2. What is aWhat is a solutionsolution??
AA homogeneous mixturehomogeneous mixture
Composed of aComposed of a solutesolute dissolved in adissolved in a
solventsolvent Solute
Solvent
3. How is a solution formed?How is a solution formed?
Through the process ofThrough the process of
Solute particlesSolute particles separate from each other and mixseparate from each other and mix
with thewith the solventsolvent
particlesparticles
Solvent particlesSolvent particles
surround thesurround the solutesolute
particlesparticles and pulland pull
them away from otherthem away from other
solute particlessolute particles
solvation
4. Solute and SolventSolute and Solvent
SolventSolvent
Does theDoes the dissolvingdissolving
GreaterGreater quantity (usually)quantity (usually)
SoluteSolute
What is dissolvedWhat is dissolved
LesserLesser quantity (usually)quantity (usually)
5. Like dissolves likeLike dissolves like
Baking soda will dissolve in water, but not inBaking soda will dissolve in water, but not in
oil…..why?oil…..why?
““Like dissolves like” refers to theLike dissolves like” refers to the bonding andbonding and
polaritypolarity of the particles in theof the particles in the solute and solventsolute and solvent
Polar means a substancePolar means a substance
has ahas a positivepositive and aand a
negativenegative endend
IonicIonic compoundscompounds
6. Ionic compounds in solutionIonic compounds in solution
Cl- Na+
Cl- Na+
Na+
Cl-
Cl-
7. SolubilitySolubility
Only a certain amount of solute can dissolve in aOnly a certain amount of solute can dissolve in a
solvent under a certain set of conditionssolvent under a certain set of conditions
When too much solute is added to a solution atWhen too much solute is added to a solution at
that temperature, the excess solute willthat temperature, the excess solute will
crystallizecrystallize
and fall out of solutionand fall out of solution
SolubilitySolubility is theis the maximummaximum
amount of a soluteamount of a solute thatthat
dissolves in a solvent atdissolves in a solvent at
aa given temperaturegiven temperature
8. SaturationSaturation
AA saturatedsaturated solutionsolution
contains thecontains the maximum amountmaximum amount of dissolvedof dissolved
solutesolute
for a givenfor a given amount of solventamount of solvent
at aat a specificspecific temperaturetemperature andand pressurepressure
9. SupersaturationSupersaturation
A supersaturated solutionA supersaturated solution
containscontains moremore dissolved solute than adissolved solute than a
saturated solutionsaturated solution
at theat the samesame temperature.temperature.
10. Solubility CurvesSolubility Curves
Shows how
much solute
will dissolve
in 100 g of
water at a
certain
temperature
The line represents the saturated amount of solute
Underneath the line represents an unsaturated amount
Above the line represents a supersaturated amount
11. • Which substance is most soluble at 40°C?
• How many grams of NH4Cl will dissolve at 50°C?
• What two substances have the same solubility at 24°C?
• If you place 70 grams of KBr into 100g of water at 60°C, what
type of solution have you made?
• How many grams of NaNO3 will dissolve in 300.0g of water at
10.0°C?
NaNONaNO33
~ 50 grams~ 50 grams
YbYb22(SO(SO44))33
KNO33
unsaturatedunsaturated
~ 240 grams~ 240 grams (80 x 3)(80 x 3)
12. Increasing Solubility - SolidsIncreasing Solubility - Solids
Increase theIncrease the temperaturetemperature
Why? Increases the amount ofWhy? Increases the amount of solute-solventsolute-solvent
collisionscollisions and increasesand increases speed and energyspeed and energy ofof
particlesparticles
AgitateAgitate the solution (stir)the solution (stir)
Why? Brings moreWhy? Brings more
solvent particlessolvent particles closer tocloser to
thethe solutesolute
Decrease the particle sizeDecrease the particle size
IncreasesIncreases thethe surface areasurface area
of the solute, making itof the solute, making it
easier for solvent particles toeasier for solvent particles to
surround the solutesurround the solute
13. Increasing Solubility –Increasing Solubility –
GasesGases
Decrease theDecrease the temperaturetemperature
Increase theIncrease the pressurepressure
If you increase the pressure,If you increase the pressure,
think of pressing the gasthink of pressing the gas
particles into the liquid.particles into the liquid.
Increasing pressure alwaysIncreasing pressure always
increases the amount ofincreases the amount of
gasgas that can bethat can be dissolveddissolved
in a liquid.in a liquid.
14. Rate of SolvationRate of Solvation
Greater solubility = Faster solvationGreater solubility = Faster solvation
The same factors that increase solubility,The same factors that increase solubility,
increase the rate of solvationincrease the rate of solvation
15. ConcentrationConcentration
The larger theThe larger the ratioratio of solute to solventof solute to solvent
becomes, the morebecomes, the more concentratedconcentrated thethe
solution is.solution is.
ConcentratedConcentrated – large ratio of solute to– large ratio of solute to
solventsolvent
DiluteDilute – small ratio of solute to solvent– small ratio of solute to solvent
16. Rates of ReactionRates of Reaction
Concentration affects the rate of reactionConcentration affects the rate of reaction
ConcentratedConcentrated solutions reactsolutions react fasterfaster thanthan
dilutedilute solutionssolutions
17. MolarityMolarity
Most commonly used in chemistryMost commonly used in chemistry
Abbreviated asAbbreviated as MM
MolesMoles of solute in perof solute in per literliter of solutionof solution
moles of solute
Liters of solution
M =
18. ElectrolytesElectrolytes
Electrolyte – ionic compound whose aqueousElectrolyte – ionic compound whose aqueous
solution conducts an electric currentsolution conducts an electric current
–– electrolyteelectrolyte
–– non-electrolytenon-electrolyte
NaClNaCl
SugarSugar
How many moles of
ions are produced by
dissolving 1 mole of
NaCl in water?
19. Colligative PropertiesColligative Properties
Colligative - depending on the collectionColligative - depending on the collection
Properties dependent onProperties dependent on concentrationconcentration,,
number of particles presentnumber of particles present
20. Boiling Point ElevationBoiling Point Elevation
When vapor pressure equals atmosphericWhen vapor pressure equals atmospheric
pressure, water boilspressure, water boils
More particles =More particles = lowerlower vapor pressurevapor pressure
Lower vapor pressure =Lower vapor pressure = higherhigher boiling pointboiling point
More particles =More particles = higherhigher boiling pointboiling point
Which raises boiling
point more, 1 mole of
NaCl in water, or 1
mole of sugar in water?
21. Freezing Point DepressionFreezing Point Depression
Solute particlesSolute particles
interfere with attractioninterfere with attraction
between solventbetween solvent
particlesparticles
MoreMore particles =particles = lowerlower
freezing pointfreezing point
22. OsmosisOsmosis
Osmosis – diffusion ofOsmosis – diffusion of solventsolvent across aacross a
semi-permeable barriersemi-permeable barrier
Solvent goes from:Solvent goes from:
Area ofArea of moremore solventsolvent → Area of→ Area of lessless solventsolvent
27. Miscible and Immiscible
Substances that are miscible will dissolve
in each other.
Example: alchohol and water
Substances that are immiscible will mix
but immediately separate.
Example: oil and vinegar
