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2. Resources Chapter Presentation Bellringer Transparencies Sample Problems Visual Concepts Standardized Test Prep

3. Solutions Chapter 13 Table of Contents Section 1What Is a Solution? Section 2Concentration and Molarity Section 3Solubility and the Dissolving Process Section 4Physical Properties of Solutions

4. Chapter 13 Section1 What Is a Solution? Bellringer • Look at the following definitions: • suspension—a solution that appears uniform while being stirred but separates quickly after stirring • solution—a homogenous mixture • colloid—a mixture in which small particles are suspended throughout • Make a list of mixture that fit into each of these categories. You might start by thinking of foods and drinks with these properties.

5. Chapter 13 Section1 What Is a Solution? Objectives • Distinguishbetween solutions, suspensions, and colloids. • Describesome techniques chemists use to separate mixtures.

6. Chapter 13 Section1 What Is a Solution? Mixtures • A mixture is the blending of two or more dissimilar substances that do not chemically combine to form compounds and that can typically be separated by non-chemical means. • Mixtures can be classified into three types: suspension mixture, colloidal mixture or solution, according to how they combine and can be separated.

7. Chapter 13 Section1 What Is a Solution? Mixtures • Mixtures can either be heterogeneous or homogeneous. • The particles of a heterogeneous mixture are large enough to see under a microscope. • In a homogeneous mixture, however, the particles are molecule-sized, so the mixture appears uniform, even under a microscope

8. Suspension mixture • A suspension mixture is usually created by stirring together two or more ingredients, where the particles are typically large enough to be seen by the unaided eye or a magnifying glass. • The ingredients of a suspension mixture are heterogeneous, meaning that they are not evenly distributed throughout. Most mixtures are suspension mixtures.

9. Solid-solid mix • Many suspension mixtures consist of solids mixed with solids. • Cake mix is an example of visible solid particles mixed together by a means of stirring. Dirt or soil is another example of a solid-solid suspension mixture. • These mixtures can be separated by sifting. Sometimes shaking will cause the heavier particles to settle to the bottom.

10. sifting

11. Solid-fluid mix If solid particles are mixed in a liquid or gas to form a suspension mixture, the ingredients will soon separate, with the heavier solid particles settling at the bottom. For example, if you mixed sand and water, the sand would soon sink to the bottom. If the solid particles are lighter than the liquid--as in the case of sawdust mixed in water--they will separate and float to the top.

13. Particle Model for a Suspension Chapter 13 Section1 What Is a Solution?

14. Suspension of Tamiflu

15. Visual Concepts Chapter 13 Suspensions

16. A major part of air pollution consists of smoke and dust particles mixed within the atmosphere. This is a suspension mixture. • After a while, these solid particles will settle to the ground. • Besides settling(sedimentation), filtration can also be used to separate the ingredients.

17. Chapter 13 Section1 What Is a Solution? Mixtures, continued Solution Is a Broad Term • Any mixture that is homogeneous on a microscopic level is a solution. According to that definition, air is a gaseous solution. • A homogeneous liquid mixture has one main component—a liquid—as well as one or more additional ingredients that are usually present in smaller amounts.

18. Chapter 13 Section1 What Is a Solution? Mixtures, continued Solution Is a Broad Term, continued • The primary ingredient in a solution is called the solvent. • The other ingredients are the solutes and are said to be dissolved in the solvent. • Water is the most common solvent. • Water is a unique solvent because so many substances can dissolve in it. • Solutions in which water is the solvent are called aqueous solutions.

19. Visual Concepts Chapter 13 Solutes, Solvents, and Solutions

20. Chapter 13 Section1 What Is a Solution? Mixtures, continued Solution Is a Broad Term, continued • Another type of solution involves one solid mixed with another solid. • Examples include solid alloys, such as brass(copper & zinc), bronze(copper & tin), and steel(iron & carbon)

21. Particle Models for Gold and Gold Alloy Chapter 13 Section1 What Is a Solution?

22. Visual Concepts Chapter 13 Types of Solutions

23. Chapter 13 Section1 What Is a Solution? Mixtures, continued Colloids Are Stable Heterogeneous Mixtures • A colloidis a mixture consisting of tiny particles that are intermediate in size between those in solutions and those in suspensions and that are suspended in a liquid, solid, or gas. • Milk appears to be homogeneous. But under a microscope you see that milk contains globules of fat and small lumps of the protein casein dispersed in a liquid called whey. Milk is colloid because the particles of casein do not settle out after standing.

24. Visual Concepts Chapter 13 Solutions

25. Visual Concepts Chapter 13 Colloids

26. Otherexamples of colloidsAerosol sprays insecticide spray smog Shaving lather whipped cream Mayonnaisecosmetic lotion lubricants Paint

27. Chapter 13 Section1 What Is a Solution? Separating Mixtures • Mixtures are separated based on their physical properties. • Mixtures may be separated by decanting, pouring off the liquid, with a centrifuge, filtering, or evaporation. • Chromatography Separates by Differences in Attraction • Chromatography separates components of a mixture based on how quickly molecules dissolved in a mobile phasesolvent move along a solid phase. • Paper chromatography is a powerful technique for separating solutions.

28. Chapter 13 Section1 What Is a Solution? Mixtures, continued Distillation Separates by Differences in Boiling Point • If the boiling points of the components are different, distillationcan separate them based on their boiling points. • As one component reaches its boiling point, it evaporates from the mixture and is allowed to cool and condense. This is called a distillate. • This process continues until all the desired components have been separated from the mixture.

29. decanting

30. Filtration

31. Centrifuge

32. Paper Chromatography

33. Distillation

34. Fractional distillation

35. Oil refinery

36. 1. Explain why a suspension is considered a heterogeneous mixture.It is a type of mixture in which the different parts spontaneously separate over time.2. Classify the following mixtures as homogeneous or heterogeneous:a. lemon juice (heterogeneous)b. tap water (homogeneous)c. blood (heterogeneous) d. house paint (heterogeneous) 3. In a solution, which component is considered the solvent? Which is the solute?The solvent is the substance in excess, and the solute is the substance dissolved in the solvent Section 13.1 Review

37. Section 13.1 Review • 4. Name the solvent and solute(s) in the following solutions: • carbonated water • ( water, CO2) • b. apple juice • ( water, apple extract) • c. Coffee • ( water, coffee filtrate) d. salt water • ( water, salt) • 5. Does a solution have to involve a liquid? Explain your answer. • No, it can be gas/gas or solid/solid6. How is a colloid distinguished from a solution or a suspension? • A colloid is heterogeneous at the microscopic level, while a solution is homogeneous all the way down to the molecular level

38. Section 13.1 Review 7. What is the basic physical principle that chromatography is based upon? Chromatography is based on differences of adhesion of substances to a solid surface. 8. How can distillation be used to prepare pure water from tap water? The tap water can be boiled, and the resulting water vapor, when recondensed, will be pure water.

39. HW Concept review (handouts)

40. Section2 Concentration and Molarity Chapter 13 Bellringer • Write a brief paragraph about how you would prepare lemonade. • Why is the amount of sugar and lemon juice important in making a good glass of lemonade?

41. Section2 Concentration and Molarity Chapter 13 Objectives • Calculateconcentration using common units. • Definemolarity, and calculate the molarity of a solution. • Describethe procedure for preparing a solution of a certain molarity. • Usemolarity in stoichiometric calculations.

42. Section2 Concentration and Molarity Chapter 13 Concentration Calculation Concentration • In a solution, the solute is distributed evenly throughout the solvent. This means that any part of a solution has the same ratio of solute to solvent as any other part of the solution. • This ratio is the concentrationof the solution. • The concentration is the amount of a particular substance in a given quantity of a solution

43. Visual Concepts Chapter 13 Concentration ( iron(II) sulfate)

44. Section2 Concentration and Molarity Chapter 13 Concentration, continued Calculating Concentration, continued • Concentrations can be expressed in many forms.

45. Section2 Concentration and Molarity Chapter 13 Calculating Parts per Million Sample Problem A A chemical analysis shows that there are 2.2 mg of lead in exactly 500 g of water. Convert this measurement to parts per million.

46. Section2 Concentration and Molarity Chapter 13 Calculating Parts per Million, continued Sample Problem A Solution mass of solute: 2.2 mg mass of solvent: 500 g parts per million = ?

47. Section2 Concentration and Molarity Chapter 13 Sample Problem A, practice pg.461 1)Helium gas, 3.0 × 10−4 g, is dissolved in 200.0 g of water. Express this concentration in parts per million.

48. Section2 Concentration and Molarity Chapter 13 Sample Problem A, practice pg.461 3) A solution of lead sulfate contains 0.425 g of lead sulfate in 100.0 g of water. What is this concentration in parts per million?

49. Homework Sample Problem A, practice pg.461 4) A 900.0 g sample of sea water is found to contain 6.7 × 10−3 g Zn. Express this concentration in parts per million. 5)A 365.0 g sample of water, contains 23 mg Au. How much gold is present in the sample in parts per million? 6) A 650.0 g hard-water sample contains 101 mg Ca. What is this concentration in parts per million? 7)An 870.0 g river water sample contains 2 mg of cadmium. Express the concentration of cadmium in parts per million.

50. Section2 Concentration and Molarity Chapter 13 Molarity • Since the mole is the unit chemists use to measure the number of particles, they often specify concentrations using molarity. • Molarity (M) is a concentration unit of a solution expressed as moles of solute dissolved per liter of solution.