3. Chapter Menu Lesson 1:SolutionsSolutions Lesson 2:Acidic, Basic, and Neutral SolutionsAcidic, Basic, and Neutral Solutions Click on a hyperlink to view the corresponding lesson.

4. substance mixture homogeneous mixture heterogeneous mixture solution solute solvent 9.1 Solutions

5. Types of Matter A substance is matter that has the same composition and properties throughout. 9.1 Solutions Most of the substances you encounter daily are solutions. Elements and compounds are substances.

6. Types of Matter (cont.) A mixture is a combination of two or more substances that can be separated by physical means. Heterogeneous mixtures are mixtures in which the substances are not evenly mixed, such as granite or mixed nuts. 9.1 Solutions

7. Types of Matter (cont.) Homogenous mixtures are two or more substances that are evenly mixed on the atomic level. 9.1 Solutions

8. Types of Matter (cont.) A solution is a homogeneous mixture. Two or more substances are evenly mixed, but they each retain their identities. –Before the drink mix dissolves, the mixture is heterogeneous. –When the drink mix has dissolved, it is a homogeneous mixture. 9.1 Solutions

9. Components of Solutions The solute in any solution is the dissolved substance. The solvent is the substance used to dissolve the solute. 9.1 Solutions

10. Types of Solutions Substances in each of the three states of matter—solid, liquid, gas—may act as solute or solvent. 9.1 Solutions

11. Alloys—Solid Solutions An alloy is the mixture of a metal and one or more additional elements. Alloys have metallic properties. Alloys are used in jewelry, statues, and automobiles. 9.1 Solutions

12. Separating Mixtures by Physical Means Components of a mixture can be separated by taking advantage of the differences in their physical properties. Dissolving, evaporating, melting, and freezing are some physical changes that can also be used to separate mixtures. 9.1 Solutions

13. Solubility—How much can dissolve? Solubility is the measure of how much solute can be dissolved in an amount of solvent. Increasing temperature increases the ability of a solvent to dissolve a solute. 9.1 Solutions

14. Saturated and Unsaturated Solutions A saturated solution has dissolved the maximum amount of solute at a given temperature—more solute will not dissolve in the solution. Unsaturated solutions are any solutions that are able to dissolve more solute at a given temperature—more solute can be added and it will dissolve. 9.1 Solutions

15. –Concentrated solutions contain a lot of solute. –Diluted solutions contain little solute. Concentration—How much is dissolved? The concentration of a solution is the amount of solute present in a solution compared to the amount of solvent. 9.1 Solutions

16. Concentration in Grams Per Liter (g/L) To be precise, describe concentration as grams of solute per liter of solvent. –10 grams of sodium chloride in 1 liter of water is a concentration of 10 g/L. 9.1 Solutions

17. Percent By Volume Percent by volume is the volume of solute in a given volume of solvent. –Hydrogen peroxide is 3 percent by volume, so 3 mL of hydrogen peroxide are in every 100 mL of solution. 9.1 Solutions

18. Water as a Solvent Most of the water on Earth is present in the form of a solution. Water is often called the universal solvent since many substances are soluble in it. 9.1 Solutions

19. Water as a Solvent (cont.) Water is a polar molecule—it has a positive end and a negative end. 9.1 Solutions

20. Polar Solvents and Polar Molecules Polar solvent molecules are likely to dissolve other polar molecules. The negative and positive ends of polar solutes are pulled into solution by the attraction to the negative and positive ends of the solvent molecules. 9.1 Solutions

21. Polar Solvents and Polar Molecules (cont.) 9.1 Solutions

22. Polar Solvents and Ionic Compounds Many ionic compounds are soluble in water. Water molecules attach themselves to the ions and pull them apart. 9.1 Solutions

23. Conductivity of Aqueous Solutions Ions in solution allow the solution to carry an electric current. Any compound that produces ions in water is called an electrolyte. 9.1 Solutions

24. Conductivity of Aqueous Solutions (cont.) Electricity flows through a sodium chloride solution but not a sugar solution. 9.1 Solutions

25. Lesson 1 Review NaCl is a ____ solution. Aheterogeneous Bhomogeneous Csaturated Dnone of the above 9.1 Solutions

26. Lesson 1 Review A polar solvent contains molecules that ____. Ahave positive and negative ends Bhave magnetic ends Care saturated Dhave ionic bonds 9.1 Solutions

27. Lesson 1 Review Which contains the largest amount of solute in 100 mL? A10 g/L B20 g/L C15 g/L D18 g/L 9.1 Solutions

28. End of Lesson 1

29. acid hydronium ion base pH indicator pH meter 9.2 Acidic, Basic, and Neutral Solutions

30. Acids The pH scale measures the acidity of a solution. The part that is H + in the water Acids are any substance that releases a hydrogen ion, H +, in water. H + in water forms a hydronium ion (H 3 O + ) 9.2 Acidic, Basic, and Neutral Solutions How is the acidic concentration of a solution determined?

31. What is a hydronium ion? The H + ion combines with water to form H 3 O +, the positively charged hydronium ion. 9.2 Acidic, Basic, and Neutral Solutions Hydrogen ionWater moleculeHydronium ion

32. What is a hydronium ion? (cont.) 9.2 Acidic, Basic, and Neutral Solutions

33. Uses and Properties of Acids Acids are also used in making many products, such as fertilizers, detergent, and cleaners. 9.2 Acidic, Basic, and Neutral Solutions Taste sour Stomach acid pH is lower than 7, strong acids near 0

34. Bases Bases are any substance that produces hydroxide ions, OH - when dissolved in water. Most bases are ionic compounds pH is greater than 7, strong bases near 14 9.2 Acidic, Basic, and Neutral Solutions

35. What is a hydroxide ion? In water, bases separate into a positive ion and the hydroxide ion (OH – ). All the properties of bases are a result of the presence of hydroxide ions that form when the base is dissolved in water. 9.2 Acidic, Basic, and Neutral Solutions

36. Uses of Bases Taste bitter Slippery to the touch Found in soap, plaster, drain cleaner Bases are also used to produce new products, such as soap, paper, and plaster. 9.2 Acidic, Basic, and Neutral Solutions Acids and Bases

37. pH is a scale to measure how acidic or basic a solution is. -Scale runs from 0 to 14. –Acids are below 7; strong acids are near 0. –Bases are above 7; strong bases near 14. –Neutral solutions have a pH of 7 9.2 Acidic, Basic, and Neutral Solutions

38. What is pH? Water is both acidic and basic H 2 O H + + OH - 1 molecules of water in 10 -7 does this –The exponent is seven! Neutral pH is 7 pH 6 is 10 times more acidic than pH 7 –These numbers are exponents each is a power of ten.

39. Hydronium Ions, Hydroxide Ions, and pH All acid and base solutions contain both hydronium (H + ) and hydroxide ions (OH - ) 9.2 Acidic, Basic, and Neutral Solutions

40. Hydronium Ions, Hydroxide Ions, and pH (cont.) Acids have more hydronium ions (H+) Bases have more hydroxide ions (OH - ) concentration. 9.2 Acidic, Basic, and Neutral Solutions

41. Neutralization pH Values Acids and bases react to neutralize each other. Water and a salt are the results Products are not acids or bases 9.2 Acidic, Basic, and Neutral Solutions

42. How is pH measured? Indicators change color depending of pH Example is Litmus paper Blue litmus turns red with acids Red litmus turns blue with bases pH meters –Electronic device 9.2 Acidic, Basic, and Neutral Solutions

43. How is pH Measured? (cont.) 9.2 Acidic, Basic, and Neutral Solutions

44. pH Meters (cont.) 9.2 Acidic, Basic, and Neutral Solutions

45. Lesson 2 Review An acid with a pH of 3 is contains how many times as many hydronium ions as an acid with a pH of 6? A1000 B3B3 C30 D100 9.2 Acidic, Basic, and Neutral Solutions

46. Lesson 2 Review When an acid and base are mixed, the products are ____ and ____. Awater; a base Bwater; ammonia Cwater; salt Dammonia; salt 9.2 Acidic, Basic, and Neutral Solutions

47. Lesson 2 Review Red litmus paper is dipped in a solution. The paper turns blue. The solution must have been ____. Aacidic Bhomogeneous Cbasic Dpolar 9.2 Acidic, Basic, and Neutral Solutions

48. End of Lesson 2

49. Chapter Assessment California Standards Practice Concepts in Motion Image Bank Science Online Chapter Resources Menu Click on a hyperlink to view the corresponding feature.

50. Blue litmus paper turns ____ in acid solutions. Ared Borange Cgreen Dblue Chapter Assessment 1

51. Which of the following is a hydroxide ion? AH3O+AH3O+ BH+BH+ COH – DNH 4 + Chapter Assessment 2

52. Which is a property of a base? Asour taste Bproduces OH – in water Cproduces H + in water Dreacts with metal to produce hydrogen gas Chapter Assessment 3

53. Which of the following is NOT a homogeneous mixture? Avinegar Bbrass Csalt water Dnone of the above Chapter Assessment 4

54. What ions are present in the greatest amount in a solution with a pH of 2.5? Ahydroxide Bhydrogen Chydronium Doxygen Chapter Assessment 5

55. When MgCl 2 is dissolved in water, what term is used to describe the MgCl 2 ? Asolution Bsolute Csolvent Dalloy CA Standards Practice 1 SCI 7.c

56. As the temperature of water decreases, its ability to dissolve NaCl ____. Aincreases Bdecreases Cstays the same Dcannot be predicted CA Standards Practice 2 SCI 7.c

57. Water is polar and easily dissolves ____ molecules. Apolar Bnonpolar Cpositively charged Dnegatively charged CA Standards Practice 3 SCI 7.c

58. Acids and bases are both ____ because they allow water to conduct electricity. Amalleable Bdiluted Cpolar Delectrolytes CA Standards Practice 4 SCI 5.e

59. What is the symbol for the hydrogen ion? AH3O+AH3O+ BH2OBH2O CH+CH+ DOH – CA Standards Practice 5 SCI 5.e

60. Concepts in Motion 1

61. Concepts in Motion 2

62. Concepts in Motion 3

63. Image Bank

64. End of Resources