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Solutions

Solutions. Definitions Types of Solution Solutions, Colloids, Suspensions Process of Dissolving Rate of Solution Concentration Solubility. Definitions. Homogenous Mixture – two or more substances which have the same composition throughout; uniform; in the same state of matter

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Solutions

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  1. Solutions Definitions Types of Solution Solutions, Colloids, Suspensions Process of Dissolving Rate of Solution Concentration Solubility

  2. 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

  3. Definitions • Solution - homogeneous mixture of two or more substances Solute - substance being dissolved, present in smaller amount Solute particles very small Solvent - present in greater amount

  4. Definitions Solute - KMnO4 Solvent - H2O

  5. Hydrogen Bonds Attract Polar Water Molecules

  6. 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

  7. Types of Solutions air O2 gas and N2 gas gas/gas soda CO2 gas in water gas/liquid seawater NaCl in water solid/liquid brass copper and zinc solid/solid

  8. Learning Check SF1 (1) element (2) compound (3) solution A. water 1 2 3 B. sugar 1 2 3 C. salt water 1 2 3 D. air 1 2 3 E. tea 1 2 3

  9. Solution SF1 (1) element (2) compound (3) solution A. water 2 B. sugar 2 C. salt water 3 D. air 3 E. tea 3

  10. 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 H2O+5 g KCl solute = 1) KCl 2) H2O solvent = 1) KCl 2) H2O

  11. Solution SF2 A. brass: 20 g zinc + 50 g copper solute = 1) zinc solvent = 2) copper B. 100 g H2O+5 g KCl solute = 1) KCl solvent = 2) H2O

  12. Dissolving • Solvation • occurs at the surface of the solute • solvent particles surround solute particles (+/- attraction) • solute particles are pulled into solution

  13. Dissolving NaCl dissolving in water

  14. NONPOLAR NONPOLAR POLAR POLAR “Like Dissolves Like” • Detergents • polar “head” with long nonpolar “tail” • can dissolve both types

  15. Learning Check SF4 Which of the following solutes will dissolve in water? Why? 1) Na2SO4 2) gasoline 3) I2 4) HCl

  16. 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 (C6H14) is needed to dissolve nonpolar solutes such as oil or grease.

  17. Solution SF4 Which of the following solutes will dissolve in water? Why? 1) Na2SO4 Yes, polar (ionic) 2) gasoline No, nonnpolar 3) I2 No, nonpolar 4) HCl Yes, Polar

  18. Colloids • Have medium size particles • Cannot be filtered • Separated with semipermeable membranes • Scatter light (Tyndall effect)

  19. Examples of Colloids • Fog • Whipped cream • Milk • Cheese • Blood plasma • Pearls

  20. Suspensions • Have very large particles • Settle out • Can be filtered • Must stir to stay suspended

  21. Examples of Suspensions • Blood platelets • Muddy water

  22. Rate of Solution - Solids • Solids dissolve faster (have greater solubility) with... • more stirring • small particle size(increased surface area) • high temperature

  23. Temperature and Solubility of Solids Temperature Solubility (g/100 g H2O) KCl(s) NaNO3(s) 0° 27.6 74 20°C 34.0 88 50°C 42.6 114 100°C 57.6 182 The solubility of most solids (decreases or increases ) with an increase in the temperature.

  24. Temperature and Solubility of Solids Temperature Solubility (g/100 g H2O) KCl(s) NaNO3(s) 0° 27.6 74 20°C 34.0 88 50°C 42.6 114 100°C 57.6 182 The solubility of most solids increases with an increase in the temperature.

  25. Rate of Solution - Gases • Gases dissolve faster and have great solubility if... • no shaking or stirring • high pressure above surface • low temperature

  26. Temperature and Solubility of Gases Temperature Solubility (g/100 g H2O) CO2(g) O2(g) 0°C 0.34 0.0070 20°C 0.17 0.0043 50°C 0.076 0.0026 The solubility of gases (decreases or increases) with an increase in temperature.

  27. Temperature and Solubility of Gases Temperature Solubility (g/100 g H2O) CO2(g) O2(g) 0°C 0.34 0.0070 20°C 0.17 0.0043 50°C 0.076 0.0026 The solubility of gases decreases with an increase in temperature.

  28. Concentration • Concentrated solution • large amount of solute • Dilute solution • small amount of solute

  29. Concentration • % by Volume: usu. liquid in liquid • EX: 10% juice = 10mL juice + 90mL water • % by Mass: usu. solid in liquid • EX: 20% NaCl = 20g NaCl + 80g water • % solution = mass of solute x 100 • mass of solution

  30. UNSATURATED SOLUTION more solute dissolves SATURATED SOLUTION no more solute dissolves SUPERSATURATED SOLUTION becomes unstable, crystals form Concentration concentration

  31. 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

  32. Learning Check S1 At 40C, the solubility of KBr is 80 g/100 g H2O. 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

  33. Solution S1 At 40C, the solubility of KBr is 80 g/100 g H2O. Indicate if the following solutions are (1) saturated or (2) unsaturated A. 2 Less than 80 g/100 g H2O 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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