1. Solution Formation The compositions of the solvent and the solute determine whether a substance will dissolve. The factors that determine how fast a substance dissolves are stirring (agitation) temperature the surface area of the dissolving particles 16.1

2. Solubility A saturated solution contains the maximum amount of solute for a given quantity of solvent at a given temperature and pressure. An unsaturated solution contains less solute than a saturated solution at a given temperature and pressure. 16.1

3. Factors Affecting Solubility A supersaturated solution contains more solute than it can theoretically hold at a given temperature. The crystallization of a supersaturated solution can be initiated if a very small crystal, called a seed crystal, of the solute is added. 16.1

4. Solubility In a saturated solution, the rate of dissolving equals the rate of crystallization, so the total amount of dissolved solute remains constant. 16.1

5. Solubility Some liquids combine in all proportions, while others don’t mix at all. Two liquids are miscible if they dissolve in each other in all proportions. Two liquids are immiscible if they are insoluble in each other. 16.1

6. Factors Affecting Solubility Temperature The solubility of most solid substances increases as the temperature of the solvent increases. The solubilities of most gases are greater in cold water than in hot. 16.1

7. Factors Affecting Solubility 16.1

8. Molarity a.The concentration of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent. A dilute solution is one that contains a small amount of solute. A concentrated solution contains a large amount of solute. 16.2

9. Molarity a.Molarity (M) is the number of moles of solute dissolved in one liter of solution. b.To calculate the molarity of a solution, divide the moles of solute by the volume of the solution. 16.2

10. Molarity 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. 16.2

11. Molarity a.Swirl the flask carefully to dissolve the solute. 16.2

12. Molarity a.Fill the flask with water exactly to the 1-L mark. 16.2

15. 16.3

16. Sample Problem 16.3 16.3

17. Making Dilutions Diluting a solution reduces the number of moles of solute per unit volume, but the total number of moles of solute in solution does not change. 16.2

18. Making Dilutions a.The total number of moles of solute remains unchanged upon dilution, so you can write this equation. a.M 1 and V 1 are the molarity and volume of the initial solution, and M 2 and V 2 are the molarity and volume of the diluted solution. 16.2

19. 16.4

22. Making Dilutions 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. 16.2

23. Making Dilutions a.She then transfers the 20 mL to a 100-mL volumetric flask. 16.2

24. Making Dilutions a.Finally she carefully adds water to the mark to make 100 mL of solution. 16.2

25. Percent Solutions Concentration in Percent (Volume/Volume) 16.2

26. Percent Solutions Concentration in Percent (Mass/Mass) 16.2

27. Molality and Mole Fraction a.The molality (m) is the number of moles of solute dissolved in 1 kilogram (1000 g) of solvent. Molality is also known as molal concentration. 16.4