1. Solutions and Solubility Chapters 15 and 16

2. Solution Homogeneous Mixture Uniform Throughout

3. Solution Components Solvent Dissolving medium in mixture Solute Dissolved particles in solution Aqueous Solution Solution with water as the solvent NaCl (aq)

4. Solubility measure of the amount of solute that can dissolve in a given quantity of solvent at certain conditions

5. Solubility Soluble Solute will dissolve in solvent Insoluble Solute will not dissolve in solvent

6. Factors that affect Solubility Temperature Pressure Chemical Nature

7. Temperature increasing temperature increases solubility of solids and liquids in other solids and liquids decreasing temperature increases solubility of gases in liquids Ex: Cold soda is fizzy

8. Pressure Increasing partial pressure of gas above liquid increases solubility of the gas in the liquid Example Soda Bottles

9. Chemical Nature “Like dissolves Like” Polar and ionic substances will dissolve in polar solvents Nonpolar substances will dissolve in nonpolar solvents

11. Solutions Concentrated General term for a lot of solute dissolved in solvent Dilute General term for not a lot of solute dissolved in solvent Opposite of concentrated

12. Table G Shows the relationship between temperature and amount of solute for a number of different compounds

13. Table G How much NaNO 3 can dissolve in 100g of H 2 O at 50°C? 115g

14. Table G At what temperature can 60g of NH 4 Cl dissolve in 100g of H 2 O? 65°C

16. Types of Solution Saturated maximum amount of solute for a given quantity of solvent At Equilibrium Unsaturated contains less than the maximum amount of solute Supersaturated Contains more solute than it can theoretically hold

17. Supersaturated Solutions Begins as saturated solution at high temp As solution cools, with no disturbance, solubility decreases Any disturbance, or place for a crystal to grow, will cause any excess solute to precipitate out back to a saturated solution

18. Solution Types Saturated On the line Unsaturated Under the line Supersaturated Above the line

20. Electrolytes Compounds that conduct an electrical current when dissolved or in a molten state (melted) Ionic compounds Including acids and bases NaCl, KNO 3, HCl

21. Dissolving vs. Dissociation Dissolving Molecules separate as solvent molecules mix C 6 H 12 O 6 (s) + H 2 O(l)  C 6 H 12 O 6 (aq) Dissociation Ions separate as solvent molecules mix NaCl(s) + H 2 O(l)  Na + (aq) + Cl - (aq)

22. Dissociation Simulation http://phet.colorado.edu/simulations/sims.php?sim=Salts_and_Solubility

24. Concentration Quantitative measure of the amount of solute dissolved in a given quantity of solvent Molarity Percent Composition by mass, by volume Parts Per Million (ppm)

25. Molarity Molarity = Moles of Solute Liters of Solution 1 mol/L = 1 M Often used for solids dissolved into liquids Most common concentration system

26. Molarity Example What is the molarity of 2 moles of glucose dissolved in 5 Liters of solution? Molarity = Moles of Solute Liters of Solution

27. Example How many moles of HCl are dissolved in 4L of a 3M solution of HCl? Molarity = Moles of Solute Liters of Solution

28. Example What volume of a 6M solution contains 0.6moles of NaCl? Molarity = Moles of Solute Liters of Solution

30. Percent Composition Percent Comp = Part x 100% Whole By mass %(m/m) Usually used for solid - solid solutions By Volume %(v/v) Usually used for liquid - liquid solutions

31. (v/v) Example A solution contains 60 mL of NH 3 in a 1 Liter solution, what is the percent by volume composition of this solution?

33. Parts Per Million (ppm) Used for very small concentrations ppm = grams of solute x 1,000,000 grams of solution Units = ppm

34. ppm example A 2 kg bar of silver contains 0.05 g of gold, what is the parts per million concentration of gold in the silver bar? 25 ppm Au

35. Example A bar of tantalum has a niobium concentration of 16ppm. How much does the bar weigh if the niobium weighs 0.004g?

37. Colligative Properties of Solutions Properties of a solution that depend only on the number of particles dissolved Vapor Pressure Boiling Point Melting Point

38. Vapor Pressure Pressure exerted by a vapor that has evaporated and is still above a liquid More solute particles get in the way of solvent particles trying to evaporate Adding more nonvolatile solute particles to pure solvent decreases vapor pressure

39. Boiling Point Temperature at which a liquid boils at a given pressure, related to vapor pressure. More solute particles get in the way of solvent particles trying to escape liquid phase Adding more solute particles to pure solvent increases boiling point

40. Freezing Point Temperature at which a liquid freezes, or the particles line up in an orderly pattern. More solute particles get in the way of the solvent particles trying to line up. Adding more solute particles to pure solvent decreases freezing point

41. Number of Particles When a covalent compound dissolves the compound stays intact. When an ionic compound dissociates the compound splits into its ions.

42. Examples When glucose, C 6 H 12 O 6, dissolves it will split into how many particles? 1, C 6 H 12 O 6 When NaCl dissociates it will split into how many particles? 2, Na + and Cl - When CaCl 2 dissociates it will split into how many particles? 3, Ca 2+, Cl -, and Cl -

43. Example For a 2M solution of each glucose, NaCl, and CaCl 2 SubstancecalculationChange in Temp Glucose(2M)(1particle)2 NaCl(2M)(2particles)4 CaCl 2 (2M)(3particles)6

44. Real Life Why do we put salt on roads in winter? Salt lowers freezing point, ice melts Which is better NaCl or CaCl 2 ? CaCl 2, more particles Why do some people use salt when cooking pasta? (Besides Taste) Raises boiling point, cooks at higher temperature