Transcript V. Physical Behavior of Matter

SOLUTIONS
TAKE OUT:
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TAKE NOTES ON PAGE 3
What is a
SOLUTION?
SOLUTION IS A HOMOGENOUS
MIXTURE OF SUBSTANCES.
What is a
SOLUTE?
SOLUTE
Solute is a substance being dissolved.
Hint: it is usually present in smaller amount

SUGAR

What is a
SOLVENT?
SOLVENT
Solvent is the substance that dissolves the
solute.
Hint: it is usually present in the greater amount.
WATER
SOLUTE + SOLVENT = SOLUTION
+
+(tea)
=
(OR)
REGENTS QUESTION: 08/02 #7
Which mixture can be separated by using the
equipment shown?
(1) NaCl(aq) and SiO2(s)
(2) NaCl(aq) and C6H12O6(aq)
(3) CO2(aq) and NaCl(aq)
(4) CO2(aq) and C6H12O6(aq)
(aq) stands for aqueous which
means dissolved in water.
Dissolved particles are too small
to be trapped by the filter.
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 Solubility:
Maximum quantity of solute that
can dissolve in an amount of solvent at a
specified temperature

Measured in grams(solute)/grams(solvent)
FACTORS THAT THE
RATE OF SOLUTION
 Rate
of Solution:
measure of how fast a substance
dissolves
FACTORS THAT THE
RATE OF SOLUTION
 Size
of Particles: (solid solute)
As surface area  rate of solution 
To increase surface area, crush large
crystals
Example: sugar granules vs. sugar cubes
FACTORS THAT THE
RATE OF SOLUTION
 Stirring:
Makes solute come in contact with solvent
 Amount of solute in solution:
The less solute in solution the faster more will
dissolve.
FACTORS THAT AFFECT THE
RATE OF SOLUTION
 Temperature:
For liquids/solids:
As T  Rate of Soln. 
For gases:
As T  Rate of Soln. 
FACTORS THAT AFFECT SOLUBILITY
 Nature
of solute and solvent:
“Like dissolves like”
polar solutes dissolve in polar solvents
example: ionic solids in water
non polar solutes in non polar solvents
FACTORS THAT AFFECT SOLUBILITY
 Temperature:
For Ionic solids:

as T solubility
example: Jell-O in boiling water
For gases: as T solubility 
example: warm soda goes flat
FACTORS THAT AFFECT SOLUBILITY
 Pressure:
For solids/liquids:
As P changes, solubility does not change
For gases: as P solubility 
Effervescence: escape of gas from soln.
SOLUBILITY OF A NONVOLATILE SOLUTE
DEPENDS ON TEMPERATURE.

Solubility is the maximum amount of solute that a
solvent can hold at a given temperature.



An unsaturated solution is one in which the solvent can
dissolve more solute
A saturated solution is one in which the solvent has as
much solute as it can hold
A supersaturated solution is one in which there is more
solute dissolved than a solvent can normally hold.
Make a supersaturated solution by cooling a saturated solution
 Supersaturated solutions are unstable and will precipitate the
excess solute when a seed crystal is added.

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NOTES TIME – TAKE OUT PAPER
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Table G shows the
solubility of some
gases and solids at
various temperatures
when dissolved in
100 grams of water.
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•A solution which
is on the line is
saturated
•A solution below
the line is
unsaturated
•A solution above
the line is
supersaturated
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ADD A TEST CRYSTAL TO SEE IF A
SOLUTION IS UNSATURATED,
SATURATED OR SUPERSATURATED.
Unsaturated – the test crystal dissolves
 Saturated – the test crystal settles to the
bottom
 Supersaturated – a large amount of
crystals precipitate from the solution

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REGENTS QUESTION: 06/02 #40
According to Reference Table G,
which solution is saturated at
30°C?
(1) 12 grams of KClO3 in 100
grams of water
(2) 12 grams of KClO3 in 200
grams of water
(3) 30 grams of NaCl in 100
grams of water
(4) 30 grams of NaCl in 200
grams of water
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REGENTS QUESTION: 08/02 #48
One hundred grams of water is saturated with NH4Cl
at 50°C. According to Table G, if the temperature
is lowered to 10°C, what is the total amount of
NH4Cl that will precipitate?
(1) 5.0 g
(3) 30. g
(2) 17 g
(4) 50. g
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REGENTS QUESTION: 01/03 #65-66
When cola, a type of soda pop, is manufactured, CO2
(g) is dissolved in it.
A capped bottle of cola contains CO2 (g) under high
pressure. When the cap is removed, how does
pressure affect the solubility of the dissolved CO2
(g)?
As the pressure decreases, the solubility decreases.
A glass of cold cola is left to stand 5 minutes at room
temperature. How does temperature affect the
solubility of the CO2 (g)?
As the temperature increases, the solubility decreases.
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REGENTS QUESTION: 06/03 #42
Hexane (C 6 H 14 ) and water do not form a solution.
Which statement explains this phenomenon?
(1) Hexane is polar and water is nonpolar.
(2) Hexane is ionic and water is polar.
(3) Hexane is nonpolar and water is polar.
(4) Hexane is nonpolar and water is ionic.
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Soluble will dissolve
 Insoluble will not dissolve

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SOLUBILITY GUIDELINES
Not all substances are soluble in water
 Reference Table F lists solubility rules and
exceptions to those rules.

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SOLUBLE
NOT SOLUBLE
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REGENTS QUESTION: 08/02 #40
Which of the following compounds is least soluble
in water?
(1) copper (II) chloride
(2) aluminum acetate
(3) iron (III) hydroxide
(4) potassium sulfate
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REGENTS QUESTION: 06/03
#14
According to Table F, which of these salts is least
soluble in water?
(1) LiCl
(2) RbCl
(3) FeCl2
(4) PbCl2
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CONCENTRATION OF SOLUTION
The concentration of a solution is a
measurement of the amount of solute
dissolved in solution.
 Dilute is very little solute
 Concentrated is at or near saturation
 Molarity is a [concentration] of moles/liter

 Table
T
REGENTS QUESTION: 06/02 #42
What is the molarity of a solution that contains 0.50
mole of NaOH in 0.50 liter of solution?
(1) 1.0 M
(3) 0.25 M
(2) 2.0 M
(4) 0.50 M
Moles
Molarity =
Liters
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REGENTS QUESTION: 08/02 #36
How many moles of solute are contained in 200
milliliters of a 1 M solution?
(1) 1
(3) 0.8
(2) 0.2
(4) 200
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REGENTS QUESTION: 08/02 #49
What is the total number of grams of NaI(s)
needed to make 1.0 liter of a 0.010 M solution?
(1) 0.015
(2) 0.15
Molarity = moles
liters
0.010M = x
1.0 L
X = 0.010 moles
(3) 1.5
(4) 15
Na 1 x 23.0 = 23.0
I
1 x 126.9 = 126.9
149.9 g / mole
0.010 moles x 149.9 g/mole =
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PARTS PER MILLION

Parts per million ppm is often used to measure
concentrations of solutes that are present in
very small amounts
Mass of Solute
Parts Per Million =
Mass of Solution
X 1,000,000
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COLLIGATIVE PROPERTIES
Some properties (like boiling point and melting
point) of substances change when non-volatile
substances are added.
 We add salt to ice and lower the freezing point.
The ice melts and we are safe. YAY!!!!!!
 Rule #1 – The more dissolved particles, the
greater the effect on FP and BP
 Rule #2 – Ionic substance dissociate so will
tend to effect FP and BP greater.

NON-ELECTROLYTES
Non-electrolytes are molecular substances that
do not break up into ions (i.e. sugar)
 C12H22O11  C12H22O11 (aq)

1 mole
1 mole
ELECTROLYTES
Electrolytes are ionic substances that break up
into ions when put in solution. (ex: NaCl)
 NaCl  Na+ + Cl1 mole NaCl  1mole Na+ + 1 mole Cl
Because there are more moles produced, this has a
greater effect on colligative properties.
COMPARE THE FOLLOWING:
Which will have the lowest freezing point?
 Which will have the highest freezing point?

1 mole of MgCl2 in 500 g water
1 mole of C6H12O6 in 500 g water
Freezing point will always be lower than 0°C.
BOILING POINT ELEVATION
Boiling point is raised when a non-volatile
substance is added.
 Example: water boils at a higher temp when
salt is added

COMPARE THE FOLLOWING:
Which will have the highest boiling point?
 Which will have the lowest boiling point?

1 mole of MgCl2 in 500 g water
1 mole of C6H12O6 in 500 g water
Boiling point will always be higher than 100°C.
REGENTS QUESTION: 06/03 #23
At standard pressure when NaCl is added to
water, the solution will have a
(1) higher freezing point and a lower boiling
point than water
(2) higher freezing point and a higher boiling
point than water
(3) lower freezing point and a higher boiling
point than water
(4) lower freezing point and a lower boiling point
than water
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REGENTS QUESTION: 01/04 #13
Compared to pure water, an aqueous solution of
calcium chloride has a
(1) higher boiling point and higher freezing point
(2) higher boiling point and lower freezing point
(3) lower boiling point and higher freezing point
(4) lower boiling point and lower freezing point
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