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A SOLUTION is a homogeneous mixture;
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Particles are evenly distributed throughout the mixture.
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Amounts may vary ____________________ solutions (variable proportions) BUT
the _____________ of amounts is the __________ throughout a particular solution
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You might like a little sugar in your Koolaid or a lot, but within a glass of Koolaid, the sugar is mixed
evenly
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No __________ __________________…no scattering of light, because particles are so small
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Red powder: flavor and color White crystals: sugar Clear liquid: water
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One substance dissolved in another
______________________: the substance being dissolved
______________________: the substance that dissolves the solute
_________________ is the SOLUTE (smaller quantity)
_________________is the SOLVENT (larger quantity)
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TYPES OF SOLUTIONS
Gas (solvent is gas)
Gas into Gas: ____________
Liquid into Gas: __________________
Solid into Gas: ________________________________
Liquid (solvent is liquid)
Gas into Liquid: ____________________
Liquid into Liquid: _______________________
Solid into Liquid: ____________________________
Solid (solvent is solid)
Gas into Solid: _________________________
Liquid into Solid: _____________________________
Solid into Solid: ______________________________
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THE DISSOLVING PROCESS
Two factors affect the dissolving process: ___________________________
The constant ________________ of the particles
(______________ ___________ __________)
The ______________ of the solute and solvent (Recall that polarity is when a
compound has partial charges because of uneven distribution of charges)
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THE ________________________________ ________________________________
_____________ ___________ particles cluster around solute molecules or particles at the
surface of the solid.
Solvent molecules pull ____________ off of the solid ___________ and into solution.
Moving solvent particles continue to __________ ___________ evenly throughout the
solution,
The process ____________ itself as fresh layers of the solute are exposed.
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ELECTROLYTE AND NONELECTROLYTES
When an ____________ substance dissolves in water, the forces of the solvent pulling on
the ions is stronger than the forces holding the ions together.
The ions separate. This is called ______________________________
Because charged ions are present in an ionic solution, ionic solutions conduct electricity and
are called ___________________________________.
EXAMPLE: NaCl
Certain ____________ substances form ions when they dissolve in water. This process is
called _________________________.
Because ions are formed, the solution conducts electricity.
These substance are also ______________________________.
EXAMPLE: HCl, HC2H3O2
Other polar substances do __________ionize in water.
Because ions are not formed, the solution does not conduct electricity.
These substances that do not ionize in water and do not conduct electricity are called
____________________________________________
EXAMPLE: sugar
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Factors that affect the rate of solution of solid and liquid solutes in liquid solvent
Factors
Solid in
Liquid
Gas in Liquid
TEMPERATURE
Temp
Temp
Rate
Rate
Agitation
Agitation
Rate
Rate
Size
NA
AGITATION
SIZE OF PARTICLES
(surface area
)
Rate
PRESSURE
NA
Pressure
Rate
WHY?
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The solute particles are
less energetic than
solvent
The solute particles are more
energetic than solvent
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SOLUBILITY…what dissolves in what?
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Solvents with non-polar molecules dissolve _________________________ substances
Oil, grease, dry cleaning fluid, paint, turpentine
Solvents with polar molecules dissolve _________________________ substances
Water dissolves sugar, ionic compounds
The rule for solubility is easy: __________ _____________________ ______________
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_________________: capable of being dissolved in a particular solvent
_________________: incapable of being dissolved in a particular solvent
_________________: liquids that dissolve freely in any proportion
_________________: liquids that are not soluble in each other
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DETERGENTS AND EMULSIFIERS
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_____________________ is non-polar
_____________________ is polar
______________________________________ has
A non-polar end that dissolves the ___________________________
A polar end that dissolves in the ___________________to rinse it away
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SOLUBILITY…how much solute can dissolve in solvent?
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There are limits to the amount of solute that will dissolve in a given amount of solvent at a
given temperature
There are some general terms:
_____________________________: a solution that can dissolve more of a given
solute at a certain temperature
A crystal of solute added to an unsaturated solution will dissolve
When you add a second spoon of sugar to your cup of tea, it dissolves. The tea was
an unsaturated solution.
_____________________________: a solution that has dissolved all of the solute
that it can at a certain temperature
A crystal of solute added to a saturated solution will drop to the bottom, undissolved.
When you add three spoons of sugar to your tea, some sugar drops to the bottom,
undissolved. It is a saturated solution.
DYNAMIC EQUILIBRIUM exists:
changing but balanced.
Some solid dissolves, but as some dissolves, some re-crystallizes
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______________________________________: an unstable solution that contains
more solute than a saturated solution at a certain temperature
A crystal of solute added to a super-saturated solution will cause crystallization. So
will any disruption of the unstable solution.
Make a saturated solution at an elevated temperature and cool it slowly. At the
lower temperature, the solute will remain dissolved in an unstable situation. If
disrupted, the solute crystallizes.
Hot-packs and rock candy
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SOLUBILITY CURVES give quantitative information about how much of a solute in a
certain amount of solvent at a certain temperature.
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HOW DO WE EXPRESS CONCENTRATION?
_______________________________: the amount of solute in a given amount of
solvent or solution
___________: a relatively small amount of solute in a relatively large amount of
solvent
____________________: a relatively large amount of solute in a relatively small
amount of solvent
Percent by volume_____________________________________________________
mL of solute /100 mL of solution
Percent by mass_______________________________________________________
g of solute/100 mL of solution
PPM and PPB__________________________________________________________
x/1,000,000
x/1,000,000,000
Serial dilutions are often used
1x, 10x, 100x, 1000x, etc.
Mass per volume______________________________________________________
g solute/1000 mL solution
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COLLIGATIVE PROPERTIES
______________________________…sounds like collective
The ___________________ of dissolved particles affect properties of solution
It does not matter WHAT the particles are
It only matters HOW MANY particles there are
Collectively (all together) the amount of the particles have an effect
___________________ _________________________
___________________________
The more particles of solute dissolved in a solution, the higher the boiling point.
More particles of solute at the surface mean fewer solvent particles can
vaporize, thus raising the boiling point.
EX] anitfreeze dissolved in the coolant of our cars raises the boiling
point to keep our engine from overheating.
____________________ _______________________ _____________________
The more particles of solute dissolved in a solution, the lower the freezing point.
More particles of solute interfere with crystal formation, lowering the freezing point.
EX] antifreeze dissolved in the coolant of our cars lowers the freezing point to keep
our engine running in cold weather
EX] Salt on the sidewalks melts the ice