1. Solutions

2. Objectives/Warm-Up SWBAT describe dilute, concentrated, saturated, unsaturated, and supersaturated solutions. SWBAT describe dilute, concentrated, saturated, unsaturated, and supersaturated solutions. What do the terms “concentrated” and “dilute” mean to you? What do the terms “concentrated” and “dilute” mean to you?

3. Objective/Warm-Up SWBAT describe solutions and be able to complete molarity and dilution calcualtions. SWBAT describe solutions and be able to complete molarity and dilution calcualtions. How do we know if something is more or less concentrated or dilute? How could we quantify (measure) concentration? How do we know if something is more or less concentrated or dilute? How could we quantify (measure) concentration?

4. Concentrated Look at the two bottles of laundry detergent. Look at the two bottles of laundry detergent. Why is one bottle smaller than the other? Why is one bottle smaller than the other? What does it mean that the smaller bottle is more “concentrated”? What does it mean that the smaller bottle is more “concentrated”? What is the difference between the two laundry detergents? What is the difference between the two laundry detergents?

5. Solute-what is being dissolved Solute-what is being dissolved Solvent-what the solute is being dissolved in Solvent-what the solute is being dissolved in Solution-the mixture of solute and solvent Solution-the mixture of solute and solvent

6. Making Kool-Aid When you make Kool-Aid, what is the solute? When you make Kool-Aid, what is the solute? What is the solvent? What is the solvent? What is the solution? What is the solution?

7. Making Kool-Aid If you make a concentrated solution of Kool-Aid. If you make a concentrated solution of Kool-Aid. –This solution has too much___________. If you make a dilute solution of Kool-Aid. If you make a dilute solution of Kool-Aid. –This solution has too much ____________. How can we use the concentrated solution of Kool-Aid to make a more dilute solution of Kool-Aid? How can we use the concentrated solution of Kool-Aid to make a more dilute solution of Kool-Aid? solute solvent

8. Saturated Solutions Is there a limit to how much Kool-Aid or sugar we can dissolve in water? Is there a limit to how much Kool-Aid or sugar we can dissolve in water? What happens when we reach that limit? What happens when we reach that limit? What can we do to the solution to make more sugar dissolve? What can we do to the solution to make more sugar dissolve? When we can add no more solute to a solution, the solution is SATURATED. When we can add no more solute to a solution, the solution is SATURATED.

9. Objective/Warm-Up SWBAT describe solutions. SWBAT describe solutions. What is a saturated solution? What is a saturated solution?

10. Ch. 15-Solutions Essential Questions What makes up a solution? What makes up a solution? What are some different types of solutions? What are some different types of solutions? How can I make a solution? How can I make a solution? What factors affect solubility? What factors affect solubility? How can I measure or calculate the solubility or concentration of a solution? How can I measure or calculate the solubility or concentration of a solution?

11. Supersaturated http://www.pbs.org/kcet/wiredscience/vid eo/259-dr_schrempp_s_chem_lab.html http://www.pbs.org/kcet/wiredscience/vid eo/259-dr_schrempp_s_chem_lab.html http://www.pbs.org/kcet/wiredscience/vid eo/259-dr_schrempp_s_chem_lab.html http://www.pbs.org/kcet/wiredscience/vid eo/259-dr_schrempp_s_chem_lab.html Watch the demonstration of the crystallization of a supersaturated solution. Watch the demonstration of the crystallization of a supersaturated solution. Supersaturated means that more solute is dissolved in the solution than should be able to dissolve at that temperature. Supersaturated means that more solute is dissolved in the solution than should be able to dissolve at that temperature. To make a supersaturated solution, heat the solution to get the solute to dissolve, then let it cool. To make a supersaturated solution, heat the solution to get the solute to dissolve, then let it cool.

12. Solubility Curves

13. Reading Using black “Connections to our changing world” Textbook, read sections 15-2 and 15-3 and complete worksheet. Using black “Connections to our changing world” Textbook, read sections 15-2 and 15-3 and complete worksheet.

14. Objective/Warm-Up SWBAT describe solutions and be able to complete molarity and dilution calcualtions. SWBAT describe solutions and be able to complete molarity and dilution calcualtions. How do we know if something is more or less concentrated or dilute? How could we quantify (measure) concentration? How do we know if something is more or less concentrated or dilute? How could we quantify (measure) concentration?

15. How do we measure concentration? MOLARITY MOLARITY M = moles solute/Liters of solution M = moles solute/Liters of solution

16. Showing saturated solutions http://www.wwnorton.com/college/chemis try/gilbert2/tutorials/interface.asp?chapter =chapter_04&folder=saturated_solutions http://www.wwnorton.com/college/chemis try/gilbert2/tutorials/interface.asp?chapter =chapter_04&folder=saturated_solutions http://www.wwnorton.com/college/chemis try/gilbert2/tutorials/interface.asp?chapter =chapter_04&folder=saturated_solutions http://www.wwnorton.com/college/chemis try/gilbert2/tutorials/interface.asp?chapter =chapter_04&folder=saturated_solutions

17. Thinking back… What is the difference between homogeneous and heterogeneous mixtures? What is the difference between homogeneous and heterogeneous mixtures?

18. What is a solution? A homogeneous mixture of two or more substances. A homogeneous mixture of two or more substances.

19. Examples of Solutions… What are the solute and solvent for each of these solutions? Kool-aid Kool-aid Tea Tea Air Air Soda Soda Brass Brass Steel Steel

20. Review from Yesterday… Solubility: “Like Dissolves Like” Solubility: “Like Dissolves Like” Fill out chart. Fill out chart.

21. Objective/Warm-Up SWBAT solve dilution problems. SWBAT solve dilution problems. How many grams of NaCl are needed to make 250 mL of a 0.100 M solution? How many grams of NaCl are needed to make 250 mL of a 0.100 M solution?

22. Volume-Measuring Devices buret graduated cylinder volumetric flask pipette

23. How do we make solutions for the lab? Using the following materials, predict how they might be used to make solutions with a particular molarity: balance, wash bottle, distilled water, volumetric flask. Using the following materials, predict how they might be used to make solutions with a particular molarity: balance, wash bottle, distilled water, volumetric flask. Procedure: Procedure: 1.Weigh solid. 2.Put some distilled water in volumetric flask. 3.Add solid and stir. 4.Fill water to line, mix completely.

24. a)To make a 0.5-molar (0.5M) solution, first add 0.5 mol of solute to a 1-L volumetric flask half filled with distilled water. b)Swirl the flask carefully to dissolve the solute. c)Fill the flask with water exactly to the 1-L mark.

25. http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/013_SOLUTF ROMSOL.MOV http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/013_SOLUTF ROMSOL.MOV http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/013_SOLUTF ROMSOL.MOV http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/013_SOLUTF ROMSOL.MOV

26. Oops, It’s too concentrated! Our solution is too concentrated. How can we dilute the solution so that it is less concentrated? Our solution is too concentrated. How can we dilute the solution so that it is less concentrated?

27. Dilution M 1 V 1 =M 2 V 2 M 1 V 1 =M 2 V 2 Because… the moles stay the same! Because… the moles stay the same!

28. Making a Dilute Solution

29. a)To prepare 100 ml of 0.40M MgSO 4 from a stock solution of 2.0M MgSO 4, a student first measures 20 mL of the stock solution with a 20-mL pipet. b)She then transfers the 20 mL to a 100-mL volumetric flask. c) Finally she carefully adds water to the mark to make 100 mL of solution.

30. Dilution Practice Problems

31. 1. To make a 1.00M aqueous solution of NaCl, 58.4 g of NaCl are dissolved in a) 1.00 liter of water. b) enough water to make 1.00 liter of solution c) 1.00 kg of water. d) 100 mL of water. 16.2 Review

32. 2. What mass of sodium iodide (NaI) is contained in 250 mL of a 0.500M solution? a) 150 g b) 75.0 g c) 18.7 g d) 0.50 g

33. 3. Diluting a solution does NOT change which of the following? a) concentration b) volume c) milliliters of solvent d) moles of solute

34. Objective/Warm-Up SWBAT calculate molality and describe types of solutions. SWBAT calculate molality and describe types of solutions. If 10.0 grams of NaOH are dissolved in enough solvent to make 100 mL of solution, what is the molarity of the solution? If 10.0 grams of NaOH are dissolved in enough solvent to make 100 mL of solution, what is the molarity of the solution?

35. Types of Solutions Alloys-mixture of two or more metals Alloys-mixture of two or more metals Miscible- mixture of two liquids that can mix in any proportion Miscible- mixture of two liquids that can mix in any proportion Immiscible- liquids that cannot mix in any proportion Immiscible- liquids that cannot mix in any proportion Aqueous- solutions with water as a solvent Aqueous- solutions with water as a solvent

36. Types of Aqueous solutions Electrolytes-conduct electricity in water, made primarily with ionic compounds Electrolytes-conduct electricity in water, made primarily with ionic compounds Non-electrolytes-do not conduct electricity in water, made primarily with covalent compounds Non-electrolytes-do not conduct electricity in water, made primarily with covalent compounds

37. Demonstration

38. Molality Molality: m =moles solute/kg solvent Molality: m =moles solute/kg solvent How is molality different than molarity? How is molality different than molarity? How would these differences affect how to make a solution based on molality as opposed to molarity? How would these differences affect how to make a solution based on molality as opposed to molarity?

39. To make a 0.500m solution of NaCl, use a balance to measure 1.000 kg of water and add 0.500 mol (29.3 g) of NaCl.

40. Practice Calculations

41. Reading Solubility Curves

42. Objective/Warm-Up SWBAT describe types of solutions and identify electrolytes. SWBAT describe types of solutions and identify electrolytes. What is the molarity of a 3.5 L solution with 4.5 g of Ca(NO 3 ) 2 ? What is the molarity of a 3.5 L solution with 4.5 g of Ca(NO 3 ) 2 ?

43. Animation of Solution Formation http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/058_Dissolut NaCl.MOV http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/058_Dissolut NaCl.MOV http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/058_Dissolut NaCl.MOV http://cwx.prenhall.com/petrucci/medialib/ media_portfolio/text_images/058_Dissolut NaCl.MOV

44. Objective/Warm-Up SWBAT solve molarity and molality problems. SWBAT solve molarity and molality problems. How many grams of FeCl 3 are needed to make 50 mL of a 0.170 M solution? How many grams of FeCl 3 are needed to make 50 mL of a 0.170 M solution?

45. Reading Article/Discussion Read the Article from the Washington Post. Read the Article from the Washington Post. In your group, create a chart/table/or graphic organizer (such as a Venn Diagram, concept map or web) describing how to get out different types of stains (oily, water-based, combination stains, carbohydrates, proteins, food pigments, wine stains) In your group, create a chart/table/or graphic organizer (such as a Venn Diagram, concept map or web) describing how to get out different types of stains (oily, water-based, combination stains, carbohydrates, proteins, food pigments, wine stains)

46. Why? Write a 1-2 sentence summary explain how and/or why different cleaning methods are needed for different stains. Write a 1-2 sentence summary explain how and/or why different cleaning methods are needed for different stains.