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Warm-up

Warm-up. Define the term solution in your own words. What are three examples of solutions?. SOLUTIONS. Solutions (ch.16). Solution – a homogeneous mixture of pure substances

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Warm-up

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  1. Warm-up • Define the term solution in your own words. • What are three examples of solutions?

  2. SOLUTIONS

  3. Solutions (ch.16) • Solution – a homogeneous mixture of pure substances • The SOLVENT is the medium in which the SOLUTESare dissolved. (The solvent is usually the most abundant substance.) • Example: • Solution: Salt Water • Solute: Salt • Solvent: Water

  4. READ ONLY SECTION: • HOW DO SUBSTANCES DISSOLVE? • “According to the kinetic theory, the water molecules in each glass of tea are always moving. Some moving water molecules collide with sugar crystals. When this happens, energy is transferred to the sugar molecules at the surface of the crystal.” (Holt, p. 192)

  5. The process of dissolution (solute dissolving in solvent) is favored by: • A decrease in the energy of the system (exothermic-releasing energy) 2) An increase in the disorder of the system (entropy)

  6. Liquids Dissolving in Liquids • Liquids that are soluble in one another (“mix”) are called MISCIBLE. • “LIKE dissolves LIKE” • POLAR liquids are generally soluble in other POLAR liquids. • NONPOLAR liquids are generally soluble in other NONPOLAR liquids.

  7. Factors affecting rate of dissolution: How can you speed up dissolution? • Think of a cube of sugar dissolving in water

  8. Factors affecting rate of dissolution: think iced tea vs. hot tea & the type of sugar you use: cubes or granulated 1) Surface area / particle size • The greater the surface area, the faster it dissolves 2) Temperature • Most solids dissolve faster at higher temperatures 3) Agitation • Stirring/shaking will speed up dissolution

  9. Saturation: • Write a definition for the following terms using the terms solute and solvent • Unsaturated solution – • Saturated solution – • Supersaturated solution –

  10. Saturation: a solid solute dissolves in a solvent until the soln is SATURATED • Unsaturated solution – is able to dissolve more solute • Saturated solution – has dissolved the maximum amount of solute • Supersaturated solution – has dissolved excess solute (at a higher temperature). Solid crystals generally form when this solution is cooled.

  11. Demo: Supersaturated NaC2H3O2 • Crystallization of a supersaturated solution: • Have more solute dissolved than a soln can theoretically hold. • Can initiate the crystallization by using a very small crystal (seed crystal) of solute. • Crystallization is RAPID & draws excess solute to crystallize • http://www.youtube.com/watch?v=BLq5NibwV5g

  12. ROCK CANDY, YUM!!

  13. Applying Concepts QUESTION • When the crystallization has stopped, will the solution be saturated or unsaturated? •  answer

  14. ANSWER: SATURATED • Solution has the maximum amount of solute for a given quantity of solvent at a constant temperature and pressure.

  15. SOLUBILITY • Solubility = the amount of solute that will dissolve in a given amount of solvent

  16. Factors Affecting Solubility • The nature of the solute and solvent: different substances have different solubilities • Temperature: many solids substances become more soluble as the temp of a solvent increases; however, gases are less soluble in liquids at higher temps. • Pressure: Only affects the solubility of gases. As pressure increases, the solubility of gases increases.

  17. Gases: solubility • Temp and Pressure (think: flat soda) • mentos in Diet Coke • Nucleation site: the following factors that contribute to the bubble formation: Diet coke • carbon dioxide is what makes the bubbles form in the first place • in synthetic mixtures aspartame, caffeine and potassium benzoate where shown give better fountains Mentos • the most important property is the rough surface which provides plenty of nucleation sites for bubble formation • the density makes them sink which is ideal as the bubbles formed at the bottom of the bottle help expel much more soda • mentos contains gelatin and gum arabic which could also reduce surface tension

  18. NOTES DRAWINGS • Write each concept/term in a square (small) • Explain the concept and draw an image to help you remember the meaning: • Solution • Solute • Solvent • Entropy • Factors affecting rate • Unsaturated • Saturated • Supersaturated • Solubility • Factors affecting solubility • Demo: heat pack • Demo: coke & mentos

  19. Concentration of Solution • Concentration refers to the amount of solute dissolved in a solution.

  20. *MOLARITY

  21. Example: Describe how you would prepare 2.50 L of 0.665 M Na2SO4 solution starting with:b) solid Na2SO4 Dissolve 236 g of Na2SO4 in enough water to create 2.50 L of solution.

  22. Example Problem from Textbook • Pg. 481 • #9 • #8

  23. MOLARITY BY DILUTION • When you dilute a solution, you can use this equation:

  24. Example: Describe how you would prepare 2.50 L of 0.665 M Na2SO4 solution starting with:a) 5.00 M Na2SO4 Add 0.333 L of Na2SO4 to 2.17 L of water.

  25. MASS PERCENT

  26. MASS PERCENT • Example: What is the percent of NaCl in a solution made by dissolving 24 g of NaCl in 152 g of water?

  27. *MOLALITY

  28. MOLALITY • Example: What is the molality of a solution that contains 12.8 g of C6H12O6 in 187.5 g water?

  29. MOLALITY • Example: How many grams of H2O must be used to dissolve 50.0 g of sucrose to prepare a 1.25 m solution of sucrose, C12H22O11?

  30. Colligative Properties of Solutions (chapter 16) Colligative properties = physical properties of solutions that depend on the # of particles dissolved, not the kind of particle.

  31. Colligative Properties • Lowering vapor pressure • Raising boiling point • Lowering freezing point • Generating an osmotic pressure

  32. 2 to focus on… • Lowering vapor pressure • Raising boiling point • Lowering freezing point • Generating an osmotic pressure

  33. Boiling Point Elevation • a solution that contains a nonvolatile solute has a higher boiling pt than the pure solvent; the boiling pt elevation is proportional to the # of moles of solute dissolved in a given mass of solvent. Like when adding salt to a pot of boiling water to make pasta 

  34. Boiling Point Elevation • Tb = kbm where: Tb = elevation of boiling pt m = molality of solute (mol solute/kg solvent) kb = the molal boiling pt elevation constant • kb values are constants; see table 16.3 pg. 495 • kb for water = 0.52 °C/m

  35. Ex: What is the normal boiling pt of a 2.50 m glucose, C6H12O6, solution? • “normal” implies 1 atm of pressure • Tb = kbm • Tb = (0.52 C/m)(2.50 m) • Tb = 1.3 C • Tb = 100.0 C + 1.3 C = 101.3 C

  36. Freezing/Melting Point Depression • The freezing point of a solution is always lower than that of the pure solvent. Like when salting roads in snowy places so the roads don’t ice over or when making ice cream 

  37. Freezing/Melting Point Depression • Tf = kfm where: Tf = lowering of freezing point m = molality of solute kf = the freezing pt depression constant • kf for water = 1.86 °C/m • kf values are constants; see table 16.2 pg. 494

  38. Ex: Calculate the freezing pt of a 2.50 m glucose solution. • Tf = kfm • Tf = (1.86 C/m)(2.50 m) • Tf = 4.65 C • Tf = 0.00C - 4.65 C = -4.65C

  39. Textbook pg. 495 #34 • Calculate the freezing-point depression (ΔTf) of a benzene solution containing 400. g of benzene and 200. g of acetone, C3H6O (solute). • Kf for benzene is 5.12 °C/m

  40. Answer • ΔTf = Kf x m • ΔTf = (5.12 °C/m) x (m) • m = So, ΔTf = (5.12 °C/m) x (8.61 m) = 44.1 °C

  41. Do the following on your paper • 1. What is the boiling point of each solution? a) 0.50 mol glucose in 1000. g water b) 1.50 mol NaCl in 1000. g water • 2. What is the freezing point of each solution? a) 1.40 mol Na2SO4 in 1750 g water b) 0.060 mol MgSO4 in 100. g water  answers

  42. ANSWERS • 1a) 100.26 °C • 1b) 100.78 °C • 2a) -1.49 °C • 2b) -1.1 °C

  43. More calcs.

  44. Ex: When 15.0 g of ethyl alcohol, C2H5OH, is dissolved in 750 grams of formic acid, the freezing pt of the solution is 7.20°C. The freezing pt of pure formic acid is 8.40°C. Determine Kf for formic acid. Tf = kfm 1.20C= (kf)( 0.4340 m) kf = 2.76 C/m

  45. EXTRA NOTES • Important info for lab, etc.

  46. Electrolytes and Colligative Properties • Colligative properties depend on the # of particles present in solution. • Because ionic solutes dissociate into ions, they have a greater effect on freezing pt and boiling pt than molecular solids of the same molal conc.

  47. Electrolytes and Colligative Properties • For example, the freezing pt of water is lowered by 1.86°C with the addition of any molecular solute at a concentration of 1 m. • Such as C6H12O6, or any other covalent compound • However, a 1 m NaCl solution contains 2 molal conc. of IONS. Thus, the freezing pt depression for NaCl is 3.72°C…double that of a molecular solute. • NaCl  Na+ + Cl- (2 particles)

  48. Electrolytes - Boiling Point Elevation and Freezing Point Depression The relationships are given by the following equations: • Tf = kf ·m·norTb = kb·m·n Tf/b = f.p. depression/elevation of b.p. m = molality of solute kf/b = b.p. elevation/f.p depression constant n = # particles formed from the dissociation of each formula unit of the solute

  49. Ex: What is the freezing pt of a 1.15 m sodium chloride solution? • NaCl  Na+ + Cl- n=2 • Tf = kf·m·n • Tf = (1.86 C/m)(1.15 m)(2) • Tf = 4.28 C • Tf = 0.00C - 4.28 C = -4.28C

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