1. Chapter 15 Solutions

2. 1.To understand the process of dissolving 2.To learn why certain substances dissolve in water 3.To learn qualitative terms describing the concentration of a solution 4.To understand the factors that affect the rate at which a solid dissolves Objectives Section 1 – Homogenous and Heterogeneous Solutions

3. Forming solutions Solution = homogeneous mixture Can be solid, liquid, or gas Solute = Solvent = – Aqueous solution

5. Solubility Solubility of ionic substances – Strong attractive forces that hold ionic crystal together are overcome by the strong attraction between the ionic crystal and the water molecule

6. – When ionic compounds dissolve they break into individual ions NaCl CaCl 2

7. Solubility of polar substances – Polar molecules can form hydrogen bonds with water and dissolve – Like dissolves like

9. Substances insoluble in water – Nonpolar molecules will not dissolve in water – Water-water hydrogen bonds keep the water from mixing with the nonpolar molecules

10. How substances dissolve – A “hole” must be made in the water structure for each solute particle. – The lost water-water interactions must be replaced by water-solute interactions. – “like dissolves like”

11. Solution Composition Saturated – solution contains as much solute as will dissolve at that temperature – If more solute is added it will not dissolve Unsaturated – solution that has not reached the limit of solute that will dissolve in it. – If more solute is added it will dissolve

12. Supersaturated - occurs when a solution is saturated at an elevated temperature and then allowed to cool but all of the solid remains dissolved Contains more dissolved solute than a saturated solution Very unstable

13. Solution Composition: An Introduction A supersaturated solution is clear before a seed crystal is added.

14. Solution Composition: An Introduction Crystals begin to form in the solution immediately after the addition of a seed crystal.

15. Solution Composition: An Introduction Excess solute crystallizes rapidly.

16. Solution concentration = the amount of solute in a given amount of solution Qualitative measurements of solution concentration – Concentrated – lots of solute – Dilute – not a lot of solute

17. Solution Composition: An Introduction Which solution is more concentrated?

18. Solution Composition: An Introduction Which solution is more concentrated?

19. Factors affecting the rate of dissolving Surface area – dissolving occurs at surface of substance being dissolved Stirring – removes newly dissolved particles from the solute surface and continuously exposes the surface to fresh solvent Temperature - molecules moving more rapidly, more interaction between solvent and solute

20. 1. To understand mass percent and how to calculate it 2. To understand and use molarity 3. To learn to calculate the concentration of a solution made by diluting a stock solution Objectives Section 2 – Concentration of Solutions

21. Solution Composition: Mass Percent

22. A solution is prepared by mixing 1.00 g of ethanol with 100.0 g of water. Calculate the mass percent of ethanol in this solution

23. Cow’s milk typically contains 4.5% by mass of lactose, calculate the mass of lactose in 175 g of milk.

24. Solution Composition: Molarity

25. What is the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in 1500 mL of solution?

26. Give the concentration of the ions in a 0.50 M solution of Co(NO 3 ) 2

27. How man moles of Ag + ions are present in 25 mL of a 0.75 M AgNO 3 solution?

28. Solution Composition: Molarity Standard solution - a solution whose concentration is accurately known To make a standard solution –Weigh out a sample of solute. –Transfer to a volumetric flask. –Add enough solvent to mark on flask.

29. Molarity 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.

30. Molarity Swirl the flask carefully to dissolve the solute.

31. Molarity Fill the flask with water exactly to the 1-L mark.

32. A chemist needs 1.00 L of 0.200 M K 2 Cr 2 O 7 solution. How much solid K 2 Cr 2 O 7 (molar mass = 294.2 g/mol) must be weighed out to make this solution?

33. Dilution Water can be added to an aqueous solution to dilute the solution to a lower concentration. Only water is added in the dilution – the amount of solute is the same in both the original and final solution.

34. Diluting a solution – Transfer a measured amount of original solution to a flask containing some water. – Add water to the flask to the mark (with swirling) and mix by inverting the flask.

35. Making Dilutions The total number of moles of solute remains unchanged upon dilution, so you can write this equation. 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.

36. If we want to prepare 500. mL of 1.00 M acetic acid from a 17.5 M stock solution, what volume of the stock solution is required?

37. 1.To learn to solve stoichiometric problems involving solution reactions 2.To do calculations involving acid-base reactions 3.To learn about normality and equivalent weight 4.To use normality in stoichiometric calculations 5.To understand the effect of a solute on solution properties Objectives Section 3 – Properties of Solutions

38. Stoichiometry of Solution Reactions

39. Calculate th mass of solid NaCl that must be added to 1.50 L of a 0.100 M AgNO 3 solution to precipitate all of the Ag + ions in the form of AgCl. Calculate the mass of AgCl formed.

40. When Ba(NO 3 ) 2 and K 2 CrO 4 react in aqueous solution the yellow solid BaCrO 4 is formed. Calculate the mass of BaCrO 4 that forms when 3.50 x 10 -3 mol of solid Ba(NO 3 ) 2 is dissolved in 265 mL of 0.0100 M K 2 CrO 4 solution.

41. Neutralization Reactions An acid-base reaction is called a neutralization reaction. Steps to solve these problems are the same as before.

42. What volume of a 0.100 M HCl solution is needed to neutralize 25.0 mL of a 0.350 M NaOH solution?

43. Normality Unit of concentration – One equivalent of acid – amount of acid that furnishes 1 mol of H + ions – One equivalent of base – amount of base that furnishes 1 mol of OH  ions – Equivalent weight – mass in grams of 1 equivalent of acid or base

44. Normality

46. Phosphoric acid, H 3 PO 4 can furnish three H+ ions per molecule. Calculate the equivalent weight of H 3 PO 4

47. Normality To find number of equivalents

48. A solution of sulfuric acid contains 86g of H 2 SO 4 per liter of solution. Calculate the normality of the solution.

49. Colligative properties a solution property that depends on the number of solute particles present The presence of solute “particles” causes the liquid range to become wider. – Boiling point increases – Freezing point decreases

50. Vapor pressure lowering – – Vapor pressure: – Adding a nonvolatile solute to a solution lowers the solvent’s vapor pressure

51. Boiling point elevation – – Boiling point – Because vapor pressure is lowered, boiling point increases

52. Freezing point depression – solute particles interfere with attractive forces holding solvent particles together