solutions chapter 12 modern chemistry

Chapter 8 Section 1 Describing Chemical Reactions p. 261-275

1

SolutionsSolutionsChapter 12 Modern Chapter 12 Modern ChemistryChemistry

Sections 1-3Sections 1-3

Types of MixturesTypes of Mixtures

The Solution ProcessThe Solution Process

Concentrations of Concentrations of SolutionSolution

Chapter 12 Section 2 The Solution Process p. 407-417

2

The Solution The Solution ProcessProcess

Section 12.2Section 12.2

Chapter 12 Section 1 Types of Mixtures p. 401-406

3

SolubilityFactors affecting

rate of dissolutionSaturatedUnsaturatedSupersaturatedSolubility equilibriumSolubility values

VocabularyVocabularyDissociation HydrationInsolubleImmiscibleMiscibleHenry’s LawEffervescence

Chapter 12 Section 1 Types of Mixtures p. 401-406

4

FACTORS AFFECTING RATE OF DISSOLUTIONFACTORS AFFECTING RATE OF DISSOLUTION

Concept Map 12.2Concept Map 12.2

UNSATURATEDUNSATURATED SATURATEDSATURATED SUPERSATURATEDSUPERSATURATED

LIQUID SOLUTELIQUID SOLUTE

SOLUBILITYEQUILIBRIUMSOLUBILITY

EQUILIBRIUM

GAS SOLUTEGAS SOLUTE

DIS

SO

CIA

TIO

ND

ISSO

CIA

TIO

N

IONIC SOLUTEIONIC SOLUTE

SOLUBILITYSOLUBILITY SOLUBILITYVALUES

SOLUBILITYVALUES

HYD

RA

TIO

NH

YD

RA

TIO

N

SOLUBLESOLUBLE

LIKES DISSOLVE

LIKES

LIKES DISSOLVE

LIKES

PRESSUREPRESSURE

TEMPERATURETEMPERATURE

HEN

RY’S

LA

WH

EN

RY’S

LA

W

EFF

ER

VE

SC

EN

CE

EFF

ER

VE

SC

EN

CE

IMM

ISC

IBLE

IM

MIS

CIB

LE

MIS

CIB

LE

MIS

CIB

LE

INSOLUBLEINSOLUBLE


5

How would you make a solute dissolve faster?

• Stir.

• Break it up.

• Heat it.

Factors Affecting the Rate of Factors Affecting the Rate of DissolutionDissolution

Agitate the solution

Heat the solvent

Increase the surface area of the solute


6Facto

rs A

ffecti

ng

Dis

solu

tion

Rate

Facto

rs A

ffecti

ng

Dis

solu

tion

Rate


7

• Solubility of a substance is the amount of that substance required to form a saturated solutions with a specific amount of solvent at a specific temperature

• Look at the chart on page 410• Dependant on

the nature of the solvent and the solute and the temperature of the solute

• The maximum amount that can be dissolved is not dependant on the rate it dissolves

SolubilitySolubility

in grams

100 g H2O20° C


8p. 410

Solubility & TemperatureSolubility & Temperature


9p. 414*Solu

bilit

y a

nd

Tem

pera

ture

Solu

bilit

y a

nd

Tem

pera

ture


10Solu

bilit

y o

f S

olid

s in

Liq

uid

sS

olu

bilit

y o

f S

olid

s in

Liq

uid

s


11

• There is a limit to the amount of solute that can be dissolved. Why?

• Solubility Equilibrium – the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates.

• In other words… the same amount of solute is dissolving and “undissolving” at the same time.

SolubilitySolubility


12Solu

bilit

y &

Solu

tion

Eq

uilib

riu

mS

olu

bilit

y &

Solu

tion

Eq

uilib

riu

m


13Solu

bilit

y E

qu

ilib

riu

mS

olu

bilit

y E

qu

ilib

riu

m

Insert Holt Disc 2Insert Holt Disc 2


14

• Saturated – A solution that contains the maximum amount of dissolved solute.

• You can tell that it is saturated because no more solute will dissolve and fall to the bottom of the container.

• Unsaturated – A solution that contains less solute than a saturated solution under the existing conditions.

Saturated & Unsaturated Saturated & Unsaturated SolnsSolns


15p. 409

Mass of Solute Added vs Mass of Solute Mass of Solute Added vs Mass of Solute DissolvedDissolved


16

• A solution that contains more dissolved solute than a saturated solution contains under the same conditions.

• HOW? Saturate a solution. Heat the solution so that more solute can be added. When the solution is cooled undisturbed it will be saturated.

Supersaturated SolutionsSupersaturated Solutions


17

UnsaturatedUnsaturated

SaturatedSaturated

SupersaturatSupersaturateded

LESS than 35.9g NaCl in 100g H2O at 20°C

EXACTLY 35.9g NaCl in 100g H2O at 20°C

MORE than 35.9g NaCl MORE than 35.9g NaCl

in 100g Hin 100g H22O at 20O at 20°C°C


18NaC

NaC

22HH

33OO

22 T

ow

er

Tow

er



19Solu

bilit

y o

f C

om

pou

nd

sS

olu

bilit

y o

f C

om

pou

nd

s

notes


20Solu

bilit

y o

f C

om

pou

nd

sS

olu

bilit

y o

f C

om

pou

nd

s

notes


21

• What is the molecule polarity of H2O? CCl4?

• How do we determine this?

Molecule Polarity REVIEW!!Molecule Polarity REVIEW!!



22

• Ionic solids that dissolve are soluble.• Ionic solids will dissolve in polar solvents

but not nonpolar solvents• Water molecules break the crystal lattice

into separate ions. This is dissociation.• Then the water molecules surround the

ions. This is hydration. • Ionic solids that do not dissolve are

insoluble.

Ionic Solute-Solvent Ionic Solute-Solvent InteractionInteraction


23p. 411

Ion

ic S

olu

te-S

olv

en

t In

tera

cti

on

Ion

ic S

olu

te-S

olv

en

t In

tera

cti

on


24Dis

socia

tion

An

imati

on

sD

issocia

tion

An

imati

on

s


Insert Glencoe Disk 2Insert Glencoe Disk 2


25Hyd

rate

d N

aH

yd

rate

d N

a++



26

• Miscible – Liquids that dissolve freely in one another in any proportion.

• Immiscible – Liquids that are not soluble in each other.

• “Likes dissolve likes”Polar solutes dissolve in polar

solvents.Nonpolar solutes dissolve in

nonpolar solvents.• Alcohols are slightly polar.

Liquid Solute-Solvent Liquid Solute-Solvent InteractionInteraction


27Mis

cib

le a

nd

Im

mis

cib

leM

iscib

le a

nd

Im

mis

cib

le


28p. 412

Immiscible & MiscibleImmiscible & Miscible


29

How Soap How Soap WorksWorks


Iodine Iodine SolubilitySolubility


30

• Effect of pressure on gas solubility• Pressure changes have little effect on

liquid or solid solutes.• Gases dissolved in a liquid are in an

equilibrium• This means that some of the gas

molecules are going into the solvent and some are going out of the solvent at equal rates.

Gas Solute-Solvent Gas Solute-Solvent InteractionsInteractions


31Solu

bilit

y o

f a G

as in

a L

iqu

idS

olu

bilit

y o

f a G

as in

a L

iqu

id


32

• Henry’s Law– The solubility

of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.



33

After being underwater for a long time, a diver will have more gases dissolved in the blood. The diver must pause during the ascent to allow the dissolved gas to come out of solution (the blood) slowly and to be exhaled. If the ascent is too fast the gas can come out of solution while flowing through blood vessels and block essential blood vessels, causing extreme pain, paralysis, or even death.



34Efe

rvescen

ce

Efe

rvescen

ce


35

Keep the fizz in your Keep the fizz in your soda!soda!

http://www.eepybird.com/dcm1.html


36

Eepy BirdEepy Birdhttp://www.eepybird.com/videos.htmlSteve Spangler ScienceSteve Spangler Sciencehttp://www.stevespanglerscience.com/experiment/00000109MythbusterMythbusterhttp://www.youtube.com/watch?v=

kMXPOqovSBs&feature=related

Mentos and Coke?Mentos and Coke?

http://www.eepybird.com/videos.html

http://www.eepybird.com/videos.html

http://www.stevespanglerscience.com/experiment/00000109

http://www.stevespanglerscience.com/experiment/00000109

http://www.youtube.com/watch?v=kMXPOqovSBs&feature=related






37

• Effect of temperature on gas solubility• Increasing temperature decreases the

solubility of a gas• An increased temperature increases the

kinetic energy so that gas molecules can escape from the solvent



38

• The net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent.

• If heat is given off when the solute dissolves, it is exothermic and the enthalpy is negative.

• If heat is taken in when the solute dissolves, it is endothermic and the enthalpy is positive.

• Look at the table of enthalpies on page 416.

Enthalpy of SolutionEnthalpy of Solution


39p. 416

Enthalpies of SolutionsEnthalpies of Solutions


40Han

dh

eld

Heate

rH

an

dh

eld

Heate

r



41p. 415

Enthalpies of SolutionsEnthalpies of Solutions


42

Ch 12 Sec 2 HomeworkCh 12 Sec 2 Homework

Section Review Page 416 # 1-7

solutions chapter 12 modern chemistry

Documents

solution processchapter

dissolved solute

solubility temperaturep

solubility of solids

rate of dissolutionhow

g nacl

specific temperaturelook

dissolution ratechapter