substance is homogeneous matter if thesmallest part of it exhibits the samepchemical and physical properties.Ex: Air , Solution of sugar with water, anEx: Air , Solution of sugar with water, anintimate mixture of two or more than twometals (alloys).metals (alloys).

Homogeneous matter can be classifiediinto two typesHomogeneous mixtures

A mixture of two components appears in a single phase is called homogeneous mixtures. These

ll d l tiare called as solutions.A homogeneous mixture of solute and

solvent are called solutions These solutions aresolvent are called solutions. These solutions are also called as true solutions or crystalloids Ex:A homogeneous mixture of sugar and water g ggives true solutions

Pure substancesPure substances

P b t Th d fPure substance: These are made ofonly one type of particles such ast l l F th thatoms or molecules. Further these are

classified as elements and compounds.

ElementSimple forms of matter which cannot bedecomposed into further simple substances are

ll d l t 118 l t di d tillcalled elements. 118 elements are discovered tilltoday, out of which 92 are naturally occurringelements and remaining are artificially preparedelements and remaining are artificially preparedelements.Ex: Hydrogen mercury gold iron etcEx: Hydrogen, mercury, gold, iron etc.

Elements are further classified as metals, non metals and metalloids

Metal

non‐metals and metalloids

The elements with the electro‐positive nature of losing one or more electrons greadily to give positively charged cations are called metalscations are called metals.

M                 M+  +  e‐

Ex :Copper,     Zinc,      Iron

Non‐metal:The electronegative elements which have a tendency to gain one which have a tendency to gain one or more electrons are called non‐

lmetals..A +  e‐ A‐A +  e A

Ex: Chlorine, Bromine, Sulphur etc

Magnesium metalg

Sodium metal

MetalloidsMetalloids

Elements possessing of both metalsElements possessing of both metalsand non‐metals properties are called

ll idmetalloids.Ex: Antimony, arsenic, Germinium etc.y, ,

CompoundsThe substances made of two or more thantwo elements in a definite ratio by massyare called compounds.Ex: 1. In water(H2O) number of hydrogenEx: 1. In water(H2O) number of hydrogenand oxygen atoms are in the ratio 2:1 or itcontains hydrogen and oxygen in the ratiocontains hydrogen and oxygen in the ratioof 1:8 by their mass. i.e. 2g of hydrogencombines with 16 g of oxygen.combines with 16 g of oxygen.

CompoundsEx: 2. Sulphuric acid (H2SO4 ):In this compound the ratio of number ofIn this compound the ratio of number ofatoms of H:S:O is 2:1:4The ratio by massof H:S:O is 1:16:32.In this compound 2 g ofof H:S:O is 1:16:32.In this compound 2 g ofhydrogen 32 g of sulpher 64 grams ofoxygen combine with each other to form 98oxygen combine with each other to form 98g of H2SO4.

SolutionSolutionA homogeneous mixtures of solute andgsolvent are called solutions. In a solution, asubstance which is in a less quantity isq ysolute and other which is in more quantityis solvent. In aqueous solution of sugar,q g ,water is solvent and sugar is solute.

Concentration of solutionThe amount of a solute present in a unit volume of

the solution is called concentration of thel tisolution.

Concentration of the solution can be expressed int h t b b lterms such as percentage by mass or by volume,molarity, molality, normality, mole fraction, ppm.Out of these terms the most familiar terms toOut of these terms the most familiar terms toexpress the concentration of the solution arepercentage by mass or volume, molarity andp g y , ynormality.

Percentage by mass: It is the massof the solute present in 100 g of theof the solute present in 100 g of thesolution.

Percentage by mass =Percentage by mass =

Percentage by volume: It is thegmass of the solute present in 100cm3of the solutioncm3of the solution.

Percentage by volume =

50 g of glucose is dissolved in 400 g 5 g g 4 gof water, then calculate  % by mass of the soluteof the solute.

Ans: Total mass of the solution = mass of glucose + mass of  water = 50  + 400   =  450 g= 50  + 400   =  450 g

Percentage by mass =

=                          =   11.11

Hence % by mass of glucose in thesolution is 11.11

300 cm3 of solution contains 20 g ofNaCl dissolved with water, thenNaCl dissolved with water, thencalculate % by volume of the solution

P t  b   l    Percentage by volume = 

= = 6.67

Hence % by volume of NaCl in theHence % by volume of NaCl in the solution is 6.67

MolarityMolarity can be defined as the number ofgram molecular mass of solute dissolved ingone dm3 of the solution. It is denoted by M

Molarity = 

orMolarity =

Where m= mass of the soluteWhere m mass of the soluteM= Molecular mass of the soluteV= volume of the solutionV= volume of the solution

MolarityMolarity

Molarity of NaOH solution is 0.5 Mmeans 0.5 mole (or 0.5 gram molecularmass) of NaOH is dissolved in one dm3

of the solution.

Problem.

Calculate the molarity of the

Problem.

y

solution obtained by dissolving 6 g

of oxalic acid in 200 cm3of solution.

Mol.mass of oxalic acid is 126.

Solution. Given things gm=6 g M= 126 V= 200cm3

Molarity =

= = 0.238M

NormalityNormality can be defined as the numberof gram equivalent mass of soluteg qdissolved in one dm3 of the solution. Itis represented by Np y

Normality =

ORNormality =

Where m= mass of the soluteE= Equivalent mass of the soluteqV= volume of the solution

NormalityNormality

N li f H SO l i i N INormality of H2SO4 solution is 0.5 N, Itmeans that 0.5 gram equivalent mass ofH2SO4 is dissolved in one dm3 of thesolutionso ut o

ProblemCalculate the normality of the solutioncontaining 4 g of sodium hydroxide in 500 cm3 ofthe solution (Equ mass of NaOH is 40)the solution. (Equ.mass of NaOH is 40)

Normality Normality  =

N= 0.2 NHence, the normality of NaOHsolution is 0.2N

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