2. LecturePLUS Timberlake1 Chapter 9 Solutions Properties of Water Solutions

3. LecturePLUS Timberlake2 Predict the % water in the following foods 88% water 94% water 85% water 86% water

4. LecturePLUS Timberlake3 Water in the Body water gainwater loss liquids1000 mLurine 1500 mL food 1200 mLperspiring 300 mL cells 300 mL exhaling 600 mL feces 100 mL Calculate the total water gain and water loss Total ______ mL _____ mL

5. LecturePLUS Timberlake4 Water Most common solvent A polar molecule O  - a hydrogen bond H  +

6. LecturePLUS Timberlake5 Hydrogen Bonds Attract Polar Water Molecules

7. LecturePLUS Timberlake6 Explore 1. Place some water on a waxy surface. Why do drops form? 2. Carefully place a needle on the surface of water. Why does it float? What happens if you push it through the water surface? 3. Sprinkle pepper on water. What does it do? Add a drop of soap. What happens?

8. LecturePLUS Timberlake7 Surface Tension Water molecules within water hydrogen bond in all directions Water molecules at surface cannot hydrogen bond above the surface, pulled inward Water surface behaves like a thin, elastic membrane or “skin” Surfactants (detergents) undo hydrogen bonding

9. LecturePLUS Timberlake8 Solute and Solvent Solutions are homogeneous mixtures of two or more substances Solute The substance in the lesser amount Solvent The substance in the greater amount

10. LecturePLUS Timberlake9 Nature of Solutes in Solutions Spread evenly throughout the solution Cannot be separated by filtration Can be separated by evaporation Not visible, solution appears transparent May give a color to the solution

11. LecturePLUS Timberlake10 Types of Solutions air O 2 gas and N 2 gas gas/gas soda CO 2 gas in water gas/liquid seawater NaCl in water solid/liquid brass copper and zinc solid/solid

12. LecturePLUS Timberlake11 Learning Check SF1 (1) element (2) compound (3) solution A. water123 B. sugar 123 C. salt water 123 D. air123 E. tea123

13. LecturePLUS Timberlake12 Learning Check SF2 Identify the solute and the solvent. A. brass: 20 g zinc + 50 g copper solute= 1) zinc 2) copper solvent = 1) zinc 2) copper B. 100 g H 2 O + 5 g KCl solute = 1) KCl 2) H 2 O solvent = 1) KCl 2) H 2 O

14. LecturePLUS Timberlake13 Like dissolves like A ____________ solvent such as water is needed to dissolve polar solutes such as sugar and ionic solutes such as NaCl. A ___________solvent such as hexane (C 6 H 14 ) is needed to dissolve nonpolar solutes such as oil or grease.

15. LecturePLUS Timberlake14 Learning Check SF4 Which of the following solutes will dissolve in water? Why? 1) Na 2 SO 4 2) gasoline 3) I 2 4) HCl

16. LecturePLUS Timberlake15 Formation of a Solution Cl - Na + Cl - Na + H2OH2O H2OH2O Cl - solute Dissolved solute Hydration

17. LecturePLUS Timberlake16 Writing An Equation for a Solution When NaCl(s) dissolves in water, the reaction can be written as H 2 O NaCl(s) Na + (aq) + Cl - (aq) solid separation of ions in water

18. LecturePLUS Timberlake17 Learning Check SF5 Solid LiCl is added to some water. It dissolves because A. The Li + ions are attracted to the 1) oxygen atom(  -) of water 2) hydrogen atom(  +) of water B.The Cl - ions are attracted to the 1) oxygen atom(  -) of water 2) hydrogen atom(  +) of water

19. LecturePLUS Timberlake18 Rate of Solution You are making a chicken broth using a bouillon cube. What are some things you can do to make it dissolve faster? Crush it Use hot water (increase temperature) Stir it

20. LecturePLUS Timberlake19 Learning Check SF6 You need to dissolve some gelatin in water. Indicate the effect of each of the following on the rate at which the gelatin dissolves as (1) increase, (2) decrease, (3) no change A. ___Heating the water B. ___Using large pieces of gelatin C. ___Stirring the solution

21. LecturePLUS Timberlake20 Chapter 8 Solution Percent Concentration

22. LecturePLUS Timberlake21 Percent Concentration Describes the amount of solute dissolved in 100 parts of solution amount of solute 100 parts solution

23. LecturePLUS Timberlake22 Mass-Mass % Concentration mass/mass % = g solute x 100% 100 g solution

24. LecturePLUS Timberlake23 Mixing Solute and Solvent Solute + Solvent 4.0 g KCl 46.0 g H 2 O 50.0 g KCl solution

25. LecturePLUS Timberlake24 Calculating Mass-Mass % g of KCl = 4.0 g g of solvent = 46.0 g g of solution = 50.0 g %(m/m) = 4.0 g KCl (solute) x 100 = 8.0% KCl 50.0 g KCl solution

26. LecturePLUS Timberlake25 Learning Check PC1 A solution contains 15 g Na 2 CO 3 and 235 g of H 2 O? What is the mass % of the solution? 1) 15% (m/m) Na 2 CO 3 2) 6.4% (m/m) Na 2 CO 3 3) 6.0% (m/m) Na 2 CO 3

27. LecturePLUS Timberlake26 Mass-Volume % mass/volume % = g solute x 100% 100 mL solution

28. LecturePLUS Timberlake27 Learning Check PC2 An IV solution is prepared by dissolving 25 g glucose (C 6 H 12 O 6 ) in water to make 500. mL solution. What is the percent (m/v) of the glucose in the IV solution? 1) 5.0% 2) 20.% 3) 50.%

29. LecturePLUS Timberlake28 Writing Factors from % A physiological saline solution is a 0.85% (m/v) NaCl solution. Two conversion factors can be written for the % value. 0.85 g NaCl and 100 mL NaCl soln 100 mL NaCl soln 0.85 g NaCl

30. LecturePLUS Timberlake29 % (m/m) Factors Write the conversion factors for a 10 %(m/m) NaOH solution NaOH a nd NaOH soln NaOH soln NaOH

31. LecturePLUS Timberlake30 Learning Check PC 3 Write two conversion factors for each of the following solutions: A. 8 %(m/v) NaOH B. 12 %(v/v) ethyl alcohol

32. LecturePLUS Timberlake31 Using % Factors How many grams of NaCl are needed to prepare 250 g of a 10.0% (m/m) NaCl solution? Complete data: ____________ g solution ____________% or (______/_100 g_) solution ____________ g solute

33. LecturePLUS Timberlake32 Learning Check PC4 How many grams of NaOH do you need to measure out to prepare 2.0 L of a 12%(m/v) NaOH solution? 1) 24 g NaOH 2)240 g NaOH 3)2400 g NaOH

34. LecturePLUS Timberlake33 Learning Check PC5 How many milliliters of 5 % (m/v) glucose solution are given if a patient receives 150 g of glucose? 1) 30 mL 2) 3000 mL 3) 7500 mL

35. LecturePLUS Timberlake34 Chapter 8 Solutions Molarity

36. LecturePLUS Timberlake35 Molarity (M) A concentration that expresses the moles of solute in 1 L of solution Molarity (M) = moles of solute 1 liter solution

37. LecturePLUS Timberlake36 Units of Molarity 2.0 M HCl = 2.0 moles HCl 1 L HCl solution 6.0 M HCl= 6.0 moles HCl 1 L HCl solution

38. LecturePLUS Timberlake37 Molarity Calculation NaOH is used to open stopped sinks, to treat cellulose in the making of nylon, and to remove potato peels commercially. If 4.0 g NaOH are used to make 500. mL of NaOH solution, what is the molarity (M) of the solution?

39. LecturePLUS Timberlake38 Learning Check M1 A KOH solution with a volume of 400 mL contains 2 mole KOH. What is the molarity of the solution? 1) 8 M 2) 5 M 3) 2 M Drano

40. LecturePLUS Timberlake39 Learning Check M2 A glucose solution with a volume of 2.0 L contains 72 g glucose (C 6 H 12 O 6 ). If glucose has a molar mass of 180. g/mole, what is the molarity of the glucose solution? 1)0.20 M 2)5.0 M 3)36 M

41. LecturePLUS Timberlake40 Molarity Conversion Factors A solution is a 3.0 M NaOH.. Write the molarity in the form of conversion factors. 3.0 moles NaOH and 1 L NaOH soln 1 L NaOH soln 3.0 moles NaOH

42. LecturePLUS Timberlake41 Learning Check M3 Stomach acid is a 0.10 M HCl solution. How many moles of HCl are in 1500 mL of stomach acid solution? 1) 15 moles HCl 2) 1.5 moles HCl 3) 0.15 moles HCl

43. LecturePLUS Timberlake42 Learning Check M4 How many grams of KCl are present in 2.5 L of 0.50 M KCl? 1) 1.3 g 2) 5.0 g 3) 93 g

44. LecturePLUS Timberlake43 Learning Check M5 How many milliliters of stomach acid, which is 0.10 M HCl, contain 0.15 mole HCl? 1) 150 mL 2) 1500 mL 3) 5000 mL

45. LecturePLUS Timberlake44 Learning Check M6 How many grams of NaOH are required to prepare 400. mL of 3.0 M NaOH solution? 1)12 g 2)48 g 3) 300 g

46. LecturePLUS Timberlake45 Chapter 8 Solutions Solubility Percent Concentration Colloids and Suspensions

47. LecturePLUS Timberlake46 Solubility The maximum amount of solute that can dissolve in a specific amount of solvent usually 100 g. g of solute 100 g water

48. LecturePLUS Timberlake47 Saturated and Unsaturated A saturated solution contains the maximum amount of solute that can dissolve. Undissolved solute remains. An unsaturated solution does not contain all the solute that could dissolve

49. LecturePLUS Timberlake48 Learning Check S1 At 40  C, the solubility of KBr is 80 g/100 g H 2 O. Indicate if the following solutions are (1) saturated or (2) unsaturated A. ___60 g KBr in 100 g of water at 40  C B. ___200 g KBr in 200 g of water at 40  C C. ___25 KBr in 50 g of water at 40  C

50. LecturePLUS Timberlake49 Temperature and Solubility of Solids TemperatureSolubility (g/100 g H 2 O) KCl(s)NaNO 3 (s) 0°27.6 74 20°C34.0 88 50°C42.6114 100°C 57.6182 The solubility of most solids (decreases or increases ) with an increase in the temperature.

51. LecturePLUS Timberlake50 Temperature and Solubility of Gases TemperatureSolubility(g/100 g H 2 O) CO 2 (g)O 2 (g) 0°C0.340.0070 20°C0.170.0043 50°C0.0760.0026 The solubility of gases (decreases or increases) with an increase in temperature.

52. LecturePLUS Timberlake51 Learning Check S2 A. Why would a bottle of carbonated drink possibly burst (explode) when it is left out in the hot sun ? B. Why would fish die in water that gets too warm?

53. LecturePLUS Timberlake52 Soluble and Insoluble Salts A soluble salt is an ionic compound that dissolves in water. An insoluble salt is an ionic compound that does not dissolve in water

54. LecturePLUS Timberlake53 Solubility Rules 1. A salt is soluble in water if it contains any one of the following ions: NH 4 + Group IA metal ion NO 3 - C 2 H 3 O 2 - Examples: soluble salts LiCl Na 2 SO 4 KBr Ca(NO 3 ) 2

55. LecturePLUS Timberlake54 Cl -, Br -, I - Salts (X - ) 2. Salts with X - are soluble, but not if the positive ion is Ag +, Pb 2+, or Hg 2 2+. Examples: solublenot soluble(will not dissolve) MgCl 2 AgBr Pbl 2

56. LecturePLUS Timberlake55 SO 4 2- Salts 3. Salts with SO 4 2- are soluble, but not if the positive ion is Ca 2+, Ba 2+, Pb 2+, or Hg 2+ Examples: solublenot soluble MgSO 4 BaSO 4 PbSO 4

57. LecturePLUS Timberlake56 Other Salts 4. Most salts containing CO 3 2-, PO 4 3-, S 2- and OH - are not soluble, except when positive ion is group IA metal or NH 4 + Examples: solublenot soluble Na 2 CO 3 CaCO 3 K 2 SCuS

58. LecturePLUS Timberlake57 Learning Check S3 Indicate if each salt is (1)soluble or (2)not soluble: A. ______ Na 2 SO 4 B. ______ MgCO 3 C. ______ PbCl 2 D. ______ MgCl 2

59. LecturePLUS Timberlake58 They happen when mixing two salt solution and a new salt forms that is insoluble in water (precipitate). You see a powder forming from mixing two clear solutions: AgNO 3(aq) + NaCl (aq) → AgCl (s) + NaNO 3(aq) KOH (aq) + Pb(NO 3 ) 2 → Precipitation Reactions

60. LecturePLUS Timberlake59 Chapter 8 Solutions Colloids and Suspensions Osmosis and Dialysis

61. LecturePLUS Timberlake60 Solutions Have small particles (ions or molecules) Are transparent Do not separate Cannot be filtered Do not scatter light.

62. LecturePLUS Timberlake61 Colloids Have medium size particles Cannot be filtered Separated with semipermeable membranes Scatter light (Tyndall effect)

63. LecturePLUS Timberlake62 Examples of Colloids Fog Whipped cream Milk Cheese Blood plasma Pearls

64. LecturePLUS Timberlake63 Suspensions Have very large particles Settle out Can be filtered Must stir to stay suspended

65. LecturePLUS Timberlake64 Examples of Suspensions Blood platelets Muddy water Calamine lotion

66. LecturePLUS Timberlake65 Osmosis In osmosis, the solvent water moves through a semipermeable membrane Water flows from the side with the lower solute concentration into the side with the higher solute concentration Eventually, the concentrations of the two solutions become equal.

67. LecturePLUS Timberlake66 Osmosis semipermeable membrane 4% starch10% starch H2OH2O

68. LecturePLUS Timberlake67 Equilibrium is reached. water flow becomes equal 7% starch H2OH2O

69. LecturePLUS Timberlake68 Osmotic Pressure Produced by the number of solute particles dissolved in a solution Equal to the pressure that would prevent the flow of additional water into the more concentrated solution Increases as the number of dissolved particles increase

70. LecturePLUS Timberlake69 Osmotic Pressure of the Blood Cell walls are semipermeable membranes The osmotic pressure of blood cells cannot change or damage occurs. The flow of water between a red blood cell and its surrounding environment must be equal

71. LecturePLUS Timberlake70 Isotonic solutions Exert the same osmotic pressure as red blood cells. Medically 5% glucose and 0.9% NaCl are used their solute concentrations provide an osmotic pressure equal to that of red blood cells H2OH2O

72. LecturePLUS Timberlake71 Hypotonic Solutions Lower osmotic pressure than red blood cells Lower concentration of particles than RBCs In a hypotonic solution, water flows into the RBC The RBC undergoes hemolysis; it swells and may burst. H 2 O

73. LecturePLUS Timberlake72 Hypertonic Solutions Has higher osmotic pressure than RBC Has a higher particle concentration In hypertonic solutions, water flows out of the RBC The RBC shrinks in size (crenation) H2OH2O

74. LecturePLUS Timberlake73 Dialysis Occurs when solvent and small solute particles pass through a semipermeable membrane Large particles retained inside Hemodialysis is used medically (artificial kidney) to remove waste particles such as urea from blood

75. LecturePLUS Timberlake74 Solutions Electrolytes Nonelectrolytes

76. LecturePLUS Timberlake75 Electrolytes  Are substances that form positive(+) and negative (-) ions in water  Conduct an electric current

77. LecturePLUS Timberlake76 Electrolytes in the Body  Carry messages send to and from the brain as electrical signals  Maintain cellular function with the correct concentrations electrolytes

78. LecturePLUS Timberlake77 Strong Electrolytes are 100% ionized salts H 2 O 100%ions NaCl(s) Na + (aq) + Cl - (aq) H 2 O CaBr 2 (s) Ca 2+ (aq) + 2Br - (aq) acids HCl(g) H 2 O H 3 O + (aq) + Cl - (aq)

79. LecturePLUS Timberlake78 Weak electrolytes Most of the solute exists as molecules in solution Only a few solute particles produce ions HF + H 2 O  H 3 O + (aq) + F - (aq) acid NH 3 + H 2 O  NH 4 + (aq) + OH - (aq) base

80. LecturePLUS Timberlake79 Nonelectrolytes þ Dissolve as molecules only þ No ions are produced in water þ Do not conduct an electric current H 2 O C 6 H 12 O 6 (s)  C 6 H 12 O 6 (aq) glucose

81. LecturePLUS Timberlake80 Learning Check E1 Select the products for each of the following in water: H 2 O A. CaCl 2 (s) 1) CaCl 2 2) Ca 2+, Cl 2 - 3) Ca 2+ + 2Cl - H 2 O B. K 3 PO 4 (s) 1) 3K +, PO 4 3- 2) K 3 PO 4 3) K 3 +, P 3-, O 4 -

82. LecturePLUS Timberlake81 Equivalents Amount of an electrolyte or an ion that provides 1 mole of electrical charge (+ or -) 1 mole Na + = 1 equivalent 1 mole Cl - = 1 equivalent 1 mole Ca 2+ = 2 equivalents 1 mole Fe 3+ = equivalents

83. LecturePLUS Timberlake82 Electrolytes in Body Fluids In replacement solutions for body fluids, the electrolytes are given in milliequivalents per liter (mEq/L). Ringer’s Solution Na + 147 mequiv/LCl - mequiv/L K + 4 mequiv/L Ca 2+ 4 mequiv/L

84. LecturePLUS Timberlake83 Learning Check E2 A. In 1 mole of Fe 3+, there are 1) 1 equiv2) 2 equiv 3) 3 equiv B. 0.5 equivalents of calcium is 1) 5 mEq2) 50 mEq 3) 500 mEq C.An IV bottle contains NaCl. If the Na + is 34 mEq/L, the Cl - is 1) 34 mEq/L2) 0 mEq/L 3) 68 mEq/L