Solutions

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Solutions

• Chapter 12

• Outline
• Solutions
• Units of Concentration
• Colligative Properties

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What are the types of colloids?
Aerosol liquid in gas
Solid Aerosol solid in gas
Sol -- solid in liquid like protein particles in
milk
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Emulsion liquid in liquid like oil droplets in
mayonnaise.
Foams gases in liquids like whipped cream
Solid emulsion liquid in a solid like milk in
butter
Gel a solid emulsion which is soft but holds
its shape like Jell-O
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What type of mixture exhibits the Tyndall Effect?
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What is Brownian motion?
Tro Chemistry A Molecular Approach, 2/e
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How do mixtures differ?
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How does the solubility of a solid change with
increasing temperature?
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What are the three types of solutions?
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How does temperature affect gas solubility?
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How does gas solubility change with increasing
temperature?
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How does pressure affect gas solubility?
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How does changing the pressure affect
equilibrium?
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Chapter 12 Examples Henrys Law

• The solubility of pure nitrogen gas at 25 C and
  1.00 atm is 6.8 x 10-4 mol/L. What is the
  solubility of nitrogen gas under those conditions
  if the partial pressure of nitrogen gas is 0.78
  atm?

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What interactions must be overcome for an ionic
compound to dissolve?
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How does a micelle interact with water?
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Are solute-solute interactions exothermic or
endothermic?
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Are solvent-solvent interactions exothermic or
endothermic?
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Are solute-solvent interactions exothermic or
endothermic?
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Chapter 12 Examples Units of Concentration

• 28.0g of NaF are dissolved in 455g of water.
  What is the concentration of this solution?

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Chapter 12 Examples Units of Concentration

• How many grams of water are required to dissolve
  13.00 g of KOH in order to prepare a 7.0 KOH
  solution?

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Chapter 12 Examples Units of Concentration

• What is the molarity of a 1.2 NaCl solution?
  The density of this solution is 1.02 g/mL.

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Chapter 12 Examples Units of Concentration

• How many grams of NH4Cl are in 313 mL of a
  12.00 ammonium chloride solution? The density of
  this ammonium chloride solution is 1.05g/mL.

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Chapter 12 Examples Units of Concentration

• How many grams of water should you add to 32.5 g
  of sucrose, C12H22O11, to get a 0.85 m solution?

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Chapter 12 Examples Units of Concentration

• What is the molality of a 40 ethylene glycol,
  C2H6O2, solution?

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Chapter 12 Examples Units of Concentration

• A 0.944 M solution of glucose, C6H12O6, in water
  has a density of 1.0624 g/mL at 20C. What is the
  concentration in mass percent, mole fraction,
  and molality?

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How does the vapor pressure change when a
nonvolatile solute is added to the solvent?
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What does the distilled water transfer to the
seawater?
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How do ions affect the vant Hoff factor?
Tro Chemistry A Molecular Approach, 2/e
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How does a solute change the phase diagram of a
solvent?
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How does a solute change the phase diagram of a
solvent?
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How do intermolecular forces affect Raoults Law?
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How does a volatile solute affect a solutions
vapor pressure?

• P total PA PB
• PA (XA)(PAo)
• PB (XB)(PBo)
• PAo is the vapor pressure of the pure solvent.

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Chapter 12 Examples Colligative Properties

• Calculate the vapor pressure of water at 100 C
  of a solution prepared by dissolving 5.00 g
  sucrose, C12H22O11, in 100 g water. The vapor
  pressure of the pure solvent is 760 torr.
  

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Chapter 12 Examples Colligative Properties

• A solution was prepared by adding 20.0 g of urea
  to 125 g of water at 25 C, a temperature at
  which pure water has a vapor pressure of 23.76
  torr. The observed vapor pressure of the solution
  was found to be 22.67 torr. Calculate the molar
  mass of urea.
  

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How does a solutions molality affect its
freezing point?
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Chapter 12 Examples Colligative Properties

• Calculate the boiling point of a solution
  containing 100 g of ethylene glycol (C2H6O2 ) in
  900 g water. kb water 0.512 C/m.
  

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Chapter 12 Examples Colligative Properties

• An elemental analysis of adrenaline is 59.0 C,
  26.2 O, 7.10 H, and 7.60 N by mass. When 0.64
  g of adrenaline was dissolved in 36.0 g benzene,
  kf 5.12 C/m, the freezing point decreased by
  0.50 C. What is the molecular formula?
  

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What is osmotic pressure?
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What is osmotic pressure?
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How is osmotic pressure measured?
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Which direction will the solvent flow?
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Chapter 12 Examples Colligative Properties

• Intravenous medications are often administered
  in 5.0 glucose, C6H12O6, aqueous solutions by
  mass (density of 1.0 g/mL). What is the osmotic
  pressure of such solutions at body temperature?
  

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Chapter 12 Examples Colligative Properties

• To determine the molar mass of a certain
  protein, 1.00 x 10-3 g of the protein was
  dissolved in enough water to make 1.00 mL of
  solution. The osmotic pressure of this solution
  is found to be 1.12 torr at 25.0 C. Calculate
  the molar mass of the protein.
  

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How is osmotic pressure affecting these cells?
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What is reverse osmosis?