2. What are some special properties of solutions? Chemistry Unit 11

3. Main Ideas Mixtures can be either heterogeneous or homogeneous Concentration can be expressed in terms of percent or in terms of moles Factors such as temperature, pressure, and polarity affect the formation of solutions Colligative properties depend on the number of solute particles in a solution

4. Types of Mixtures 11.1

5. Objectives Compare the properties of suspensions, colloids, and solutions Identify types of colloids and types of solutions. Describe the electrostatic forces in colloids

6. Types of Mixtures Heterogeneous Mixtures are a combination of two or more pure substances in which each pure substance retains its individual properties. There are two main types of heterogeneous mixtures:

7. Types of Mixtures 1.Suspensions – A suspension is a mixture containing particles that settle out if left undisturbed but, when stirred, the substance will flow like a liquid. These substances are called thixotropic. These particles can be filtered out. These substances are called thixotropic. These particles can be filtered out. Example : muddy water

8. Types of Solutions 2.Colloids – A colloid is made of smaller sizes of suspension particles and these particles do not settle out. Particles cannot be filtered out. The most abundant substance in a mixture is the dispersion medium. Example: Milk Colloids are categorized according to the phases of their particles. Colloids are categorized according to the phases of their particles.

9. Types of Colloids

10. Colloids The dispersed particles in a colloid are prevented from settling out because they often have polar or charged atomic groups on their surfaces. This results in the formation of electrostatic layers around the particles. The layers electrostatically repel each other when the dispersed particles collide, thus, the particles remain in the colloid.

11. Colloids If you interfere with the electrostatic layering, colloid particles will settle out of the mixture. Heating also destroys a colloid because it gives colliding particles enough kinetic energy to overcome the electrostatic forces and settle out.

12. Brownian Motion Brownian motion is the jerky, random movements of particles in a liquid colloid, from the results of particle collisions.

13. Tyndall Effect Concentrated colloids are often cloudy or opaque. Dilute colloids sometimes appear as clear as solutions. Dilute colloids appear to be homogeneous solutions because their dispersed particles are so small. The Tyndall effect is when dispersed colloid particles scatter light. The Tyndall effect is when dispersed colloid particles scatter light. Examples: sunlight through smoke filled air or fog

14. Homogeneous Mixtures A homogeneous mixture is a solution of two or more substances that blend easily and constant composition throughout. There are different types of homogeneous solutions: A solution might exist as a gas, a liquid, or a solid, depending on the state of its solvent. Water is the most common liquid solvent. Examples: salt water and steel

15. Types of Solutions

16. Forming Solutions Some combinations of substances readily form solutions, and others do not. A substance that dissolves in a solvent is said to be soluble in that solvent. Example: Sugar in water Two liquids that are soluble in each other are called miscible.

17. Forming Solutions A substance that does not dissolve in a solvent is said to be insoluble. Two liquids that cannot be mixed together but separate shortly after are said to be immiscible

18. Questions Miscible substances are: A.two liquids that are not soluble in each other B.solids that dissolve in liquids C.solids that do not dissolve in liquids D.two liquids that are soluble in each other

19. Questions The jerky, random movement of particles in a liquid colloid is known as ____. A.Brownian motion B.Tyndall effect C.Charles’s Law D.kinetic energy

20. Homework CALM 11.1 p 479 #2, 4, 6,7

21. Solution Concentration 11.2

22. Objectives Describe concentration using different units Determine the concentrations of solutions Calculate the molarity of a solution.

23. Expressing Concentration Concentration can be expressed in terms of percent or in terms of moles. The concentration of a solution is a measure of how much solute is dissolved in a specific amount of solvent or solution. concentration

24. Expressing Concentration

25. Practice Problem #1 In order to maintain a sodium chloride (NaCl) concentration similar to ocean water, an aquarium must contain 3.6g NaCl per 100g of water. What is the percent by mass of NaCl in the solution? Answer: 3.5%

26. Molarity MolarityMolarity is the number of moles of solute dissolved per liter of solution. Molarity Dilution equation: M 1 V 1 = M 2 V 2

27. Practice Problem #2 A 100.5 ml intravenous (IV) solution contains 5.10 g of glucose (C 6 H 12 O 6 ). What is the molarity of this solution? Ans: 0.282M

28. Practice Problem #3 If you needed to make a 1.0 M solution of CaCl 2, how many grams would you need to make 500 ml of it? 5.5g

29. Practice Problem#4: Dilution What volume of 2.00 M calcium chloride stock solution would you use to make 0.50 L of 0.300 M calcium chloride solution? 75 ml or.075L

30. Molality MolalityMolality is the ratio of moles of solute dissolved in 1 kg of solvent. Molality

31. Practice Problem #5 In the lab, a student adds 4.5g of sodium chloride (NaCl) to 100.0g of water. Calculate the molality of the solution. 0.77 mol/kg

32. Mole Fraction Mole fractionMole fraction is the ratio of the number of moles of solute in solution to the total number of moles of solute and solvent. Mole fraction where X A and X B represent mole fractions of each substance

33. Practice Problem #6 100 g of a hydrochloric acid solution contains 36 g of HCl and 64 g of H 2 O. What are the mole fractions of HCl and water?.22 HCl.78 H 2 O

34. Question Which is NOT a quantitative measure of concentration? A.molarity B.molality C.percent by mass D.dilute

35. Question The number of moles of solute divided by liters of solvution is called ____. A.molarity B.molality C.percent by volume D.percent by mass

36. Homework CALM 11.2 p481-483 #9,10, 16-18 p485-487 # 20-22, 24, 25, 27, 29

37. Factors Affecting Solvation 11.3

38. Objectives Describe how intermolecular forces affect solvation. Define solubility. Understand what factors affect solubility.

39. Solvation The process of surrounding solute particles with solvent particles to form a solution is called solvation. Solvation in water is called hydration. “like dissolves like”

40. Solvation

41. Factors that Affect Solvation Agitation – shaken or stirred – agitation of the mixture allows for more contact between solute and solvent. Surface area – breaking the solute into small pieces helps solvation. A greater surface area allows more collisions to occur.

42. Factors that Affect Solvation Temperature – As temperature increases, the rate of solvation also increases. Additionally, hotter solvents generally can dissolve more solid solute.

43. Solubility Solubility is the ability of a solvent to dissolve a solute. In an aqueous solution, a precipitate forms when a mixture produces an insoluble product.

44. Solubility Guidelines 1.All common salts of the group 1 elements and ammonium ions are soluble. 2.All common acetates and nitrates are soluble. 3.All binary compounds of group 17 elements (other than F) with metals are soluble except hoes of silver, mercury (I), and lead.

45. Solubility Guidelines 4.All sulfates are soluble except those of barium, strontium, lead, calcium, silver, and mercury (I). 5.Except for those in Rule 1, carbonates, hydroxides, oxides, sulfides, and phosphates are insoluble.

46. Practice Problem #7 Which of the following substances would be a precipitate in an aqueous solution? Why? a)NaCl b)CaCO 3 c)Fe(NO 3 ) d)KOH

47. Solubility Unsaturated solutions – An unsaturated solution is one that contains less dissolved solute than the solvent can handle at a certain temperature and pressure. In other words, more solute can be dissolved in an unsaturated solution.

48. Solubility Saturated solution – The maximum amount of solute has been dissolved in the solvent. The amount of crystallization is at equilibrium with the amount of solvation. In other words: The solution cannot dissolve anymore solute.

49. Solubilty A supersaturated solution contains more dissolved solute than a saturated solution at the same temperature and are considered unstable. To make a supersaturated solution, a saturated solution is formed at a high temperature and then cooled slowly. The slow cooling allows the excess solute to remain dissolved in solution at the lower temperature.

50. Solubility of Gases Gases, in general, are less soluble at higher temperatures than at lower temperatures. At higher temperatures, the gases have a higher kinetic energy that allows them to escape from a solution.

51. Henry’s Law Pressure affects the solubility of gaseous solutes in solutions. The solubility of a gas in any solvent increases as its external pressure increases. Carbonated beverages rely on the container to provide enough pressure to keep gas dissolved in the solution.

52. Henry’s Law Henry’s law states that at a given temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas.

53. Practice Problem #8 If 0.85 g of a gas at 4.0 atm of pressure dissolves in 1.0 L of water at 25°C, how much will dissolve in 1.0 L of water at 1.0 atm of pressure and the same temperature?.21 g/ liter

54. Question For a given amount, which type of solution contains the LEAST amount of solute? A.solvated B.saturated C.supersaturated D.unsaturated

55. Question At a given temperature, the solubility of a gas is directly proportional to what? A.volume B.mass C.molarity D.pressure

56. Homework CALM 11.3 p497 #36, 37, 39, 41

57. Solution Stoichiometry 11.4

58. Objectives Solve solution stoichiometry problems and solution limiting reactant problems. Determine excess concentration of ions after a reaction.

59. Solution Stoichiometry Stoichiometry applies to solutions too. The number of moles of a reactant and/or product can be found with concentration using the concentration equations. Most solution stoichiometry utilizes the net ionic equation.

60. Solution Stoichiometry Concentration of ions can be found in a solution by using the ratios in a compound. For example: 1.0 M CaCl 2 has 1.0 mole of Calcium (Ca 2+ ) in 1 liter of solution and 2.0 moles of chloride (Cl - )

61. Practice Problem #9 What is the concentration of sodium ions in 1 liter of a 2.0 M solution of sodium sulfate? 4.0 M

62. Practice Problem #10 What mass of solid aluminum hydroxide can be produced when 50.0ml of 0.200 M Al(NO 3 ) 3 is added to 200.0 ml of 0.100 M KOH? What mass of solid aluminum hydroxide can be produced when 50.0ml of 0.200 M Al(NO 3 ) 3 is added to 200.0 ml of 0.100 M KOH?

63. Practice Problem #11 A 100.0 ml of 0.200 M aqueous potassium hydroxide is mixed with 100.0 ml of 0.200 M aqueous magnesium nitrate. Write a balanced equation and net ionic equation. What mass of precipitate is produced and what is the concentration of each ion remaining in solution after the reaction is complete.

64. Practice Problem #12 What mass of silver chloride can be prepared by the reaction of 100.0ml of 0.20 M silver nitrate with 100.0 ml of 0.15 M calcium chloride? Write the balanced equation and net ionic equation. Calculate the concentration of each ion remaining in solution after precipitation is complete.

65. Accumulating Content 11.5

66. How does the net ionic change the way stoichiometry is calculated? What are the pros and cons?

67. Accumulating Content How does concentration affect solutions?

68. Accumulating Content How is solvation similar to ionic compounds?

69. Key Concepts The individual substances in a heterogeneous mixture remain distinct. Two types of heterogeneous mixtures are suspensions and colloids. Brownian motion is the erratic movement of colloid particles. Colloids exhibit the Tyndall effect.

70. Key Concepts A solution can exist as a gas, a liquid, or a solid, depending on the solvent. Solutes in a solution can be gases, liquids, or solids. Concentrations can be measured qualitatively and quantitatively. Concentrations can be measured qualitatively and quantitatively.

71. Key Concepts Molarity is the number of moles of solute dissolved per liter of solution. Molality is the ratio of the number of moles of solute dissolved in 1 kg of solvent.

72. Key Concepts The number of moles of solute does not change during a dilution. M 1 V 1 = M 2 V 2 The process of solvation involves solute particles surrounded by solvent particles.

73. Key Concepts Solutions can be unsaturated, saturated, or supersaturated. Henry’s law states that 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.

74. The END