1. Aim: Using Table G to Predict Solubility  Do Now: Take out HW  Complete #7-12 on page 9 of the packet  Do Now: Take out HW  Complete #7-12 on page 9 of the packet

2. Aim: Using Table F to Predict Solubility  Table F gives us information on the solubility of various compounds in solution  You can predict the solubility of a compound or of the two products of a double replacement reaction  Table F gives us information on the solubility of various compounds in solution  You can predict the solubility of a compound or of the two products of a double replacement reaction

4. Recognizing & Understanding Double Replacement Reactions  Double reactions contain 2 ionic compounds  Not every potential double replacement reaction will occur  3 situations that ensure a DR reaction occurs:  One of the products is a solid (a precipitate)  One of the products is a gas  A molecular substance such as water is formed  Double reactions contain 2 ionic compounds  Not every potential double replacement reaction will occur  3 situations that ensure a DR reaction occurs:  One of the products is a solid (a precipitate)  One of the products is a gas  A molecular substance such as water is formed

5. 3 Possible Outcomes of Double Replacement  One of the products must be:  A solid  A gas  A molecular compound, like water  One of the products must be:  A solid  A gas  A molecular compound, like water

8. Predicting Solubility with Table F Directions  Circle the symbol of the first ion or element  Underline the symbol of the second ion or element  Switch them around  Use Table F to predict the solubility Directions  Circle the symbol of the first ion or element  Underline the symbol of the second ion or element  Switch them around  Use Table F to predict the solubility

9. Predicting Double Replacement Products & Solubility  KI + Pb(NO 3 ) 2  +  1. Predict products: reactants swap places  2. Determine solubility of products  Example: For the reaction between LiBr and BaNO 3, predict the products and determine their solubility  KI + Pb(NO 3 ) 2  +  1. Predict products: reactants swap places  2. Determine solubility of products  Example: For the reaction between LiBr and BaNO 3, predict the products and determine their solubility

11. Homework  Complete page 11 of the packet

12. Aim: What are some factors that affect solubility?  Do Now: packet page 12

13. Dissolving Demo  Styrofoam  Salt  Sugar  Styrofoam  Salt  Sugar

14. Unequal Solubilities  Not all solutes dissolve to the same extent in the same solvent  Examples:  NaNO 3 : 125g/100g water at 60° C  NaCl: ~39g/100g water at 60° C  Not all solutes dissolve to the same extent in the same solvent  Examples:  NaNO 3 : 125g/100g water at 60° C  NaCl: ~39g/100g water at 60° C

15. But Why?

16. Factors Affecting Solubility  Temperature  Pressure  Particle size  Nature of the solute & solvent (polarity)  Temperature  Pressure  Particle size  Nature of the solute & solvent (polarity)

17. Solubility Factors: Temperature  Solids: as temp , solubility   Liquids: as temp , solubility   Gas: as temp , solubility   Solids: as temp , solubility   Liquids: as temp , solubility   Gas: as temp , solubility 

18. Solubility Factors: Pressure  Solids: as pressure , no effect  Liquids: as pressure , no effect  Gas: as pressure , solubility   Solids: as pressure , no effect  Liquids: as pressure , no effect  Gas: as pressure , solubility  Applying principles of solubility and pressure, explain why soda goes flat when you open the can.

19. Soda Carbonation

20. Solubility Factors: Particle Size  Particle size: smaller particles dissolve faster than larger particles  Stirring can increase the rate of dissolving and the solubility  Particle size: smaller particles dissolve faster than larger particles  Stirring can increase the rate of dissolving and the solubility

21. Solubility Factors: Polarity  “Like Dissolves Like” Rule  Nonpolar solutes dissolve in nonpolar solvents  Polar solutes dissolve in polar solvents  “Like Dissolves Like” Rule  Nonpolar solutes dissolve in nonpolar solvents  Polar solutes dissolve in polar solvents

23. Solution Video  http://www.youtube.com/watch?v=VTmfQUNLl MY http://www.youtube.com/watch?v=VTmfQUNLl MY  http://www.youtube.com/watch?v=VTmfQUNLl MY http://www.youtube.com/watch?v=VTmfQUNLl MY

24.  Complete pages 13 & 14 in the packet  HW: page 15 in the packet  Complete pages 13 & 14 in the packet  HW: page 15 in the packet

25. Colligative Properties  Colligative properties are physical properties of solutions that depend on the concentration of solute in a given amount of solvent  Dependent on how much solute is present, which is influenced by the nature of the solute  Greater concentration gives greater effects  Colligative properties are physical properties of solutions that depend on the concentration of solute in a given amount of solvent  Dependent on how much solute is present, which is influenced by the nature of the solute  Greater concentration gives greater effects

26. Electrolytes  Electrolytes are substances that separate to produce ions when dissolved in a solution  Conduct electricity, turn on light bulb tester  Ex: ionic compounds (salts), acids, bases  Nonelectrolytes do not produce ions (stay in one piece) in solution  Do not conduct electricity, do not turn on light bulb tester  Ex: sugars, alcohols  Electrolytes are substances that separate to produce ions when dissolved in a solution  Conduct electricity, turn on light bulb tester  Ex: ionic compounds (salts), acids, bases  Nonelectrolytes do not produce ions (stay in one piece) in solution  Do not conduct electricity, do not turn on light bulb tester  Ex: sugars, alcohols

27. Electrolytes vs. Nonelectrolytes  Electrolytes  Nonelectrolytes  Electrolytes  Nonelectrolytes

28. Electrolyte or Nonelectrolyte?  Electrolytes  Ionic substances  Acids: X-H  Bases M-OH  Electrolytes  Ionic substances  Acids: X-H  Bases M-OH  Nonelectrolytes  Sugars  Alcohols

29. Colligative Properties  Boiling Point Elevation  the temperature at which a liquid normally boils goes up when solute particles are dissolved  Freezing Point Depression  the temperature at which a liquid normally freezes goes down when solute particles are dissolved  Boiling Point Elevation  the temperature at which a liquid normally boils goes up when solute particles are dissolved  Freezing Point Depression  the temperature at which a liquid normally freezes goes down when solute particles are dissolved

30. Boiling Point Elevation  The boiling point of a solution increases when solute particles are added  Example:  Adding salt to water raises the water’s boiling point  Water now gets hotter than 100° C (102-103°) before it boils, and pasta will cook faster  The boiling point of a solution increases when solute particles are added  Example:  Adding salt to water raises the water’s boiling point  Water now gets hotter than 100° C (102-103°) before it boils, and pasta will cook faster

31. Freezing Point Depression  The freezing point of a solution decreases when solute particles are added  Example:  Putting salt on roads causes ice to melt  Ice’s freezing point becomes lower than 0°, so water stays liquid at temperatures where it would normally be solid ice  The freezing point of a solution decreases when solute particles are added  Example:  Putting salt on roads causes ice to melt  Ice’s freezing point becomes lower than 0°, so water stays liquid at temperatures where it would normally be solid ice

32. Vapor Pressure  When a substance that is normally solid or liquids at room temperature enters the gas phase, it is called a vapor  Pressure exerted by this vapor is vapor pressure  When a substance that is normally solid or liquids at room temperature enters the gas phase, it is called a vapor  Pressure exerted by this vapor is vapor pressure

33. Do Now and HW  Now: Complete pages 16 to 18 of the packet  HW: Complete pages 24 and 25 of the packets  Now: Complete pages 16 to 18 of the packet  HW: Complete pages 24 and 25 of the packets

34. Concentration  Concentration is the amount of solute dissolved in a solution  Several ways to express concentration:  Grams solute/100mL solvent (Table G)  % composition by mass  % composition by volume  Parts per Million  Molarity  Concentration is the amount of solute dissolved in a solution  Several ways to express concentration:  Grams solute/100mL solvent (Table G)  % composition by mass  % composition by volume  Parts per Million  Molarity

35. Percent Composition  Labels often list ingredients as a percent by mass or percent by volume

36. Percent Composition by Mass and by Volume Ratio of the mass (or volume) of one part compared to the mass (or volume) of the whole Used w/ solids Used w/ liquids

37. Percent Composition  What is the percent by mass of sodium hydroxide if 5g of NaOH are added to 50g of water?  What is the percent by volume of alcohol is 50mL of ethanol is diluted with water to form a total volume of 3000mL?  What is the percent by mass of sodium hydroxide if 5g of NaOH are added to 50g of water?  What is the percent by volume of alcohol is 50mL of ethanol is diluted with water to form a total volume of 3000mL?

38. Parts Per Million (ppm)  If you divide a pie into 10 equal pieces, each piece is a part-per-ten (1/10th)  Divide the pie into a million pieces, and each piece is a part per million, (1/1,000,000th)

39. Parts Per Million (ppm)  Similar to percent composition, parts per million is a ratio between mass of the solute and the total mass of solution  Useful for very dilute solutions  In swimming pools, only 2g of chlorine for every 2 million g of water  Similar to percent composition, parts per million is a ratio between mass of the solute and the total mass of solution  Useful for very dilute solutions  In swimming pools, only 2g of chlorine for every 2 million g of water

40.  At 40 C, carbon dioxide has a solubility of 0.0972g/100g H 2 O. What is the concentration of CO 2, expressed in parts per million?

41.  A substance has a solubility of 350ppm. How many grams of the substance are present in 1.0L of a saturated solution?

42.  Now: find review book q’s  HW: complete page 27 of the packet  Now: find review book q’s  HW: complete page 27 of the packet

43. Molarity (M)  Measures concentration in moles  Higher molarity = more concentrated  Important to note that molarity is moles of solute per liter of solution, not solvent

44. Molarity (M)  Example: What is the molarity of a solution that contains 4.0 moles of NaOH in 0.50 L of solution?

45.  Now: complete pages 21 and 22 of the packet  HW: complete page 26 of the packet  Now: complete pages 21 and 22 of the packet  HW: complete page 26 of the packet