Transcript Slide 1

Table of Contents
Chapter: Substances, Mixtures,
and Solubility
Section 2: Solubility
Solubility
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Water—The Universal Solvent
• A solution in which water is the solvent is
called an aqueous (A kwee us) solution.
• Because water can dissolve so many
different solutes, chemists often call it the
universal solvent.
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Molecular Compounds
• When certain atoms form compounds, they
share electrons. Sharing electrons is called
covalent bonding.
• Compounds that
contain covalent
bonds are called
molecular
compounds, or
molecules.
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Molecular Compounds
• If a molecule has an even distribution of
electrons it is called nonpolar.
• In a water molecule, the
electrons spend more
time around the oxygen
atom than the hydrogen
atoms.
• Such a molecule is polar.
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Ionic Bonds
• Atoms with a charge are called ions.
• Bonds between ions that are formed by the
transfer of electrons are called ionic bonds,
and the compound that is formed is called
and ionic compound.
• Table salt is an ionic compound that is made
of sodium ions and chloride ions.
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How Water Dissolves
Ionic Compounds
• Because water molecules are polar, they
attract positive and negative ions.
• The more positive part of a water
molecule—where the hydrogen atoms are—
is attracted to negatively charged ions.
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How Water Dissolves
Ionic Compounds
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How Water Dissolves
Ionic Compounds
• The more negative part of a water molecule—
where the oxygen atom is—attracts positive
ions.
• When an ionic compound is mixed with
water, the different ions of the compound
are pulled apart by the water molecules.
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How Water Dissolves
Molecular Compounds
• Water does dissolve
molecular compounds,
such as sugar, although
it doesn’t break each
sugar molecule apart.
• Water simply moves
between different
molecules of sugar,
separating them.
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What will dissolve?
• When you stir a spoonful of sugar into iced
tea, all of the sugar dissolves but none of the
metal in the spoon does.
• A substance that dissolves in another is said
to be soluble in that substance.
• You would say that the sugar is soluble in
water but the metal of the spoon is insoluble
in water.
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Like Dissolves Like
• When trying to predict which solvents can
dissolve which solutes, chemists use the rule
of “like dissolves like.”
• Polar solvents dissolve polar solutes and
nonpolar solvents dissolve nonpolar solutes.
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Like Dissolves Like
• On the other hand, if a solvent and a solute
are not similar, the solute won’t dissolve.
• For example, oil and
water do not mix.
• Oil molecules are
nonpolar, so polar
water molecules are
not attracted to them.
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How much will dissolve?
• Solubility (sahl yuh BIH luh tee) is a
measurement that describes how much solute
dissolves in a given amount of solvent.
• The solubility of a material has been
described as the amount of the material that
can dissolve in 100 g of solvent at a given
temperature.
• When a substance has an extremely low
solubility, it usually is considered insoluble.
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Solubility in Liquid-Solid Solutions
• The solubility of many solutes changes if
you change the temperature of the solvent.
• For example, if you heat water, not only
does the sugar dissolve at a faster rate, but
more sugar can dissolve in it.
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Solubility in Liquid-Solid Solutions
• This graph shows
how the temperature
of the solvent affects
the solubility of some
solutes.
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Solubility in Liquid-Gas Solutions
• Unlike liquid-solid solutions, an increase
in temperature decreases the solubility of a
gas in a liquid-gas solution.
• You might notice this if you have ever
opened a warm carbonated beverage and it
bubbled up out of control while a chilled
one barely fizzed.
• Carbon dioxide is less soluble in a warm
solution.
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Saturated Solutions
• A solution that contains all of the solute
that it can hold under the given conditions
is called a saturated solution.
• If a solution is a liquid-solid solution, the
extra solute that is added will settle to the
bottom of the container.
• It’s possible to make solutions that have
less solute than they would need to become
saturated. Such solutions are unsaturated.
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Saturated Solutions
• A hot solvent usually can hold more solute
than a cool solvent can.
• If a saturated solution is cooled slowly,
sometimes the excess solute remains
dissolved for a period of time.
• Such a solution is said to be supersaturated,
because it contains more than the normal
amount of solute.
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Rate of Dissolving
• Some solutes dissolve
quickly, but others take a
long time to dissolve.
• A solute dissolves faster
when the solution is
stirred or shaken or when
the temperature of the
solution is increased.
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Rate of Dissolving
• These methods increase
the rate at which the
surfaces of the solute
come into contact with
the solvent.
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Concentration
• The concentration of a solution tells you
how much solute is present compared to
the amount of solvent.
• You can give a simple description of a
solution’s concentration by calling it either
concentrated or dilute.
• A concentrated solution has more solute
per given amount of solvent than a dilute
solution.
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Measuring Concentrations
• One way of giving the exact concentration
is to state the percentage of the volume of
the solution that is made up of solute.
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Measuring Concentrations
• Labels on fruit drinks show their
concentration.
• Another way to
describe the
concentration of a
solution is to give a
percentage of the
total mass that is
made up of solute.
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Effects of Solute Particles
• The effect that a solute has on the freezing
or boiling point of a solvent depends on the
number of solute particles.
• When a solvent such as water begins to
freeze, its molecules arrange themselves
in a particular pattern.
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Effects of Solute Particles
• Adding a solute such as sodium chloride to
this solvent changes the way the molecules
arrange themselves.
• To overcome this interference of the solute,
a lower temperature is needed to freeze the
solvent.
End of Chapter Section 2