1. Notes – Properties of Water: Solubility/Acids-Bases

2. v v

6. Properties of Water Hydrogen Bonds – Weak forces between some covalently bonded molecules (polar molecules)

8. Properties of Water Cohesion – polar molecules attract and stick together Adhesion – water molecules stick to other molecules Examples Surface tension, capillary action, high boiling point, water in sphere droplets, high heat capacity (storage)

10. Fig. 3-3 Water-conducting cells Adhesion Cohesion 150 µm Direction of water movement

11. Fig. 3-4

13. Properties of Water Solutions - Mixtures in which one or more substances are uniformly distributed in another. A Solute is dissolved in a solvent. Examples: Aqueous solutions (water solvent), blood plasma, plant sap, seawater.

14. Properties of Water Universal solvent – More substances dissolve in water than any other molecule. Solvent – The substance other substances dissolve in. Solute – The substance being dissolved

15. Properties of Solutions Properties of Water Universal solvent – More substances dissolve in water than any other molecule. Solvent – The substance other substances dissolve in. Solute – The substance being dissolved

16. Properties of Solutions Properties of Water Universal solvent – More substances dissolve in water than any other molecule. Solvent – The substance other substances dissolve in. Solute – The substance being dissolved

17. Properties of Solutions Properties of Water Universal solvent – More substances dissolve in water than any other molecule. Solvent – The substance other substances dissolve in. Solute – The substance being dissolved

19. Properties of Solutions Solution are said to be: Homogeneous mixtures – they look the “same” throughout Examples: Salt water, coffee, orange juice Mixtures that look “different” are called: Heterogeneous mixtures

20. Properties of Solutions Solution are said to be: Homogeneous mixtures – they look the “same” throughout Examples: Salt water, coffee, orange juice Mixtures that look “different” are called: Heterogeneous mixtures

21. Solutions Colloid - The type of mixture which contains small solid particles suspended in a solution. Example: Milk, fog, gelatin

22. Solutions Suspension -A type of heterogeneous mixture where the solid particles are large enough to settle out or can be separated by using filtration. Ex: Snow globe, muddy water

23. Salt in Water Salt in water dissolves and becomes positive and negative ions. Saltwater conducts electricity

24. Salt in Water Salt in water dissolves and lowers the freezing point of water. –Ex: Applying salt on icy roads causes ice to melt Salt in water dissolves and raises the boiling point of water

25. Salt in Water Salt in water dissolves and lowers the freezing point of water. –Ex: Applying salt on icy roads causes ice to melt Salt in water dissolves and raises the boiling point of water –Ex: Adding salt to water makes water boil hotter and cooks food faster

26. Salt in Water Salt in water dissolves and lowers the freezing point of water. –Ex: Applying salt on icy roads causes ice to melt Salt in water dissolves and raises the boiling point of water

27. Salt in Water Salt in water dissolves and lowers the freezing point of water. –Ex: Applying salt on icy roads causes ice to melt Salt in water dissolves and raises the boiling point of water –Ex: Adding salt to water makes water boil hotter and cooks food faster

28. Solubility – The maximum quantity of a substance that will dissolve in a certain quantity of water at a specified temperature Solubility curve – Graphical representation of the amount of solute that dissolves in a given amount of solvent

29. Solubility – The maximum quantity of a substance that will dissolve in a certain quantity of water at a specified temperature Solubility curve – Graphical representation of the amount of solute that dissolves in a given amount of solvent

30. Concentration – How much solute is dissolved in a specific quantity of solvent or solution Solubility can be measured in : per cent % - parts per hundred ppm – parts per million ppb – parts per billion

31. Solubility - concentrations depend on the amount/type of solvent and the temperature Saturated – solutions holding the maximum amount of solute Unsaturated – solutions holding less than the max. amount Supersaturated – solutions holding more than the max amount of solute

32. Solubility - concentrations depend on the amount/type of solvent and the temperature Saturated – solutions holding the maximum amount of solute Unsaturated – solutions holding less than the max. amount Supersaturated – solutions holding more than the max amount of solute

33. Solubility - concentrations depend on the amount/type of solvent and the temperature Saturated – solutions holding the maximum amount of solute Unsaturated – solutions holding less than the max. amount Supersaturated – solutions holding more than the max amount of solute

34. Solubility

35. Substances that dissolve in H2O are soluble. If substances do not dissolve in water they are insoluble. Substances that dissolve in water are ionic compounds or other polar molecules

36. Solubility Substances that dissolve in H2O are soluble. If substances do not dissolve in water they are insoluble. Substances that dissolve in water are ionic compounds or other polar molecules Ex: Salts, Alcohol

37. Solubility Nonpolar substances do not have partial charges. They do not readily dissolve in water Nonpolar substances include oils, petroleum products, kerosene

38. Solubility Nonpolar substances will dissolve in other nonpolar substances. Ex: Paint thinner for oil-based paints Like dissolves in like Soap breaks nonpolar molecules into smaller particles to make them more soluble in water

39. Solubility Nonpolar substances will dissolve in other nonpolar substances. Ex: Paint thinner for oil-based paints Like dissolves in like Soap breaks nonpolar molecules into smaller particles to make them more soluble in water

40. Measuring Solubility

42. Water Dissociation – Self Ionization Water can break down into ionized particles H 2 0 ( l ) = H + ( aq ) + OH - ( aq ) H 2 0 + H + = H 3 0 + Hydronium ion

43. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (H 3 0 + ) (hydronium) (acids) or Hydroxide (OH-) ions (charged particles) dissolved in water (base)

44. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (H 3 0 + ) (hydronium) (acids)or Hydroxide (OH-) ions (charged particles) dissolved in water (base)

45. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (H 3 0 + ) (hydronium) (acids)or Hydroxide (OH-) ions (charged particles) dissolved in water (base) pH = Scale to measure H+ concentration (-log) pH 1= 1/10=1/10 1 H+ pH 2 = 1/100=1/10 2 pH 3 = 1/1000= 1/10 3 pH 1 = highest H+ pH 14= lowest H+

46. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (H 3 0 + ) (hydronium) (acids)or Hydroxide (OH-) ions (charged particles) dissolved in water (base) pH = Scale to measure H+ concentration (-log) pH 1= 1/10=1/10 1 H+ pH 2 = 1/100=1/10 2 pH 3 = 1/1000= 1/10 3 pH 1 = highest H+ pH 14= lowest H+

47. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (hydronium) (acids)or Hydroxide (OH-) ions (charged particles) dissolved in water (base) pH = Scale to measure H+ concentration (-log) pH 1= 1/10=1/10 1 H+ pH 2 = 1/100=1/10 2 pH 3 = 1/1000= 1/10 3 pH 1 = highest H+ pH 14= lowest H+

48. Acids Made up of molecules including one or more hydrogen (H+) (H 3 0 + ) atoms that can be easily released in water solutions Substances in common have a sour taste Ex: Lemons, vinegar

49. Acid / Base Acid (H+) (H 3 0 + ) = Hydronium ion pH 1-6 1 is strongest, 6 is weakest

50. Acids Made up of molecules including one or more hydrogen (H+) (H 3 0 + ) atoms that can be easily released in water solutions Substances in common have a sour taste Ex: Lemons, vinegar Acids contain (H+) ions and compounds are renamed as acids Example: HCl = Hydrogen Chloride renamed: Hydrochloric Acid

51. Naming and Writing Acids and Bases Acids- Compounds that contain one or more Hydrogen atoms and produce Hydrogen ions (H+) when dissolved in water. Formula HnX H = Hydrogen n = Subscript (# of H) X = Monatomic or Polyatomic anion

52. Naming and Writing Acids and Bases Acids- Compounds that contain one or more Hydrogen atoms and produce Hydrogen ions (H+) when dissolved in water. Formula HnX H = Hydrogen n = Subscript (# of H) X = Monatomic or Polyatomic anion

53. Naming and Writing Acids and Bases Naming Acids 1) If anion ends in –ide: begin with Hydro-, change anion to – ic, and add “acid” HCl = Hydrogen Chloride = Hydrochloric Acid HBr = H 2 S =

54. Naming and Writing Acids and Bases Naming Acids 1) If anion ends in –ide: begin with Hydro-, change anion to – ic, and add “acid” HCl = Hydrogen Chloride = Hydrochloric Acid HBr = Hydrogen Bromide = Hydrobromic Acid H 2 S =

55. Naming and Writing Acids and Bases Naming Acids 1) If anion ends in –ide: begin with Hydro-, change anion to – ic, and add “acid” 2) If anion ends in –ite: anion changes to –ous followed by “acid” HCl = Hydrogen Chloride = Hydrochloric Acid HBr = Hydrobromic Acid H 2 S = Hydrogen Sulfide =Hydrosulfuric Acid

56. Naming and Writing Acids and Bases Naming Acids 2) If anion ends in –ite: anion changes to –ous followed by “acid” H 2 SO 3 = Hydrogen Sulfite = Sulfurous Acid HNO 2 = HClO 2 =

57. Naming and Writing Acids and Bases Naming Acids 2) If anion ends in –ite: anion changes to –ous followed by “acid” H 2 SO 3 = Hydrogen Sulfite = Sulfurous Acid HNO 2 = Hydrogen Nitrite = Nitrous Acid HClO 2 =

58. Naming and Writing Acids and Bases Naming Acids 2) If anion ends in –ite: anion changes to –ous followed by “acid” 3) If anion ends in –ate: anion changes to –ic followed by “acid”. H 2 SO 3 = Hydrogen Sulfite = Sulfurous Acid HNO 2 = Hydrogen Nitrite = Nitrous Acid HClO 2 = Hydrogen chlorite = Chlorous Acid

59. Naming and Writing Acids and Bases Naming Acids 3) If anion ends in –ate: anion changes to –ic followed by “acid”. H 2 SO 4 = Hydrogen Sulfate = Sulfuric Acid HNO 3 = H 3 PO 4 =

60. Naming and Writing Acids and Bases Naming Acids 3) If anion ends in –ate: anion changes to –ic followed by “acid”. H 2 SO 4 = Hydrogen Sulfate = Sulfuric Acid HNO 3 = Hydrogen Nitrate = Nitric Acid H 3 PO 4 =

61. Naming and Writing Acids and Bases Naming Acids 3) If anion ends in –ate: anion changes to –ic followed by “acid”. H 2 SO 4 = Hydrogen Sulfate = Sulfuric Acid HNO 3 = Hydrogen Nitrate = Nitric Acid H 3 PO 4 = Hydrogen Phosphate = Phosphoric Acid

63. Acids Formula name HCl = H 2 CO 3 = HC 2 H 3 O 2 = HNO 2 = H 3 PO 3 = H 2 SO 4 = HBr = Acid Name HCl = H 2 CO 3 = HC 2 H 3 O 2 = HNO 2 = H 3 PO 3 = H 2 SO 4 = HBr =

64. Acids Formula name HCl = Hydrogen Chloride H 2 CO 3 = Hydrogen Carbonate HC 2 H 3 O 2 = Hydrogen Acetate HNO 2 = Hydrogen Nitrite H 3 PO 3 = Hydrogen Phosphite H 2 SO 4 = Hydrogen Sulfate HBr = Hydrogen Bromide Acid Name HCl =Hydrochloric Acid H 2 CO 3 = Carbonic Acid HC 2 H 3 O 2 = Acetic Acid HNO 3 = Nitrous Acid H 3 PO 3 = Phosphorous Acid H 2 SO 4 = Sulfuric acid HBr = Hydrobromic Acid

65. Bases Ionic substances that include (OH-) hydroxide ions or generate (OH-) ions in solution In common substances have a bitter taste and slippery feel Ex: soap, peppers

66. Naming Bases Bases – Ionic compounds that produce hydroxide ions (OH - ) in solution

67. Naming Bases Bases – Ionic compounds that produce hydroxide ions (OH - ) in solution Naming bases: Bases follow the same rules as ionic compounds

68. Naming Bases Naming bases: Bases follow the same rules as ionic compounds. Name metal or polyatomic cation, name polyatomic anion NaOH = Sodium Hydroxide Ca(OH) 2 = NH 4 (OH)

69. Naming Bases Naming bases: Bases follow the same rules as ionic compounds. Name metal or polyatomic cation, name polyatomic anion NaOH = Sodium Hydroxide Ca(OH) 2 = Calcium Hydroxide NH 4 (OH) =

70. Naming Bases Naming bases: Bases follow the same rules as ionic compounds. Name metal or polyatomic cation, name polyatomic anion NaOH = Sodium Hydroxide Ca(OH) 2 = Calcium Hydroxide NH 4 (OH) = Ammonium Hydroxide

71. Bases Ionic substances that include (OH-) hydroxide ions or generate (OH-) ions in solution In common substances have a bitter taste and slippery feel Ex: soap, peppers Bases keep their original compound name Ca(OH) 2 = Mg(OH) 2 = KOH = NaOH =

72. Bases Ionic substances that include (OH-) hydroxide ions or generate (OH-) ions in solution In common substances have a bitter taste and slippery feel Ex: soap, peppers Bases keep their original compound name Ca(OH) 2 = Calcium Hydroxide Mg(OH) 2 = Magnesium Hydroxide KOH = Potassium Hydroxide NaOH = Sodium Hydroxide

74. Base (OH - ) = Hydroxide ion pH 8-14 14 is strongest, 8 is weakest

76. Acid / Base Acid (H+) = Hydronium ion pH 1-6 1 is strongest, 6 is weakest Base (OH-) = Hydroxide ion pH 8-14 14 is strongest, 8 is weakest

77. Neutral pH pH 7 H + = (OH) - = neutral H + + (OH) - =HOH=H 2 O Ex: Distilled water

78. pH indicators Indicators – show pH with color changes. H+ or (OH)- concentrations Ex: Litmus paper, phenolphthalein

79. Acid / Base Neutralization Equation ReactantsProducts 1M HCl + 1M NaOH = 1M NaCl + 1M H 2 O Acid + Base = Salt + Water pH1 pH14 pH7 pH7 Buffer – Baking Soda (HCO 3 -) prevents pH change Titration – adding known quantities of acids and/or bases together to determine M or pH quantities

80. Acid / Base Neutralization Equation ReactantsProducts HCl + NaOH = NaCl + H 2 O Acid Base Salt Water pH1 pH14 pH7 pH7 Buffer – Baking Soda (HCO 3 -) prevents pH change

83. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (hydronium) (acids)or Hydroxide (OH-) ions (charged particles) dissolved in water (base)

84. ACID / BASE Acid/Base – Special compounds containing excess : Hydrogen (H+) (hydronium) (acids)or Hydroxide (OH-) ions (charged particles) dissolved in water (base) pH = Scale to measure H+ concentration (-log) pH 1= 1/10=1/10 1 H+ pH 2 = 1/100=1/10 2 pH 3 = 1/1000= 1/10 3 pH 1 = highest H+ pH 14= lowest H+