1. SOLUTIONS Chapter 15

2. Solution = homogeneous mixture Solute = gets dissolved (minor component) Solvent = dissolving agent (major component)

4. A substance that dissolves in a solvent is said to be soluble. These two substances are miscible.

5. A substance that does not dissolve in a solvent is insoluble. These two substances are immiscible.

6. (See Table 15-1, p.454) Page 454 in Book

7. Solvation = the process of surrounding solute particles with solvent particles to form a solution. Solute particles must separate from one another and the solute and solvent particles must mix.

8. “Like dissolves like.” Polar solutes dissolve in polar solvents Nonpolar solutes dissolve in nonpolar solvents

9. Water is polar and dissolves many ionic and polar substances.

10. Salt is ionic and dissolves in water.

11. Table sugar is polar and dissolves in water.

12. Water is an excellent solvent. It is the “universal solvent.” Solutions made with water are called aqueous solutions.

13. Factors that affect rate of solvation Stirring the mixture Increasing the surface area of the solute Increasing the temperature of the solvent Increasing the pressure when dissolving a gas

14. Solubility = maximum amount of solute that will dissolve in a given amount of solvent at a specified temperature and pressure Saturated = maximum amount of solute is dissolved Unsaturated = more solute can be dissolved Supersaturated = contains more dissolved solute than a saturated solution at the same temperature.

16. Factors that affect solubility Increased Temperature – solubility of solids increases; solubility of gases decreases. Increased Pressure – solubility of gases increases. (This process is called aeration) Henry’s Law –at a given temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas above the liquid.

17. Ch.15.2- Solution Concentration The concentration of a solution is a measure of how much solute is dissolved in a specific amount of solvent or solution. solute or solute solvent solution (solution = solute + solvent)

18. Expressing Concentration Concentration may be described qualitatively as concentrated or dilute.

19. Concentration= solute or solute solvent solution

20. Percent by Mass (p.463 #8) What is the percent by mass of NaHCO 3 in a solution containing 20 g NaHCO 3 dissolved in 600 mL H 2 O? Density of H 2 O = 1.00 g/mL % by mass = 20 g x 100 = 3.2% 620 g

21. Percent by Mass (p.463 #9) You have 1500.0 g of a bleach solution. The percent by mass of the solute sodium hypochlorite, NaOCl, is 3.62%. How many grams of NaOCl are in the solution? % Mass = mass solute x 100 mass solution 3.62 = x g X 100 1500.0 g x = 54.3 g NaOCl

22. Percent by Volume (p.464 #12) If you have 100.0 mL of a 30.0% aqueous solution of ethanol, what volumes of ethanol and water are in the solution? % Volume = volume of solute x 100% volume of solution 30.0 % = x mL x 100 100.0 mL x = 30 mL ethanol 70 mL water

23. Molarity (p.465 #14) What is the molarity of an aqueous solution containing 40.0 g of glucose (C 6 H 12 O 6 ) in 1.5 L of solution? 1 mole C 6 H 12 O 6 = 180.16 g 40.0 g C 6 H 12 O 6 x 1 mole = 0.222 mol 180.16 g Molarity = 0.222 mol = 0.15 M C 6 H 12 O 6 1.5 liter

24. Molarity (p.465 #15) What is the molarity of a bleach solution containing 9.5 g NaOCl per liter of bleach?

25. Molarity (p.465 #16) Calculate the molarity of 1.60 L of a solution containing 1.55 g of dissolved KBr.

26. Molarity (p.466 #17) How many grams of CaCl 2 would be dissolved in 1.0 L of a 0.10 M solution of CaCl 2 ?

27. Molarity (p.466 #18) A liter of 2M NaOH solution contains how many grams of NaOH?

28. Molarity (p.466 #19) How many grams of CaCl 2 should be dissolved in 500.0 mL of water to make a 0.20M solution of CaCl 2 ?

29. Molarity (p.466 #20) How many grames of NaOH are in 250 mL of a 3.0M NaOH solution?

30. Diluting Solutions- p.467 In the laboratory, you may use concentrated solutions called stock solutions. For example, concentrated hydrochloric acid (HCl) is 12 M. You can dilute the stock solution by adding more solvent. Would you still have the same number of moles of solute particles that were in the stock solution?

31. Diluting Solutions- p.467 Molarity (M) = moles solute liters solution moles solute = Molarity x liters solution Because the total number of moles of solute does not change during dilution, moles solute in stock solution = moles solute after dilution M 1 V 1 = M 2 V 2

32. Diluting Solutions- p.468 #21 What volume of a 3.00 M KI stock solution would you use to make 0.300 L of a 1.25 M KI solution?

33. Diluting Solutions- p.468 #23 If you dilute 20.0 mL of a 3.5 M solution to make 100.0 mL of solution, what is the molarity of the dilute solution?

34. Molality- p.469 Molality (m) = moles solute = moles solute kilogram solvent 1000 g solvent What is the molality of a solution containing 10. 0 g Na 2 SO 4 dissolved in 1000.0 g of water? What is the molality of a solution containing 30.0 g of naphthalene dissolved in 500.0g of toluene?

35. Mole Fraction- p.470

36. Mole Fraction- p.470 #26 What is the mole fraction of NaOH in an aqueous solution that contains 22.8% NaOH by mass?

37. Mole Fraction- p.470 #27 An aqueous solution of NaCl has a mole fraction of 0.21. What is the mass of NaCl dissolved in 100.0 mL of solution?

38. Parts per million (ppm)