States of Matter VIKASANA VIGNANA PATHADEDEGE NIMMA NADIGE Bridge Course Program for SSLC Students who want to take up Science in I PUC in 2012
States of Matter Matter: It is something that occupies space possessing certain ti mass. Hence all the Substances present in this universe are matters.
Classification of matter on the basis of their physical state: On the basis of physical state, matter can be classified as solid, liquid, gas and plasma.
Solid: Substances which possess definite mass, volume and shape are called solids.in this state particles are held hldvery close to each other. These particles have no freedom of movement. Ex: Wood, stone, copper etc.
Liquid Substances which possess definite mass and volume but indefinite shape are called liquid. In this state particles are close to each other and they can move within their volume. Ex: water, Benzene, Carbon Tetrachloride, Kerosene.
Gas Substances which possess definite mass but indefinite volume and shape are called gases. In gases particles are far apart as compared to solid and liquid. The particles can move freely from one point to another. Ex: Nitrogen, Oxygen, Carbon dioxide etc.
Classification of matter on the basis of composition: On O the ebasis s of the echemical ca composition matter can be classified as fallows. Heterogeneous matter Homogeneous matter
Heterogeneous matter A substance is heterogeneous if it exhibits different properties at its different position. Different types of ht heterogeneous matter are a)suspension b) Colloid c) Hetero mixture
Heterogeneous matter Matter Heterogeneous matter Homogeneous matter Suspension colloid Hetero mixture Homogeneous mixture Element Pure substance Compound Metal Non metal metalloid
Suspension It is a heterogeneous matter in which the solute particles do not dissolve but remain suspended throughout h the bulk of the medium. Ex: Dirt particles in water, Butter milk.
Colloid Colloids are the heterogeneous mixture of two components with the size of the 100nm(or 10 A 0 particle is 1nm to to 1000A 0 ).These particles of colloid are uniformly spread throughouth t thesolution. ti Ex: Blood,Milk,Butter,Cloud.,,
Heteromixture It is obtained by mixing two or more substance in any ratio. These are possessing the mixed properties of the combined substance. These can be separated by physical method. Ex: A mixture of sand and common salt.
Homogeneous matter A substance is homogeneous matter if the smallest part of it exhibits the same chemical and physical properties. Ex: Air, Solution of sugar with water, an intimate mixture of two or more than two metals (alloys).
Homogeneous matter can be classified into two types (a)homogeneous mixtures A mixture of two components appears in a single phase is called homogeneous mixtures. These are called as solutions. A homogeneous mixture of solute and solvent are called solutions. These solutions are also called as true solutions or crystalloids Ex: A homogeneous mixture of sugar and water gives true solutions
Homogeneous matter can be classified into two types: (Contd.) (b)pure substances These are made of only one type of particles such as atoms or molecules. Further these are classified as elements and compounds.
Element Simple forms of matter which cannot be decomposed into further simple substances are called elements. 118 elements are discovered till today, out of which 92 are naturally occurring elements and remaining are artificially prepared elements. Ex: Hydrogen, mercury, gold, iron etc.
Elements are further classified as metals, non-metals and metalloids Mtl Metal The elements with the electro-positive nature of losing one or more electrons readily to give positively charged cations are called metals. M M + + e - Ex :Copper, Zinc, Iron
Non-metal: The electronegative elements which have a tendency to gain one or more electrons are called non-metals.. A + e - A - Ex: Chlorine, Bromine, Sulphur etc
Magnesium metal
Sodium metal
Metalloids Elements possessing of both metals and non-metals properties are called metalloids. Ex: Antimony, arsenic, Germinium etc.
Compounds The substances made of two or more than two elements in a definite ratio by mass are called compounds. Ex: (1) In water (H 2 O) number of hydrogen and oxygen atoms are in the ratio 2:1 or it contains hydrogen and oxygen in the ratio of 1:8 by their mass. i.e. 2g of hydrogen combines with 16 g of oxygen.
Compounds Ex: (2) Sulphuric acid (H 2 SO 4 ): In this compound the ratio of number of atoms of H:S:O is 2:1:4The ratio by mass of H:S:O is 1:16:32.In16 this compound 2 g of hydrogen 32 g of sulpher 64 grams of oxygen combine with each other to form 98 g of H 2 SO 4. g 2 4
Solution A homogeneous mixtures of solute and solvent are called solutions. In a solution, a substance which is in a less quantity is solute and other which is in more quantity is solvent. In aqueous solution of sugar, water is solvent and sugar is solute.
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Concentration of solution The amount of asolute present in aunit volume of the solution is called concentration of the solution. Concentration of the solution can be expressed in terms such as percentage by mass or by volume, molarity, molality, normality, mole fraction, ppm. Out of these terms the most familiar terms to express the concentration of the solution are percentage by mass or volume, molarity and normality.
Percentageby mass: It is the mass of the solute present in 100 gof the solution. Percentage by mass =
Percentage by volume: It is the mass of the solute present in 100 cm 3 of the solution. Percentage by volume =
Problem 50 g of glucose is dissolved in 400 g of water, then calculate % by mass of the solute. Ans: Total mass of the solution = mass of glucose + mass of water = 50 + 400 = 450 g
Percentage by mass = 11.11 Hence % by mass of glucose in the solution is 11.11
Problem 300 cm 3 of solution contains 20 g of NaCl dissolved with water, then calculate l % by volume of the solution Percentage by volume =
. = = 6.67 Hence % by volume of NaCl in the solution is 6.67 67
Molarity Molarity can be defined as the number of gram molecular mass of solute dissolved in one dm 3 of the solution. It is denoted by M Molarity =
or Molarity = Where m= mass of the solute M= Molecular l mass of thesolute V= volume of the solution
Molarity Molarity of NaOH solution is 0.5 M means 0.5 mole ( or 0.5 gram molecular mass )of NaOH is dissolved in one dm 3 of the solution.
Problem. Calculate the molarity of the solution obtained by dissolving i 6 g of oxalic acid in 200 cm 3 of solution. Mol. mass of oxalic acid is 126.
Solution. S l Given things m=6 g M= 126 V= 200cm 3 Molarity = = = 0.238M
Normality Normality can be dfi definedd as the number of gram equivalent mass of solute dissolved in one dm 3 of the solution. It is represented by N Normality =
OR Normality = Where m= mass of the solute E= Equivalent mass of the solute V= volume of the solution
Normality Normality of H 2 SO 4 solution is 0.5 N, It means that 0.5 gram equivalent mass of H 2 SO 4 is dissolved in one dm 3 of the solution
Problem Calculate the normality of the solution containing 4 g of sodium hydroxide in 500 cm 3 of the solution. (Equ.mass of NaOH is 40) Normality = = 0.2 N Hence the normality of NaOH solution is 0.2N