Solutions Unit

Honors Chemistry

Solution

bull Definition a homogeneous mixture of 2 or more substances in a single physical state

bull Parts solute and solvent (usually water)bull Types ndash Physical states solid (alloys) liquid gasndash Miscible vs Immiscible

bull Miscible Liquids that dissolve freely in one another in any proportion

bull Immiscible Liquid solutes and solvents that are not soluble

ndash Saturated Unsaturated and Supersaturatedndash Dilute vs Concentratedndash Electrolyte vs Nonelectrolyte

bull Saturated ndash soln containing the max amt of solute

bull Unsaturated ndash soln containing less solute than a sat soln under the existing conditions

bull Supersaturated ndash contains more dissolved solute than a saturated solution under the same conditions

Solubility Curves

supersaturated solution(stirred)

Supersaturated Solution of Sodium Thiosulfate

Solution

bull Definition a homogeneous mixture of 2 or more substances in a single physical state

bull Parts solute and solvent (usually water)bull Types ndash Physical states solid (alloys) liquid gasndash Miscible vs Immiscible

bull Miscible Liquids that dissolve freely in one another in any proportion

bull Immiscible Liquid solutes and solvents that are not soluble

ndash Saturated Unsaturated and Supersaturatedndash Dilute vs Concentratedndash Electrolyte vs Nonelectrolyte

bull Saturated ndash soln containing the max amt of solute

bull Unsaturated ndash soln containing less solute than a sat soln under the existing conditions

bull Supersaturated ndash contains more dissolved solute than a saturated solution under the same conditions

Solubility Curves

supersaturated solution(stirred)

Supersaturated Solution of Sodium Thiosulfate

bull Saturated ndash soln containing the max amt of solute

bull Unsaturated ndash soln containing less solute than a sat soln under the existing conditions

bull Supersaturated ndash contains more dissolved solute than a saturated solution under the same conditions

Solubility Curves

supersaturated solution(stirred)

Supersaturated Solution of Sodium Thiosulfate

supersaturated solution(stirred)

Supersaturated Solution of Sodium Thiosulfate

Solubility (physical change)

bull Definition mass of solute needed to make a saturated solution at a given temperaturendash solution equilibrium in

a closed systemndash dissolution harr

crystallizationndash Unit = g solute100 g

H2O

Solubility of solids in liquids

bull For most solids increasing temperature increases solubility

bull In general ldquolike dissolves likerdquo Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute

and solvent

Solubility Graph for NaNO3

0

10

20

30

40

50

60

70

80

90

100

110

120

130

140

150

160

170

180

0 10 20 30 40 50 60 70 80 90 100 110

Temperature (deg C)

So

lub

ilit

y (

g1

00 g

wat

er )

Saturated solrsquon

Supersaturated solution

Unsaturated solution

At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC

135 g100 g water

What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC

unsaturated

What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC

supersaturated

90 g

Solubility of Gases

bull Gases are less soluble at high temperatures than at low temperatures

bull Increasing temperature decreases solubility

bull Increasing pressure increases solubility

bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a

certain volume of liquid is directly proportional to the pressure of the gas (above the solution)

bull Effervescence ndash rapid escape of gas dissolved in liquid

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

Solubility of solids in liquids

bull For most solids increasing temperature increases solubility

bull In general ldquolike dissolves likerdquo Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute

and solvent

Solubility Graph for NaNO3

0

10

20

30

40

50

60

70

80

90

100

110

120

130

140

150

160

170

180

0 10 20 30 40 50 60 70 80 90 100 110

Temperature (deg C)

So

lub

ilit

y (

g1

00 g

wat

er )

Saturated solrsquon

Supersaturated solution

Unsaturated solution

At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC

135 g100 g water

What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC

unsaturated

What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC

supersaturated

90 g

Solubility of Gases

bull Gases are less soluble at high temperatures than at low temperatures

bull Increasing temperature decreases solubility

bull Increasing pressure increases solubility

bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a

certain volume of liquid is directly proportional to the pressure of the gas (above the solution)

bull Effervescence ndash rapid escape of gas dissolved in liquid

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

Solubility Graph for NaNO3

0

10

20

30

40

50

60

70

80

90

100

110

120

130

140

150

160

170

180

0 10 20 30 40 50 60 70 80 90 100 110

Temperature (deg C)

So

lub

ilit

y (

g1

00 g

wat

er )

Saturated solrsquon

Supersaturated solution

Unsaturated solution

At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC

135 g100 g water

What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC

unsaturated

What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC

supersaturated

90 g

Solubility of Gases

bull Gases are less soluble at high temperatures than at low temperatures

bull Increasing temperature decreases solubility

bull Increasing pressure increases solubility

bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a

certain volume of liquid is directly proportional to the pressure of the gas (above the solution)

bull Effervescence ndash rapid escape of gas dissolved in liquid

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

Solubility of Gases

bull Gases are less soluble at high temperatures than at low temperatures

bull Increasing temperature decreases solubility

bull Increasing pressure increases solubility

bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a

certain volume of liquid is directly proportional to the pressure of the gas (above the solution)

bull Effervescence ndash rapid escape of gas dissolved in liquid

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a

certain volume of liquid is directly proportional to the pressure of the gas (above the solution)

bull Effervescence ndash rapid escape of gas dissolved in liquid

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

bull Effervescence ndash rapid escape of gas dissolved in liquid

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

Factors Affecting Solubility

bull Increase surface area of solute (crushing)

bull Stirshakebull Increase temperature

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

Dissolution Processbull Ionic Compounds

NaCl(s) Na+1(aq) + Cl-1(aq)

ndash For dissolution to occur must overcome solute attractions and solvent attractions

ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)

ndash Try calcium chloride

hexahydrated for Na+1 most cations have 4-9 H2O molecules

6 is most common

Solvation process of solvent moleculessurrounding solute

Hydration solvation with water

nonelectrolyte

electrolyte

Dissolving NaCl in water

Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in

polar solvents bull naphthalene

ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte

ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by

action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)

Electrolyte vs Nonelectrolyte

Concentrationbull Percent concentration by mass (mass

ndash (solutesolution) x 100 = Concentrationbull Molarity (M)

ndash Moles of soluteLiters of solution = molLbull Molality (m)

ndash Moles of solutemass of solvent = molkgbull ppm and ppb

ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is

added to a solutionndash How is this solution different

bull Volume color molarityndash How is it the same

bull Same mass of solute same moles of solute

ndash In Dilution ONLY ndash M1V1 = M2V2

Net Ionic Equationsbull Net ionic equations are equations that show

only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into

ionsndash Substances that pure solids liquids or gases do

not break down in solution ndash Hint Remember to check solubility rules to

determine if a precipitate forms

Energy Changesbull Heat of solution = Hsoln

bull Endothermicndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter

liquidndash Energy absorbed

bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released

Colligative Properties

bull Definition physical properties of solutions that differ from properties of its solvent ndash Property depends upon the number of

solute particles in solution

bull Types1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Electrolyte vs Nonelectrolyte

Concentrationbull Percent concentration by mass (mass

ndash (solutesolution) x 100 = Concentrationbull Molarity (M)

ndash Moles of soluteLiters of solution = molLbull Molality (m)

ndash Moles of solutemass of solvent = molkgbull ppm and ppb

ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is

added to a solutionndash How is this solution different

bull Volume color molarityndash How is it the same

bull Same mass of solute same moles of solute

ndash In Dilution ONLY ndash M1V1 = M2V2

Net Ionic Equationsbull Net ionic equations are equations that show

only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into

ionsndash Substances that pure solids liquids or gases do

not break down in solution ndash Hint Remember to check solubility rules to

determine if a precipitate forms

Energy Changesbull Heat of solution = Hsoln

bull Endothermicndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter

liquidndash Energy absorbed

bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released

Colligative Properties

bull Definition physical properties of solutions that differ from properties of its solvent ndash Property depends upon the number of

solute particles in solution

bull Types1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Concentrationbull Percent concentration by mass (mass

ndash (solutesolution) x 100 = Concentrationbull Molarity (M)

ndash Moles of soluteLiters of solution = molLbull Molality (m)

ndash Moles of solutemass of solvent = molkgbull ppm and ppb

ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is

added to a solutionndash How is this solution different

bull Volume color molarityndash How is it the same

bull Same mass of solute same moles of solute

ndash In Dilution ONLY ndash M1V1 = M2V2

Net Ionic Equationsbull Net ionic equations are equations that show

only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into

ionsndash Substances that pure solids liquids or gases do

not break down in solution ndash Hint Remember to check solubility rules to

determine if a precipitate forms

Energy Changesbull Heat of solution = Hsoln

bull Endothermicndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter

liquidndash Energy absorbed

bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released

Colligative Properties

bull Definition physical properties of solutions that differ from properties of its solvent ndash Property depends upon the number of

solute particles in solution

bull Types1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Net Ionic Equationsbull Net ionic equations are equations that show

only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into

ionsndash Substances that pure solids liquids or gases do

not break down in solution ndash Hint Remember to check solubility rules to

determine if a precipitate forms

Energy Changesbull Heat of solution = Hsoln

bull Endothermicndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter

liquidndash Energy absorbed

bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released

Colligative Properties

bull Definition physical properties of solutions that differ from properties of its solvent ndash Property depends upon the number of

solute particles in solution

bull Types1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Energy Changesbull Heat of solution = Hsoln

bull Endothermicndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter

liquidndash Energy absorbed

bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released

Colligative Properties

bull Definition physical properties of solutions that differ from properties of its solvent ndash Property depends upon the number of

solute particles in solution

bull Types1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Colligative Properties

bull Definition physical properties of solutions that differ from properties of its solvent ndash Property depends upon the number of

solute particles in solution

bull Types1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Vapor PressureA measure of the tendency of molecules to escape from a liquid

bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the

boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the

concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to

leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS

than pure water

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

H2O H2O H2O Sugar H2O

Same Temperature

Temperature (ordmC)

Vapor Pressure (kPa)

100

40

20

60

80

100H2O solution

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Boiling Point Elevation

bull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash bp of solution = bp of solvent + tb

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance

deviates for more concentrated solutions

bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic

compounds adjust for of ions actually present in solution (dissociation process)

ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O

moles of solute (ions or molecules)ndash m = molality = moles solute

kg of solventndash fp of solution = fp of solvent - tf

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Boiling Point Elevation and Freezing Point Problems

1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute

2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid

Ex) HCl hydrochloric acid

Ex) H3P hydrophosphoric acid

B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo

(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid

Ex) H2SO4 sulfuric acid

Ex) H2SO3 sulfurous acid

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Properties of Acids and Bases

Taste Touch Reactions with Metals

Electrical Conductivity

Acid sour

looks like water burns stings

Yes-produces

H2 gas

electrolyte in solution

Base(alkali)

bitter

looks like water feels

slippery

No Reaction

electrolyte in solution

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Indicators Turn 1 color in an acid and another color in a base

A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue

B Phenolphthalein colorless in an acid and pink in a base

C pH paper range of colors from acidic to basic

D pH meter measures the concentration of H+ in solution

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form

Acid + Base rarr Salt + Water

Ex) HCl + NaOH rarr NaCl + HOH

Reactions

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Arrhenius Definition (1884)A An acid dissociates in water to produce more

hydrogen ions H+HCl H+1 + Cl-1

B A base dissociates in water to produce more hydroxide ions OH-

NaOH Na+1 + OH-1

C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids

dissolve in waterbull Does not include certain compounds that have

characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions

Ex) HCl rarr H+ + Cl-

ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)

B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4

+

ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition

bullAcids and bases are defined independently of how they behave in water

bullFocuses solely on hydrogen ions

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Hydronium Ion

Hydronium Ion ndash H3O+ This is a complex ion that forms in water

H+1 + H2O H3O+1

To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

STRONG AcidBase versus WEAK AcidBase

Strength refers to the of molecules that form IONS

A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow

HNO3 + H2O H3O+ + NO3-

A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow

HOCl + H2O harr H3O+ + ClO-

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

HF lt HCl lt HBr lt HIincreasing strength

7 Strong AcidsHNO3 H2SO4 HClO3

HClO4 HCl HBrHI

8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2

Sr(OH)2 Ba(OH)2

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Strength vs Concentration

bull Strength refers to the percent of molecules that form ions

bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Ionization of Acids amp Bases

bull H2SO4 2 H+ + SO4-2

ndash Sulfuric acid

bull H3PO3 ndash Phosphorous acid

bull Ca(OH)2 ndash Calcium hydroxide

3 H+ + PO3-3

Ca+2 + 2 OH-1

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion

A Acid donates a proton to become a conjugate base

B Base accepts proton to become a conjugate acid

bull A strong acid will have a weak conjugate base

bull A strong base will have a weak conjugate acid

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)

NH3 + H2O harr NH4+ + OH-

HCl + H2O harr Cl- + H3O+

bull Base and Conjugate Acid are a Conjugate Pair

bull Acid and Conjugate Base are a Conjugate Pair

B

B

A

A

CA CB

CB CA

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

1 H2O + H2O harr H3O+ + OHminus B A CA CB

2 H2SO4 + OHminus harr HSO4minus + H2O

A B CB CA

3 HSO4minus + H2O harr SO4

minus2 + H3O+ A B CB CA

4 OHminus + H3O+ harr H2O + H2O B A CA CB

AciDonates amp Bases accept

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the

same reaction

Ex) H2O(l) + H2O(l) harr H3O+(aq) + OH-

(aq)

Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is

not included in the equilibrium expression

25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water

Kw = [H3O+] [OH-] = 1 x 10-14 M2

10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]

10 x 10-14 = [H3O+] [OH-]

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M

Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral

Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]

25 x 10-7 M = [OH-] slightly basic

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

The pH scale (1909) the power of Hydrogen

A Measure of H3O+ in solution

B pH = -log[H3O+]

C Range of pH 0-14

pH lt 7 acid

pH gt 7 base

pH = 7 neutralD pOH = -log[OH-]

E pH + pOH = 14

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

H+

OH

-

pH [H3O+] [OH-]

14 1x10-14 1x100

13 1x10-13 1x10-1

12 1x10-12 1x10-2

11 1x10-11 1x10-3

10 1x10-10 1x10-4

9 1x10-9 1x10-5

8 1x10-8 1x10-6

7 1x10-7 1x10-7

6 1x10-6 1x10-8

5 1x10-5 1x10-9

4 1x10-4 1x10-10

3 1x10-3 1x10-11

2 1x10-2 1x10-12

1 1x10-1 1x10-131

14

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule

Significant Digits Rule

bull The number of digits AFTER THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number

bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306

• Solutions Unit
• Solution
• Slide 3
• Slide 4
• supersaturated solution (stirred)
• Solubility (physical change)
• Solubility of solids in liquids
• Slide 8
• Solubility of Gases
• Slide 10
• Slide 11
• Factors Affecting Solubility
• Dissolution Process
• Slide 14
• Dissolution Process (2)
• Electrolyte vs Nonelectrolyte
• Concentration
• Net Ionic Equations
• Energy Changes
• Colligative Properties
• Vapor Pressure A measure of the tendency of molecules to escape
• Slide 22
• Boiling Point Elevation
• Freezing Point Depression when a solution freezes the solvent
• Boiling Point Elevation and Freezing Point Problems
• Naming Acids Review
• Properties of Acids and Bases
• Indicators Turn 1 color in an acid and another color in a base
• Slide 29
• Reactions
• Slide 31
• Bronsted-Lowry Definition (1923)
• Hydronium Ion
• STRONG AcidBase versus WEAK AcidBase
• HF lt HCl lt HBr lt HI increasing strength
• Strength vs Concentration
• Ionization of Acids amp Bases
• Slide 38
• Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
• AciDonates amp Bases accept
• The Self-ionization of Water amp pH
• Slide 42
• The pH scale (1909) the power of Hydrogen
• Slide 44
• Significant Digits Rule