1 P a g e B Y : M. Z I A D O G A R

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1 Q: WHY SOLUTIONS ARE OMPORTANT FOR US? Brass, steel, german silver, air, soft drinks, juices, shampoo, crude oil, cough syrup and many others are all solutions. These solutions are widely used for making cooking utensils, surgical tools, cutlery, musical instruments, health tonics, motor fuel and many other objects. Gases when dissolved in liquid also produce some important solutions. For example, water dissolves small amount of air giving a solution whose oxygen content (Solute) is important for the survival of fish and other aquatic animals. Carbon dioxide gas dissolves readily in water, for this reason, it is used in making carbonated drinks. In food industries, vegetable oil is converted into vegetable ghee by passing H 2 gas through the oil. Nickel (used as catalyst) accelerates this process by absorbing H 2 gas on its surface, producing a solution, which is gas in solid solution. Q; DEFINE FOLLOWING WITH EXAMPLE? Solution A homogenous mixture of two or more different chemical substances with uniform chemical and physical properties is called SOLUTION. : Sugar solution is a mixture of sugar and water. Salt solution is a mixture of salt and water. Binary Solution A solution which consist of only two substances is called BINARY SOLUTION. Sugar solution (sugar+water) Salt solution (salt + water) Aqueous Solution The word aqueous is derived from the Latin word Aqua which means water. A solution in which water is used as a solvent is called AQUEOUS SOLUTION. Sugar solution and salt solution. In both solutions, water is used as a solvent Solute The substance or component present in lesser amount in solution is called SOLUTE. In salt sugar solutions, salt and sugar act as a solute. Solvent The substance or component of solution present in relatively large amount in solution is called SOLVENT. In salt and sugar solutions, water is a solvent. Q; DEFINE FOLLOWING WITH SUITABLE EXAMPLES? Unsaturated Solution A solution which can dissolve further amount of solute at a particular temperature is called an unsaturated solution. Take a beaker half filled with water. Add a spoon of sugar in it. It will dissolve. Such a solution is unsaturated because it can still dissolve more amount of solute in it. Saturated Solution A solution which contains the maximum amount, of a solute at a particular temperature and which is unable to dissolve further amount of solute in it is saturated solution. : Go on adding sugar in the above solution till it starts settling down at the bottom of the beaker at a particular temperature, it will be saturated solution. Supersaturated Solution A solution which contains more amount of a solute in a particular amount of solvent then the saturated solution is called supersaturated solution. For Add more sugar in the above solution, stir it, it will dissolve. Go on a adding more sugar and stir it. A stage will come when no more sugar will dissolve and will start settling down at the bottom of the beaker. This solution is called saturated solution. Now heat the above solution, some more solute will dissolves. This solution will be called supper, saturated solution. 1 P a g e B Y : M. Z I A D O G A R

2 Q: How to know whether a solution is unsaturated, saturated or supersaturated? A supersaturated solution is not stable in the presence of crystals of solute. If we add a crystal of sodium thiosulphate to its saturated solution, it will simply drop to the bottom, without dissolving but if we add a crystal of sodium thiosulphate to a Supersaturated solution of sodium thiosulphate, crystallization will starts while in unsaturated solution the crystal will be dissolved. When crystallization has finished, we will have a saturated solution in presence of sodium Thiosulphate. SELF ASSESSMENT EXERCISE 6.1 The maximum amount of sodium acetate that dissolves in 100g of water at 0 o C is 119g and 170g at 100 o C. (a) If you add 170g of sodium acetate in 100g of water at 0 o C, how much will dissolve? ANS: 119g of Sodium acetate will dissolve in 100g of water at 0 o C. (b) Is the solution saturated unsaturated or supersaturated? ANS: The solution will be saturated (c) If the solution in heated to 100 o C, is the solution now saturated, unsaturated or supersaturated. ANS: The solution will be saturated (d) If the solution is cooled back to 0 o C and no crystals appear. Is the solution saturated, unsaturated or supersaturated? ANS: the solution will be supersaturated Q: Descibe various types of solutions? TYPES OF SOLUTIONS Solution exists in any one of the three states of matter i.e. solid, liquid or gas. Physical state of solution is same as that for solvent. In fact, nine different types of solutions can be prepared by mixing together substances. These substances, in any physical state can serve as a solute or solvent. Common types of solutions S. No. Solute Solvent State of resulting solution s 1 Gas Gas Gas Air (a mixture of O 2, N 2, CO 2, etc.), water gas (CO + Hz) 2 Gas Liquid Liquid Soda water (carbonated drink) Hydrochloric Acid 3 Gas Solid Solid H 2 absorbed on Ni, Pt, Pd 4 Liquid Gas Gas Mist, fog, clouds 5 Liquid Liquid Liquid Alcohol in water 6 Liquid Solid Solid Amalgams Hg in Ag, wet NaCl in rainy season 7 Solid Gas Gas Carbon particles in air (smoke) 8 Solid Liquid Liquid Sugar in water, salt in water 9 Solid Solid Solid Alloys such as Solder (Pb + Zn), Bronze (Cu + Zn) SELF ASSESSMENT EXERCISE 6.2 What are the physical states of solute and solvent in each of the following solutions. Also identify the type of solution. (a) Deep sea divers use a breathing mixture of helium and oxygen. 2 P a g e B Y : M. Z I A D O G A R

3 (b) Brass contains 80% copper and 20% zinc. (c) Dental filling. (d) Brine (salt in water). (e) Drinking water containing chlorine as disinfectant. (f) Gemstone, Ruby contains Cr 2 O 3 and Al 2 O 3. (g) Conc. H 2 SO 4, we use in the laboratory is 98% H 2 SO 4 and contains only 2% H 2 O. S.No. Solutions State of Solute State of Solvent Type of Solution a. Mixture of Helium and Helium (g) Oxygen (g) Gas is Gas Oxygen b. Brass Zinc(s) Copper(s) Solid in Solid c. Dental filling Mercury-Hg (l) Silver- Ag (s) Liquid in solid d. Brine solution Salt (s) Water (l) Solid in liquid e. Drinking water with Chlorine (g) Water (l) Gas in liquid chlorine f. Gem stone- Ruby Cr 2 O 3 (s) Al 2 O 3 (s) Solis in solid g. H 2 SO 4, 98% 2%, H 2 O H 2 SO 4, 98% Q: Write note on following? (i) Solutions of gases (ii) Solutions of liquids (iii) Solutions of solids ANSWER Solutions of Gases Gaseous solutions are commonly used by chemical industries to prepare chemical substances. For i) Ammonia synthesis: A gaseous mixture of nitrogen and Hydrogen is used with ratio of N 2 : H 2 is 1:3 which is strictly maintained under varying reaction conditions. ii) Urea Fertilizer: A gaseous mixture of Ammonia and C0 2 is used for synthesis of urea. iii) Nitric Acid: A gaseous mixture of NH 3 and oxygen is used for the preparation of nitric acid. In all these cases, gaseous mixture or solution of gases is used. In these solutions, solute and solvent both are gases. Solutions of Liquids Solution of liquid in gas, liquid or solid solvents are also very common. For 1) Fog, clouds or mist: In this liquid in gas mixture, water vapours are dissolved in air (solvent). 2) When a person feels weakness. So 0.85% m/m NaCl solution is used in intravenous solution to persons suffering from dehydration. 3) Amalgam is mixture of mercury as solute in solid like Ag or tin as solvent. It is widely used for dental cavity filling. Solution of Solids 1. Smoke: It spreads in air forming solution that contains solid carbon particles. In this solution solid particles are solute and air is solvent. We call such a solution as solid in gas. 2. Saline solution: it contains 0.85% m/m NaCl solution is used in intravenous solution that is given to persons suffering from dehydration. 3. Alloys: It is mixture of solids in solids and is used on commercial basis. Brass is an alloy of copper and zinc Steel is an alloy of iron with carbon and silicon Gemstones are also solutions e.g Ruby, Opal etc Q: Define concentration of solution with example? Concentration of Solution Def: It is the amount of solute present in a given amount of solvent or solution is called concentration of solution. Since both parts of the ratio (solute and solvent) can be given in terms of mass, volume or moles, therefore chemists use a variety of concentration terms e.g.: 5g of solute required to dissolve in 95g of solute to make 100 g of m/m solution. 3 P a g e B Y : M. Z I A D O G A R

4 Q: Differentiate between dilute & conc. Solution? Dilute Solution and Concentrated Solution A solution which contains small amount of solute in a solvent is called a dilute solution while a solution which contains large amount of solute in a solvent is called concentrated solution. 1. 5g of NaCl in 95g of solvent in beaker A to make 100 g solution of NaCl 2. while in beaker B, 10 g of NaCl in 90g of solvent (water) to make 100 gm solution of NaCl The beaker-a solution will be called dilute solution and beaker-b solution will be called concentrated solution. Q: What are different units of concentration? Ans: Units of Concentration Chemists uses many concentration units in routine work which are: 1) Percentage composition 2) Molarity 3) Normality 4) Molality 5) Mole fraction 6) Parts per million (ppm) Q: What is Percentage Composition? Percentage Composition The percentage composition is the unit of concentration that specifies the quantity of solute in 100 parts of solution Quantity of solute and solvent can be expressed by mass in grams or volume in cm 3. Therefore, by the percentage of a solution we mean the mass or volume of solute dissolved in 100g or 100cm 3 of solution. There are four different ways of expression for percentage composition. i. Mass by Mass Percentage (m/m) It is the mass of the solute dissolved per 100 parts by mass of solution. 10% m/m NaCl solution means that 10 g NaCl in 90g water to make 100g of solute % of solution by m/m x100 ii. Mass by Volume percent (m/v) It is the mass of the solute dissolved per 100 parts by volume of solution. For 10% m/v NaCl solutions means that 10g NaCl in 90cm 3 water to make 100cm 3 of solution. % of solution by m/v x100 iii. Volume by mass Percent (v/m) It is the volume of solute dissolved per 100 parts by mass of solution. For 10% v/m Alcohol solution and means that 10cm 3 of Alcohol in 90g of water to make 100g of solution % of solution by v/m x100 iv. Volume by volume percent (v/v) It is the volume of solute dissolved per 100 parts by volume of solution. For 10% v/v Alcohol solution means that 10cm 3 of Alcohol in 90 cm 3 of water to make 100 cm 3 of solution. % of solution by v/v x100 SELF ASSESSMENT EXERCISE P a g e B Y : M. Z I A D O G A R

5 1. Write four ways to express percentage of solutions. Ans:See above topic (percentage composition) 2. A saline solution is administered intravenously to a person suffering from severe dehydration. This is labeled as 0.85% m/v of NaCl. What does it mean? Ans: It means that 0.85g of NaCl in cm 3 of water to make 100cm 3 of solution. Q Define molarity. What is the formula for finding molarity? What are the units of molarity? Molarity Molarity is the concentration unit in which the number of moles of solute dissolved per dm 3 of solution. It is denoted by M. Mathematically, the formula for finding Molarity can be written as: Number of moles of solute Molarity (M) Volume of Solution (dm 3 ) or Or molar Volume of Solution (dm 3 ) 000 molar Volume of Solution (cm 3 ) Units of Molarity Its units are mol per dm 3 (mol.dm -3 ) Q: what these terms refers? a. 18 M Sulfuric acid? b M Hydrochloric acid ANS: a. 18M concentrated H 2 SO 4 means that there are 18 moles of H 2 SO 4 in each dm 3 of solution. b. 12.1M concentrated HCl means that there are 12.1 moles of HCl in each dm 3 of solution. Problems Involving the Molarity of a Solution 1. Urea (NH 2 CONH 2 ) is a white solid used as fertilizer and starting material for synthetic plastic. A solution contains 40g urea dissolved in 500cm 3 of solution. Calculate the molarity of this solution. Solution Mass of urea 40g Molar mass of urea (NH2CONH x x2 60g /mole Molarity (M ) 40 x 1000 Molarity (M ) 60 x 500 Mass of solute x 1000 molar x Volume of Solution (cm 3 ) Mol/dm Calculating molarity from moles of solute and volume of solution Potassium permanganate (KMnO 4 ) is a dark blue-black compound. When it dissolves in water, it forms a bright purple solution. It is used as disinfectant in water tanks. It is also known as pinky. A solution contains 0.05 moles of KMnO4 in 600cm 3 of solution. Calculate molarity of this solution. Answer Moles of KMnO mol Volume of KMnO4 600 Cm 3 Molarity (M) Number of moles of solute x 1000 Volume of Solution (cm 3 ) Molarity (M) 0.05 x mol/dm 3 5 P a g e B Y : M. Z I A D O G A R

6 SELF ASSESSMENT EXERCISE 6.4 Potassium chlorate (KClO 3 ) is a white solid. It is used in making matches and dyes. Calculate the molarity of solution that contains. (a) 1.5 moles of this compound dissolved in 250cm 3 of solution (b) 75g of this compound dissolved to produce 1.25dm 3 of solution.(c) What is the molarity of a 50cm 3 sample of potassium chlorate solution that yields 0.25g residue after evaporation of the water. (a) Number of moles of KClO moles Volume of solution 250 cm 3 Molarity of KClO 3? Molarity of KClO 3 Number of moles of solute x 1000 Volume of Solution (cm 3 ) 1.5 x M (b) mass of KClO 3 75g Molar mass of KClO x g Volume of solution 1.25dm 3 Molarity of KClO 3? molar Volume of Solution (dm 3 ) mol.dm 3 or 0.49 M Converting the molarity of a solution into its concentration in g/dm 3 A flask contains 0.25M NaOH solution. What mass of NaOH is present per dm 3 of solution? Molarity: 0.25 M Volume of solution: 1 dm 3 Molar mass od NaOH 40g/mol Mass of NaOH? molar Volume of Solution (dm 3 ) molarity x molar mass x volume of soluton Mass of NaOH 0.25x 40x 1 10 g Converting concentration in g/dm 3 into molarity Potassium hydroxide (KOH) is used in the manufacture of shaving creams, paints and varnish. An analyst makes up a solution by dissolving 5.8g of KOH in one dm 3 of solution. Calculate the molarity of this solution. Mass of KOH dissolved in one dm 3 of solution 5.6g 6 P a g e B Y : M. Z I A D O G A R

7 Molar mass of KOH g/mole molar Volume of Solution (dm 3 ) M SELF ASSESSMENT EXERCISE Sodium hydroxide solutions are used to neutralize acids and in the preparation of soaps and rayon. If you dissolve 25g of NaOH to make 1 dm 3 of solution, what is the molarity of this solution? SOLUTION: Mass of NaOH 25 g Volume of solution: 1 dm 3 Molar mass of NaOH 40g/mol Molarity of NaOH solution? molar Volume of Solution (dm 3 ) 25 x M 2. A solution of NaOH has concentration 1.2M. Calculate the mass of NaOH in g/dm 3 in this solution. SOLUTION: Molarity: 1.2 M Volume of solution: 1 dm 3 Molar mass od NaOH 40g/mol Mass of NaOH? molar Volume of Solution (dm 3 ) molarity x molar mass x volume of soluton Mass of NaOH 1.2x 40x 1 48 g 3. A solution is prepared by dissolving 10g of haemoglobin in enough water to make up 1dm 3 in volume. Calculate molarity of this solution. Molar mass of haemoglobin is 6.51x10 4 g/mole. SOLUTION: Mass of haemolobin 10 g Volume of solution: 1 dm 3 Molar mass of haemoglobin 6.51x 10 4 g/mol Molarity of NaOH solution? molar Volume of Solution (dm 3 ) 10. ~ x x 10-4 M 7 P a g e B Y : M. Z I A D O G A R

8 Q: How you can Prepare a solution of given molarity Prepare 0.2M KMnO 4 solution. Hint Volumetric flasks of capacity 1 dm 3, 500cm 3, 250cm 3, 100cm 3, 50cm 3 can be used to prepare a solution. Suppose you use a 100cm 3 volumetric flask. First find the mass of KMnO 4 to give 100 cm 3 of 0.2 M KMnO 4 solution. Required volume of solution 100cm 3 Molarity of solution 0.2 M Molar mass of KMnO x g/mole 000 molar Volume of Solution (cm 3 ) molarity x molar mass x volume of soluton Mass of KMnO 4 Mass of KMnO x158 x g To prepare 0.2M KMnO 4 in 100cm 3 volumetric flask, you will add 3.16g of KMnO 4. SELF ASSESSMENT EXERCISE How can you prepare 500cm 3 of 0.2M KMnO 4 solution. SOLUTION: Required volume of solution 500cm 3 Molarity of solution 0.2 M Molar mass of KMnO x g/mole 000 molar Volume of Solution (cm 3 ) molarity x molar mass x volume of soluton Mass of KMnO 4 Mass of KMnO x158 x g To prepare 0.2M KMnO 4 in 500cm 3 volumetric flask, you will add 15.8g of KMnO How can you prepare 25cm 3 of 0.25M solution of CuSO 4.5H 2 O (Blue vitriol). 8 P a g e B Y : M. Z I A D O G A R

9 SOLUTION: Required volume of solution 25cm 3 Molarity of solution 0.25 M Molar mass of CuSO 4.5H 2 O x4+18X g/mole 000 molar Volume of Solution (cm 3 ) molarity x molar mass x volume of soluton Mass of CuSO 4.5H 2 O Mass of CuSO 4.5H 2 O 0.25 x249.5 x g 3. To prepare25 cm 3 and 0.25M CuSO 4.5H 2 O, you will add 1.56 g of CuSO 4.5H 2 O in 25 cm 3 of solvent. Preparing a solution of given molarity by diluting a solution of known molarity Concentrated sulphuric acid is 18M H 2 SO 4. How many cm 3 of this acid is needed to produce 250cm 3 of 0.1M H 2 SO 4? M 1 molarity of given conc H 2 SO 4 18M V 1 volume of conc H 2 SO 4 needed to dilute? M 2 molarity of required H 2 SO 4 solution 0.1M V 2 volume of required H 2 SO 4 250cm 3 Give H 2 SO 4 Desired H 2 SO 4 M 1 V 1 M 2 V 2 M V M V M2V2 V 1 M 0.1 x cm Transfer 1.39cm 3 of 18M H 2 SO 4 to a 250cm 3 volumetric flask and dilute it by adding water up to the mark and mix. Resulting solution is 0.1M H 2 SO 4. 1 SELF ASSESSMENT EXERCISE A stock solution of hydrochloric acid is 12.1 M. How many cm 3 of this solution should you use to prepare 500cm 3 of 0.1 M HCl. SOLUTION: 9 P a g e B Y : M. Z I A D O G A R

10 M 1 molarity of given HCl 12.1M V 1 volume of HCl needed to dilute? M 2 molarity of required HCl solution 0.1M V 2 volume of required H 2 SO cm 3 Given HCl Desired HCl M 1 V 1 M 2 V 2 V 1 M cm 3 2. Potassium dichromate (K 2 Cr 2 O 7 ) is a red-orange compound. It is a strong oxidizing agent and is used in the estimation of iron content in ores. A stock solution is 2.5M K 2 Cr 2 O 7. How many cm 3 of this solution you need to dilute to make 50 cm 3 of 0.05 M K 2 Cr 2 O 7. M 1 molarity of given K 2 Cr 2 O M V 1 volume of HCl needed to dilute? M 2 molarity of required HCl solution 0.05 M V 2 volume of required H 2 SO 4 50 cm 3 Given K 2 Cr 2 O 7 Desired K 2 Cr 2 O 7 M 1 V 1 M 2 V 2 V 1 M cm 3 3. Commercial acetic acid is 17.8 molar. How can you convert this into 0.1 M acetic acid. M 1 molarity of given acetic acid 17.8 M V 1 volume of HCl needed to dilute? M 2 molarity of required HCl solution 0.1 M V 2 volume of required H 2 SO cm 3 Given acetic acid Desired acetic acid M 1 V 1 M 2 V 2 V 1 M cm 3 Q: What do you know about solubility of solution, define and give example? Solubility 10 P a g e B Y : M. Z I A D O G A R

11 Solubility of a substance in a particular solvent at a definite temperature is, the maximum amount of the solute in grams that can dissolve in 100g of the solvent to form a saturated solution. Solubility of NaCl in 100g of water at room temperature (25 C) is 35.7g while at 100 C it is 39.12g where as sodium thiosulphate is 50 per 100g water at 25 C but when we add 60g in 100g water at 20 C, the solubility will decrease. Q: How does solubility take place in different compounds or How nature of solute and solvent could effect the solubility? Ans: Solubility and Solute-Solvent Interactions In chemistry analysis, Like dissolves like is a general rule for guiding in solubility of substances. It has been observed that nonpolar covalent solutes are soluble in non polar covalent solvents while Ionic and polar solutes dissolve in polar solvent. Explanation with s 1. Methanol and water are miscible with all proportions because water molecules are polar and having Hydrogen bonding between partial positive charge H +Ϭ and partial negative charge on O -Ϭ. Similarly methanol molecules are also polar and exhibit hydrogen bonding like water molecules. Thus both have similar structure and intermolecular force and therefore miscible with each other in all proportions. 2. Glucose, whose molecule has many -O -H bonds creates Hydrogen bonding with water so it is very soluble in water. 3. When we place a crystal of sodium chloride in water, it dissociate into Na + and Cl - As a result of which, the negative end of water molecule is attracted to Na + and the positive end to Cl - ions. Thus sodium chloride dissolves readily. Figure shows attraction of Na + and Cl - ions for water molecules called Ions dipole forces. Thus the interaction of ions of solute with the molecules of solvent (water) is called Hydration or salvation and the ions will be called Hydrated ions or solvated ions. Attraction of Na + and Cl - ions for water molecules 11 P a g e B Y : M. Z I A D O G A R

12 4. Gasoline and oils are non-polar in nature and do not dissolve in water (Polar). Gasoline and oils as both non polar molecules, are soluble in one another. Q: How does the change of temperature effect the solubility of certain compounds? Justify with. Answer Effect of Temperature on Solubility We can divide the substance in three groups as far as solubility is concerned. 1. Those substance whose solubility is increased on increasing the temperature e.g. KCl, KBr, NaNO 3, NH 4 Cl. Heat is a absorbed when solutions of these substances are prepared in water. When these substances are dissolved, the vessel cools down. Reason is that during dissolution the heat of solvent and the vessel is taken up in the process, of solution formation. Whenever temperature of such solution is increased, solubility s of solutes increase. 2. Those substance whose solubility decreases on increasing the temperature, e.g. Na 2 SO 4. These substances heat produce when dissolved in water. The vessel in which these substances are dissolved becomes hot and its temperature increases. The solubility of gases e.g, air in water decreases with increasing temperature because when water is heated, we will see small bubbles form at the side of the beaker before the water boils. These bubbles are composed of air and come out of water in the form of bubbles. This means that solubility of air in water decreases with increasing temperature.. 3. Similarly we have observed in a home aquarium, that the fish shows signs of stress on a hot day. This is because less oxygen from air dissolves in the warm water. 4. The solubility of some substances is least affected by change in temperature e.g. NaCl. The reason is that a very small amount of heat is absorbed during their solution formation as shown in a graph. The Graph shows the variation of solubility with temperature. Q (a) What do you understand by i) True Solution ii) Suspension iii) Colloids (iv)give the characteristics of each (v)give the comparison of each Answer (i)solution or True Solution A homogenous mixture in which solute particles are completely homegnized in the solvent is called solution or True solution, e.g. solution of NaCl, sugar in water. (ii)suspension A heterogeneous mixture containing particles large enough to be seen with the naked eye and clearly distinct from the surrounding fluid is called a suspension. or A mixture in which solute particles do not dissolve in solvents is called suspension. (iii)colloids A heterogeneous mixture of tiny particles of a substance dispersed through a medium is called a colloid Solute particles pass through the filter paper. Solute particles do not settle down in the bottom by keeping the solution for some time. c) Comparison of properties of solutions, suspension and colloids. S.No. Solutions Suspensions Colloids 1. Homogeneous Heterogeneous Heterogeneous 2. Particles size vary from 0.1 to 1nm Particles size is greater than 10 3 nm Particles size vary from 1 to 10 3 nm 3. Particles are invisible by naked eye, ordinary microscope as well as electron microscope Particles are visible by naked eye Particles are invisible by naked eye and in ordinary microscope but visible under electron microscope 12 P a g e B Y : M. Z I A D O G A R

13 4. Particles can pass through Particles can not pass Particles can pas through ordinary as well as ultra through ordinary as well ordinary filter paper but filter paper as ultra filter paper cannot pass through ultra filter paper 5. Cannot scatter light Scatter light Scatter light Importance of solutions in our daily life Most of the substances we need for our existence are solutions. The air we breathe is a gaseous solution containing N2, O 2, CO 2 and rare gases. The water we use for drinking, cooking and washing is not pure. It contains dissolved gases and many minerals that are essential for our health. In fact natural water is a liquid solution. Beverages, vinegar, soft drinks etc. are liquid solutions. Commercial products such as window cleaners, sanitary cleaners, shampoo, gasoline, kerosene, diesel, etc. are also liquid solutions. Most medicines are dispensed in solution form. We also use many solid solutions in our daily life. Gold is a solid solution of gold containing some copper. Brass and steel are used for making utensils, musical instruments, buses, cars, trains etc are solid solution of metals. Parts of aero plane are made of solid solution of metals such as Al and Mg. Dental filling are liquid solutions of metals in mercury. Science tit bits (suspensions) Many medicine bottles contain an insoluble solid in water. The bottle has to be shaken before use to produce a suspension, so that the solid is spread evenly throughout the bottle and the patient takes the correct amount of the medicine. 13 P a g e B Y : M. Z I A D O G A R