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Solutions Solutions
DefinitionsTypes of SolutionSolutions, Colloids, SuspensionsProcess of DissolvingRate of SolutionConcentrationSolubility
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DefinitionsDefinitions
Homogenous Mixture – two or more substances which have the same composition throughout; uniform; in the same state of matter
• Solutions, Colloids, Suspensions Heterogeneous Mixture – two or more
substances which have a mixture in which the ingredients are not uniformly dispersed.
• Fruity Pebbles
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Definitions Definitions
Solution - Solution - homogeneous mixture of two or more substances
Solvent Solvent - present in greater amount
Solute Solute - substance being dissolved, present in smaller amount Solute
particles very small
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Definitions Definitions
Solute Solute - KMnO4 Solvent Solvent - H2O
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Hydrogen Bonds Attract Polar Water Molecules
Hydrogen Bonds Attract Polar Water Molecules
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Types of Solutions Types of Solutions
Based on state of solvent. All solid-liquid-gas combos are
possible. EX: dental amalgam (alloy of silver,
mercury, etc.)• liquid solute, solid solvent• solid solution
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Types of SolutionsTypes of Solutions
air O2 gas and N2 gas gas/gas
soda CO2 gas in water gas/liquid
seawater NaCl in water solid/liquid
brass copper and zinc solid/solid
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Learning Check SF1Learning Check SF1
(1) element (2) compound (3) solution
A. water 1 2 3
B. sugar 1 2 3
C. salt water 1 2 3
D. air 1 2 3
E. tea 1 2 3
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Solution SF1Solution SF1
(1) element (2) compound (3) solution
A. water 2
B. sugar 2
C. salt water 3
D. air 3
E. tea 3
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Learning Check SF2Learning Check SF2
Identify the solute and the solvent.
A. brass: 20 g zinc + 50 g copper
solute = 1) zinc 2) copper
solvent = 1) zinc 2) copper
B. 100 g H2O + 5 g KCl
solute = 1) KCl 2) H2O
solvent = 1) KCl 2) H2O
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Solution SF2Solution SF2
A. brass: 20 g zinc + 50 g copper
solute = 1) zinc solvent = 2) copper
B. 100 g H2O + 5 g KCl
solute = 1) KCl
solvent = 2) H2O
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Dissolving Dissolving
SolvationSolvation
• occurs at the surface of the solute
• solvent particles surround solute particles (+/- attraction)
• solute particles are pulled into solution
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Dissolving Dissolving
NaCl dissolving in waterNaCl dissolving in water
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“Like Dissolves Like” “Like Dissolves Like”
NONPOLAR
NONPOLAR
POLAR
POLAR
DetergentsDetergents• polar “head” with long nonpolar “tail”• can dissolve both types
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Learning Check SF4Learning Check SF4
Which of the following solutes will dissolve in water? Why?
1) Na2SO4
2) gasoline
3) I2
4) HCl
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Like dissolves likeLike dissolves like
A ____________ solvent such as water is needed
to dissolve polar solutes such as sugar and
ionic solutes such as NaCl.
A ___________solvent such as hexane (C6H14)
is needed to dissolve nonpolar solutes such
as oil or grease.
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Solution SF4Solution SF4
Which of the following solutes will dissolve in water? Why?
1) Na2SO4 Yes, polar (ionic)
2) gasoline No, nonnpolar
3) I2 No, nonpolar
4) HCl Yes, Polar
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ColloidsColloids
Have medium size particles
Cannot be filtered
Separated with semipermeable membranes
Scatter light
(Tyndall effect)
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Examples of ColloidsExamples of Colloids
Fog
Whipped
cream
Milk
Cheese
Blood plasma
Pearls
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SuspensionsSuspensions
Have very large particles
Settle out
Can be filtered
Must stir to stay suspended
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Examples of SuspensionsExamples of Suspensions
Blood platelets
Muddy water
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Rate of Solution - SolidsRate of Solution - Solids
Solids dissolve faster (have greater solubility) with...Solids dissolve faster (have greater solubility) with...
• more stirring
• small particle size(increased surface area)
• high temperature
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Temperature and Solubility of SolidsTemperature and Solubility of Solids
Temperature Solubility (g/100 g H2O) KCl(s) NaNO3(s)
0° 27.6 74 20°C 34.0 88 50°C 42.6 114100°C 57.6 182
The solubility of most solids (decreases or increases ) with an increase in the temperature.
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Temperature and Solubility of SolidsTemperature and Solubility of Solids
Temperature Solubility (g/100 g H2O)
KCl(s) NaNO3(s)
0° 27.6 74
20°C 34.0 88
50°C 42.6 114
100°C 57.6 182
The solubility of most solids increases with an increase in the temperature.
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Rate of Solution - GasesRate of Solution - Gases
Gases dissolve faster and have great Gases dissolve faster and have great solubility if...solubility if...
• no shaking or stirring
• high pressure above surface
• low temperature
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Temperature and Solubility of GasesTemperature and Solubility of Gases
Temperature Solubility (g/100 g H2O)
CO2(g) O2(g)
0°C 0.34 0.0070 20°C 0.17 0.0043 50°C 0.076 0.0026
The solubility of gases (decreases or increases) with an increase in temperature.
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Temperature and Solubility of GasesTemperature and Solubility of Gases
Temperature Solubility(g/100 g H2O)
CO2(g) O2(g)
0°C 0.34 0.0070
20°C 0.17 0.0043
50°C 0.076 0.0026
The solubility of gases decreases with an increase in temperature.
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ConcentrationConcentration
Concentrated solutionConcentrated solution • large amount of solute
Dilute solutionDilute solution • small amount of solute
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ConcentrationConcentration
% by Volume% by Volume: usu. liquid in liquid• EX: 10% juice = 10mL juice + 90mL
water
% by Mass% by Mass: usu. solid in liquid• EX: 20% NaCl = 20g NaCl + 80g water• % solution = mass of solute x 100
mass of solution
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ConcentrationConcentration
SATURATED SOLUTION
no more solute dissolves
UNSATURATED SOLUTIONmore solute dissolves
SUPERSATURATED SOLUTION
becomes unstable, crystals form
concentration
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SolubilitySolubility
SolubilitySolubility• maximum grams of solute that will
dissolve in 100 g of solvent at a given temperature
• varies with temperature• based on a saturated solution
g of solute 100 g water
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Learning Check S1Learning Check S1
At 40C, the solubility of KBr is 80 g/100 g H2O.
Indicate if the following solutions are
(1) saturated or (2) unsaturated
A. ___60 g KBr in 100 g of water at 40C
B. ___200 g KBr in 200 g of water at 40C
C. ___25 KBr in 50 g of water at 40C
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Solution S1Solution S1
At 40C, the solubility of KBr is 80 g/100 g H2O.
Indicate if the following solutions are
(1) saturated or (2) unsaturated
A. 2 Less than 80 g/100 g H2O
B. 1 Same as 100 g KBr in 100 g of water
at 40C, which is greater than its solubility
C. 2 Same as 60 g KBr in 100 g of water,
which is less than its solubility