1. Chapter 13 Properties of Solutions
Chemistry, The Central Science, 11th edition
Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
Chapter 13 Properties of Solutions
John D. Bookstaver
St. Charles Community College
Cottleville, MO
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2. Aim: What is a solution, and how is it formed?
Do Now: Write down 1 fact/idea you remember from solutions in regents chemistry.
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3. Solutions
Solutions are homogeneous mixtures of two or more pure substances.
In a solution, the solute is dispersed uniformly throughout the solvent.
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4. Solutions
The intermolecular forces between solute and solvent particles must be strong enough to compete with those between solute particles and those between solvent particles.
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5. How Does a Solution Form?
As a solution forms, the solvent pulls solute particles apart and surrounds, or solvates, them.
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6. How Does a Solution Form
If an ionic salt is soluble in water, it is because the ion-dipole interactions are strong enough to overcome the lattice energy of the salt crystal.
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7. Energy Changes in Solution
Simply put, three processes affect the energetics of solution:
separation of solute particles,
separation of solvent particles,
new interactions between solute and solvent.
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8. Energy Changes in Solution
The enthalpy change of the overall process depends on H for each of these steps.
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9. Why Do Endothermic Processes Occur?
Things do not tend to occur spontaneously (i.e., without outside intervention) unless the energy of the system is lowered.
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10. Why Do Endothermic Processes Occur?
Yet we know the in some processes, like the dissolution of NH4NO3 in water, heat is absorbed, not released.
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11. Enthalpy Is Only Part of the Picture
The reason is that increasing the disorder or randomness (known as entropy) of a system tends to lower the energy of the system.
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12. Enthalpy Is Only Part of the Picture
So even though enthalpy may increase, the overall energy of the system can still decrease if the system becomes more disordered.
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13. Aim: What are some of the factors that affect solubility?
Do Now: Would you expect stearic acid, CH3(CH2)16COOH, to be more soluble in water or in carbon tetrachloride?
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14. Student, Beware!
Just because a substance disappears when it comes in contact with a solvent, it doesn’t mean the substance dissolved.
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15. Student, Beware!
Dissolution is a physical change — you can get back the original solute by evaporating the solvent.
If you can’t, the substance didn’t dissolve, it reacted.
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16. Give It Some Thought (Pg. 535)
Label the following processes as exothermic or endothermic:
Breaking solvent-solvent interactions to form separated particles
Forming solvent-solute interactions from separated particles
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17. Types of Solutions Saturated
In a saturated solution, the solvent holds as much solute as is possible at that temperature.
Dissolved solute is in dynamic equilibrium with solid solute particles.
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18. Types of Solutions Unsaturated
If a solution is unsaturated, less solute than can dissolve in the solvent at that temperature is dissolved in the solvent.
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19. Types of Solutions Supersaturated
In supersaturated solutions, the solvent holds more solute than is normally possible at that temperature.
These solutions are unstable; crystallization can usually be stimulated by adding a “seed crystal” or scratching the side of the flask.
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20. Give It Some Thought (Pg. 537)
What happens if a solute is added to a saturated solution?
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21. Factors Affecting Solubility
Chemists use the axiom “like dissolves like."
Polar substances tend to dissolve in polar solvents.
Nonpolar substances tend to dissolve in nonpolar solvents.
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22. Factors Affecting Solubility
The more similar the intermolecular attractions, the more likely one substance is to be soluble in another.
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23. Factors Affecting Solubility
Glucose (which has hydrogen bonding) is very soluble in water, while cyclohexane (which only has dispersion forces) is not.
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24. Factors Affecting Solubility
Vitamin A is soluble in nonpolar compounds (like fats).
Vitamin C is soluble in water.
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25. Sample Exercise 13.1 (Pg. 540)
Predict whether each of the following substances is more likely to dissolve in the nonpolar solvent carbon tetracholoride(CCl4) or in water:
C7H16, Na2SO4, HCl, I2
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26. Gases in Solution
In general, the solubility of gases in water increases with increasing mass.
Larger molecules have stronger dispersion forces.
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27. Gases in Solution
The solubility of liquids and solids does not change appreciably with pressure.
The solubility of a gas in a liquid is directly proportional to its pressure.
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28. Henry’s Law Sg = kPg where Sg is the solubility of the gas,
k is the Henry’s Law constant for that gas in that solvent, and
Pg is the partial pressure of the gas above the liquid.
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29. Sample Exercise 13.2 (Pg.543)
Calculate the concentration of CO2 in a soft drink that is bottled with a partial pressure of CO2 of 4.0 atm over the liquid at 25 degrees Celsius. The Henry’s law constant for CO2 in water at this temperature is 3.4 x 10-2 mol/L-atm.
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30. Temperature
Generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
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31. Temperature The opposite is true of gases.
Carbonated soft drinks are more “bubbly” if stored in the refrigerator.
Warm lakes have less O2 dissolved in them than cool lakes.
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32. Give it some Thought (Pg. 343)
Why do bubbles form on the inside wall of a cooking pot when water is heated on the stove, even though the water temperature is well below the boiling point of water?
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33. Chromatography : A method used to separate and purify substances
A mobile solution phase carries a mixture of compounds over a stationary insoluble phase
Gas, Liquid, and Paper Chromatography
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34. Gas Chromatography: the mobile phase is a gas, and the stationary phase is a liquid bound to a solid support
Liquid/Paper Chromatography: a liquid mobile phase, and a solid stationary phase.
Rates of movement of the compounds in the mixture depend on the strengths of attraction for the mobile phase and the stationary phase
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35. What is the mobile phase? What is the stationary phase?
Paper Chromatography
What is the mobile phase?
What is the stationary phase?
Why do the dyes separate?
Which dye has the fastest rate of movement?
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36. Acetone
Glucose
Pentane
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37. Ways of Expressing Concentrations of Solutions
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38. Mass Percentage mass of A in solution Mass % of A =
total mass of solution
Mass % of A =
 100
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39. Parts per Million and Parts per Billion
Parts per Million (ppm)
mass of A in solution
total mass of solution
ppm =
 106
Parts per Billion (ppb)
mass of A in solution
total mass of solution
ppb =
 109
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40. total moles in solution
Mole Fraction (X)
moles of A
total moles in solution
XA =
In some applications, one needs the mole fraction of solvent, not solute — make sure you find the quantity you need!
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41. Molarity (M) mol of solute M = L of solution
You will recall this concentration measure from Chapter 4.
Since volume is temperature-dependent, molarity can change with temperature.
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42. Colligative Properties
Changes in colligative properties depend only on the number of solute particles present, not on the identity of the solute particles.
Among colligative properties are
Vapor pressure lowering
Boiling point elevation
Melting point depression
Osmotic pressure
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43. Vapor Pressure
Because of solute-solvent intermolecular attraction, higher concentrations of nonvolatile solutes make it harder for solvent to escape to the vapor phase.
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44. Vapor Pressure
Therefore, the vapor pressure of a solution is lower than that of the pure solvent.
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