Properties of Solutions

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Properties of Solutions
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Classification of Matter
Solutions are homogeneous mixtures
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Solute
A solute is the dissolved substance in a solution.
Salt in salt water
Sugar in soda drinks
Carbon dioxide in soda drinks
Solvent
A solvent is the dissolving medium in a solution.
Water in salt water
Water in soda
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Calculations of Solution Concentration
Mass percent - the ratio of mass units of solute
to mass units of solution, expressed as a percent
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Calculations of Solution Concentration
Mole fraction the ratio of moles of solute to
total moles of solution
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Calculations of Solution Concentration
Molality moles of solute per kilogram of
solvent
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Calculations of Solution Concentration
Molarity - the ratio of moles of solute to liters
of solution
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Heat of Solution
The Heat of Solution is the amount of heat energy
absorbed (endothermic) or released (exothermic)
when a specific amount of solute dissolves in a
solvent.
Substance Heat of Solution (kJ/mol)
NaOH -44.51
NH4NO3 25.69
KNO3 34.89
HCl -74.84
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Steps in Solution Formation
?H1 Expanding the solute
Separating the solute into individual components
?H2 Expanding the solvent
Overcoming intermolecular forces of the solvent
molecules
?H3 Interaction of solute and solvent to
form the solution
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Like Dissolves Like
Nonpolar solutes dissolve best in nonpolar
solvents
Fats Benzene
Steroids Hexane
Waxes Toluene
Polar and ionic solutes dissolve best in polar
solvents
Inorganic Salts Water
Sugars Small alcohols
Acetic acid
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Predicting Solution Formation
Solvent/ Solute ?H1 ?H2 ?H3 ?Hsoln Outcome
Polar/ Polar large large - large /-small Solution forms
Polar/ Nonpolar small large /- small large No solution forms
Nonpolar/ Nonpolar small small /- small /- small Solution forms
Nonpolar/ polar large small /- small large No solution forms
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Solubility Trends

• The solubility of MOST solids increases with
  temperature.
• The rate at which solids dissolve increases with
  increasing surface area of the solid.
• The solubility of gases decreases with increases
  in temperature.
• The solubility of gases increases with the
  pressure above the solution.

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Therefore
Solids tend to dissolve best when

• Heated
• Stirred
• Ground into small particles

Liquids tend to dissolve best when

• The solution is cold
• Pressure is high

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Saturation of Solutions

• A solution that contains the maximum amount of
  solute that may be dissolved under existing
  conditions is saturated.
• A solution that contains less solute than a
  saturated solution under existing conditions is
  unsaturated.
• A solution that contains more dissolved solute
  than a saturated solution under the same
  conditions is supersaturated.

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Solubility Chart
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Henrys Law
The concentration of a dissolved gas in a
solution is directly proportional to the pressure
of the gas above the solution
Applies most accurately for dilute solutions of
gases that do not dissociate or react with the
solvent
Yes ? CO2, N2, O2
No ? HCl, HI
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Raoults Law
The presence of a nonvolatile solute lowers the
vapor pressure of the solvent.
Psolution Observed Vapor pressure of
the solution
?solvent Mole fraction of the solvent
P0solvent Vapor pressure of the pure solvent
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Liquid-liquid solutions in which both components
are volatile
Modified Raoult's Law
P0 is the vapor pressure of the pure solvent PA
and PB are the partial pressures
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Raoults Law Ideal Solution
A solution that obeys Raoults Law is called an
ideal solution
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Negative Deviations from Raoults Law
Strong solute-solvent interaction results in a
vapor pressure lower than predicted
Exothermic mixing Negative deviation
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Positive Deviations from Raoults Law
Weak solute-solvent interaction results in a
vapor pressure higher than predicted
Endothermic mixing Positive deviation
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Definition of Electrolytes and Nonelectrolytes
An electrolyte is

• A substance whose aqueous solution conducts
• an electric current.

A nonelectrolyte is

• A substance whose aqueous solution does not
• conduct an electric current.

Try to classify the following substances as
electrolytes or nonelectrolytes
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Electrolytes vs. Nonelectrolytes
The ammeter measures the flow of electrons
(current) through the circuit.

• If the ammeter measures a current, and the bulb
• glows, then the solution conducts.

• If the ammeter fails to measure a current, and
  the
• bulb does not glow, the solution is
  non-conducting.

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Electrolytes?

1. Pure water
2. Tap water
3. Sugar solution
4. Sodium chloride solution
5. Hydrochloric acid solution
6. Lactic acid solution
7. Ethyl alcohol solution
8. Pure sodium chloride

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Answers to Electrolytes
NONELECTROLYTES
ELECTROLYTES

• Pure water
• Sugar solution
• Ethanol solution
• Pure NaCl

• Tap water (weak)
• NaCl solution
• HCl solution
• Lactate solution (weak)

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Colligative Properties
Colligative properties are those that depend on
the concentration of particles in a solution, not
upon the identity of those properties.

• Boiling Point Elevation
• Freezing Point Depression
• Osmotic Pressure

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Freezing Point Depression
Each mole of solute particles lowers the freezing
point of 1 kilogram of water by 1.86 degrees
Celsius.
Kf 1.86 ?C ? kilogram/mol
m molality of the solution
i vant Hoff factor
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Boiling Point Elevation
Each mole of solute particles raises the boiling
point of 1 kilogram of water by 0.51 degrees
Celsius.
Kb 0.51 ?C ? kilogram/mol
m molality of the solution
i vant Hoff factor
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Freezing Point Depression and Boiling Point
Elevation Constants, ?C/m
Solvent Kf Kb
Acetic acid 3.90 3.07
Benzene 5.12 2.53
Nitrobenzene 8.1 5.24
Phenol 7.27 3.56
Water 1.86 0.512
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The vant Hoff Factor, i
Electrolytes may have two, three or more times
the effect on boiling point, freezing point, and
osmotic pressure, depending on its dissociation.
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Dissociation Equations and the Determination of i
i 2
NaCl(s) ?
Na(aq) Cl-(aq)
i 2
AgNO3(s) ?
Ag(aq) NO3-(aq)
i 3
MgCl2(s) ?
Mg2(aq) 2 Cl-(aq)
i 3
Na2SO4(s) ?
2 Na(aq) SO42-(aq)
AlCl3(s) ?
Al3(aq) 3 Cl-(aq)
i 4
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Ideal vs. Real vant Hoff Factor
The ideal vant Hoff Factor is only achieved in
VERY DILUTE solution.
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Osmotic Pressure
The minimum pressure that stops the osmosis is
equal to the osmotic pressure of the solution
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Osmotic Pressure Calculations
p Osmotic pressure
M Molarity of the solution
R Gas Constant 0.0821 L?atm/mol?K
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Suspensions and Colloids
Suspensions and colloids are NOT solutions.
Suspensions The particles are so large that they
settle out of the solvent if not constantly
stirred.
Colloids The particles intermediate in size
between those of a suspension and those of a
solution.
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Types of Colloids
Examples Dispersing Medium Dispersed Substance Colloid Type
Fog, aerosol sprays Gas Liquid Aerosol
Smoke, airborn germs Gas Solid Aerosol
Whipped cream, soap suds Liquid Gas Foam
Milk, mayonnaise Liquid Liquid Emulsion
Paint, clays, gelatin Liquid Solid Sol
Marshmallow, Styrofoam Solid Gas Solid Foam
Butter, cheese Solid Liquid Solid Emulsion
Ruby glass Solid Solid Solid sol
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The Tyndall Effect
Colloids scatter light, making a beam visible.
Solutions do not scatter light.
Which glass contains a colloid?
colloid
solution