1. Chapter 18 Solutions

2. Section 18.1 Properties of Solutions l OBJECTIVES: – Identify the factors that determine the rate at which a solute dissolves.

3. Section 18.1 Properties of Solutions l OBJECTIVES: – Calculate the solubility of a gas in a liquid under various pressure conditions.

4. Solution formation l Nature of the solute and the solvent – Whether a substance will dissolve – How much will dissolve l Factors determining rate of solution... – stirred or shaken (agitation) – particles are made smaller – temperature is increased l Why?

5. Making solutions l In order to dissolve, the solvent molecules must come in contact with the solute. l Stirring moves fresh solvent next to the solute. l The solvent touches the surface of the solute. l Smaller pieces increase the amount of surface area of the solute.

6. Temperature and Solutions l Higher temperature makes the molecules of the solvent move around faster and contact the solute harder and more often. – Speeds up dissolving. l Usually increases the amount that will dissolve (exception is gases)

7. How Much? l Solubility- The maximum amount of substance that will dissolve at a specific temperature (g solute/100 g solvent) l Saturated solution- Contains the maximum amount of solute dissolved l Unsaturated solution- Can still dissolve more solute l Supersaturated- solution that is holding more than it theoretically can; seed crystal will make it come out; Fig. 18.7, p.506

8. Liquids l Miscible means that two liquids can dissolve in each other – water and antifreeze, water and ethanol l Partially miscible- slightly – water and ether l Immiscible means they can’t – oil and vinegar

9. Solubility? l For solids in liquids, as the temperature goes up-the solubility usually goes up (Fig. 18.4, p.504) l For gases in a liquid, as the temperature goes up-the solubility goes down l For gases in a liquid, as the pressure goes up-the solubility goes up

10. Gases in liquids... l Henry’s Law - says the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid – think of a bottle of soda pop, removing the lid releases pres. l Equation: S 1 S 2 P 1 P 2 =

11. Cloud seeding l Ever heard of seeding the clouds to make them produce rain? l Clouds- mass of air supersaturated with water vapor l Silver Iodide (AgI) crystals are dusted into the cloud l The AgI attracts the water, forming droplets to attract others

12. Section 18.2 Concentration of Solutions l OBJECTIVES: – Solve problems involving the molarity of a solution.

13. Section 18.2 Concentration of Solutions l OBJECTIVES: – Describe how to prepare dilute solutions from more concentrated solutions of known molarity.

14. Section 18.2 Concentration of Solutions l OBJECTIVES: – Explain what is meant by percent by volume [ % (v/v) ], and percent by mass [ % (m/v) ] solutions.

15. Concentration is... l a measure of the amount of solute dissolved in a given quantity of solvent l A concentrated solution has a large amount of solute l A dilute solution has a small amount of solute – thus, only qualitative descriptions l But, there are ways to express solution concentration quantitatively

16. Molarity - most important l The number of moles of solute in 1 Liter of the solution. l M = moles/Liter; such as 6.0 molar l What is the molarity of a solution with 2.0 moles of NaCl in 250 mL of solution? l Sample 18-2, page 510

17. Making solutions l Pour in a small amount of solvent l Then add the solute (to dissolve it) l Carefully fill to final volume. – Fig. 18-10, page 509 l Also: M x L = moles l How many moles of NaCl are needed to make 6.0 L of a 0.75 M NaCl solution?

18. Making solutions l 10.3 g of NaCl are dissolved in a small amount of water, then diluted to 250 mL. What is the concentration? l How many grams of sugar are needed to make 125 mL of a 0.50 M C 6 H 12 O 6 solution?

19. Dilution Adding water to a solution

20. Dilution l The number of moles of solute doesn’t change if you add more solvent! l The # moles before = the # moles after l M 1 x V 1 = M 2 x V 2 l M 1 and V 1 are the starting concentration and volume. l M 2 and V 2 are the final concentration and volume. l Stock solutions are pre-made to known Molarity

21. Practice l 2.0 L of a 0.88 M solution are diluted to 3.8 L. What is the new molarity? l You have 150 mL of 6.0 M HCl. What volume of 1.3 M HCl can you make? l Need 450 mL of 0.15 M NaOH. All you have available is a 2.0 M stock solution of NaOH. How do you make the required solution?

22. Percent solutions... l Percent means parts per 100, so l Percent by volume: = Volume of solute x 100% Volume of solution l indicated %(v/v) l What is the percent solution if 25 mL of CH 3 OH is diluted to 150 mL with water?

23. Percent solutions l Percent by mass: = Mass of solute(g) x 100% Volume of solution(mL) l Indicated %(m/v) l More commonly used l 4.8 g of NaCl are dissolved in 82 mL of solution. What is the percent of the solution? l How many grams of salt are there in 52 mL of a 6.3 % solution?

24. Section 18.3 Colligative Properties of Solutions l OBJECTIVES: – Explain on a particle basis why a solution has a lower vapor pressure than the pure solvent of that solution.

25. Section 18.3 Colligative Properties of Solutions l OBJECTIVES: – Explain on a particle basis why a solution has an elevated boiling point, and a depressed freezing point compared with the pure solvent.

26. Colligative Properties Depend only on the number of dissolved particles Not on what kind of particle

27. Vapor Pressure decreased l The bonds between molecules keep molecules from escaping. l In a solution, some of the solvent is busy keeping the solute dissolved. l Lowers the vapor pressure l Electrolytes form ions when they are dissolved = more pieces. NaCl  Na + + Cl - (= 2 pieces) l More pieces = bigger effect

28. Boiling Point Elevation l The vapor pressure determines the boiling point. l Lower vapor pressure = higher boiling point. l Salt water boils above 100ºC l The number of dissolved particles determines how much, as well as the solvent itself.

29. Freezing Point Depression l Solids form when molecules make an orderly pattern. l The solute molecules break up the orderly pattern. l Makes the freezing point lower. l Salt water freezes below 0ºC l How much depends on the number of solute particles dissolved.

30. Section 18.4 Calculations Involving Colligative Properties l OBJECTIVES: – Calculate the molality and mole fraction of a solution.

31. Section 18.4 Calculations Involving Colligative Properties l OBJECTIVES: – Calculate the molar mass of a molecular compound from the freezing point depression or boiling point elevation of a solution of the compound.

32. Molality l a new unit for concentration l m = Moles of solute kilogram of solvent l m = Moles of solute 1000 g of solvent l What is the molality of a solution with 9.3 mole of NaCl in 450 g of water?

33. Why molality? l The size of the change in boiling point is determined by the molality.  T b = K b x m x n  T b is the change in the boiling point l K b is a constant determined by the solvent (Table 18.2, page 523). l m is the molality of the solution. l n is the number of pieces it falls into when it dissolves.

34. What about Freezing? l The size of the change in freezing point is also determined by molality.  T f = -K f x m x n  T f is the change in freezing point l K f is a constant determined by the solvent (Table 18.3, page 524). l m is the molality of the solution. l n is the number of pieces it falls into when it dissolves.

35. Problems l What is the boiling point of a solution made by dissolving 1.20 moles of NaCl in 750 g of water? l What is the freezing point? l What is the boiling point of a solution made by dissolving 1.20 moles of CaCl 2 in 750 g of water? l What is the freezing point?

36. Mole fraction l This is another way to express concentration l It is the ratio of moles of solute to total number of moles of solute + solvent (Fig. 18-19, p.522) n a n a + n b X = Sample 18-8, page 521

37. Molar Mass l We can use changes in boiling and freezing to calculate the molar mass of a substance l Find: 1) molality 2) moles, and then 3) molar mass l Sample 18-10, page 524