solutions - gakall.com · characteristics of solutions return to toc section 8.1 in a homogenous...
TRANSCRIPT
Chapter 8
Solutions
Chapter 8
Chapter Outline
Copyright ©2016 Cengage Learning. All Rights Reserved. 2
8.1 Characteristics of solutions 8.2 Solubility 8.3 Solution formation 8.4 Solubility rules 8.5 Percent concentration units 8.6 Molarity concentration unit 8.7 Dilution 8.8 Colloidal dispersions and suspensions 8.9 Colligative properties of solutions 8.10 Osmosis and osmotic pressure
Characteristics of Solutions
Return to TOC
Section 8.1
3
• A homogeneous mixture of two or more substances with each substance retaining its own chemical identity
• Components of a solution: – Solvent: Component of a solution that is present in
the greatest amount – Solute: Component of a solution that is present in a
lesser amount relative to that of the solvent • Substance being dissolved
Solution
Copyright ©2016 Cengage Learning. All Rights Reserved.
Characteristics of Solutions
Return to TOC
Section 8.1
4
Figure 8.1 - Colored Crystals (Solute) Mixed with Water (Solvent)
Copyright ©2016 Cengage Learning. All Rights Reserved.
Characteristics of Solutions
Return to TOC
Section 8.1
5
• Contains 2 or more components • Has variable composition • Properties change as the ratio of solute to
solvent is changed • Dissolved solutes are present as individual
particles (molecules, atoms, or ions) • Solutes remain uniformly distributed and will not
settle out with time • Solute(s) can be separated from the solvent by
physical means such as evaporation
General Properties of a Solution
Copyright ©2016 Cengage Learning. All Rights Reserved.
Characteristics of Solutions
Return to TOC
Section 8.1
In a homogenous mixture containing 80 mL of water and 20 mL of alcohol, identify the solvent and the solute. a. Water is the solute, and alcohol is the solvent. b. Water is the solvent, and alcohol is the solute. c. Neither, since it is a homogenous mixture. d. Both, since one is dissolving the other.
6 Copyright ©2016 Cengage Learning. All Rights Reserved.
Characteristics of Solutions
Return to TOC
Section 8.1
In a homogenous mixture containing 80 mL of water and 20 mL of alcohol, identify the solvent and the solute. a. Water is the solute, and alcohol is the solvent. b. Water is the solvent, and alcohol is the solute. c. Neither, since it is a homogenous mixture. d. Both, since one is dissolving the other.
7 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
8
• The maximum amount of solute that will dissolve in a given amount of solvent under a given set of conditions
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
9
• Most solids become more soluble in water with increasing temperature
• In contrast, gas solubilities in water decrease with increasing temperature
Effect of Temperature on Solubility
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
10
Table 8.1 - Solubilities of Various Compounds in Water at 0°C, 50°C, and 100°C
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
11
• Pressure has little effect on the solubility of solids and liquids in water
• Pressure has major effect on the solubility of gases in water
Effect of Pressure on Solubility
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
12
• The amount of gas that will dissolve in a liquid at a given temperature is directly proportional to the partial pressure of the gas above the liquid – As the pressure of a gas above the liquid increases,
the solubility of the gas increases
Henry’s Law
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
13
• A solution that contains the maximum amount of solute that can be dissolved under the conditions at which the solution exists
Saturated Solution
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
14
• An unstable solution that temporarily contains more dissolved solute than that present in a saturated solution – Excess solute crystallizes out with time and the
solution reverts to a saturated solution
Supersaturated Solution
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
15
• A solution that contains less than the maximum amount of solute that can be dissolved under the conditions at which the solution exists – Most commonly encountered solutions fall into this
category
Unsaturated Solution
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
16
• Concentrated solution: A solution that contains a large amount of solute relative to the amount that could dissolve
• Dilute solution: A solution that contains a small amount of solute relative to the amount that could dissolve
Concentrated and Dilute Solutions
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
17
Figure 8.4 - Concentrated and Dilute Solutions
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
18
• Aqueous solution: A solution in which water is the solvent
• Nonaqueous solution: A solution in which a substance other than water is the solvent
Aqueous and Nonaqueous Solutions
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
How does the temperature and pressure affect the solubility of a gas in water?
a. Increased temperature decreases gas solubility, and increased pressure increases gas solubility. b. Increased temperature increases gas solubility, and increased pressure increases gas solubility. c. Increased temperature decreases gas solubility, and increased pressure decreases gas solubility. d. Decreased temperature decreases gas solubility, and decreased pressure increases gas solubility.
19 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.2
Solubility
Return to TOC
How does the temperature and pressure affect the solubility of a gas in water?
a. Increased temperature decreases gas solubility, and increased pressure increases gas solubility. b. Increased temperature increases gas solubility, and increased pressure increases gas solubility. c. Increased temperature decreases gas solubility, and increased pressure decreases gas solubility. d. Decreased temperature decreases gas solubility, and decreased pressure increases gas solubility.
20 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.3
Solution Formation
Return to TOC
21
• Two types of interparticle attractions must be overcome: – Attractions between solute particles (solute–solute
attractions) – Attractions between solvent particles (solvent–
solvent attractions) • New type of interaction arises
– Attraction between solute and solvent particles (solute–solvent attractions)
For a Solute to Dissolve in a Solvent
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.3
Solution Formation
Return to TOC
22
1. The state of subdivision of the solute 2. The degree of agitation during solution
preparation 3. The temperature of the solution components
Factors Affecting the Rate of Solution Formation
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.3
Solution Formation
Return to TOC
What three factors increase the rate of solution formation? a. State of subdivision of the solute; increase in rate of solute–solvent interaction; decrease in temperature b. State of subdivision of the solute; decrease in rate of solute–solvent interaction; decrease in temperature c. State of subdivision of the solute; decrease in rate of solute–solvent interaction; increase in temperature d. State of subdivision of the solute; increase in rate of solute–solvent interaction; increase in temperature
23 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.3
Solution Formation
Return to TOC
What three factors increase the rate of solution formation? a. State of subdivision of the solute; increase in rate of solute–solvent interaction; decrease in temperature b. State of subdivision of the solute; decrease in rate of solute–solvent interaction; decrease in temperature c. State of subdivision of the solute; decrease in rate of solute–solvent interaction; increase in temperature d. State of subdivision of the solute; increase in rate of solute–solvent interaction; increase in temperature
24 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.4
Solubility Rules
Return to TOC
25
• In general, it is found that the greater the difference in solute–solvent polarity, the less soluble is the solute
• Substances of like polarity tend to be more soluble in each other than substances that differ in polarity – “Like dissolves like” (but not in all cases) – Use table 8.2 - Solubility guidelines for ionic
compounds in water
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.4
Solubility Rules
Return to TOC
26
Table 8.2 - Solubility Guidelines for Ionic Compounds in Water
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.4
Solubility Rules
Return to TOC
Greater difference in solute–solvent polarity results in: a. greater solubility of the solute. b. less solubility of the solute. c. no effect on the solubility of the solute. d. an increase in the solvent’s ability to dissolve the solute.
27 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.4
Solubility Rules
Return to TOC
Greater difference in solute–solvent polarity results in: a. greater solubility of the solute. b. less solubility of the solute. c. no effect on the solubility of the solute. d. an increase in the solvent’s ability to dissolve the solute.
28 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.4
Solubility Rules
Return to TOC
Concept Check
• Which of the following ions that are generally soluble in water form compounds with Pb2+?
a) S2–
b) Cl–
c) NO3–
d) SO42–
e) Na+
29 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.4
Solubility Rules
Return to TOC
Concept Check
• Which of the following ions that are generally soluble in water form compounds with Pb2+?
a) S2–
b) Cl–
c) NO3–
d) SO42–
e) Na+
30 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
31
• The amount of solute present in a specified amount of solution
• Two methods of expressing concentration: – Percent concentration – Molarity concentration
Concentration
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
32
• Three different ways of representing percent concentration: – Percent by mass (mass–mass percent) – Percent by volume (volume–volume percent) – Mass–volume percent
Percent Concentration
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
33
Percent by Mass
mass of solutePercent by mass = × 100mass of solution
Mass of solution = mass of solute + mass of solvent
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
Exercise
• What is the percent by mass concentration of glucose in a solution made by dissolving 5.5 g of glucose in 78.2 g of water?
34 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
Exercise
• What is the percent by mass concentration of glucose in a solution made by dissolving 5.5 g of glucose in 78.2 g of water?
6.6%
35 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
36
Percent by Volume
volume of solutePercent by volume = ×100volume of solvent
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
Exercise
• Calculate the volume percent of solute in 30.0 mL of methyl alcohol in enough water to give 435 mL of solution.
37 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
Exercise
• Calculate the volume percent of solute in 30.0 mL of methyl alcohol in enough water to give 435 mL of solution.
6.90%
38 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
39
Mass–Volume Percent
( )( )
mass of solute gMass – volume percent = × 100
volume of solution mL
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
40
Table 8.3 - Conversion Factors Obtained From Percent Concentration Units
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
A solution having a mass percent concentration of 10% contains: a. 10 g of solute and 90 g of solvent. b. 10 g of solvent and 10 g of solute. c. 10 g of solute per 100 g of solvent. d. 10 g of solvent per 100 g of solute.
41 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
A solution having a mass percent concentration of 10% contains: a. 10 g of solute and 90 g of solvent. b. 10 g of solvent and 10 g of solute. c. 10 g of solute per 100 g of solvent. d. 10 g of solvent per 100 g of solute.
42 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
How many grams of sodium chloride are needed to prepare 150 mL of 0.9% (m/v) sodium chloride? a. 135 g b. 13.5 g c. 1.35 g d. 0.135 g
43 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.5
Percent Concentration Units
Return to TOC
How many grams of sodium chloride are needed to prepare 150 mL of 0.9% (m/v) sodium chloride? a. 135 g b. 13.5 g c. 1.35 g d. 0.135 g
44 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Molarity
• Moles of solute in a solution divided by the liters of solution
45
( ) moles of soluteMolarity M =liters of solution
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
What is the definition of molarity? a. Moles of solute per mole of solution b. Moles of solute per liter of solution c. Liters of solute per mole of solution d. Liters of solute per liter of solution
46 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
What is the definition of molarity? a. Moles of solute per mole of solution b. Moles of solute per liter of solution c. Liters of solute per mole of solution d. Liters of solute per liter of solution
47 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Exercise
• You have 1.00 mol of sugar in 125.0 mL of solution. Calculate the concentration in units of molarity.
48 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Exercise
• You have 1.00 mol of sugar in 125.0 mL of solution. Calculate the concentration in units of molarity.
8.00 M
49 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Exercise
• You have a 10.0 M sugar solution. What volume of this solution do you need to have 2.00 mol of sugar?
50 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Exercise
• You have a 10.0 M sugar solution. What volume of this solution do you need to have 2.00 mol of sugar?
0.200 L
51 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Exercise
• Consider separate solutions of NaOH and KCl made by dissolving 100.0 g of each solute in 250.0 mL of solution. Calculate the concentration of each solution.
52 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.6
Molarity Concentration Unit
Return to TOC
Exercise
• Consider separate solutions of NaOH and KCl made by dissolving 100.0 g of each solute in 250.0 mL of solution. Calculate the concentration of each solution.
10.0 M NaOH
5.37 M KCl
53 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
• The process in which more solvent is added to a solution in order to lower its concentration
54
Concentration of volume of concentration of volume of × = ×
stock solution stock solution diluted solution diluted solution
s C × V
⎛ ⎞ ⎛ ⎞ ⎛ ⎞ ⎛ ⎞⎜ ⎟ ⎜ ⎟ ⎜ ⎟ ⎜ ⎟⎝ ⎠ ⎝ ⎠ ⎝ ⎠ ⎝ ⎠
s d d= C × V
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
How would you prepare 100 mL of 0.9% saline solution in water from a 10% saline solution?
a. 90 mL of 10% saline solution + 100 mL of water b. 90 mL of 10% saline solution + 10 mL of water c. 9 mL of 10% saline solution + 100 mL of water d. 9 mL of 10% saline solution + 91 mL of water
55 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
How would you prepare 100 mL of 0.9% saline solution in water from a 10% saline solution?
a. 90 mL of 10% saline solution + 100 mL of water b. 90 mL of 10% saline solution + 10 mL of water c. 9 mL of 10% saline solution + 100 mL of water d. 9 mL of 10% saline solution + 91 mL of water
56 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
Concept Check
• A 0.50 M solution of sodium chloride sits on a lab bench. Which of the following would decrease the concentration of the salt solution?
a) Add water to the solution. b) Pour some of the solution down the sink drain. c) Add more sodium chloride to the solution. d) Let the solution sit out in the open air for a couple of days. e) At least two of the above would decrease the concentration
of the salt solution.
57 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
Concept Check
• A 0.50 M solution of sodium chloride sits on a lab bench. Which of the following would decrease the concentration of the salt solution?
a) Add water to the solution. b) Pour some of the solution down the sink drain. c) Add more sodium chloride to the solution. d) Let the solution sit out in the open air for a couple of days. e) At least two of the above would decrease the concentration
of the salt solution.
58 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
Exercise
• What is the minimum volume of a 2.00 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?
59 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.7
Dilution
Return to TOC
Exercise
• What is the minimum volume of a 2.00 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?
60.0 mL
60 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
Colloidal Dispersion
• A homogeneous mixture that contains dispersed particles that are intermediate in size between those of a true solution and those of an ordinary heterogeneous mixture – Dispersed phase (similar to the solute) – Dispersing medium (similar to the solvent)
61 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
Tyndall Effect
• The light-scattering phenomenon that causes the path of a beam of visible light through a colloidal dispersion to be observable – When we shine a beam of light through a true
solution, we cannot see the track of the light – A beam of light passing through a colloidal dispersion
can be observed because the light is scattered by the dispersed phase
62 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
Figure 8.10 - Scattering of Light in a Colloidal Dispersion vs. a True Solution
63 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
Suspension
• A heterogeneous mixture that contains dispersed particles that are heavy enough that they settle out under the influence of gravity
64 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
Table 8.4 - Property Comparison for Solutions, Colloidal Dispersions, and Suspensions
65 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
What is a colloidal dispersion?
a. It is a mixture that contains small particles not visible to the naked eye. b. It is a mixture that contains particles that do not settle out under the influence of gravity. c. It is a mixture that contains particles that cannot be filtered out through large pore filter paper. d. All of these.
66 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.8
Colloidal Dispersions and Suspensions
Return to TOC
What is a colloidal dispersion?
a. It is a mixture that contains small particles not visible to the naked eye. b. It is a mixture that contains particles that do not settle out under the influence of gravity. c. It is a mixture that contains particles that cannot be filtered out through large pore filter paper. d. All of these.
67 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
Colligative Property
• A physical property of a solution that depends only on the number of solute particles (molecules or ions) present in a given quantity of solvent and not on their chemical identities – Lowering of vapor-pressure – Elevation of boiling-point – Depression of freezing-point – Osmotic pressure
68 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
Vapor-Pressure Lowering
• Adding a nonvolatile solute to a solvent lowers the vapor pressure of the resulting solution below that of the pure solvent at the same temperature
69 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
Figure 8.11 - Surface of Liquid Solvent (a) Before and (b) After Addition of Solute
70 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
Boiling-Point Elevation
• Adding a nonvolatile solute to a solvent raises the boiling point of the resulting solution above that of the pure solvent
71 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
Freezing-Point Depression
• Adding a nonvolatile solute to a solvent lowers the freezing point of the resulting solution below that of the pure solvent
72 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
How does the addition of a nonvolatile solute to a solvent affect the vapor pressure of the resulting solution? a. Decreases the vapor pressure b. Increases the vapor pressure c. Has no affect on the vapor pressure d. No correct response
73 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.9
Colligative Properties of Solutions
Return to TOC
How does the addition of a nonvolatile solute to a solvent affect the vapor pressure of the resulting solution? a. Decreases the vapor pressure b. Increases the vapor pressure c. Has no affect on the vapor pressure d. No correct response
74 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Osmosis
• The passage of a solvent through a semipermeable membrane separating a dilute solution (or pure solvent) from a more concentrated solution – Semi-permeable membrane: A membrane that
allows certain types of molecules to pass through it but prohibits the passage of other types of molecules
75 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Figure 8.13 - An Illustration of the Process of Osmosis
76 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Figure 8.14 - An Illustration of a Semi-Permeable Membrane
77 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Osmotic Pressure
• The pressure that must be applied to prevent the net flow of solvent through a semipermeable membrane from a solution of lower solute concentration to a solution of higher solute concentration
78 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Osmolarity
• Used to compare the osmotic pressures of solutions
• i is the number of particles produced from the
dissociation of one formula unit of solute
79
Osmolarity = molarity × i
Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Exercise
• What is the osmolarity of a 3 M NaCl solution?
80 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Exercise
• What is the osmolarity of a 3 M NaCl solution?
6 osmol
81 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Hypotonic Solution
• A solution with a lower osmotic pressure than that within cells
82 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Hypertonic Solution
• A solution with a higher osmotic pressure than that within cells
83 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Isotonic Solution
• A solution with an osmotic pressure that is equal to that within cells
84 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Figure 8.17 - Effects of Bathing Red Blood Cells in Various Types of Solutions
85 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
Table 8.5 - Characteristics of Hypotonic, Hypertonic, and Isotonic Solutions
86 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
What is an isotonic solution? a. A solution with a lower osmotic pressure than that within cells b. A solution with a higher osmotic pressure than that within cells c. A solution with an osmotic pressure equal to that within cells d. A solution which results in a flow of water out of cells
87 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
What is an isotonic solution? a. A solution with a lower osmotic pressure than that within cells b. A solution with a higher osmotic pressure than that within cells c. A solution with an osmotic pressure equal to that within cells d. A solution which results in a flow of water out of cells
88 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
How is the osmolarity of a solution determined?
a. Calculate the molarity of the solution, since a solution’s osmolarity is equal to its molarity. b. Divide the molarity of the solution by the number of particles produced per formula unit if the solute dissociates. c. Multiply the molarity of the solution by the number of particles produced per formula unit if the solute dissociates. d. Add the number of dissociated solute particles to the molarity of the solution.
89 Copyright ©2016 Cengage Learning. All Rights Reserved.
Section 8.10
Osmosis and Osmotic Pressure
Return to TOC
How is the osmolarity of a solution determined?
a. Calculate the molarity of the solution, since a solution’s osmolarity is equal to its molarity. b. Divide the molarity of the solution by the number of particles produced per formula unit if the solute dissociates. c. Multiply the molarity of the solution by the number of particles produced per formula unit if the solute dissociates. d. Add the number of dissociated solute particles to the molarity of the solution.
90 Copyright ©2016 Cengage Learning. All Rights Reserved.
Chapter 8
Return to TOC
Concept Question 1
How would you prepare 200 mL of a 0.8 M sodium hydroxide, molar mass = 40 g/mole, solution in water? Identify the solute and solvent. a. Add 64 g of sodium hydroxide to 200 mL of water. The solvent is water, and the solute is sodium hydroxide. b. Add 64 g of sodium hydroxide to 200 mL of water. The solvent is sodium hydroxide, and the solute is water. c. Add 6.4 g of sodium hydroxide to 200 mL of water. The solvent is water, and the solute is sodium hydroxide. d. Add 6.4 g of sodium hydroxide to 200 mL of water. The solvent is sodium hydroxide, and the solute is water.
91 Copyright ©2016 Cengage Learning. All Rights Reserved.
Chapter 8
Return to TOC
Concept Question 1
How would you prepare 200 mL of a 0.8 M sodium hydroxide, molar mass = 40 g/mole, solution in water? Identify the solute and solvent. a. Add 64 g of sodium hydroxide to 200 mL of water. The solvent is water, and the solute is sodium hydroxide. b. Add 64 g of sodium hydroxide to 200 mL of water. The solvent is sodium hydroxide, and the solute is water. c. Add 6.4 g of sodium hydroxide to 200 mL of water. The solvent is water, and the solute is sodium hydroxide. d. Add 6.4 g of sodium hydroxide to 200 mL of water. The solvent is sodium hydroxide, and the solute is water.
92 Copyright ©2016 Cengage Learning. All Rights Reserved.
Chapter 8
Return to TOC
Concept Question 2
If you add 2.6 g of sodium chloride, molar mass = 58 g/mole, to 300 mL water, what is the molarity, percent (m/v), and osmolarity of this solution? a. 0.15 M, 0.9%, and 0.30 osmol b. 0.15 M, 8.7%, and 0.30 osmol c. 0.045 M, 0.09%, and 0.09 osmol d. 0.15 M, 0.9%, and 0.075 osmol
93 Copyright ©2016 Cengage Learning. All Rights Reserved.
Chapter 8
Return to TOC
Concept Question 2
If you add 2.6 g of sodium chloride, molar mass = 58 g/mole, to 300 mL water, what is the molarity, percent (m/v), and osmolarity of this solution? a. 0.15 M, 0.9%, and 0.30 osmol b. 0.15 M, 8.7%, and 0.30 osmol c. 0.045 M, 0.09%, and 0.09 osmol d. 0.15 M, 0.9%, and 0.075 osmol
94 Copyright ©2016 Cengage Learning. All Rights Reserved.