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Solutions Definitions Types of Solution Solutions, Colloids, Suspensions Process of Dissolving Rate of Solution Concentration Solubility
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Definitions Homogenous Mixture – two or more substances which have the same composition throughout; uniform; in the same state of matter Solutions, Colloids, Suspensions Heterogeneous Mixture – two or more substances which have a mixture in which the ingredients are not uniformly dispersed. Fruity Pebbles
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Definitions Solution - Solution - homogeneous mixture of two or more substances Solvent Solvent - present in greater amount Solute Solute - substance being dissolved, present in smaller amount Solute particles very small
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Definitions Solute Solute - KMnO 4 Solvent Solvent - H 2 O
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Hydrogen Bonds Attract Polar Water Molecules
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Types of Solutions Based on state of solvent. All solid-liquid-gas combos are possible. EX: dental amalgam (alloy of silver, mercury, etc.) liquid solute, solid solvent solid solution
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Types of Solutions air O 2 gas and N 2 gas gas/gas soda CO 2 gas in water gas/liquid seawater NaCl in water solid/liquid brass copper and zinc solid/solid
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Learning Check SF1 (1) element (2) compound (3) solution A. water123 B. sugar 123 C. salt water 123 D. air123 E. tea123
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Solution SF1 (1) element (2) compound (3) solution A. water2 B. sugar 2 C. salt water 3 D. air3 E. tea3
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Learning Check SF2 Identify the solute and the solvent. A. brass: 20 g zinc + 50 g copper solute= 1) zinc 2) copper solvent = 1) zinc 2) copper B. 100 g H 2 O + 5 g KCl solute = 1) KCl 2) H 2 O solvent = 1) KCl 2) H 2 O
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Solution SF2 A. brass: 20 g zinc + 50 g copper solute= 1) zinc solvent = 2) copper B. 100 g H 2 O + 5 g KCl solute = 1) KCl solvent = 2) H 2 O
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Dissolving Solvation occurs at the surface of the solute solvent particles surround solute particles (+/- attraction) solute particles are pulled into solution
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Dissolving NaCl dissolving in water
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“Like Dissolves Like” NONPOLAR POLAR Detergents polar “head” with long nonpolar “tail” can dissolve both types
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Learning Check SF4 Which of the following solutes will dissolve in water? Why? 1) Na 2 SO 4 2) gasoline 3) I 2 4) HCl
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Like dissolves like A ____________ solvent such as water is needed to dissolve polar solutes such as sugar and ionic solutes such as NaCl. A ___________solvent such as hexane (C 6 H 14 ) is needed to dissolve nonpolar solutes such as oil or grease.
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Solution SF4 Which of the following solutes will dissolve in water? Why? 1) Na 2 SO 4 Yes, polar (ionic) 2) gasoline No, nonnpolar 3) I 2 No, nonpolar 4) HClYes, Polar
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Colloids Have medium size particles Cannot be filtered Separated with semipermeable membranes Scatter light (Tyndall effect)
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Examples of Colloids Fog Whipped cream Milk Cheese Blood plasma Pearls
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Suspensions Have very large particles Settle out Can be filtered Must stir to stay suspended
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Examples of Suspensions Blood platelets Muddy water
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Rate of Solution - Solids Solids dissolve faster (have greater solubility) with... more stirring small particle size (increased surface area) high temperature
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Temperature and Solubility of Solids TemperatureSolubility (g/100 g H 2 O) KCl(s)NaNO 3 (s) 0°27.6 74 20°C34.0 88 50°C42.6114 100°C 57.6182 The solubility of most solids (decreases or increases ) with an increase in the temperature.
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Temperature and Solubility of Solids TemperatureSolubility (g/100 g H 2 O) KCl(s)NaNO 3 (s) 0°27.6 74 20°C34.0 88 50°C42.6114 100°C 57.6182 The solubility of most solids increases with an increase in the temperature.
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Rate of Solution - Gases Gases dissolve faster and have great solubility if... no shaking or stirring high pressure above surface low temperature
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Temperature and Solubility of Gases TemperatureSolubility(g/100 g H 2 O) CO 2 (g)O 2 (g) 0°C0.340.0070 20°C0.170.0043 50°C0.0760.0026 The solubility of gases (decreases or increases) with an increase in temperature.
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Temperature and Solubility of Gases TemperatureSolubility(g/100 g H 2 O) CO 2 (g)O 2 (g) 0°C0.340.0070 20°C0.170.0043 50°C0.0760.0026 The solubility of gases decreases with an increase in temperature.
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Concentration Concentrated solution large amount of solute Dilute solution small amount of solute
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Concentration % by Volume % by Volume: usu. liquid in liquid EX: 10% juice = 10mL juice + 90mL water % by Mass % by Mass: usu. solid in liquid EX: 20% NaCl = 20g NaCl + 80g water % solution = mass of solute x 100 mass of solution
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Concentration SATURATED SOLUTION no more solute dissolves UNSATURATED SOLUTION more solute dissolves SUPERSATURATED SOLUTION becomes unstable, crystals form concentration
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Solubility Solubility maximum grams of solute that will dissolve in 100 g of solvent at a given temperature varies with temperature based on a saturated solution g of solute 100 g water
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Learning Check S1 At 40 C, the solubility of KBr is 80 g/100 g H 2 O. Indicate if the following solutions are (1) saturated or (2) unsaturated A. ___60 g KBr in 100 g of water at 40 C B. ___200 g KBr in 200 g of water at 40 C C. ___25 KBr in 50 g of water at 40 C
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Solution S1 At 40 C, the solubility of KBr is 80 g/100 g H 2 O. Indicate if the following solutions are (1) saturated or (2) unsaturated A. 2 Less than 80 g/100 g H 2 O B. 1 Same as 100 g KBr in 100 g of water at 40 C, which is greater than its solubility C. 2 Same as 60 g KBr in 100 g of water, which is less than its solubility
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