BDChapter 4: Solutions 111
VOCABULARY
solution p. 111
solute p. 112
solvent p. 112
suspension p. 113
BEFORE, you learned
• Ionic or covalent bonds hold acompound together
• Chemical reactions producechemical changes
• Chemical reactions alter thearrangements of atoms
NOW, you will learn
• How a solution differs fromother types of mixtures
• About the parts of a solution
• How properties of solutionsdiffer from properties of theirseparate components
KEY CONCEPT
A solution is a type of mixture.
EXPLORE Mixtures
Which substances dissolve in water?
PROCEDURE
Pour equal amounts of water into each cup.
Pour one spoonful of table salt into one
of the cups. Stir.
Pour one spoonful of flour into the other
cup. Stir.
Record your observations.
WHAT DO YOU THINK?• Did the salt dissolve? Did the flour dissolve?
• How can you tell?
4
3
2
1
MATERIALS• tap water
• 2 clear plastic cups
• plastic spoon
• table salt
• flour
The parts of a solution are mixed evenly.
A mixture is a combination of substances, such as a fruit salad.
The ingredients of any mixture can be physically separated from each
other because they are not chemically changed—they are still the same
substances. Sometimes, however, a mixture is so completely blended
that its ingredients cannot be identified as different substances.
A is a type of mixture, called a homogeneous mixture, that
is the same throughout. A solution can be physically separated, but all
portions of a solution have the same properties.
If you stir sand into a glass of water, you can identify the sand as a
separate substance that falls to the bottom of the glass. Sand in water is
a mixture that is not a solution. If you stir sugar into a glass of water,
you cannot identify the sugar as a separate substance. Sugar in water is
a common solution, as are examples such as seawater, gasoline, and the
liquid part of your blood.
solution
VOCABULARY
Remember to use the strategy of your choice. You might use a four squarediagram for solution.
� � � � � � � �
reading tip
The words solute and solvent
are both related to the Latinword solvere, which means“to loosen.”
Solutes and Solvents
Like other mixtures, a solution has definite components. A
(SAHL-yoot) is a substance that is dissolved to make a solution.
When a solute dissolves, it separates into individual particles. A
is a substance that dissolves a solute. Because a solute dissolves into
individual particles in a solvent, it is not possible to identify the solute
and solvent as different substances when they form a solution.
In a solution of table salt and water, the salt is the solute and the
water is the solvent. In the cells of your body, substances such as
calcium ions and sugar are solutes, and water is the solvent. Water is
the most common and important solvent, but other substances can
also be solvents. For example, if you have ever used an oil-based paint
you know that water will not clean the paintbrushes. Instead, a solvent
like turpentine must be used.
Check Your Reading What is the difference between a solute and a solvent?
Types of Solutions
Many solutions are made of solids dissolved in liquids. However, solutes,
solvents, and solutions can be gases, liquids, or solids. For example,
oxygen, a gas, is dissolved in seawater. The bubbles in carbonated
drinks come from the release of carbon dioxide gas that was
dissolved in the drink.
In some solutions, both the solute and the solvent are in the
same physical state. Vinegar, for example, is a solution of acetic
acid in water. In a solution of different liquids, it may be difficult
to say which substance is the solute and which is the solvent.
In general, the substance present in the greater amount is the
solvent. Since there is more water than acetic acid in vinegar,
water is the solvent and acetic acid is the solute.
Although you may usually think of a solution as a liquid,
solid solutions also exist. For example, bronze is a solid
solution in which tin is the solute and copper is the solvent.
Solid solutions are not formed as solids. Instead, the solvent
metal is heated until it melts and becomes a liquid. Then the
solute is added, and the substances are thoroughly mixed
together. When the mixture cools, it is a solid solution.
Solutions made of combinations of gases are also common.
The air you breathe is a solution. Because nitrogen makes up
the largest portion of air, it is the solvent. Other gases present,
such as oxygen and carbon dioxide, are solutes.
When substances in a solution are in the same physicalstate, which is the solvent?
solvent
solute
112 Unit: Chemical Interactions
Liquid SolutionWater often contains manydissolved substances.
Solid Solution Bronze consistsof tin dissolvedin copper.
Gas SolutionAir is oxygenand other gasesdissolved innitrogen.
BD
� � � � � � � �
BDChapter 4: Solutions 113
How can you separate the parts of a solution?
PROCEDURE
Draw a solid black circular region 6 cm in diameter around the point of the filter.
Place the filter, point up, over the top of the bottle.
Squeeze several drops of water onto the point of the filter.
Observe the filter once every minute for 10 minutes.
Record your observations.
WHAT DO YOU THINK?
• What happened to the ink on the filter?
• Identify, in general, the solutes and the solution in
this investigation.
CHALLENGE Relate your observations of the ink and
water on the coffee filter to the properties of solutions.
4
3
2
1
SolutionsSolutions
Suspensions
When you add flour to water, the mixture turns cloudy, and you cannot
see through it. This mixture is not a solution but a suspension.
In a the particles are larger than those found in a solution.
Instead of dissolving, these larger particles turn the liquid cloudy.
Sometimes you can separate the components of a suspension by
filtering the mixture.
suspension,
SKILL FOCUSObserving
MATERIALS• black marker• coffee filter• plastic bottle• eyedropper• tap water
TIME15 minutes
Solution Dissolved particles cannotbe identified as a substance differentfrom the solvent.
Suspension Particles that do not dissolve make a suspension look cloudy.
suspended particledissolved particle
solvent solvent
� � � � � � �
BD
Solvent and solute particles interact.
The parts of a solution—that is, the solute and the solvent—can be
physically separated because they are not changed into new substances.
However, individual particles of solute and solvent do interact. When a
solid dissolves in a liquid, the particles of the solute are surrounded by
particles of the liquid. The solute particles become evenly distributed
through the solvent.
The way in which a solid compound dissolves in a liquid depends
on the type of bonds in the compound. Ionic compounds such as table
salt (NaCl) split apart into individual ions. When table salt dissolves in
water, the sodium and chloride ions separate, and each ion is surrounded
by water molecules. When a covalent compound such as table sugar
(C12H22O11) dissolves, each molecule stays together and is surrounded
by solvent molecules. The general processes that take place when ionic
compounds dissolve and when covalent compounds dissolve are
shown below.
114 Unit: Chemical Interactions
How Solutes Dissolve
What difference between the two illustrations tells you whether a compound is ionic or covalent?
Ionic Compound Dissolved in Solvent Covalent Compound Dissolved in Solvent
Ionic compounds separate into ions. Covalent compounds separate into individual molecules.
added to solvent added to solvent
ionic compound
covalent compound
� � � � � � �
reminder
In temperature measure-ments, C stands for“Celsius” and F standsfor “Fahrenheit.”
Properties of solvents change in solutions.
In every solution—solid, liquid, and gas—solutes change the physical
properties of a solvent. Therefore, a solution’s physical properties differ
from the physical properties of the pure solvent. The amount of solute
in the solution determines how much the physical properties of the
solvent are changed.
Lowering the Freezing Point
Recall that the freezing point is the temperature at which a liquid
becomes a solid. The freezing point of a liquid solvent decreases—becomes
lower—when a solute is dissolved in it. For example, pure water freezes
at 0°C (32°F) under normal conditions. When a solute is dissolved in
water, the resulting solution has a freezing point below 0°C.
Lowering the freezing point of water can be very useful in winter.
Road crews spread salt on streets and highways during snowstorms
because salt lowers the freezing point of water. When snow mixes with
salt on the roads, a saltwater solution that does not freeze at 0°C is
formed. The more salt that is used, the lower the freezing point of
the solution.
Since salt dissolves in the small amount of water usually
present on the surface of ice, it helps to melt any ice already
present on the roads. However, there is a limit to salt’s effective-
ness because there is a limit to how much will dissolve.
No matter how much salt is used, once the temperature goes
below –21°C (–6°F), the melted ice will freeze again.
Check Your Reading How does the freezing point of a solvent change when a solute is dissolved in it?
Making ice cream also depends on lowering the freezing
point of a solvent. Most hand-cranked ice cream makers hold
the liquid ice cream ingredients in a canister surrounded by a
mixture of salt and ice. The salt added to the ice lowers the
freezing point of this mixture. This causes the ice
to melt—absorbing heat from its surroundings,
including the ice cream ingredients. The ice
cream mix is chilled while its ingredients are
constantly stirred. As a result, tiny
ice crystals form all at once in the
ice cream mixture instead of a
few crystals forming and growing
larger as the mix freezes. This whole
process helps to make ice cream that
is smooth and creamy.
115
Adding salt tolower the freezingpoint of ice helpsto make ice cream.
Adding salt tolower the freezingpoint of ice helpsto make ice cream.
BD
� � � � � � � �
BD 116 Unit: Chemical Interactions
Raising the Boiling Point
The boiling point of a liquid is the temperature at which the liquid forms
bubbles in its interior and becomes a gas. Under normal conditions,
a substance cannot exist as a liquid at a temperature greater than its
boiling point. However, the boiling point
of a solution is higher than the boiling point
of the pure solvent. Therefore, a solution
can remain a liquid at a higher temperature
than its pure solvent.
For example, the boiling point of pure
water is 100˚C (212˚F) under normal
conditions. Saltwater, however, can be a
liquid at temperatures above 100˚C
because salt raises the boiling point of
water. The amount of salt in the water
determines how much the boiling point
is increased. The more solute that is
dissolved in a solution, the greater the
increase in boiling point.
Check Your Reading How does the boiling point of a solution depend on the amountof solute in it?
A solute lowers the freezing point and raises the boiling point of
the solvent in the solution. The result is that the solute extends the
temperature range in which the solvent remains a liquid. One way in
which both a decrease in freezing point and an increase in boiling
point can be useful in the same solution involves a car’s radiator.
Antifreeze, which is mostly a chemical called ethylene glycol, is often
added to the water in the radiator. This solution prevents the water from
freezing in the winter and also keeps it from boiling in the summer.
KEY CONCEPTS
1. How is a solution different
from other mixtures?
2. Describe the two parts of a
solution. How can you tell
them apart?
3. How does the boiling point
of a solvent change when a
solute is dissolved in it?
How does the freezing
point change?
CRITICAL THINKING
4. Compare Contrast the way
in which an ionic compound,
such as table salt, dissolves
with the way in which a
covalent compound, such
as sugar, dissolves.
5. Infer Pure water freezes at
0˚C and boils at 100˚C. Would
tap water likely freeze and boil
at those exact temperatures?
Why or why not?
CHALLENGE
6. Synthesize People often
sprinkle salt on icy driveways
and sidewalks. Would a sub-
stance like flour have a similar
effect on the ice? Explain.
APPLY Why might theaddition of antifreeze tothe water in this car’sradiator have preventedthe car from overheating?
� � � � � � � �