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Solutions Chapter 12 Modern Chemistry

Solutions Chapter 12 Modern Chemistry. Sections 1-3 Types of Mixtures The Solution Process Concentrations of Solution. Section 12.2. The Solution Process. Vocabulary. Dissociation Hydration Insoluble Immiscible Miscible Henry’s Law Effervescence. Solubility

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Solutions Chapter 12 Modern Chemistry

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  1. SolutionsChapter 12 Modern Chemistry Sections 1-3 Types of Mixtures The Solution Process Concentrations of Solution

  2. Section 12.2 The Solution Process Chapter 12 Section 2 The Solution Process p. 407-417

  3. Vocabulary Dissociation Hydration Insoluble Immiscible Miscible Henry’s Law Effervescence Solubility Factors affecting rate of dissolution Saturated Unsaturated Supersaturated Solubility equilibrium Solubility values Chapter 12 Section 1 Types of Mixtures p. 401-406

  4. UNSATURATED SATURATED SUPERSATURATED Concept Map 12.2 SOLUBILITYEQUILIBRIUM SOLUBILITYVALUES SOLUBILITY FACTORS AFFECTING RATE OF DISSOLUTION IONIC SOLUTE LIQUID SOLUTE GAS SOLUTE TEMPERATURE PRESSURE SOLUBLE LIKES DISSOLVE LIKES DISSOCIATION HYDRATION MISCIBLE IMMISCIBLE INSOLUBLE HENRY’S LAW EFFERVESCENCE Chapter 12 Section 1 Types of Mixtures p. 401-406

  5. Factors Affecting the Rate of Dissolution How would you make a solute dissolve faster? • Stir. • Break it up. • Heat it. Agitate the solution Increase the surface area of the solute Heat the solvent Chapter 12 Section 2 The Solution Process p. 407-417

  6. Factors Affecting Dissolution Rate Chapter 12 Section 2 The Solution Process p. 407-417

  7. Solubility in grams • Solubility of a substance is the amount of that substance required to form a saturated solutions with a specific amount of solvent at a specific temperature • Look at the chart on page 410 • Dependant on the nature of the solvent and the solute and the temperature of the solute • The maximum amount that can be dissolved is not dependant on the rate it dissolves 100 g H2O 20° C Chapter 12 Section 2 The Solution Process p. 407-417

  8. Solubility & Temperature p. 410 Chapter 12 Section 2 The Solution Process p. 407-417

  9. Solubility and Temperature p. 414* Chapter 12 Section 2 The Solution Process p. 407-417

  10. Solubility of Solids in Liquids Chapter 12 Section 2 The Solution Process p. 407-417

  11. Solubility • There is a limit to the amount of solute that can be dissolved. Why? • Solubility Equilibrium – the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates. • In other words… the same amount of solute is dissolving and “undissolving” at the same time. Chapter 12 Section 2 The Solution Process p. 407-417

  12. Solubility & Solution Equilibrium Chapter 12 Section 2 The Solution Process p. 407-417

  13. Solubility Equilibrium Insert Holt Disc 2 Chapter 12 Section 2 The Solution Process p. 407-417

  14. Saturated & Unsaturated Solns • Saturated – A solution that contains the maximum amount of dissolved solute. • You can tell that it is saturated because no more solute will dissolve and fall to the bottom of the container. • Unsaturated – A solution that contains less solute than a saturated solution under the existing conditions. Chapter 12 Section 2 The Solution Process p. 407-417

  15. Mass of Solute Added vs Mass of Solute Dissolved p. 409 Chapter 12 Section 2 The Solution Process p. 407-417

  16. Supersaturated Solutions • A solution that contains more dissolved solute than a saturated solution contains under the same conditions. • HOW? Saturate a solution. Heat the solution so that more solute can be added. When the solution is cooled undisturbed it will be saturated. Chapter 12 Section 2 The Solution Process p. 407-417

  17. UnsaturatedSaturatedSupersaturated LESS than 35.9g NaCl in 100g H2O at 20°C EXACTLY 35.9g NaCl in 100g H2O at 20°C MORE than 35.9g NaCl in 100g H2O at 20°C Chapter 12 Section 2 The Solution Process p. 407-417

  18. NaC2H3O2 Tower Insert Holt Disc 2 Chapter 12 Section 2 The Solution Process p. 407-417

  19. Solubility of Compounds notes Chapter 12 Section 2 The Solution Process p. 407-417

  20. Solubility of Compounds notes Chapter 12 Section 2 The Solution Process p. 407-417

  21. Molecule Polarity REVIEW!! • What is the molecule polarity of H2O? CCl4? • How do we determine this? Insert Holt Disc 2 Chapter 12 Section 2 The Solution Process p. 407-417

  22. Ionic Solute-Solvent Interaction • Ionic solids that dissolve are soluble. • Ionic solids will dissolve in polar solvents but not nonpolar solvents • Water molecules break the crystal lattice into separate ions. This is dissociation. • Then the water molecules surround the ions. This is hydration. • Ionic solids that do not dissolve are insoluble. Chapter 12 Section 2 The Solution Process p. 407-417

  23. Ionic Solute-Solvent Interaction p. 411 Chapter 12 Section 2 The Solution Process p. 407-417

  24. Dissociation Animations Insert Holt Disc 2 Insert Glencoe Disk 2 Chapter 12 Section 2 The Solution Process p. 407-417

  25. Hydrated Na+ Insert Holt Disc 2 Chapter 12 Section 2 The Solution Process p. 407-417

  26. Liquid Solute-Solvent Interaction • Miscible – Liquids that dissolve freely in one another in any proportion. • Immiscible – Liquids that are not soluble in each other. • “Likes dissolve likes” Polar solutes dissolve in polar solvents. Nonpolar solutes dissolve in nonpolar solvents. • Alcohols are slightly polar. Chapter 12 Section 2 The Solution Process p. 407-417

  27. Miscible and Immiscible Chapter 12 Section 2 The Solution Process p. 407-417

  28. Immiscible & Miscible p. 412 Chapter 12 Section 2 The Solution Process p. 407-417

  29. How Soap Works Iodine Solubility Insert Holt Disc 2 Chapter 12 Section 2 The Solution Process p. 407-417

  30. Gas Solute-Solvent Interactions • Effect of pressure on gas solubility • Pressure changes have little effect on liquid or solid solutes. • Gases dissolved in a liquid are in an equilibrium • This means that some of the gas molecules are going into the solvent and some are going out of the solvent at equal rates. Chapter 12 Section 2 The Solution Process p. 407-417

  31. Solubility of a Gas in a Liquid Chapter 12 Section 2 The Solution Process p. 407-417

  32. Gas Solute-Solvent Interactions • Henry’s Law • The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid. Chapter 12 Section 2 The Solution Process p. 407-417

  33. Gas Solute-Solvent Interactions After being underwater for a long time, a diver will have more gases dissolved in the blood. The diver must pause during the ascent to allow the dissolved gas to come out of solution (the blood) slowly and to be exhaled. If the ascent is too fast the gas can come out of solution while flowing through blood vessels and block essential blood vessels, causing extreme pain, paralysis, or even death. Chapter 12 Section 2 The Solution Process p. 407-417

  34. Efervescence Chapter 12 Section 2 The Solution Process p. 407-417

  35. Keep the fizz in your soda! Chapter 12 Section 2 The Solution Process p. 407-417

  36. Mentos and Coke? Eepy Bird http://www.eepybird.com/videos.html Steve Spangler Science http://www.stevespanglerscience.com/experiment/00000109 Mythbuster http://www.youtube.com/watch?v=kMXPOqovSBs&feature=related Chapter 12 Section 2 The Solution Process p. 407-417

  37. Gas Solute-Solvent Interactions • Effect of temperature on gas solubility • Increasing temperature decreases the solubility of a gas • An increased temperature increases the kinetic energy so that gas molecules can escape from the solvent Chapter 12 Section 2 The Solution Process p. 407-417

  38. Enthalpy of Solution • The net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent. • If heat is given off when the solute dissolves, it is exothermic and the enthalpy is negative. • If heat is taken in when the solute dissolves, it is endothermic and the enthalpy is positive. • Look at the table of enthalpies on page 416. Chapter 12 Section 2 The Solution Process p. 407-417

  39. Enthalpies of Solutions p. 416 Chapter 12 Section 2 The Solution Process p. 407-417

  40. Handheld Heater Insert Holt Disc 2 Chapter 12 Section 2 The Solution Process p. 407-417

  41. Enthalpies of Solutions p. 415 Chapter 12 Section 2 The Solution Process p. 407-417

  42. Ch 12 Sec 2 Homework Section Review Page 416 # 1-7 Chapter 12 Section 2 The Solution Process p. 407-417

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