Chapter 10 Liquids and Solids Solids vs Liquids
![Chapter 10 Liquids and Solids Chapter 10 Liquids and Solids](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-1.jpg)
![Solids vs. Liquids vs. Gases Distance Between Solid Liquid Gas Close together Density Attractive Solids vs. Liquids vs. Gases Distance Between Solid Liquid Gas Close together Density Attractive](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-2.jpg)
![Intermolecular Forces • Occur between (not within) molecules • Covalent/Ionic Bonding • Dipole-Dipole • Intermolecular Forces • Occur between (not within) molecules • Covalent/Ionic Bonding • Dipole-Dipole •](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-3.jpg)
![Important to Note • Changing states is a PHYSICAL (not chemical) change • The Important to Note • Changing states is a PHYSICAL (not chemical) change • The](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-4.jpg)
![Dipole-Dipole Forces • Two molecules with dipoles (polarity) can have an attraction to one Dipole-Dipole Forces • Two molecules with dipoles (polarity) can have an attraction to one](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-5.jpg)
![Hydrogen Bonding • Dipole-dipole attractions that are unusually strong • Hydrogen is small and Hydrogen Bonding • Dipole-dipole attractions that are unusually strong • Hydrogen is small and](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-6.jpg)
![London Dispersion Forces • Dipole-dipole force between noble gas atoms and nonpolar molecules • London Dispersion Forces • Dipole-dipole force between noble gas atoms and nonpolar molecules •](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-7.jpg)
![Surface Tension • Molecules at a liquids’ surface are attracted to other molecules near Surface Tension • Molecules at a liquids’ surface are attracted to other molecules near](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-8.jpg)
![Capillary Action • Spontaneous rising of a liquid in a narrow tube • Typically Capillary Action • Spontaneous rising of a liquid in a narrow tube • Typically](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-9.jpg)
![How Interesting • When a liquid is polar, it forms a concave meniscus. When How Interesting • When a liquid is polar, it forms a concave meniscus. When](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-10.jpg)
![Viscosity • Measures a liquids resistance to flow • Higher IMF = higher viscosity Viscosity • Measures a liquids resistance to flow • Higher IMF = higher viscosity](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-11.jpg)
![Modeling • Solids and gases are easy to model • Liquids are not… • Modeling • Solids and gases are easy to model • Liquids are not… •](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-12.jpg)
![SOLIDS • Classified into crystalline and amorphous – Crystalline: highly regular arrangement – Amorphous: SOLIDS • Classified into crystalline and amorphous – Crystalline: highly regular arrangement – Amorphous:](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-13.jpg)
![Types of Solids • Ionic Solids: have ions at lattice points • Molecular Solids: Types of Solids • Ionic Solids: have ions at lattice points • Molecular Solids:](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-14.jpg)
![Solid Classification Solid Classification](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-15.jpg)
![Packing In Solids • Metals have characteristics based on their packing/bonding • “Closest Packing” Packing In Solids • Metals have characteristics based on their packing/bonding • “Closest Packing”](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-16.jpg)
![king Pac es o f Typ • Hexagonal Closest Packed (hcp) = hexagonal unit king Pac es o f Typ • Hexagonal Closest Packed (hcp) = hexagonal unit](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-17.jpg)
![Molecular Solids • Contain strong covalent bonding within the molecules but relatively weak forces Molecular Solids • Contain strong covalent bonding within the molecules but relatively weak forces](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-18.jpg)
![Ionic Solids • Stable, high-melting substances held together by strong electrostatic forces • Packing Ionic Solids • Stable, high-melting substances held together by strong electrostatic forces • Packing](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-19.jpg)
![• Trigonal holes formed by 3 spheres in one layer (smallest) • Tetrahedral • Trigonal holes formed by 3 spheres in one layer (smallest) • Tetrahedral](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-20.jpg)
![Vaporization • Endothermic (requires energy) • Heat of vaporization (∆Hvap) = amount of energy Vaporization • Endothermic (requires energy) • Heat of vaporization (∆Hvap) = amount of energy](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-21.jpg)
![Dynamic Equilibrium • Rate of evaporation = rate of condensation Dynamic Equilibrium • Rate of evaporation = rate of condensation](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-22.jpg)
![Clausius-Clapeyron Equation • Can be used to determine the (∆Hvap) by measuring Pvap at Clausius-Clapeyron Equation • Can be used to determine the (∆Hvap) by measuring Pvap at](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-23.jpg)
![Example • The vapor pressure of water at 25°C is 23. 8 torr, and Example • The vapor pressure of water at 25°C is 23. 8 torr, and](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-24.jpg)
![Sublimation • Solid directly to gas without passing a liquid state Sublimation • Solid directly to gas without passing a liquid state](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-25.jpg)
![Heat/Enthalpy of Fusion(∆Hfus) • Occurs when solids melt • Energy is used to disrupt Heat/Enthalpy of Fusion(∆Hfus) • Occurs when solids melt • Energy is used to disrupt](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-26.jpg)
![Heating Curve Heating Curve](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-27.jpg)
![Normal Melting/Boiling Point • Temperature at which melting/boiling occurs at STANDARD pressure (1 atm) Normal Melting/Boiling Point • Temperature at which melting/boiling occurs at STANDARD pressure (1 atm)](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-28.jpg)
![Fancy Vocab • Supercooling: Liquid remains a liquid at temperatures below 0 C at Fancy Vocab • Supercooling: Liquid remains a liquid at temperatures below 0 C at](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-29.jpg)
![Phase Diagram • Shows different conditions of temperature and pressure and the phases that Phase Diagram • Shows different conditions of temperature and pressure and the phases that](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-30.jpg)
![Critical Point: temp/press at which neither a true liquid/gas is present Critical Point: temp/press at which neither a true liquid/gas is present](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-31.jpg)
![Chapter 11 Properties of Solutions Chapter 11 Properties of Solutions](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-32.jpg)
![Important Vocabulary • Homogeneous means there is only one phase (compositions do not vary) Important Vocabulary • Homogeneous means there is only one phase (compositions do not vary)](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-33.jpg)
![Dilute vs. Concentrated • Can’t be used in calculations • Molarity, mass percent, and Dilute vs. Concentrated • Can’t be used in calculations • Molarity, mass percent, and](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-34.jpg)
![Molarity • Moles of solute/liters of solution • Represented by M • Example: A Molarity • Moles of solute/liters of solution • Represented by M • Example: A](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-35.jpg)
![Mass Percent • Percent by mass of the solute in the solution • Mass Mass Percent • Percent by mass of the solute in the solution • Mass](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-36.jpg)
![Mole Fraction • Represented by X • Moles of part/moles of solution X 100% Mole Fraction • Represented by X • Moles of part/moles of solution X 100%](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-37.jpg)
![Molality • Represented by m • Moles of solute per kilogram of solvent Molality Molality • Represented by m • Moles of solute per kilogram of solvent Molality](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-38.jpg)
![NEW: Normality (N) • Number of “equivalents” per liter of solution • Equivalents - NEW: Normality (N) • Number of “equivalents” per liter of solution • Equivalents -](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-39.jpg)
![Normality Example • Given the following reaction: H 3 PO 4 + 3 Na. Normality Example • Given the following reaction: H 3 PO 4 + 3 Na.](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-40.jpg)
![Solubility • Shows what will dissolve in what • “Like dissolves like” = polar Solubility • Shows what will dissolve in what • “Like dissolves like” = polar](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-41.jpg)
![Factors Affecting Solubility 1. Structure 2. Pressure 3. Temperature Factors Affecting Solubility 1. Structure 2. Pressure 3. Temperature](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-42.jpg)
![1. Structure Effects • Polarity of solute/solvent (like dissolves like) • Example: vitamins are 1. Structure Effects • Polarity of solute/solvent (like dissolves like) • Example: vitamins are](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-43.jpg)
![2. Pressure Effects • Doesn’t affect liquids/solids, but has a large affect on gases 2. Pressure Effects • Doesn’t affect liquids/solids, but has a large affect on gases](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-44.jpg)
![Henry’s Law • Shows relationship between gas pressure and concentration of dissolved gas: C Henry’s Law • Shows relationship between gas pressure and concentration of dissolved gas: C](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-45.jpg)
![Henry’s Law Example • The solubility of O 2 is 2. 2 X 10 Henry’s Law Example • The solubility of O 2 is 2. 2 X 10](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-46.jpg)
![3. Temperature Effects • For most solids, solubility increases as temperature increases • For 3. Temperature Effects • For most solids, solubility increases as temperature increases • For](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-47.jpg)
![Vapor Pressure of Solutions • If a solution contains a nonvolitile (not easily vaporized) Vapor Pressure of Solutions • If a solution contains a nonvolitile (not easily vaporized)](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-48.jpg)
![• Molecules that do not dissociate (break up) in water (solvent) have higher • Molecules that do not dissociate (break up) in water (solvent) have higher](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-49.jpg)
![Answer This… • Which compound affects the vapor pressure of a solution the least: Answer This… • Which compound affects the vapor pressure of a solution the least:](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-50.jpg)
![Raoult’s Law • Calculates the expected vapor pressure of a solution based on the Raoult’s Law • Calculates the expected vapor pressure of a solution based on the](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-51.jpg)
![Example • Glycerin, C 3 H 8 O 3, is a nonvolatile liquid. What Example • Glycerin, C 3 H 8 O 3, is a nonvolatile liquid. What](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-52.jpg)
![Example #2 • What is the vapor pressure of a solution made by adding Example #2 • What is the vapor pressure of a solution made by adding](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-53.jpg)
![Colligative Properties • Depend on the number of solute particles, NOT their identity in Colligative Properties • Depend on the number of solute particles, NOT their identity in](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-54.jpg)
![1. Boiling-Point Elevation • Review boiling point definition: when vapor pressure = atmospheric pressure 1. Boiling-Point Elevation • Review boiling point definition: when vapor pressure = atmospheric pressure](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-55.jpg)
![• Antifreeze in car engines (solute) makes it so car engines don’t boil • Antifreeze in car engines (solute) makes it so car engines don’t boil](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-56.jpg)
![Boiling-Point Elevation Calculation • Change in boiling point ∆Tb is the difference between the Boiling-Point Elevation Calculation • Change in boiling point ∆Tb is the difference between the](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-57.jpg)
![Example • What is the boiling point of a solution containing 96. 7 g Example • What is the boiling point of a solution containing 96. 7 g](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-58.jpg)
![2. Freezing-Point Depression • When solute is present, the normal molecular freezing pattern is 2. Freezing-Point Depression • When solute is present, the normal molecular freezing pattern is](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-59.jpg)
![• The more solute particles dissolved, the more the freezing point decreases (identity • The more solute particles dissolved, the more the freezing point decreases (identity](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-60.jpg)
![Freezing-Point Depression Calculation • Change in freezing point ∆Tf is the difference between the Freezing-Point Depression Calculation • Change in freezing point ∆Tf is the difference between the](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-61.jpg)
![Example • Determine the freezing point of a solution made by adding 27. 5 Example • Determine the freezing point of a solution made by adding 27. 5](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-62.jpg)
![3. Osmotic Pressure • Solution and solvent are separated by a semipermeable membrane which 3. Osmotic Pressure • Solution and solvent are separated by a semipermeable membrane which](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-63.jpg)
![• Pressure can be applied to make it so this doesn’t happen (osmotic • Pressure can be applied to make it so this doesn’t happen (osmotic](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-64.jpg)
![Molar Mass From Osmotic Pressure • Useful b/c small concentration of solute can lead Molar Mass From Osmotic Pressure • Useful b/c small concentration of solute can lead](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-65.jpg)
![Example • The osmotic pressure of a solution containing 26. 5 mg of aspartame Example • The osmotic pressure of a solution containing 26. 5 mg of aspartame](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-66.jpg)
![Osmosis vs. Dialysis • Osmosis only allows SOLVENT to travel across the semipermeable membrane Osmosis vs. Dialysis • Osmosis only allows SOLVENT to travel across the semipermeable membrane](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-67.jpg)
![Reverse Osmosis • An external pressure greater than osmotic pressure allows a semipermeable membrane Reverse Osmosis • An external pressure greater than osmotic pressure allows a semipermeable membrane](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-68.jpg)
![Watch Out! • Ionic compounds break up in water, so the concentration is significantly Watch Out! • Ionic compounds break up in water, so the concentration is significantly](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-69.jpg)
![Adjustment…van’t Hoff Factor, i • i = moles of particles in solution moles of Adjustment…van’t Hoff Factor, i • i = moles of particles in solution moles of](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-70.jpg)
![Example • Find the boiling point of a 1. 50 m solution of calcium Example • Find the boiling point of a 1. 50 m solution of calcium](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-71.jpg)
![Example - WATCH OUT! • Use data from Table 11. 6 in your textbook Example - WATCH OUT! • Use data from Table 11. 6 in your textbook](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-72.jpg)
![Additional Definitions • Colloid/colloidal dispersion: suspension of tiny particles in a medium • Tyndall Additional Definitions • Colloid/colloidal dispersion: suspension of tiny particles in a medium • Tyndall](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-73.jpg)
- Slides: 73
![Chapter 10 Liquids and Solids Chapter 10 Liquids and Solids](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-1.jpg)
Chapter 10 Liquids and Solids
![Solids vs Liquids vs Gases Distance Between Solid Liquid Gas Close together Density Attractive Solids vs. Liquids vs. Gases Distance Between Solid Liquid Gas Close together Density Attractive](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-2.jpg)
Solids vs. Liquids vs. Gases Distance Between Solid Liquid Gas Close together Density Attractive Fills Compressibility Force Container High Large No Barely (rigid) Somewhere in between…but generally more similar to solids Far apart Low Small Yes High
![Intermolecular Forces Occur between not within molecules CovalentIonic Bonding DipoleDipole Intermolecular Forces • Occur between (not within) molecules • Covalent/Ionic Bonding • Dipole-Dipole •](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-3.jpg)
Intermolecular Forces • Occur between (not within) molecules • Covalent/Ionic Bonding • Dipole-Dipole • London Dispersion Forces
![Important to Note Changing states is a PHYSICAL not chemical change The Important to Note • Changing states is a PHYSICAL (not chemical) change • The](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-4.jpg)
Important to Note • Changing states is a PHYSICAL (not chemical) change • The molecules do NOT break apart in a physical (phase) change!
![DipoleDipole Forces Two molecules with dipoles polarity can have an attraction to one Dipole-Dipole Forces • Two molecules with dipoles (polarity) can have an attraction to one](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-5.jpg)
Dipole-Dipole Forces • Two molecules with dipoles (polarity) can have an attraction to one another called a dipole attraction • This will make the most +, - attractions and -, and +, + repulsions • Hydrogen bonding is a common (stronger) example Dipole-Dipole < Covalent < Ionic
![Hydrogen Bonding Dipoledipole attractions that are unusually strong Hydrogen is small and Hydrogen Bonding • Dipole-dipole attractions that are unusually strong • Hydrogen is small and](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-6.jpg)
Hydrogen Bonding • Dipole-dipole attractions that are unusually strong • Hydrogen is small and can arrange itself closely to other atoms/molecules • Bond polarities also allow hydrogen to be attracted to the slightly negative end of a polar molecule • Causes higher boiling points • Important in organic molecules (especially large ones)
![London Dispersion Forces Dipoledipole force between noble gas atoms and nonpolar molecules London Dispersion Forces • Dipole-dipole force between noble gas atoms and nonpolar molecules •](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-7.jpg)
London Dispersion Forces • Dipole-dipole force between noble gas atoms and nonpolar molecules • Instantaneous dipole (NO permanent dipole) which causes a similar dipole in an adjacent atom • Weak, short-lived attraction causes the freezing points of LARGER molecules to be lower • Larger molecules have greater LDF’s
![Surface Tension Molecules at a liquids surface are attracted to other molecules near Surface Tension • Molecules at a liquids’ surface are attracted to other molecules near](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-8.jpg)
Surface Tension • Molecules at a liquids’ surface are attracted to other molecules near the surface (next to) and directly below them • To increase the surface area, energy is required to move molecules from the inside out (combatting surface tension) • Liquids with large IMF will have higher surface tensions
![Capillary Action Spontaneous rising of a liquid in a narrow tube Typically Capillary Action • Spontaneous rising of a liquid in a narrow tube • Typically](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-9.jpg)
Capillary Action • Spontaneous rising of a liquid in a narrow tube • Typically exhibited by polar liquids • Cohesive forces: intermolecular forces between liquid molecules • Adhesive forces: forces between liquid molecules and a container
![How Interesting When a liquid is polar it forms a concave meniscus When How Interesting • When a liquid is polar, it forms a concave meniscus. When](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-10.jpg)
How Interesting • When a liquid is polar, it forms a concave meniscus. When a liquid is nonpolar, it forms a convex meniscus.
![Viscosity Measures a liquids resistance to flow Higher IMF higher viscosity Viscosity • Measures a liquids resistance to flow • Higher IMF = higher viscosity](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-11.jpg)
Viscosity • Measures a liquids resistance to flow • Higher IMF = higher viscosity • More complex molecules = higher viscosity
![Modeling Solids and gases are easy to model Liquids are not Modeling • Solids and gases are easy to model • Liquids are not… •](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-12.jpg)
Modeling • Solids and gases are easy to model • Liquids are not… • Spectroscopy is used
![SOLIDS Classified into crystalline and amorphous Crystalline highly regular arrangement Amorphous SOLIDS • Classified into crystalline and amorphous – Crystalline: highly regular arrangement – Amorphous:](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-13.jpg)
SOLIDS • Classified into crystalline and amorphous – Crystalline: highly regular arrangement – Amorphous: disorderly structure • Crystalline represented by various lattice structures (3 D positioning) called crystal lattice structures
![Types of Solids Ionic Solids have ions at lattice points Molecular Solids Types of Solids • Ionic Solids: have ions at lattice points • Molecular Solids:](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-14.jpg)
Types of Solids • Ionic Solids: have ions at lattice points • Molecular Solids: have covalently bonded molecules at lattice points • Atomic Solids: have atoms at lattice points (examples: metallic solids, network solids, and Group 8 A solids) – Metallic: delocalized nondirectional covalent bonding – Network: atoms bonded with strong directional covalent bonds – Group 8 A: noble gas elements attracted with LDF
![Solid Classification Solid Classification](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-15.jpg)
Solid Classification
![Packing In Solids Metals have characteristics based on their packingbonding Closest Packing Packing In Solids • Metals have characteristics based on their packing/bonding • “Closest Packing”](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-16.jpg)
Packing In Solids • Metals have characteristics based on their packing/bonding • “Closest Packing” spherical atoms are packed together in an arrangement that most efficiently uses the available space
![king Pac es o f Typ Hexagonal Closest Packed hcp hexagonal unit king Pac es o f Typ • Hexagonal Closest Packed (hcp) = hexagonal unit](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-17.jpg)
king Pac es o f Typ • Hexagonal Closest Packed (hcp) = hexagonal unit cell…abab… • Cubic Closest Packed (ccp) = face-centered cubic unit cell…abcabcabc…
![Molecular Solids Contain strong covalent bonding within the molecules but relatively weak forces Molecular Solids • Contain strong covalent bonding within the molecules but relatively weak forces](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-18.jpg)
Molecular Solids • Contain strong covalent bonding within the molecules but relatively weak forces between the molecules • The type of bond that forms between molecules will depend on the atoms present (LDF, hydrogen bonding, etc. )
![Ionic Solids Stable highmelting substances held together by strong electrostatic forces Packing Ionic Solids • Stable, high-melting substances held together by strong electrostatic forces • Packing](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-19.jpg)
Ionic Solids • Stable, high-melting substances held together by strong electrostatic forces • Packing occurs so that the electrostatic forces among oppositely charged ions are maximized and repulsions are minimized • Larger ions (anions) are packed in hcp or ccp • Smaller ions (cations) are packed into holes made by the larger ions.
![Trigonal holes formed by 3 spheres in one layer smallest Tetrahedral • Trigonal holes formed by 3 spheres in one layer (smallest) • Tetrahedral](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-20.jpg)
• Trigonal holes formed by 3 spheres in one layer (smallest) • Tetrahedral holes formed by one sphere sitting in a dimple formed by three other spheres (medium) • Octahedral holes formed between two sets of three spheres (largest)
![Vaporization Endothermic requires energy Heat of vaporization Hvap amount of energy Vaporization • Endothermic (requires energy) • Heat of vaporization (∆Hvap) = amount of energy](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-21.jpg)
Vaporization • Endothermic (requires energy) • Heat of vaporization (∆Hvap) = amount of energy required to vaporize 1 mole of a liquid at 1 atm • Liquids with high vaporization - VOLATILE • Vapor pressure is partly determined by intermolecular forces (large IMF = lower VP) • Vapor pressure increases with temperature
![Dynamic Equilibrium Rate of evaporation rate of condensation Dynamic Equilibrium • Rate of evaporation = rate of condensation](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-22.jpg)
Dynamic Equilibrium • Rate of evaporation = rate of condensation
![ClausiusClapeyron Equation Can be used to determine the Hvap by measuring Pvap at Clausius-Clapeyron Equation • Can be used to determine the (∆Hvap) by measuring Pvap at](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-23.jpg)
Clausius-Clapeyron Equation • Can be used to determine the (∆Hvap) by measuring Pvap at different temperatures and evaluating a line of best fit… ln(Pvap, T 1/Pvap, T 2) = (∆Hvap/R)(1/T 2 -1/T 1) ∆Hvap = must be in J (X 1000) R = constant (8. 3145 J/Kmol) T = Kelvin ***to solve ln(x), do e^ for both sides
![Example The vapor pressure of water at 25C is 23 8 torr and Example • The vapor pressure of water at 25°C is 23. 8 torr, and](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-24.jpg)
Example • The vapor pressure of water at 25°C is 23. 8 torr, and the heat of vaporization of water at 25°C is 43. 9 k. J/mol. Calculate the vapor pressure of water at 50°C. • Answer: 93. 7 torr
![Sublimation Solid directly to gas without passing a liquid state Sublimation • Solid directly to gas without passing a liquid state](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-25.jpg)
Sublimation • Solid directly to gas without passing a liquid state
![HeatEnthalpy of FusionHfus Occurs when solids melt Energy is used to disrupt Heat/Enthalpy of Fusion(∆Hfus) • Occurs when solids melt • Energy is used to disrupt](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-26.jpg)
Heat/Enthalpy of Fusion(∆Hfus) • Occurs when solids melt • Energy is used to disrupt the bonds present between solid molecules • Temperature remains constant
![Heating Curve Heating Curve](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-27.jpg)
Heating Curve
![Normal MeltingBoiling Point Temperature at which meltingboiling occurs at STANDARD pressure 1 atm Normal Melting/Boiling Point • Temperature at which melting/boiling occurs at STANDARD pressure (1 atm)](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-28.jpg)
Normal Melting/Boiling Point • Temperature at which melting/boiling occurs at STANDARD pressure (1 atm)
![Fancy Vocab Supercooling Liquid remains a liquid at temperatures below 0 C at Fancy Vocab • Supercooling: Liquid remains a liquid at temperatures below 0 C at](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-29.jpg)
Fancy Vocab • Supercooling: Liquid remains a liquid at temperatures below 0 C at 1 atm due to lack of solid arrangement necessary – When orderly arrangement necessary occurs, liquid will rapidly solidify • Superheating: liquid temperature raises above boiling point. Bubbles make it so the molecules with the most KE/highest temp collect in one area – Boiling chips are used to avoid these bubbles
![Phase Diagram Shows different conditions of temperature and pressure and the phases that Phase Diagram • Shows different conditions of temperature and pressure and the phases that](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-30.jpg)
Phase Diagram • Shows different conditions of temperature and pressure and the phases that occur for different substances • Only works with a closed system • Triple Point: all three phases exist in equilibrium
![Critical Point temppress at which neither a true liquidgas is present Critical Point: temp/press at which neither a true liquid/gas is present](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-31.jpg)
Critical Point: temp/press at which neither a true liquid/gas is present
![Chapter 11 Properties of Solutions Chapter 11 Properties of Solutions](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-32.jpg)
Chapter 11 Properties of Solutions
![Important Vocabulary Homogeneous means there is only one phase compositions do not vary Important Vocabulary • Homogeneous means there is only one phase (compositions do not vary)](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-33.jpg)
Important Vocabulary • Homogeneous means there is only one phase (compositions do not vary) • Ex: Kool Aid, air, steel • Solute: Gets dissolved • Solvent: Does the dissolving • Solution: Homogeneous mixture consisting of a solute and solvent
![Dilute vs Concentrated Cant be used in calculations Molarity mass percent and Dilute vs. Concentrated • Can’t be used in calculations • Molarity, mass percent, and](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-34.jpg)
Dilute vs. Concentrated • Can’t be used in calculations • Molarity, mass percent, and mole fraction can be used to show solution concentrations
![Molarity Moles of soluteliters of solution Represented by M Example A Molarity • Moles of solute/liters of solution • Represented by M • Example: A](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-35.jpg)
Molarity • Moles of solute/liters of solution • Represented by M • Example: A solution was prepared by adding 5. 84 g of formaldehyde, H 2 CO, to 100. 0 g of water. The final volume of the solution was 104. 0 m. L. Calculate the molarity. • Answer: 1. 87 M H 2 CO
![Mass Percent Percent by mass of the solute in the solution Mass Mass Percent • Percent by mass of the solute in the solution • Mass](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-36.jpg)
Mass Percent • Percent by mass of the solute in the solution • Mass Percent = (mass of solute/mass of solution) X 100% • Example: A solution was prepared by adding 5. 84 g of formaldehyde, H 2 CO, to 100. 0 g of water. The final volume of the solution was 104. 0 m. L. Calculate the mass percent. • Answer: 5. 52 % H 2 CO, 94. 48% H 2 O
![Mole Fraction Represented by X Moles of partmoles of solution X 100 Mole Fraction • Represented by X • Moles of part/moles of solution X 100%](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-37.jpg)
Mole Fraction • Represented by X • Moles of part/moles of solution X 100% Mole Frac. A = XA = n. A/(n. A+n. B) • Example: A solution was prepared by adding 5. 84 g of formaldehyde, H 2 CO, to 100. 0 g of water. The final volume of the solution was 104. 0 m. L. Calculate the mole fraction. • Answer: XH 2 CO = 0. 0338, XH 2 O = 0. 9662
![Molality Represented by m Moles of solute per kilogram of solvent Molality Molality • Represented by m • Moles of solute per kilogram of solvent Molality](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-38.jpg)
Molality • Represented by m • Moles of solute per kilogram of solvent Molality = moles of solute/kilogram of solvent • Example: A solution was prepared by adding 5. 84 g of formaldehyde, H 2 CO, to 100. 0 g of water. The final volume of the solution was 104. 0 m. L. Calculate the molality. • Answer: 1. 94 m H 2 CO
![NEW Normality N Number of equivalents per liter of solution Equivalents NEW: Normality (N) • Number of “equivalents” per liter of solution • Equivalents -](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-39.jpg)
NEW: Normality (N) • Number of “equivalents” per liter of solution • Equivalents - depends on reaction: – Acid-base reactions…mass of acid/base that can use/accept ONE mole of protons – Oxidation-reduction…quantity of oxidizing/reducing agent that will react with ONE mole of electrons • NOT ON AP EXAM!!
![Normality Example Given the following reaction H 3 PO 4 3 Na Normality Example • Given the following reaction: H 3 PO 4 + 3 Na.](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-40.jpg)
Normality Example • Given the following reaction: H 3 PO 4 + 3 Na. OH --> PO 43 - + 3 H 2 O + 3 Na+ If we have 28. 42 g H 3 PO 4 in 800 m. L of water, what is the normality of the solution? Answer: 1. 09 N H 3 PO 4
![Solubility Shows what will dissolve in what Like dissolves like polar Solubility • Shows what will dissolve in what • “Like dissolves like” = polar](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-41.jpg)
Solubility • Shows what will dissolve in what • “Like dissolves like” = polar solvents will dissolve polar/ionic solutes and nonpolar solvents will dissolve nonpolar solutes
![Factors Affecting Solubility 1 Structure 2 Pressure 3 Temperature Factors Affecting Solubility 1. Structure 2. Pressure 3. Temperature](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-42.jpg)
Factors Affecting Solubility 1. Structure 2. Pressure 3. Temperature
![1 Structure Effects Polarity of solutesolvent like dissolves like Example vitamins are 1. Structure Effects • Polarity of solute/solvent (like dissolves like) • Example: vitamins are](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-43.jpg)
1. Structure Effects • Polarity of solute/solvent (like dissolves like) • Example: vitamins are fat-soluble and watersoluble – Fat-soluble = nonpolar, hydrophobic (water-fearing), build up/stored in fatty tissue, too much = hypervitaminosis – Water-soluble = polar, hydrophilic (water-loving), extra are excreted by the body
![2 Pressure Effects Doesnt affect liquidssolids but has a large affect on gases 2. Pressure Effects • Doesn’t affect liquids/solids, but has a large affect on gases](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-44.jpg)
2. Pressure Effects • Doesn’t affect liquids/solids, but has a large affect on gases • Gas solubility increases as the partial pressure of the gas above the solution increases
![Henrys Law Shows relationship between gas pressure and concentration of dissolved gas C Henry’s Law • Shows relationship between gas pressure and concentration of dissolved gas: C](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-45.jpg)
Henry’s Law • Shows relationship between gas pressure and concentration of dissolved gas: C = k. P • C = concentration of dissolved gas • K = constant for particular solution • P = partial pressure of gas above solution • Works best with gases that don’t dissociate in/react with solvent
![Henrys Law Example The solubility of O 2 is 2 2 X 10 Henry’s Law Example • The solubility of O 2 is 2. 2 X 10](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-46.jpg)
Henry’s Law Example • The solubility of O 2 is 2. 2 X 10 -4 M at 0 C and 0. 10 atm. Calculate the solubility of O 2 at 0 C and 0. 35 atm. • Answer: 7. 7 X 10 -4 M O 2
![3 Temperature Effects For most solids solubility increases as temperature increases For 3. Temperature Effects • For most solids, solubility increases as temperature increases • For](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-47.jpg)
3. Temperature Effects • For most solids, solubility increases as temperature increases • For most gases, solubility decreases as temperature increases – Thermal Pollution in lakes: increase in temp. lowers dissolved oxygen concentrations
![Vapor Pressure of Solutions If a solution contains a nonvolitile not easily vaporized Vapor Pressure of Solutions • If a solution contains a nonvolitile (not easily vaporized)](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-48.jpg)
Vapor Pressure of Solutions • If a solution contains a nonvolitile (not easily vaporized) solute, its vapor pressure is LOWER than the pure solvent. • Shells of water solvation make it so it’s harder for the solvent to vaporize
![Molecules that do not dissociate break up in water solvent have higher • Molecules that do not dissociate (break up) in water (solvent) have higher](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-49.jpg)
• Molecules that do not dissociate (break up) in water (solvent) have higher vapor pressures than ionic compounds that do dissociate • The decrease in a solution’s vapor pressure is proportional to the number of particles the solute makes in solution.
![Answer This Which compound affects the vapor pressure of a solution the least Answer This… • Which compound affects the vapor pressure of a solution the least:](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-50.jpg)
Answer This… • Which compound affects the vapor pressure of a solution the least: glucose, sodium chloride, or calcium chloride? • Solutions with covalent compounds > Solutions with ionic compounds
![Raoults Law Calculates the expected vapor pressure of a solution based on the Raoult’s Law • Calculates the expected vapor pressure of a solution based on the](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-51.jpg)
Raoult’s Law • Calculates the expected vapor pressure of a solution based on the solute/solvent Psoln = Xsolvent. P 0 solvent • Psoln = observed vapor pressure of solution • Xsolvent = mole fraction of solvent • P 0 solvent = vapor pressure of the pure solvent
![Example Glycerin C 3 H 8 O 3 is a nonvolatile liquid What Example • Glycerin, C 3 H 8 O 3, is a nonvolatile liquid. What](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-52.jpg)
Example • Glycerin, C 3 H 8 O 3, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding 164 g of glycerin to 338 m. L of H 2 O at 39. 8 C? The vapor pressure of pure water at 39. 8 C is 54. 74 torr and its density is 0. 992 g/m. L. • Answer: 50. 0 torr
![Example 2 What is the vapor pressure of a solution made by adding Example #2 • What is the vapor pressure of a solution made by adding](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-53.jpg)
Example #2 • What is the vapor pressure of a solution made by adding 52. 9 g of Cu. Cl 2, a strong electrolyte, to 800. 0 m. L of water at 52. 0 C? The vapor pressure of water is 102. 1 torr, and its density is 0. 987 g/m. L. • Answer: 99. 4 torr
![Colligative Properties Depend on the number of solute particles NOT their identity in Colligative Properties • Depend on the number of solute particles, NOT their identity in](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-54.jpg)
Colligative Properties • Depend on the number of solute particles, NOT their identity in an ideal solution 1. Boiling-Point Elevation 2. Freezing-Point Depression 3. Osmotic Pressure
![1 BoilingPoint Elevation Review boiling point definition when vapor pressure atmospheric pressure 1. Boiling-Point Elevation • Review boiling point definition: when vapor pressure = atmospheric pressure](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-55.jpg)
1. Boiling-Point Elevation • Review boiling point definition: when vapor pressure = atmospheric pressure • When solute is added to solvent, it lowers the vapor pressure. • More kinetic energy must be added to bring the solution to boiling • Boiling point is HIGHER in solutions than in pure solvents
![Antifreeze in car engines solute makes it so car engines dont boil • Antifreeze in car engines (solute) makes it so car engines don’t boil](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-56.jpg)
• Antifreeze in car engines (solute) makes it so car engines don’t boil in high temperatures • The more solute particles dissolved, the higher the boiling point (identity doesn’t matter)
![BoilingPoint Elevation Calculation Change in boiling point Tb is the difference between the Boiling-Point Elevation Calculation • Change in boiling point ∆Tb is the difference between the](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-57.jpg)
Boiling-Point Elevation Calculation • Change in boiling point ∆Tb is the difference between the boiling point of the solution and the pure solvent • Unit: °C/m • Calculated using ∆Tb = Kb X msolute Kb is a molal boiling-point elevation constant of the solvent found on pg. 517
![Example What is the boiling point of a solution containing 96 7 g Example • What is the boiling point of a solution containing 96. 7 g](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-58.jpg)
Example • What is the boiling point of a solution containing 96. 7 g of sucrose (C 12 H 22 O 11) in 250. 0 g water at 1 atm? • Answer: 100. 579°C
![2 FreezingPoint Depression When solute is present the normal molecular freezing pattern is 2. Freezing-Point Depression • When solute is present, the normal molecular freezing pattern is](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-59.jpg)
2. Freezing-Point Depression • When solute is present, the normal molecular freezing pattern is disrupted • This makes it so the solution has to lose more kinetic energy (get colder) in order to solidify • Freezing point of the solution is LOWER than that of the pure solvent
![The more solute particles dissolved the more the freezing point decreases identity • The more solute particles dissolved, the more the freezing point decreases (identity](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-60.jpg)
• The more solute particles dissolved, the more the freezing point decreases (identity doesn’t matter) • Sidewalk salt and car antifreeze work this way
![FreezingPoint Depression Calculation Change in freezing point Tf is the difference between the Freezing-Point Depression Calculation • Change in freezing point ∆Tf is the difference between the](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-61.jpg)
Freezing-Point Depression Calculation • Change in freezing point ∆Tf is the difference between the freezing point of the solution and the pure solvent • Unit: °C/m • Calculated using ∆Tf = Kf X msolute Kf is a molal freezing-point depression constant of the solvent found on pg. 517
![Example Determine the freezing point of a solution made by adding 27 5 Example • Determine the freezing point of a solution made by adding 27. 5](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-62.jpg)
Example • Determine the freezing point of a solution made by adding 27. 5 g of methanol (CH 3 OH) to 250. 0 g of water. • Answer: -6. 39°C
![3 Osmotic Pressure Solution and solvent are separated by a semipermeable membrane which 3. Osmotic Pressure • Solution and solvent are separated by a semipermeable membrane which](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-63.jpg)
3. Osmotic Pressure • Solution and solvent are separated by a semipermeable membrane which allows the solvent (not solute) through • OSMOSIS happens until equilibrium occurs
![Pressure can be applied to make it so this doesnt happen osmotic • Pressure can be applied to make it so this doesn’t happen (osmotic](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-64.jpg)
• Pressure can be applied to make it so this doesn’t happen (osmotic pressure)
![Molar Mass From Osmotic Pressure Useful bc small concentration of solute can lead Molar Mass From Osmotic Pressure • Useful b/c small concentration of solute can lead](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-65.jpg)
Molar Mass From Osmotic Pressure • Useful b/c small concentration of solute can lead to a large osmotic pressure ∏ = MRT • • ∏ = osmotic pressure (atm) M = molarity of solution R = ideal gas law constant (0. 08206 Latm/Kmol) T = temperature (K)
![Example The osmotic pressure of a solution containing 26 5 mg of aspartame Example • The osmotic pressure of a solution containing 26. 5 mg of aspartame](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-66.jpg)
Example • The osmotic pressure of a solution containing 26. 5 mg of aspartame per liter is 1. 70 torr at 30 C. Calculate the molar mass of aspartame. • Answer: 294 g/mol
![Osmosis vs Dialysis Osmosis only allows SOLVENT to travel across the semipermeable membrane Osmosis vs. Dialysis • Osmosis only allows SOLVENT to travel across the semipermeable membrane](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-67.jpg)
Osmosis vs. Dialysis • Osmosis only allows SOLVENT to travel across the semipermeable membrane • Dialysis allows solvent and small solute molecules and ions to travel across the membrane – Occurs in most plant and animal cells • Isotonic = when solutions have identical osmotic pressures
![Reverse Osmosis An external pressure greater than osmotic pressure allows a semipermeable membrane Reverse Osmosis • An external pressure greater than osmotic pressure allows a semipermeable membrane](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-68.jpg)
Reverse Osmosis • An external pressure greater than osmotic pressure allows a semipermeable membrane to be used as a “molecular filter”, removing solute • Desalination - removal of dissolved salts from water - happens via this process
![Watch Out Ionic compounds break up in water so the concentration is significantly Watch Out! • Ionic compounds break up in water, so the concentration is significantly](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-69.jpg)
Watch Out! • Ionic compounds break up in water, so the concentration is significantly more… • If the concentration says 0. 25 m Na. Cl it means 0. 25 m Na AND 0. 25 m Cl. Total molality is 0. 50 • If the concentration says 0. 35 m Ca. Cl 2 it means 0. 35 m Ca, 0. 35 m Cl, and 0. 35 m Cl. Total molality is 1. 05 m
![Adjustmentvant Hoff Factor i i moles of particles in solution moles of Adjustment…van’t Hoff Factor, i • i = moles of particles in solution moles of](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-70.jpg)
Adjustment…van’t Hoff Factor, i • i = moles of particles in solution moles of solute dissolved • This modifies the equations for freezing/boiling point changes: ∆T = im. K • Also modifies the equation for osmotic pressure: ∏ = i. MRT
![Example Find the boiling point of a 1 50 m solution of calcium Example • Find the boiling point of a 1. 50 m solution of calcium](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-71.jpg)
Example • Find the boiling point of a 1. 50 m solution of calcium chloride, Ca. Cl 2 and water. • Answer: 2. 30°C so the new boiling point would be 102. 30°C.
![Example WATCH OUT Use data from Table 11 6 in your textbook Example - WATCH OUT! • Use data from Table 11. 6 in your textbook](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-72.jpg)
Example - WATCH OUT! • Use data from Table 11. 6 in your textbook to calculate the freezing point and expected osmotic pressure of a 0. 50 m Fe. Cl 3 solution at 25. 0 C. (Assume the density of the final solution equals 1. 0 g/m. L and that the liquid volume is unchanged by the addition of Fe. Cl 3. ) • Answer: FP: -0. 32 C, OP: 4. 16 atm
![Additional Definitions Colloidcolloidal dispersion suspension of tiny particles in a medium Tyndall Additional Definitions • Colloid/colloidal dispersion: suspension of tiny particles in a medium • Tyndall](https://slidetodoc.com/presentation_image_h2/61b60f6d0d96cca730ad8892360bd186/image-73.jpg)
Additional Definitions • Colloid/colloidal dispersion: suspension of tiny particles in a medium • Tyndall Effect: scattering of light by particles • Coagulation: destruction of a colloid through heat or electrolyte addition
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