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Agenda:

Homework : New Element Project. Agenda: . Warm-up: Explain the solvation process Review – terms, importance, “likes dissolve likes” Solubility Curves What can they tell us about solutions? Measuring concentration of solutions. Warm-up: Solvation Process.

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Agenda:

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  1. Homework: New Element Project Agenda: • Warm-up: Explain the solvation process • Review – terms, importance, “likes dissolve likes” • Solubility Curves • What can they tell us about solutions? • Measuring concentration of solutions

  2. Warm-up: Solvation Process • Explain what is happening when an ionic compound is dissolved in water (called solvation or hydration) • View the video - what are key steps that need? • How does the water molecules interact with the ionic compound? • http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/thermochem/solutionSalt.html

  3. a. Making Solutions: Molecules (Covalent compounds) • General Rule: “Likes dissolve likes” Polar solutes can dissolve in polar solvents. Examples:

  4. Organic solvents • Non-polar solute can dissolve in non-polar solvents • Examples: • To remove oily stains in dry-cleaning • Lipids will dissolve in hydrocarbon • To clean oil based paints • To manufacture plastics, man-made fibers, adhesives

  5. Solution process

  6. Solution process • Animations • https://www.youtube.com/watch?v=EBfGcTAJF4o

  7. b. Making Solutions: Factors that impact the solubility of solids in liquids • Energy is involved – 2 steps • Endothermic to separate solute & solvent particles • Exothermics – attraction between solvent & solute particles

  8. c. Measuring Concentration • Solubility: number of grams of solute in 100 grams of water at 20℃ • Solubility Curves • Saturated solutions • Unsaturated • Supersaturated • http://www.youtube.com/watch?v=XSGvy2FPfCw • http://www.youtube.com/watch?v=1y3bKIOkcmk&feature=related

  9. Interpreting solubility curves Y axis X axis Lines If the amount needed is more or less than 100 g of H₂O 1 g H₂0 = 1 mL H₂0

  10. c. Making solutions: Factors that affect the solubility of gases in liquids Think about soda (carbonated drinks)

  11. Solubility Rules determined under specified concentration (often 0.1% molarity)

  12. d. Measuring Concentrations • Molarity (M) by definition = • Molarity = Moles of solute • 1 Liter of solution • Therefore: 2 molar solution = __________________ • Discovery Education video • Standard Deviants School Chemistry: solutions & dilutions

  13. Molarity: moles of solute liters of solution

  14. Molarity problems M= moles_______ 1 Liter solution • What I s the molarity of a solution in which 58 gram of NaCl are dissolved in 1.0 L of solution? • What is the molarity of a solution in which 10.0 grams of silver I nitrate is dissolved in 500 mL of solution? • How many grams of potassium nitrate should be used to prepare a 2.0 L of a 0.5 molar solution?

  15. Steps needed in molarity calculations • Moles For grams: • Liters of solution • If less than 1L ? mL = 1L • Comparison __________ = moles of solute 1 liter of solution

  16. Molarity practice • To what volume should 5.0 g of KCl be diluted in order to prepare a 0.25M solution? • How many grams of copper II sulfate – penta hydrate are needed to prepare 100 mL of a 0.10M solution?

  17. 9g. Dilution of concentrated solutions: V₁M₁= V₂M₂ • Molarity by dilution practice problems • Most reagents are sold & sorted in concentrated solutions • How much concentrated 18M sulfuric acid is needed to prepare 250mL of a 6.0M solution? • How much concentrated 12M hydrochloric acid is needed to prepare 100 mL of a 2.0 M solution?

  18. To what volume should 25 mL of 15 M nitric actid be diluted to prepare a 3.0 M solution? • To how much water should 50 mL of 12 M hydrochloric acid be added to produce a 4.0 M solution? • To how much water should 100 mL of 18M sulfuric acid be added to prepare 1.5 M solution?

  19. Colligative Properties • The properties of the solution that depend on the number of particles in solution, not the identity of the solute. • The solvent properties will be changed. • NaCl • CaCl₂ • AlCl₃ • Melting point depression; boiling point elevation; • Vapor pressure lowering

  20. Resources • http://www.karentimberlake.com/solution.htm • http://www.afn.org/~afn02809/powerpoint-list.htm • http://www.chemistrygeek.com/chemistrypowerpoint/Student%20Ch%2015%20Solutions.ppt • http://college.cengage.com/chemistry/general/zumdahl/world_of_chem/1e/instructors/ppt/figures/viewindex.html

  21. Solution process

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