1C.
Solubility
1
Objectives
1)
2)
3)
4)
5)
6)
Define the following words: solute, solvent
and solution.
Learn why water is a good solvent.
Define the terms: insoluble, unsaturated,
saturated and supersaturated.
Interpret solubility curves.
Learn about concentration vs.
temperature and solubility.
Learn about polarity and ionic compounds
2
1C.1: SOLUBILITY OF SOLIDS
IN WATER
3
What is solubility?
• Imagine dissolving a
spoonful of salt in water
• How much will
dissolve?
• What is the solute?
• What is the solvent?
4
What is solubility?
• The salt is the ____________
• The water is the ______________
• The mixture of the salt & the water is a
__________________
• As you stir, the white crystals dissolve in the
water
• The solution is colorless & clear
5
What is solubility?
The salt is the: solute
 The water is the: solvent
 The mixture of the salt & the water is a:
solution

As you stir, the white crystals dissolve in
the water
 The solution is colorless & clear

6
Solutions - Review
Homogeneous mixture – uniform or
evenly distributed
 All solutions are homogeneous mixtures
 A solute dissolves in a solvent to make a
solution
 Solutions are clear but not
necessarily colorless

7
Do Now
Define the following words:
Solute
Solvent
Solution
Provide an example of each
8
What is solubility?
• What would happen if you added another
spoonful of salt?
• And another…. And another?
• Eventually, you wouldn’t be able to dissolve
any more. Some salt would fall to the bottom,
no matter how long you stirred.
• The solution would be saturated; it would
hold all the solute it could.
9
No more salt can dissolve.
The solution is saturated.
10
What is solubility?
• If you heated the water, you might be able to
dissolve a little more salt.
• The maximum quantity of a substance that
can dissolve in a certain quantity of water – at
a specified temperature – is called its
solubility.
• You might say grams of salt per 100 grams of
water at 20oC
11
What is solubility?
• Although size of the salt crystals &
how vigorously you stir affect how long
it would take for the salt to dissolve,
they do not affect how much can
dissolve at a specified temperature
• The amount of solute that can dissolve
is affected by temperature.
• Usually, the higher the temperature
the more solute that can be dissolved.
12
Temperature & Solubility
 The amount of solute
that can dissolve in a
specified amount of
solvent varies with
temperature
 The graphical
representation of this
relationship is called
the solute’s solubility
curve: page 54
13
Temperature & Solubility
 Each point on the
solubility curve
indicates a solution in
which the solvent
contains as much
dissolved solute as it
normally can at that
temperature
 Such a solution is
called a saturated
solution
14
Temperature & Solubility
• Question: At 40oC,
how much KNO3
will dissolve in 100
g water to form a
saturated solution?
• Answer:
15
Temperature & Solubility
Question: At
40oC, how much
KNO3 will dissolve
in 100 g water to
form a saturated
solution?
 Answer: 60 grams

16
Temperature & Solubility
• Question: At 90oC,
how much KCl will
dissolve in 100 g
water to form a
saturated solution?
• Answer:
17
Temperature & Solubility

Question: At 90oC,
how much KCl will
dissolve in 100 g
water to form a
saturated solution?

Answer: 52 grams
18
Temperature & Solubility
Question: At
50oC, how much
KNO3 will
dissolve in 100 g
water to form a
saturated
solution?
 Answer:

19
Temperature & Solubility
Question: At
50oC, how much
KNO3 will dissolve
in 100 g water to
form a saturated
solution?
 Answer: 80 grams

20
Temperature & Solubility
• Question: At what
temperature will 70 g
of KNO3 dissolve in
100 g of water to
make a saturated
solution?
• Answer:
21
Temperature & Solubility
Question: At what
temperature will
70 g of KNO3
dissolve in 100 g
of water to make a
saturated
solution?
 Answer: 45oC

22
Temperature & Solubility
• Question: Which one
of the three solutes is
the most affected by
temperature?
• Answer:
• Question: The least
affected?
• Answer:
23
An unsaturated solution is a solution that
contains less dissolved solute than the
amount that the solvent can normally hold
at that temperature.
On a solubility curve this is area below
the line.
24
Unsaturated solution
25
Temperature & Solubility
• Think about a
solution that
contains 80 g of
KNO3 in 100 g of
water at 60 oC
• The point is below
the curve
• This is an
unsaturated
solution
26
Classwork
Review sample problems on
page 55 and 56.
27
Temperature & Solubility
• What do you expect would happen if you
cooled a saturated solution?
• Crystals would form and fall to the bottom
– usually
• Sometimes, cooling a saturated solution
does not cause crystals to fall out
• This is an unstable solution called a
supersaturated solution
28
A supersaturated solution is a solution
that contains more dissolved solute than
the amount that the solvent can normally
hold at that temperature.
This normally occurs if you cool a
saturated solution.
This new point lies above the solubility
curve.
29
Supersaturated solution
30
Rock Candy
When seed crystals are added to a supersaturated sugar
solution, they cause excess dissolved sugar to crystallize onto a
string
31
Hot Springs
As the water in Emerald Pool (Yellowstone National Park) cools
and evaporates at the edges, it becomes supersaturated, and
precipitates begin to form.
32
1C.2 : SOLUBILITY &
SOLUBILITY CURVES
33
Solubility curves are quite useful when
working with 100 grams of water.
But what happens when you work with
other quantities of water.
A mathematical expression sing
proportions can be used.
34
Question
• How much potassium nitrate will dissolve
in 150g of water at 40°C?
refer to chart: At 100 grams water 60 grams
will dissolve at 40°C
• Answer:
The quantity of solvent has increased from
100 grams to 150 grams – 1.5 times as much
solvent. That means 1.5 times as much solute
can be dissolved.
Thus 1.5 x 60 grams KNO3 = 90 grams KNO3
35
Another way to solve:
60 g KNO3 =
100 g H2O
x g KNO3
150 g H2O
(150 g)(60 g) = (100 g)(X)
X = 90 g
36
Classwork
Page 56
Questions 1-3
37
Homework
Solubility Worksheet
Due: Wednesday, Nov 13th
38
1C.3: Constructing a
Solubility Curve
Lab
39
Lab: Constructing a solubility curve
Investigating Matter, pp.
57-59
40
Do Now
• Explain why the crystals formed in the
experiment yesterday.
41
1C.4: DISSOLVING IONIC
COMPOUNDS
42
IONIC COMPOUNDS
Formed from a cation (+) and an anion (-)
Example: Na+ Cl-
NaCl
43
Dissolving Process
• When you dissolve Potassium Nitrate (KNO3),
an ionic compound, in water in a lab
experiment this is referred to as a:
• macroscopic phenomenon (observable)
• Chemistry is concerned with what happens at
the particulate level – atomic and molecular
phenomenon, which cannot be observed
easily.
44
Dissolving Process
• Factors that contribute to dissolving a solid
material (macroscopic ):
– Temperature
– Agitation
– Time
• But how do the particles of solute & solvent
interact to make dissolving happen?
• This occurs at the microscopic level.
45
Water’s Role
• Water is a polar molecule
• Although it is neutral
overall, it has an uneven
distribution of electrical
charge.
• Partial positive region at
one end (hydrogen side).
• Partial negative region at
other end (oxygen side).
46
Polar Molecule – A molecule which has an uneven
distribution of electrical charge.
One half of the molecule is more positive (+) and
the other half is more negative (-).
47
Water’s Role
• It has a bent or V-shape
• The Oxygen end has
greater concentration of
electrons (-) than the
two Hydrogen ends (+)
48
Water’s Role
 Polar water molecules
are attracted to other
polar substances & to
substances composed
of electrically charged
particles
 Electrical attractions
make it possible for
water to dissolve many
kinds of substances
49
Salt Dissolving
in Water
Think about the ions & molecules interacting at different times.
50
Salt Dissolving in Water
• Q. What forces hold
the ionic lattice
together?
• A. Opposing ionic
charges (+ and –
charges). An electrical
attraction.
51
Salt Dissolving in Water
• Q. Why do the water
molecules interact with
ions?
• A. Water’s molecular
polarity allows it to
interact with both
positive & negative
ions.
52
Salt Dissolving in Water
• Q. What do the
dissolved ions have in
common with each
other?
• A. They are all solvated
– surrounded – by
water molecules.
53
Salt Dissolving in Water
• Q. How are the
dissolved ions different?
• A. Positive H ends of
H2O are aligned with
negative Cl ions, and
negative O ends of H2O
are aligned with
positive Na ions
54
Salt Dissolving in Water
 Q. On the particulate
level, what would
evaporating water
imply for this system?
 A. The crystal lattice
would begin to reform
with fewer water
molecules to overcome
the ion-ion attractive
forces.
55
Water’s Role
 View “Modeling Matter: Attraction Between
Particles”
 Q. What factors influence whether or not an
ionic compound dissolves in water?
 A. Properties of both solute & solvent, because
dissolving involves competition among 3 types of
attractions:
◦ Solvent – Solute
◦ Solvent – Solvent
◦ Solute – Solute
56
Water Video
• Go to:
• http://www.sumanasinc.com/webcontent
/animations/content/propertiesofwater/
water.html
• Show video
57
Do Now
• Draw a calcium ion solvated by water
molecules.
58
Do Now
• What is meant by unsaturated and
supersaturated?
• How does water interact with ionic
compounds?
59
1C.6: SOLUTION
CONCENTRATION
60
Objectives
• 1. Define solute concentration.
• 2. Explain the relevance to environmental
chemists
61

The terms saturated and unsaturated are
not always adequate to describe the
properties of solutions.

Solution concentration refers to how much
solute is dissolved in a specific quantity of
solution.

Ways to express solution concentration:
1) water-solubility curves
2) percent values (parts of solute per
hundred parts solution (pph)
62
Example
Dissolving 5 grams of table salt in 95 grams of
water produces 100 grams of solution
solute + solvent = solution
The percent solution of table salt is 5%
grams solute / grams solution x 100 = % solution
5 grams / 100 grams x 100 = 5%
63
Why is solution concentration important?
It is used in your daily lives. For example,
preparing beverages from premixed
concentrate, adding antifreeze to water in
automobile radiators and mixing pesticide
or fertilizer solutions all require use of
solution concentration.
Other uses:
Determining percentage of heavy metal
pollutants (lead and mercury) in water.
64
1C.7: DESCRIBING SOLUTION
CONCENTRATIONS
65
Sample Problem 1
A common intravenous saline solution used in
medical practice contains 4.5 grams NaCl
dissolved in 495.5 grams distilled water.
What is the concentration of this solution
expressed as a percentage?
66
Solute – 4.5 grams NaCl
Solvent – 495.5 grams distilled water
Solution total – 500 grams
grams solute / grams solution x 100 = % solution
4.5 grams / 500 grams x 100 = 0.90%
67
Sample Problem 2
One teaspoon of sugar, with a mass of 10.0
grams is dissolved onto 240.0 grams of water.
What is the concentration of this solution
expressed as a percentage?
68
Solute – 10.0 grams sugar
Solvent – 240.0 grams water
Solution total – 250 grams
grams solute / grams solution x 100 = % solution
10 grams / 250 grams x 100 = 4%
69
Classwork

Worksheet Unit 1C Section 6
70
Homework

Worksheet

Solution concentration problems
71
1C.8: INAPPROPRIATE
HEAVY-METAL ION
CONCENTRATIONS?
72
Objectives (1C.8 AND IC.9)
• 1. Define heavy metals, green chemistry,
regulatory limits, acids, bases, alkaline,
and pH.
• 2. Describe the health concerns for Pb2+
and Hg2+.
• 3. Describe the pH ranges that affect the
health of fish
73
Heavy Metals
• Many metal ions are essential to our health
– Iron(II)
– Potassium
– Calcium
Fe2+
K1+
Ca2+
• Some “heavy-metal” ions are harmful.
– Masses are heavier than the essential metal
ions.
– Toxic: bind to proteins, preventing them from
performing their normal tasks
– Nervous system, brain, kidneys, liver, death
– Lead
Pb2+
– Mercury
Hg2+
74
Heavy Metals
• Not removed as waste as they move through
the food chain
• Concentrated in bodies of fish & shellfish –
even when present in low concentrations in
surrounding water
• Hard to detect in low concentrations
• Difficult & costly to remove
• How to prevent poisoning?
• Prevention: “Green Chemistry” (replace
harmful chemicals)
75
Lead Ions (Pb2+)
• Plumbum – Plumber – ancient Roman water pipes
• Pottery, automobile batteries, solder, cooking
vessels, pesticides, paints (primary ingredient in red
paint that protects bridges & other steel structures
from corrosion), candy wrappers.
• Leaded gasoline – phased out in the 1970s – was a
better burning fuel. Soils around heavily traveled
roads are still contaminated (tetraethyl lead)
76
Mercury Ions (Hg 2+)
• Only metallic element
that is a liquid at room
temperature
• Hydragyrum – liquid
silver or quicksilver
• “silent” light switches,
street lamps,
thermometers,
thermostats,
fluorescent light bulbs,
paints, antiseptics,
fungicides, pesticides
77
During the 18th & 19th
centuries, mercury
compounds were used
in the making of felt
hats.
78
Ultimately, mercury
poisoning caused
symptoms such as
numbness, staggered
walk, tunnel vision,
and brain damage,
giving rise to the
expression “mad as a
hatter.”
79
Heavy Metals
• A sudden release of a large amount of a
heavy-metal ion might cause a fish kill
• It would depend on:
–
–
–
–
what ion
its concentration
species of fish
other factors
80
1C.9: INAPPROPRIATE pH
LEVELS?
SKIP
ACID/BASE POWERPOINT
81
1C.9: pH LAB
HANDOUT
82
SKIP
83
83
pH
• pH scale reports: acid, bases, or chemically
neutral
• pH usually between 0 to 14
< 7 - acid (lower numbers, more acidic)
= 7 - neutral
> 7 - base/alkaline (higher numbers, more
basic)
• Change in 1 pH unit = 10X difference
• Ex. Soft drinks = pH of 3
• Lemon juice = pH of 2
• Lemon juice is 10X more acidic than soft
drinks
84
pH Scale
• Draw the pH scale and label the following on it
– Weak acid
– Strong Base
– Strong Acid
– Neutral
– Weak Base
0
1
3
5
7
9
11
13
14
85
Acids
What comes to mind when you hear the
word acid?
Do you think of a substance that will burn
your skin or burn a hole in your clothes?
Do you think about sour foods?
All acids have some properties in
common
86
Characteristics of Acids
ACIDS
• Form H+ in water
– HCl, H2SO4, H3PO4
• Litmus: blue to red
• Sour – Don’t taste!
• Conduct electricity
87
88
Bases
You don’t consume many foods with
bases.
Some foods like eggs whites are slightly
basic.
Some bases are used in medicines.
Bases are commonly used in soaps and
household cleaners.
89
Characteristics of Bases
Some contain OH- ions :
• sodium hydroxide (NaOH) – drain and oven
cleaners
• calcium hydroxide (Ca(OH)2) – used in cement
Other bases do not contain OH- ions
• ammonia (NH3) – household cleaners
• Baking soda (NaHCO3)
• Litmus: red to blue
• Bitter – Don’t taste!
• Conduct electricity
90
91
pH of Common Substances
92
93
94
Do Now
• Where are acids located on the pH scale?
• Where are bases located on the pH scale?
95
pH continued
• Neutral solutions (pH = 7) are neither acids
nor bases
– NaCl (table salt) is an ionic compound that is
neutral
– C12H22O12 (sugar) is a molecular compound that
is neutral
• Rainwater is slightly acidic (pH ≈ 5.8)
• Both acids & bases effect living things
• EPA requires drinking water be between 6.5
to 8.5
96
pH continued
• Too low a pH in rivers, lakes, & streams
– Impairs fish egg development – affects
reproduction
– Increases concentration of metal ions –
by leaching metal ions from
surrounding soil – Al3+ can be toxic to
fish in high concentrations
• Too high a pH
– Can dissolve skin & scales
97
pH continued
• EPA requires pH of drinking water be
between 6.5 to 8.5
• Fish can tolerate a pH between 5.0 to 9.0
• Expert anglers try to fish in water with a
pH between 6.5 and 8.2
98
pH balance in swimming pools
pH balance in swimming pools is possibly the most
critical element of pool water maintenance. If you
consider that chlorine's ability to do its job is
directly linked to the pH, high or low levels
inevitably lead to sanitization problems.
The ideal range for pH in swimming pool water is
7.0 - 7.6 . The pH of our eyes is typically 7.2 - 7.4 .
If the pH is kept at the same level as that in our
eyes, the side-effects of burning red eyes is kept to
a minimum. The ability of chlorine to disinfect at
this level is also optimum.
99
High pH in swimming pool water
High pH in swimming pool water may result in one or
more of the following problems:
•scaling or calcium buildup on pool surfaces,
waterline and accessories;
•dull or cloudy pool water;
•clogging of filter medium or elements;
•drop in disinfection potential of chlorine resulting in
algae growth;
•burning eyes and nose;
•dry, itchy skin and scalp.
100
To lower the pH in pool water
Adding an acid to the pool water reduces the pH.
The most common chemicals used to reduce high
pool water pH are:
•muriatic acid - typically 30% - 35% liquid
hydrochloric acid.
•sodium bisulfate - granule or powder pH reducer,
dry acid.
•sulfuric acid
•nitric acid - highly corrosive but is known to work
well.
101
Low pH in swimming pool water
Low pH in swimming pool water may cause
one or more of these problems:
•eroding of the pool plaster or grouting;
•corroding of the metal pool accessories (steps,
heater . . .);
•staining resulting from metal corrosion;
•rapid dissipation of chlorine requiring
increased dosage;
•burning eyes and nose;
•dry and itchy skin and scalp;
•perishing of swimwear, pool toys and
accessories.
102
To raise the pH in pool water
Adding a base raises the pH of the pool water. The
active ingredient is usually sodium carbonate.
Often low pH is a result of acid rain and occurs
after periods of heavy precipitation.
103
1C.10:
MOLECULAR SUBSTANCE
SKIP
104
Objectives
1. Explain what are molecular substances.
2. Compare ionic versus molecular compounds.
3. Distinguish between polar and non polar
substances.
105
Molecular Substances
• Ionic substances are
solids at room
temperature
• Ionic substances
release ions when
they dissolve in
water (NaCl)
• Composed of a metal
and non-metal
• Molecular substances
are found as solids,
liquids, or gases at
room temperature
• Composed of nonmetals only (C, H, O)
• Molecular substances
remain as whole
molecules when they
dissolve in water
106
Molecular Substances
• Molecular substances are found as solids, liquids, or
gases at room temperature – physical state depends
on strength of attraction among the molecules.
• Examples:
• O2 – weak attraction between oxygen atoms – gas
• Ethanol and water – slightly stronger attraction
between atoms – liquids.
• Sugar – very strong attraction between atoms – solid.107
Molecular Substances
• What determines the solubility of a
molecular substance in water?
• Attraction of a substance’s molecules for
each other compared to their attraction
for water molecules
• Distribution of electric charge within the
molecules is a major factor
108
Molecular Substances
• Most molecular compounds contain atoms of
nonmetallic elements (right side of periodic
table).
• Remember, these atoms are linked together
by the attraction of one atom’s positive
nucleus to another atom’s negative electrons
109
Molecular Substances
• If the differences in attractions between the
two atoms are big enough, electrons move
from one atom to another, forming ions
(NaCl). A metal and non-metal.
• If the differences in attraction between the
two atoms exist but are not that big, they may
cause the electrons to shift around and
become unevenly distributed (H2O).
• The ability of an atom to attract electrons is
known as its electronegativity.
110
Polar Molecule – A molecule which has an uneven
distribution of electrical charge.
One half of the molecule is more positive (+) and
the other half is more negative (-). Oxygen is
more electronegative.
111
Molecular Substances
• “Like Dissolves Like”
• Polar molecules dissolve in polar solvents
• Examples: sugar in water, alcohol in water,
antifreeze in water. All are polar molecules.
• Nonpolar molecules dissolve in nonpolar
solvents
• Examples: oil-based paint in paint thinner,
• The reason to use soap and shampoo to remove
dirt and oil from skin and hair.
• Nonpolar molecules (gas and oil) do not
dissolve well in polar molecules (water). This is
why oil and water do not mix.
112
Common Nonpolar substances
•
•
•
•
•
•
Hexane
Lamp Oil
Paint Thinner
Fats
Motor oil
Cooking oils
113
Concept Chart
Solubility
Ionic compounds
Molecular Substances
Explain how it
dissolves:
Polar compounds
Explain how it
dissolves:
Non polar compounds
Explain how it
dissolves:
114
Homework
• Page 83
• Questions: 17, 18, 19, 20, 21, 23, 24 and 25
• Due: Today
115
Problem
• Explain why oil and water do not dissolve in
each other.
116
Problem
• Explain why oil and water do not dissolve in
each other.
• Polar substances dissolve polar substances.
• Polar substances dissolve ionic compounds.
• Non-polar dissolves non-polar substances.
117
117
Solubility Review
• Polar Substances dissolve other
__________ or ____________.
• Non Polar Substances dissolve
_______________.
118
1C.12: DISSOLVING GASES
INTO WATER?
119
Objectives
• 1. Describe the difference between
solubility of solids and gases.
• 2. Explain the metabolic changes of fish as
temperature and dissolve oxygen
change.
• 3. Describe factors that can change the
amount of dissolved oxygen.
120
Oxygen & Other Gases
• Ionic & molecular
solids tend to have a
higher solubility at
higher temperatures.
• The opposite tends to
be true for gases.
• Also, most gases are
much less soluble in
water than solids are –
at any temperature.
121
Problem
• Turn to page 75 and use the chart:
• What mass of O2 can be dissolved in
1000.0 g of water at 25.0 °C?
122
Oxygen & Other Gases
• In addition to the temperature & the type
of solvent, the solubility of a gas also
depends on gas pressure.
• Is this relationship directly or inversely
proportional?
123
Oxygen & Other Gases
• Is this relationship directly or inversely
proportional?
• Solubility of gases are directly proportional
to pressure if temperature remains constant.
• As pressure doubles, so
does solubility.
124
Example
• Turn to page 76 and use the chart:
• What mass of O2 can be dissolved in
1000.0 g of water at 3 atm pressure and
25.0 °C?
125
Gases
• Soda has extra CO2 forced into it
under high pressure. More CO2
dissolved.
• When can is opened the pressure
is reduced.
• When a can or bottle of soda is
opened, the solution is now
supersaturated at the lower
pressure, & some excess
dissolved CO2 escapes as bubbles.
• The “flat” soda is still saturated
with the gas at the lower
pressure.
126
1.C. 13: TEMPERATURE,
DISSOLVED OXYGEN, AND LIFE
SKIP
127
Objectives
• Examine what happens to fish when too
much or too little oxygen dissolves in water.
• You just learned how the solubility of gases is
affected by temperature.
128
Temperature & Dissolved Oxygen
• Does the temperature of water affect fish survival?
• Dissolved-oxygen requirements for fish.
• The metabolism of fish increase with water temperature.
129
Temperature & Dissolved Oxygen
• How does a temperature change affect fish?
• Cold-blooded: body temperatures rise & fall
with the water temperature
• Rise
–
–
–
–
–
Increases metabolism
Eat more
Swim more
Require more dissolved oxygen
Also increases metabolism of other aquatic
organisms (i.e., aerobic bacteria) that compete with
fish for dissolved oxygen
130
Temperature & Dissolved Oxygen
• Rise in temperature,
decreases the amount of
dissolved O2 in the
water while it increases
the fish’s need for it
• A long stretch of hot
summer days
sometimes kills fish
because there is not
enough oxygen
dissolved in the water.
131
Temperature & Dissolved Oxygen
• Hot, summer days
are not always the
cause.
• Many industries use
water to cool their
heat-producing
processes, dumping
the heated up water
back into the rivers
or lakes.
132
Temperature & Dissolved Oxygen
• Can too much dissolved oxygen be a
problem?
• When oxygen gas dissolves, so does
nitrogen which is found in the
atmosphere.
• When the total amount of dissolved gas
reaches between 110% to 124% of
saturation (a supersaturated state), gasbubble trauma may develop in fish
133
Temperature & Dissolved Oxygen
• Gas bubbles form in the blood and tissues
of fish.
• Nitrogen bubbles block the capillaries.
• Death within hours or days.
• Prompt dissection after death can find gas
bubbles in the gills.
• Bubbling of gas in the blood in humans is
known as the “bends” and affect scuba
divers.
134
Supersaturation of
water with oxygen &
nitrogen can occur at
the base of a dam or
hydroelectric project,
as the released water
forms “froth,” trapping
large quantities of air
135
Problem
• Explain what happens to the amount of
dissolved oxygen as the temperature
increases?
• How about when the pressure increases?
136
Homework
• Pg. 83; Questions: 28 - 31,
• Pg. 84; Questions: 33 and 35
137
End of Unit
138
1C.11: SOLVENTS
139
1C.11: SOLVENTS
LAB
Investigating Matter, pp. 72-75
140
Dissolving Substances (Lab)
• List several substances that will dissolve in
water and why….
• Hexane is NON POLAR, list several
substances that will dissolve in hexane.
141