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Raffi Hovasapian

Raffi Hovasapian

Acid-Base Reactions

Slide Duration:

Table of Contents

I. Review
Naming Compounds

41m 24s

Intro
0:00
Periodic Table of Elements
0:15
Naming Compounds
3:13
Definition and Examples of Ions
3:14
Ionic (Symbol to Name): NaCl
5:23
Ionic (Name to Symbol): Calcium Oxide
7:58
Ionic - Polyatoms Anions: Examples
12:45
Ionic - Polyatoms Anions (Symbol to Name): KClO
14:50
Ionic - Polyatoms Anions (Name to Symbol): Potassium Phosphate
15:49
Ionic Compounds Involving Transition Metals (Symbol to Name): Co₂(CO₃)₃
20:48
Ionic Compounds Involving Transition Metals (Name to Symbol): Palladium 2 Acetate
22:44
Naming Covalent Compounds (Symbol to Name): CO
26:21
Naming Covalent Compounds (Name to Symbol): Nitrogen Trifluoride
27:34
Naming Covalent Compounds (Name to Symbol): Dichlorine Monoxide
27:57
Naming Acids Introduction
28:11
Naming Acids (Name to Symbol): Chlorous Acid
35:08
% Composition by Mass Example
37:38
Stoichiometry

37m 19s

Intro
0:00
Stoichiometry
0:25
Introduction to Stoichiometry
0:26
Example 1
5:03
Example 2
10:17
Example 3
15:09
Example 4
24:02
Example 5: Questions
28:11
Example 5: Part A - Limiting Reactant
30:30
Example 5: Part B
32:27
Example 5: Part C
35:00
II. Aqueous Reactions & Stoichiometry
Precipitation Reactions

31m 14s

Intro
0:00
Precipitation Reactions
0:53
Dissociation of ionic Compounds
0:54
Solubility Guidelines for ionic Compounds: Soluble Ionic Compounds
8:15
Solubility Guidelines for ionic Compounds: Insoluble ionic Compounds
12:56
Precipitation Reactions
14:08
Example 1: Mixing a Solution of BaCl₂ & K₂SO₄
21:21
Example 2: Mixing a Solution of Mg(NO₃)₂ & KI
26:10
Acid-Base Reactions

43m 21s

Intro
0:00
Acid-Base Reactions
1:00
Introduction to Acid: Monoprotic Acid and Polyprotic Acid
1:01
Introduction to Base
8:28
Neutralization
11:45
Example 1
16:17
Example 2
21:55
Molarity
24:50
Example 3
26:50
Example 4
30:01
Example 4: Limiting Reactant
37:51
Example 4: Reaction Part
40:01
Oxidation Reduction Reactions

47m 58s

Intro
0:00
Oxidation Reduction Reactions
0:26
Oxidation and Reduction Overview
0:27
How Can One Tell Whether Oxidation-Reduction has Taken Place?
7:13
Rules for Assigning Oxidation State: Number 1
11:22
Rules for Assigning Oxidation State: Number 2
12:46
Rules for Assigning Oxidation State: Number 3
13:25
Rules for Assigning Oxidation State: Number 4
14:50
Rules for Assigning Oxidation State: Number 5
15:41
Rules for Assigning Oxidation State: Number 6
17:00
Example 1: Determine the Oxidation State of Sulfur in the Following Compounds
18:20
Activity Series and Reduction Properties
25:32
Activity Series and Reduction Properties
25:33
Example 2: Write the Balance Molecular, Total Ionic, and Net Ionic Equations for Al + HCl
31:37
Example 3
34:25
Example 4
37:55
Stoichiometry Examples

31m 50s

Intro
0:00
Stoichiometry Example 1
0:36
Example 1: Question and Answer
0:37
Stoichiometry Example 2
6:57
Example 2: Questions
6:58
Example 2: Part A Solution
12:16
Example 2: Part B Solution
13:05
Example 2: Part C Solution
14:00
Example 2: Part D Solution
14:38
Stoichiometry Example 3
17:56
Example 3: Questions
17:57
Example 3: Part A Solution
19:51
Example 3: Part B Solution
21:43
Example 3: Part C Solution
26:46
III. Gases
Pressure, Gas Laws, & The Ideal Gas Equation

49m 40s

Intro
0:00
Pressure
0:22
Pressure Overview
0:23
Torricelli: Barometer
4:35
Measuring Gas Pressure in a Container
7:49
Boyle's Law
12:40
Example 1
16:56
Gas Laws
21:18
Gas Laws
21:19
Avogadro's Law
26:16
Example 2
31:47
Ideal Gas Equation
38:20
Standard Temperature and Pressure (STP)
38:21
Example 3
40:43
Partial Pressure, Mol Fraction, & Vapor Pressure

32m

Intro
0:00
Gases
0:27
Gases
0:28
Mole Fractions
5:52
Vapor Pressure
8:22
Example 1
13:25
Example 2
22:45
Kinetic Molecular Theory and Real Gases

31m 58s

Intro
0:00
Kinetic Molecular Theory and Real Gases
0:45
Kinetic Molecular Theory 1
0:46
Kinetic Molecular Theory 2
4:23
Kinetic Molecular Theory 3
5:42
Kinetic Molecular Theory 4
6:27
Equations
7:52
Effusion
11:15
Diffusion
13:30
Example 1
19:54
Example 2
23:23
Example 3
26:45
AP Practice for Gases

25m 34s

Intro
0:00
Example 1
0:34
Example 1
0:35
Example 2
6:15
Example 2: Part A
6:16
Example 2: Part B
8:46
Example 2: Part C
10:30
Example 2: Part D
11:15
Example 2: Part E
12:20
Example 2: Part F
13:22
Example 3
14:45
Example 3
14:46
Example 4
18:16
Example 4
18:17
Example 5
21:04
Example 5
21:05
IV. Thermochemistry
Energy, Heat, and Work

37m 32s

Intro
0:00
Thermochemistry
0:25
Temperature and Heat
0:26
Work
3:07
System, Surroundings, Exothermic Process, and Endothermic Process
8:19
Work & Gas: Expansion and Compression
16:30
Example 1
24:41
Example 2
27:47
Example 3
31:58
Enthalpy & Hess's Law

32m 34s

Intro
0:00
Thermochemistry
1:43
Defining Enthalpy & Hess's Law
1:44
Example 1
6:48
State Function
13:11
Example 2
17:15
Example 3
24:09
Standard Enthalpies of Formation

23m 9s

Intro
0:00
Thermochemistry
1:04
Standard Enthalpy of Formation: Definition & Equation
1:05
∆H of Formation
10:00
Example 1
11:22
Example 2
19:00
Calorimetry

39m 28s

Intro
0:00
Thermochemistry
0:21
Heat Capacity
0:22
Molar Heat Capacity
4:44
Constant Pressure Calorimetry
5:50
Example 1
12:24
Constant Volume Calorimetry
21:54
Example 2
24:40
Example 3
31:03
V. Kinetics
Reaction Rates and Rate Laws

36m 24s

Intro
0:00
Kinetics
2:18
Rate: 2 NO₂ (g) → 2NO (g) + O₂ (g)
2:19
Reaction Rates Graph
7:25
Time Interval & Average Rate
13:13
Instantaneous Rate
15:13
Rate of Reaction is Proportional to Some Power of the Reactant Concentrations
23:49
Example 1
27:19
Method of Initial Rates

30m 48s

Intro
0:00
Kinetics
0:33
Rate
0:34
Idea
2:24
Example 1: NH₄⁺ + NO₂⁻ → NO₂ (g) + 2 H₂O
5:36
Example 2: BrO₃⁻ + 5 Br⁻ + 6 H⁺ → 3 Br₂ + 3 H₂O
19:29
Integrated Rate Law & Reaction Half-Life

32m 17s

Intro
0:00
Kinetics
0:52
Integrated Rate Law
0:53
Example 1
6:26
Example 2
15:19
Half-life of a Reaction
20:40
Example 3: Part A
25:41
Example 3: Part B
28:01
Second Order & Zero-Order Rate Laws

26m 40s

Intro
0:00
Kinetics
0:22
Second Order
0:23
Example 1
6:08
Zero-Order
16:36
Summary for the Kinetics Associated with the Reaction
21:27
Activation Energy & Arrhenius Equation

40m 59s

Intro
0:00
Kinetics
0:53
Rate Constant
0:54
Collision Model
2:45
Activation Energy
5:11
Arrhenius Proposed
9:54
2 Requirements for a Successful Reaction
15:39
Rate Constant
17:53
Arrhenius Equation
19:51
Example 1
25:00
Activation Energy & the Values of K
32:12
Example 2
36:46
AP Practice for Kinetics

29m 8s

Intro
0:00
Kinetics
0:43
Example 1
0:44
Example 2
6:53
Example 3
8:58
Example 4
11:36
Example 5
16:36
Example 6: Part A
21:00
Example 6: Part B
25:09
VI. Equilibrium
Equilibrium, Part 1

46m

Intro
0:00
Equilibrium
1:32
Introduction to Equilibrium
1:33
Equilibrium Rules
14:00
Example 1: Part A
16:46
Example 1: Part B
18:48
Example 1: Part C
22:13
Example 1: Part D
24:55
Example 2: Part A
27:46
Example 2: Part B
31:22
Example 2: Part C
33:00
Reverse a Reaction
36:04
Example 3
37:24
Equilibrium, Part 2

40m 53s

Intro
0:00
Equilibrium
1:31
Equilibriums Involving Gases
1:32
General Equation
10:11
Example 1: Question
11:55
Example 1: Answer
13:43
Example 2: Question
19:08
Example 2: Answer
21:37
Example 3: Question
33:40
Example 3: Answer
35:24
Equilibrium: Reaction Quotient

45m 53s

Intro
0:00
Equilibrium
0:57
Reaction Quotient
0:58
If Q > K
5:37
If Q < K
6:52
If Q = K
7:45
Example 1: Part A
8:24
Example 1: Part B
13:11
Example 2: Question
20:04
Example 2: Answer
22:15
Example 3: Question
30:54
Example 3: Answer
32:52
Steps in Solving Equilibrium Problems
42:40
Equilibrium: Examples

31m 51s

Intro
0:00
Equilibrium
1:09
Example 1: Question
1:10
Example 1: Answer
4:15
Example 2: Question
13:04
Example 2: Answer
15:20
Example 3: Question
25:03
Example 3: Answer
26:32
Le Chatelier's principle & Equilibrium

40m 52s

Intro
0:00
Le Chatelier
1:05
Le Chatelier Principle
1:06
Concentration: Add 'x'
5:25
Concentration: Subtract 'x'
7:50
Example 1
9:44
Change in Pressure
12:53
Example 2
20:40
Temperature: Exothermic and Endothermic
24:33
Example 3
29:55
Example 4
35:30
VII. Acids & Bases
Acids and Bases

50m 11s

Intro
0:00
Acids and Bases
1:14
Bronsted-Lowry Acid-Base Model
1:28
Reaction of an Acid with Water
4:36
Acid Dissociation
10:51
Acid Strength
13:48
Example 1
21:22
Water as an Acid & a Base
25:25
Example 2: Part A
32:30
Example 2: Part B
34:47
Example 3: Part A
35:58
Example 3: Part B
39:33
pH Scale
41:12
Example 4
43:56
pH of Weak Acid Solutions

43m 52s

Intro
0:00
pH of Weak Acid Solutions
1:12
pH of Weak Acid Solutions
1:13
Example 1
6:26
Example 2
14:25
Example 3
24:23
Example 4
30:38
Percent Dissociation: Strong & Weak Bases

43m 4s

Intro
0:00
Bases
0:33
Percent Dissociation: Strong & Weak Bases
0:45
Example 1
6:23
Strong Base Dissociation
11:24
Example 2
13:02
Weak Acid and General Reaction
17:38
Example: NaOH → Na⁺ + OH⁻
20:30
Strong Base and Weak Base
23:49
Example 4
24:54
Example 5
33:51
Polyprotic Acids

35m 34s

Intro
0:00
Polyprotic Acids
1:04
Acids Dissociation
1:05
Example 1
4:51
Example 2
17:30
Example 3
31:11
Salts and Their Acid-Base Properties

41m 14s

Intro
0:00
Salts and Their Acid-Base Properties
0:11
Salts and Their Acid-Base Properties
0:15
Example 1
7:58
Example 2
14:00
Metal Ion and Acidic Solution
22:00
Example 3
28:35
NH₄F → NH₄⁺ + F⁻
34:05
Example 4
38:03
Common Ion Effect & Buffers

41m 58s

Intro
0:00
Common Ion Effect & Buffers
1:16
Covalent Oxides Produce Acidic Solutions in Water
1:36
Ionic Oxides Produce Basic Solutions in Water
4:15
Practice Example 1
6:10
Practice Example 2
9:00
Definition
12:27
Example 1: Part A
16:49
Example 1: Part B
19:54
Buffer Solution
25:10
Example of Some Buffers: HF and NaF
30:02
Example of Some Buffers: Acetic Acid & Potassium Acetate
31:34
Example of Some Buffers: CH₃NH₂ & CH₃NH₃Cl
33:54
Example 2: Buffer Solution
36:36
Buffer

32m 24s

Intro
0:00
Buffers
1:20
Buffer Solution
1:21
Adding Base
5:03
Adding Acid
7:14
Example 1: Question
9:48
Example 1: Recall
12:08
Example 1: Major Species Upon Addition of NaOH
16:10
Example 1: Equilibrium, ICE Chart, and Final Calculation
24:33
Example 1: Comparison
29:19
Buffers, Part II

40m 6s

Intro
0:00
Buffers
1:27
Example 1: Question
1:32
Example 1: ICE Chart
3:15
Example 1: Major Species Upon Addition of OH⁻, But Before Rxn
7:23
Example 1: Equilibrium, ICE Chart, and Final Calculation
12:51
Summary
17:21
Another Look at Buffering & the Henderson-Hasselbalch equation
19:00
Example 2
27:08
Example 3
32:01
Buffers, Part III

38m 43s

Intro
0:00
Buffers
0:25
Buffer Capacity Part 1
0:26
Example 1
4:10
Buffer Capacity Part 2
19:29
Example 2
25:12
Example 3
32:02
Titrations: Strong Acid and Strong Base

42m 42s

Intro
0:00
Titrations: Strong Acid and Strong Base
1:11
Definition of Titration
1:12
Sample Problem
3:33
Definition of Titration Curve or pH Curve
9:46
Scenario 1: Strong Acid- Strong Base Titration
11:00
Question
11:01
Part 1: No NaOH is Added
14:00
Part 2: 10.0 mL of NaOH is Added
15:50
Part 3: Another 10.0 mL of NaOH & 20.0 mL of NaOH are Added
22:19
Part 4: 50.0 mL of NaOH is Added
26:46
Part 5: 100.0 mL (Total) of NaOH is Added
27:26
Part 6: 150.0 mL (Total) of NaOH is Added
32:06
Part 7: 200.0 mL of NaOH is Added
35:07
Titrations Curve for Strong Acid and Strong Base
35:43
Titrations: Weak Acid and Strong Base

42m 3s

Intro
0:00
Titrations: Weak Acid and Strong Base
0:43
Question
0:44
Part 1: No NaOH is Added
1:54
Part 2: 10.0 mL of NaOH is Added
5:17
Part 3: 25.0 mL of NaOH is Added
14:01
Part 4: 40.0 mL of NaOH is Added
21:55
Part 5: 50.0 mL (Total) of NaOH is Added
22:25
Part 6: 60.0 mL (Total) of NaOH is Added
31:36
Part 7: 75.0 mL (Total) of NaOH is Added
35:44
Titration Curve
36:09
Titration Examples & Acid-Base Indicators

52m 3s

Intro
0:00
Examples and Indicators
0:25
Example 1: Question
0:26
Example 1: Solution
2:03
Example 2: Question
12:33
Example 2: Solution
14:52
Example 3: Question
23:45
Example 3: Solution
25:09
Acid/Base Indicator Overview
34:45
Acid/Base Indicator Example
37:40
Acid/Base Indicator General Result
47:11
Choosing Acid/Base Indicator
49:12
VIII. Solubility
Solubility Equilibria

36m 25s

Intro
0:00
Solubility Equilibria
0:48
Solubility Equilibria Overview
0:49
Solubility Product Constant
4:24
Definition of Solubility
9:10
Definition of Solubility Product
11:28
Example 1
14:09
Example 2
20:19
Example 3
27:30
Relative Solubilities
31:04
Solubility Equilibria, Part II

42m 6s

Intro
0:00
Solubility Equilibria
0:46
Common Ion Effect
0:47
Example 1
3:14
pH & Solubility
13:00
Example of pH & Solubility
15:25
Example 2
23:06
Precipitation & Definition of the Ion Product
26:48
If Q > Ksp
29:31
If Q < Ksp
30:27
Example 3
32:58
Solubility Equilibria, Part III

43m 9s

Intro
0:00
Solubility Equilibria
0:55
Example 1: Question
0:56
Example 1: Step 1 - Check to See if Anything Precipitates
2:52
Example 1: Step 2 - Stoichiometry
10:47
Example 1: Step 3 - Equilibrium
16:34
Example 2: Selective Precipitation (Question)
21:02
Example 2: Solution
23:41
Classical Qualitative Analysis
29:44
Groups: 1-5
38:44
IX. Complex Ions
Complex Ion Equilibria

43m 38s

Intro
0:00
Complex Ion Equilibria
0:32
Complex Ion
0:34
Ligan Examples
1:51
Ligand Definition
3:12
Coordination
6:28
Example 1
8:08
Example 2
19:13
Complex Ions & Solubility

31m 30s

Intro
0:00
Complex Ions and Solubility
0:23
Recall: Classical Qualitative Analysis
0:24
Example 1
6:10
Example 2
16:16
Dissolving a Water-Insoluble Ionic Compound: Method 1
23:38
Dissolving a Water-Insoluble Ionic Compound: Method 2
28:13
X. Chemical Thermodynamics
Spontaneity, Entropy, & Free Energy, Part I

56m 28s

Intro
0:00
Spontaneity, Entropy, Free Energy
2:25
Energy Overview
2:26
Equation: ∆E = q + w
4:30
State Function/ State Property
8:35
Equation: w = -P∆V
12:00
Enthalpy: H = E + PV
14:50
Enthalpy is a State Property
17:33
Exothermic and Endothermic Reactions
19:20
First Law of Thermodynamic
22:28
Entropy
25:48
Spontaneous Process
33:53
Second Law of Thermodynamic
36:51
More on Entropy
42:23
Example
43:55
Spontaneity, Entropy, & Free Energy, Part II

39m 55s

Intro
0:00
Spontaneity, Entropy, Free Energy
1:30
∆S of Universe = ∆S of System + ∆S of Surrounding
1:31
Convention
3:32
Examining a System
5:36
Thermodynamic Property: Sign of ∆S
16:52
Thermodynamic Property: Magnitude of ∆S
18:45
Deriving Equation: ∆S of Surrounding = -∆H / T
20:25
Example 1
25:51
Free Energy Equations
29:22
Spontaneity, Entropy, & Free Energy, Part III

30m 10s

Intro
0:00
Spontaneity, Entropy, Free Energy
0:11
Example 1
2:38
Key Concept of Example 1
14:06
Example 2
15:56
Units for ∆H, ∆G, and S
20:56
∆S of Surrounding & ∆S of System
22:00
Reaction Example
24:17
Example 3
26:52
Spontaneity, Entropy, & Free Energy, Part IV

30m 7s

Intro
0:00
Spontaneity, Entropy, Free Energy
0:29
Standard Free Energy of Formation
0:58
Example 1
4:34
Reaction Under Non-standard Conditions
13:23
Example 2
16:26
∆G = Negative
22:12
∆G = 0
24:38
Diagram Example of ∆G
26:43
Spontaneity, Entropy, & Free Energy, Part V

44m 56s

Intro
0:00
Spontaneity, Entropy, Free Energy
0:56
Equations: ∆G of Reaction, ∆G°, and K
0:57
Example 1: Question
6:50
Example 1: Part A
9:49
Example 1: Part B
15:28
Example 2
17:33
Example 3
23:31
lnK = (- ∆H° ÷ R) ( 1 ÷ T) + ( ∆S° ÷ R)
31:36
Maximum Work
35:57
XI. Electrochemistry
Oxidation-Reduction & Balancing

39m 23s

Intro
0:00
Oxidation-Reduction and Balancing
2:06
Definition of Electrochemistry
2:07
Oxidation and Reduction Review
3:05
Example 1: Assigning Oxidation State
10:15
Example 2: Is the Following a Redox Reaction?
18:06
Example 3: Step 1 - Write the Oxidation & Reduction Half Reactions
22:46
Example 3: Step 2 - Balance the Reaction
26:44
Example 3: Step 3 - Multiply
30:11
Example 3: Step 4 - Add
32:07
Example 3: Step 5 - Check
33:29
Galvanic Cells

43m 9s

Intro
0:00
Galvanic Cells
0:39
Example 1: Balance the Following Under Basic Conditions
0:40
Example 1: Steps to Balance Reaction Under Basic Conditions
3:25
Example 1: Solution
5:23
Example 2: Balance the Following Reaction
13:56
Galvanic Cells
18:15
Example 3: Galvanic Cells
28:19
Example 4: Galvanic Cells
35:12
Cell Potential

48m 41s

Intro
0:00
Cell Potential
2:08
Definition of Cell Potential
2:17
Symbol and Unit
5:50
Standard Reduction Potential
10:16
Example Figure 1
13:08
Example Figure 2
19:00
All Reduction Potentials are Written as Reduction
23:10
Cell Potential: Important Fact 1
26:49
Cell Potential: Important Fact 2
27:32
Cell Potential: Important Fact 3
28:54
Cell Potential: Important Fact 4
30:05
Example Problem 1
32:29
Example Problem 2
38:38
Potential, Work, & Free Energy

41m 23s

Intro
0:00
Potential, Work, Free Energy
0:42
Descriptions of Galvanic Cell
0:43
Line Notation
5:33
Example 1
6:26
Example 2
11:15
Example 3
15:18
Equation: Volt
22:20
Equations: Cell Potential, Work, and Charge
28:30
Maximum Cell Potential is Related to the Free Energy of the Cell Reaction
35:09
Example 4
37:42
Cell Potential & Concentration

34m 19s

Intro
0:00
Cell Potential & Concentration
0:29
Example 1: Question
0:30
Example 1: Nernst Equation
4:43
Example 1: Solution
7:01
Cell Potential & Concentration
11:27
Example 2
16:38
Manipulating the Nernst Equation
25:15
Example 3
28:43
Electrolysis

33m 21s

Intro
0:00
Electrolysis
3:16
Electrolysis: Part 1
3:17
Electrolysis: Part 2
5:25
Galvanic Cell Example
7:13
Nickel Cadmium Battery
12:18
Ampere
16:00
Example 1
20:47
Example 2
25:47
XII. Light
Light

44m 45s

Intro
0:00
Light
2:14
Introduction to Light
2:15
Frequency, Speed, and Wavelength of Waves
3:58
Units and Equations
7:37
Electromagnetic Spectrum
12:13
Example 1: Calculate the Frequency
17:41
E = hν
21:30
Example 2: Increment of Energy
25:12
Photon Energy of Light
28:56
Wave and Particle
31:46
Example 3: Wavelength of an Electron
34:46
XIII. Quantum Mechanics
Quantum Mechanics & Electron Orbitals

54m

Intro
0:00
Quantum Mechanics & Electron Orbitals
0:51
Quantum Mechanics & Electron Orbitals Overview
0:52
Electron Orbital and Energy Levels for the Hydrogen Atom
8:47
Example 1
13:41
Quantum Mechanics: Schrodinger Equation
19:19
Quantum Numbers Overview
31:10
Principal Quantum Numbers
33:28
Angular Momentum Numbers
34:55
Magnetic Quantum Numbers
36:35
Spin Quantum Numbers
37:46
Primary Level, Sublevels, and Sub-Sub-Levels
39:42
Example
42:17
Orbital & Quantum Numbers
49:32
Electron Configurations & Diagrams

34m 4s

Intro
0:00
Electron Configurations & Diagrams
1:08
Electronic Structure of Ground State Atom
1:09
Order of Electron Filling
3:50
Electron Configurations & Diagrams: H
8:41
Electron Configurations & Diagrams: He
9:12
Electron Configurations & Diagrams: Li
9:47
Electron Configurations & Diagrams: Be
11:17
Electron Configurations & Diagrams: B
12:05
Electron Configurations & Diagrams: C
13:03
Electron Configurations & Diagrams: N
14:55
Electron Configurations & Diagrams: O
15:24
Electron Configurations & Diagrams: F
16:25
Electron Configurations & Diagrams: Ne
17:00
Electron Configurations & Diagrams: S
18:08
Electron Configurations & Diagrams: Fe
20:08
Introduction to Valence Electrons
23:04
Valence Electrons of Oxygen
23:44
Valence Electrons of Iron
24:02
Valence Electrons of Arsenic
24:30
Valence Electrons: Exceptions
25:36
The Periodic Table
27:52
XIV. Intermolecular Forces
Vapor Pressure & Changes of State

52m 43s

Intro
0:00
Vapor Pressure and Changes of State
2:26
Intermolecular Forces Overview
2:27
Hydrogen Bonding
5:23
Heat of Vaporization
9:58
Vapor Pressure: Definition and Example
11:04
Vapor Pressures is Mostly a Function of Intermolecular Forces
17:41
Vapor Pressure Increases with Temperature
20:52
Vapor Pressure vs. Temperature: Graph and Equation
22:55
Clausius-Clapeyron Equation
31:55
Example 1
32:13
Heating Curve
35:40
Heat of Fusion
41:31
Example 2
43:45
Phase Diagrams & Solutions

31m 17s

Intro
0:00
Phase Diagrams and Solutions
0:22
Definition of a Phase Diagram
0:50
Phase Diagram Part 1: H₂O
1:54
Phase Diagram Part 2: CO₂
9:59
Solutions: Solute & Solvent
16:12
Ways of Discussing Solution Composition: Mass Percent or Weight Percent
18:46
Ways of Discussing Solution Composition: Molarity
20:07
Ways of Discussing Solution Composition: Mole Fraction
20:48
Ways of Discussing Solution Composition: Molality
21:41
Example 1: Question
22:06
Example 1: Mass Percent
24:32
Example 1: Molarity
25:53
Example 1: Mole Fraction
28:09
Example 1: Molality
29:36
Vapor Pressure of Solutions

37m 23s

Intro
0:00
Vapor Pressure of Solutions
2:07
Vapor Pressure & Raoult's Law
2:08
Example 1
5:21
When Ionic Compounds Dissolve
10:51
Example 2
12:38
Non-Ideal Solutions
17:42
Negative Deviation
24:23
Positive Deviation
29:19
Example 3
31:40
Colligatives Properties

34m 11s

Intro
0:00
Colligative Properties
1:07
Boiling Point Elevation
1:08
Example 1: Question
5:19
Example 1: Solution
6:52
Freezing Point Depression
12:01
Example 2: Question
14:46
Example 2: Solution
16:34
Osmotic Pressure
20:20
Example 3: Question
28:00
Example 3: Solution
30:16
XV. Bonding
Bonding & Lewis Structure

48m 39s

Intro
0:00
Bonding & Lewis Structure
2:23
Covalent Bond
2:24
Single Bond, Double Bond, and Triple Bond
4:11
Bond Length & Intermolecular Distance
5:51
Definition of Electronegativity
8:42
Bond Polarity
11:48
Bond Energy
20:04
Example 1
24:31
Definition of Lewis Structure
31:54
Steps in Forming a Lewis Structure
33:26
Lewis Structure Example: H₂
36:53
Lewis Structure Example: CH₄
37:33
Lewis Structure Example: NO⁺
38:43
Lewis Structure Example: PCl₅
41:12
Lewis Structure Example: ICl₄⁻
43:05
Lewis Structure Example: BeCl₂
45:07
Resonance & Formal Charge

36m 59s

Intro
0:00
Resonance and Formal Charge
0:09
Resonance Structures of NO₃⁻
0:25
Resonance Structures of NO₂⁻
12:28
Resonance Structures of HCO₂⁻
16:28
Formal Charge
19:40
Formal Charge Example: SO₄²⁻
21:32
Formal Charge Example: CO₂
31:33
Formal Charge Example: HCN
32:44
Formal Charge Example: CN⁻
33:34
Formal Charge Example: 0₃
34:43
Shapes of Molecules

41m 21s

Intro
0:00
Shapes of Molecules
0:35
VSEPR
0:36
Steps in Determining Shapes of Molecules
6:18
Linear
11:38
Trigonal Planar
11:55
Tetrahedral
12:45
Trigonal Bipyramidal
13:23
Octahedral
14:29
Table: Shapes of Molecules
15:40
Example: CO₂
21:11
Example: NO₃⁻
24:01
Example: H₂O
27:00
Example: NH₃
29:48
Example: PCl₃⁻
32:18
Example: IF₄⁺
34:38
Example: KrF₄
37:57
Hybrid Orbitals

40m 17s

Intro
0:00
Hybrid Orbitals
0:13
Introduction to Hybrid Orbitals
0:14
Electron Orbitals for CH₄
5:02
sp³ Hybridization
10:52
Example: sp³ Hybridization
12:06
sp² Hybridization
14:21
Example: sp² Hybridization
16:11
σ Bond
19:10
π Bond
20:07
sp Hybridization & Example
22:00
dsp³ Hybridization & Example
27:36
d²sp³ Hybridization & Example
30:36
Example: Predict the Hybridization and Describe the Molecular Geometry of CO
32:31
Example: Predict the Hybridization and Describe the Molecular Geometry of BF₄⁻
35:17
Example: Predict the Hybridization and Describe the Molecular Geometry of XeF₂
37:09
XVI. AP Practice Exam
AP Practice Exam: Multiple Choice, Part I

52m 34s

Intro
0:00
Multiple Choice
1:21
Multiple Choice 1
1:22
Multiple Choice 2
2:23
Multiple Choice 3
3:38
Multiple Choice 4
4:34
Multiple Choice 5
5:16
Multiple Choice 6
5:41
Multiple Choice 7
6:20
Multiple Choice 8
7:03
Multiple Choice 9
7:31
Multiple Choice 10
9:03
Multiple Choice 11
11:52
Multiple Choice 12
13:16
Multiple Choice 13
13:56
Multiple Choice 14
14:52
Multiple Choice 15
15:43
Multiple Choice 16
16:20
Multiple Choice 17
16:55
Multiple Choice 18
17:22
Multiple Choice 19
18:59
Multiple Choice 20
20:24
Multiple Choice 21
22:20
Multiple Choice 22
23:29
Multiple Choice 23
24:30
Multiple Choice 24
25:24
Multiple Choice 25
26:21
Multiple Choice 26
29:06
Multiple Choice 27
30:42
Multiple Choice 28
33:28
Multiple Choice 29
34:38
Multiple Choice 30
35:37
Multiple Choice 31
37:31
Multiple Choice 32
38:28
Multiple Choice 33
39:50
Multiple Choice 34
42:57
Multiple Choice 35
44:18
Multiple Choice 36
45:52
Multiple Choice 37
48:02
Multiple Choice 38
49:25
Multiple Choice 39
49:43
Multiple Choice 40
50:16
Multiple Choice 41
50:49
AP Practice Exam: Multiple Choice, Part II

32m 15s

Intro
0:00
Multiple Choice
0:12
Multiple Choice 42
0:13
Multiple Choice 43
0:33
Multiple Choice 44
1:16
Multiple Choice 45
2:36
Multiple Choice 46
5:22
Multiple Choice 47
6:35
Multiple Choice 48
8:02
Multiple Choice 49
10:05
Multiple Choice 50
10:26
Multiple Choice 51
11:07
Multiple Choice 52
12:01
Multiple Choice 53
12:55
Multiple Choice 54
16:12
Multiple Choice 55
18:11
Multiple Choice 56
19:45
Multiple Choice 57
20:15
Multiple Choice 58
23:28
Multiple Choice 59
24:27
Multiple Choice 60
26:45
Multiple Choice 61
29:15
AP Practice Exam: Multiple Choice, Part III

32m 50s

Intro
0:00
Multiple Choice
0:16
Multiple Choice 62
0:17
Multiple Choice 63
1:57
Multiple Choice 64
6:16
Multiple Choice 65
8:05
Multiple Choice 66
9:18
Multiple Choice 67
10:38
Multiple Choice 68
12:51
Multiple Choice 69
14:32
Multiple Choice 70
17:35
Multiple Choice 71
22:44
Multiple Choice 72
24:27
Multiple Choice 73
27:46
Multiple Choice 74
29:39
Multiple Choice 75
30:23
AP Practice Exam: Free response Part I

47m 22s

Intro
0:00
Free Response
0:15
Free Response 1: Part A
0:16
Free Response 1: Part B
4:15
Free Response 1: Part C
5:47
Free Response 1: Part D
9:20
Free Response 1: Part E. i
10:58
Free Response 1: Part E. ii
16:45
Free Response 1: Part E. iii
26:03
Free Response 2: Part A. i
31:01
Free Response 2: Part A. ii
33:38
Free Response 2: Part A. iii
35:20
Free Response 2: Part B. i
37:38
Free Response 2: Part B. ii
39:30
Free Response 2: Part B. iii
44:44
AP Practice Exam: Free Response Part II

43m 5s

Intro
0:00
Free Response
0:12
Free Response 3: Part A
0:13
Free Response 3: Part B
6:25
Free Response 3: Part C. i
11:33
Free Response 3: Part C. ii
12:02
Free Response 3: Part D
14:30
Free Response 4: Part A
21:03
Free Response 4: Part B
22:59
Free Response 4: Part C
24:33
Free Response 4: Part D
27:22
Free Response 4: Part E
28:43
Free Response 4: Part F
29:35
Free Response 4: Part G
30:15
Free Response 4: Part H
30:48
Free Response 5: Diagram
32:00
Free Response 5: Part A
34:14
Free Response 5: Part B
36:07
Free Response 5: Part C
37:45
Free Response 5: Part D
39:00
Free Response 5: Part E
40:26
AP Practice Exam: Free Response Part III

28m 36s

Intro
0:00
Free Response
0:43
Free Response 6: Part A. i
0:44
Free Response 6: Part A. ii
3:08
Free Response 6: Part A. iii
5:02
Free Response 6: Part B. i
7:11
Free Response 6: Part B. ii
9:40
Free Response 7: Part A
11:14
Free Response 7: Part B
13:45
Free Response 7: Part C
15:43
Free Response 7: Part D
16:54
Free Response 8: Part A. i
19:15
Free Response 8: Part A. ii
21:16
Free Response 8: Part B. i
23:51
Free Response 8: Part B. ii
25:07
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Lecture Comments (35)

1 answer

Last reply by: Professor Hovasapian
Mon Jul 9, 2018 3:02 AM

Post by Nick Jiang on July 7 at 07:06:00 PM

Hi Professor,
How do I know how many hydrogens will dissociate from an acid? For example, HCL will have one dissociated hydrogen ion. However, are there cases when not all the hydrogens in the acid dissociate? If so, how can we determine which acids do that?

3 answers

Last reply by: Professor Hovasapian
Sun Jun 24, 2018 11:20 PM

Post by Shamreethaa Seeniraj on June 21 at 05:55:57 PM

Hello,
For the limiting reaction part of Example 4, isn't the moles of Chorine 0.5 because 1 male of chlorine is 0.025 and PbCl2 has 2 moles of Cl?
Thanks

1 answer

Last reply by: Professor Hovasapian
Fri Nov 18, 2016 8:07 PM

Post by Temitope Olasusi on November 18, 2016

In order for compounds to react, does it require dissociation? Because since Lead II Hydroxide is insoluble, how is it able to react to form Lead II Chloride?

1 answer

Last reply by: Professor Hovasapian
Tue Aug 30, 2016 10:51 PM

Post by Yosef Charkatli on August 30, 2016

Greetings professor Raffi Hovaspain

I came back to this just to ask one slight question
Isn't dissociation the reason beyond desolving and our inability to see things/salts we drop in water? If so how can something dissolve but not dissociate?

Thank you very much for your hardwork and rewarding lectures

2 answers

Last reply by: Professor Hovasapian
Thu Aug 18, 2016 6:33 PM

Post by Yosef Charkatli on August 15, 2016

Hello mr Raffi Hovasapian

In one of your examples, you added NH3 to H2O and got NH4+ and OH-. In this case water was the acid and NH3 was the base so y didn’t we have water in the products since this is an acid base reaction

Thanks in advance

1 answer

Last reply by: Professor Hovasapian
Mon Jun 27, 2016 6:55 PM

Post by Jeffrey McNeary on June 26, 2016

In example 1, how did you know that H2CO3 would be dissolved but would not dissociate? Is that something you need to memorize/ information that can be found in a textbook, or is it result of some chemistry concept you need to learn?

3 answers

Last reply by: Professor Hovasapian
Mon Jun 27, 2016 6:52 PM

Post by Jeffrey McNeary on June 25, 2016

for example 1, I have a question about the HOH that was created. I don't understand where the H+ within HOH (HOH is made up of H+ and OH-) came from, because H2CO3 never dissociated and gave off an H+, according to 20:00. So I guess my question is, what is the source of the H+?

1 answer

Last reply by: Professor Hovasapian
Wed Nov 11, 2015 4:16 AM

Post by Jeffrey Tao on November 9, 2015

If the hydrogen ion is what causes the damage, why is an acid like HF far weaker than HCl if they both have the hydrogen ions?

1 answer

Last reply by: Professor Hovasapian
Sat Aug 8, 2015 10:41 PM

Post by Herjot Gill on May 22, 2015

For "Example 2" the net and total ionic equations are the same. Isn't the chlorine ion on the left supposed to have a coefficient 2 in front of it?

1 answer

Last reply by: Professor Hovasapian
Wed Jul 9, 2014 6:11 PM

Post by Jessica Lee on July 9, 2014

Is polyprotic acid multiple hydrogens to give up or only 2 hydrogen to give up?

1 answer

Last reply by: Professor Hovasapian
Sat Apr 12, 2014 4:37 PM

Post by Matthew Palmer on April 12, 2014

Molarity it is total liters of solution right so don't you have to include the volume the solute not just the solvent

1 answer

Last reply by: Professor Hovasapian
Sat Apr 12, 2014 4:35 PM

Post by Matthew Palmer on April 12, 2014

Is this info still valid for the New ap chem test?

1 answer

Last reply by: Professor Hovasapian
Mon Aug 13, 2012 10:09 PM

Post by Suresh Sundarraj on August 13, 2012

0.0414 * 2 is 0.0828, not 0.0818

1 answer

Last reply by: Professor Hovasapian
Fri Aug 10, 2012 8:17 PM

Post by Kevin Kaminski on August 9, 2012

In example 2, say you dropped Pb(OH)2 into the HCl. How would this reaction occur if Pb(OH)2 wouldn't disassociate initially, based on the solubility guidelines? Would PbCl2 form?

1 answer

Last reply by: S.V. Savitha
Mon Oct 1, 2012 11:39 PM

Post by chenyu liu on April 26, 2012

will the ap exam include solubility guidelines??
or do we need to remember some of it??

Related Articles:

Acid-Base Reactions

  • An acid is a compound that dissociates in water to give up one Hydrogen Ion at a time.
  • A Base is something that dissociates to release Hydroxide Ion, or reacts with water to form Hydroxide Ion.
  • An acid produces Hydrogen Ion – Base can accept Hydrogen Ion.
  • An Acid plus a Base produces a Salt and Water
  • The reaction of Hydrogen Ion and Hydroxide Ion ALWAYS produces water. This is called a Neutralization reaction.
  • Molarity is defined as Moles of Solute per Liter of Solution

Acid-Base Reactions

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Acid-Base Reactions 1:00
    • Introduction to Acid: Monoprotic Acid and Polyprotic Acid
    • Introduction to Base
    • Neutralization
    • Example 1
    • Example 2
    • Molarity
    • Example 3
    • Example 4
    • Example 4: Limiting Reactant
    • Example 4: Reaction Part

Transcription: Acid-Base Reactions

Welcome back to Educator.com; welcome back to AP Chemistry.0000

In our last lesson, we talked about precipitation reactions, which is when you mix soluble salts, one solution with another.0004

Some combinations of cation and anion might actually be insoluble, so they bind together and they drop to the bottom like a stone, as a solid.0012

Well, today, we're going to be talking about the second class of really, really important reactions in chemistry, acid-base reactions.0021

This particular topic, acid-base reactions, and the next one, oxidation-reduction, really constitute the heart and soul of the most important chemistry that you're going to be working on in your career.0030

So, if nothing else, do your best to understand acids and bases really well, and oxidation-reduction really well, and I promise it will pay handsome dividends as you go on in your career, whether it's in biology or chemistry or even in physics, believe it or not.0041

Let's go ahead and get started.0057

Let's define what we mean by an acid.0061

Now, I have to warn you: if some of what we discuss today is not altogether clear, don't worry about it; acid-base chemistry is something that we will revisit again in great detail when we discuss the mathematics of acid-base chemistry--when we quantify some of what we discuss more qualitatively today.0064

So, again, as we do more and more problems, this whole acid-base, oxidation-reduction theme will come up over and over and over again, and as we do the problems, we will be discussing theory.0083

That is what I tend to do: as I'm doing the problems, I will go over theory; so don't feel bad if you don't immediately understand what is happening.0094

Let's define an acid--very, very simple: an acid is a compound that ionizes to form a hydrogen ion.0101

Ionizes--you can also substitute the word dissociates.0125

You can think of an acid--you remember when we were naming acids; we did it a little differently than the ionic compounds--well, hydrogen is in the first column of the periodic table, on the left; right below it, you have the lithium, potassium, and things like that.0130

Well, even though hydrogen is not a metal, in many ways, it actually behaves like a metal.0143

So, if I have something like HCl, even though we named it as an acid, it's not inappropriate to call it hydrogen chloride, which is exactly what it is when we make it in the lab.0149

It only turns into an acid when we drop it in water.0158

When we drop it in water, that is when it dissociates, and it gives up its hydrogen ion; it's soluble, like anything else.0161

But, because it's so important, we have just given it a different name; but the chemistry is actually the same--you drop something like lithium chloride in water; lithium and chloride break apart; well, you drop something like hydrogen chloride in water--the hydrogen and the chloride break apart.0169

What makes it different is that, where lithium doesn't react with anything, and chloride doesn't react with anything, hydrogen--very, very reactive.0185

Probably the most important single thing in chemistry is that hydrogen ion.0193

So, that's it; it's just a compound that ionizes, that dissociates to form a hydrogen ion, as one of its free ions.0198

Another way of looking at it, if you want to, is a compound that actually has a hydrogen to give up.0206

More often than not, it will give it up when it's actually involved in some chemistry.0215

A compound that has H+ to give up--that's all; there is nothing mysterious about it.0219

And, when we talk about an acid, we're talking about the hydrogen ion.0229

That is what an acid is; that is the most important part of the acid.0232

Let's see what we're looking at.0235

If we had hydrogen chloride, and we drop it in some water, well, the hydrogen and the chloride come apart, like ionic compounds tend to.0237

You have H+ floating around, and you have Cl- floating around.0246

You're welcome to put (aq) if you want; it just means that they are floating around in solution.0250

This is dissociation; this is the acid part--this is what does the damage, if you were to put your hand in some acid--this H+, not the Cl-.0256

OK, this is called a monoprotic acid, and as you know, if you take hydrogen (it has one proton and one electron), well, you rip off that electron, and now you have a hydrogen ion; it's the same as a proton.0267

You might have energy levels there that electrons can occupy, but essentially, it's just a free proton--that's all it is.0280

That is why a hydrogen ion is also referred to as a proton; monoprotic means an acid that only has one proton to give up--one hydrogen ion to give up; monoprotic.0289

Let's do an example of a polyprotic acid.0299

The most popular: sulfuric acid, H2SO4.0301

When that one dissociates--it is also a strong electrolyte--it doesn't give up both hydrogens simultaneously; acids only give up one hydrogen at a time.0305

It breaks up into one hydrogen, and what is left over--HSO4-, the bisulfate ion.0314

Notice, this is actually--it has another H that it can give up.0322

It does so, to some extent, which is why, when we write this reaction, we use a double arrow.0329

It breaks up into H+ + SO42-.0338

This dissociates, but it actually doesn't dissociate completely; it depends on the circumstance--what is going on in the reaction.0343

This one is a single arrow because it gives up that hydrogen completely--it just doesn't want it.0351

It wants to be this way and this way; we just call this polyprotic, and again, just fancy words for a chemistry that you completely understand.0356

One hydrogen to give up; a second hydrogen to give up; phosphoric happens to have three hydrogens that it will give up.0365

Very important, phosphoric acid, by the way--which is how the acidity inside of your cells is actually regulated--by the phosphate buffer system.0374

So, those of you who are in biology: that will be a big part of the work that you do.0381

OK, I'm going to write another representation; generally, when we do these acid-base problems, this is really what we're concerned with--the dissociation of the acid and the stoichiometry involved.0385

There is an alternative way that has become fashionable in the last fifteen to twenty years, and well, let me just write it out.0399

We can also write this this way: HCl + H2O goes to H3O+ + Cl-.0407

Now, this thing right here is exactly the same as this thing right here.0417

H+ is the same as H3O+; they write it this way--it has become fashionable--because it's a little bit more consistent with the idea of acid-base.0421

So, we said above that an acid is something that has a hydrogen to give up; well, a base is something that actually takes that hydrogen.0432

So, acid-base reactions, like oxidation-reduction later on, come in pairs; you have something that acts as an acid, something that acts as a base--the acid is the thing that gives up the hydrogen ion; the base is the thing that takes the hydrogen ion.0438

Here, what has happened is: water (if I rewrite water as HOH, which I'll do in the examples that follow, because I think it's a little bit more clear)--well, this H is actually given over to this; HCl gives up the H; the H2O, or the HOH, takes the H; and now, it becomes H3O+, since now it's carrying that extra ion, a plus charge; and then you are left with Cl-.0451

This is just an alternate way to write it.0479

I'll just put that there; sometimes, depending on the problem and what it is that we want to emphasize, how we want to look at it, we might use different versions of it; but as long as you know that this H+ hydrogen ion and this H3+ are the same thing...it is called the hydronium ion.0484

Again, it's just a name; it's just the same species--it's really just the H+ that is reacting here.0501

OK, now let's talk about a base.0508

We'll give a couple of definitions for base, because there are a couple of different types of bases.0511

A base is just a compound that dissociates to produce a hydroxide ion, OH-.0517

And when we say "dissociates," it can be partial dissociation; it can be complete dissociation; there is always some little bit of dissociation.0533

Or, we could say it's a compound that takes or accepts a hydrogen ion.0541

So, let's go back up to this one right here: in this particular case, HCl was the acid; it gave the H+.0555

In this case, H2O acted as the base; it took, it accepted, the hydrogen ion to form this and this.0562

An example of a base that dissociates to form hydroxide directly is sodium hydroxide.0570

We dissolve it in water; what you end up with is sodium ion floating around and hydroxide ion floating around; this is a base.0578

Base chemistry, acid chemistry--even though they come in pairs, they actually behave differently--they do different things.0585

Another example would be calcium hydroxide: Ca(OH)2.0595

Drop some of that in water, and what you get is a calcium 2+ ion and these two hydroxides; they come apart completely; they don't come apart one at a time, like H+ does.0600

You're going to end up with 2 free hydroxide ions.0610

OK, now we'll give an example of a base that doesn't dissociate to release hydroxide ion; it actually does something else, but in the process produces hydroxide ions.0615

So, the net effect is hydroxide ion floating around in solution that wasn't there before.0628

Here, the base has hydroxide that it released into the solution; now, we'll do something...the most common base is ammonia.0635

So, NH3; this time, I'm going to write it like I did before--the H2O--instead of on top of the arrow, and I'll tell you why in a minute.0644

It's going to be NH4+ + OH-; so you notice, the OH- still showed up, but it showed up indirectly.0652

In this case, now, the NH3 is acting as the base; it's going to take a hydrogen from this H2O, which I will write as HOH.0661

It's going to take this hydrogen to become NH4+, and it's going to leave behind this OH-.0672

This is one of the reasons why they started writing acids the way we did a minute ago--acid + H2O.0679

It shows the acid-base behavior; in the last equation, the water was behaving as the base; it took the hydrogen from the acid, HCl.0685

Here, water is acting as the acid; it is giving up one of its hydrogens to the base, ammonia.0694

There is a consistency here; that is why they started doing that about 15 or 20 years ago.0700

OK, so now that we have just a nice, general idea of what acids and bases are, let's talk about acid-base reactions.0705

When we talk about acid-base reactions, we are talking about neutralization reactions.0715

Neutralization reaction: any time you put an acid together with a base, you always get a salt plus water, HOH, or H2O.0720

Salt: again, salt is just a fancy word for ionic compound.0733

So, if I had an acid, which is dangerous; if I had a base, which is also dangerous; if I mix them together in the appropriate amount, and there was neutralization, and the salt wasn't too unpalatable, I could actually drink that solution, and it wouldn't harm me, because most of it would be water with some dissolved salt.0737

Or maybe not necessarily dissolved salt--maybe the salt would have precipitated, and I could filter it out, and I could drink just plain old water.0755

It's kind of extraordinary, when you think about it.0763

Well, here is what is happening: in neutralization reactions, this is going to be the net ionic reaction.0765

An acid, as we said, was something that has H+ floating around.0774

A base is something that has OH- floating around.0778

When I put H and OH- together, they really, really, really want to form water--liquid water.0782

And that is exactly what they will do; any time there is H+ and OH- in the vicinity of each other, they will bind very quickly, very strongly, to form liquid water.0790

OK, that's it; this is your basic neutralization reaction; this is neutralization.0803

H is dangerous alone; OH- is dangerous alone; put them together; they form water--not dangerous.0808

Let's do some examples.0816

We have HCl, hydrochloric acid; we'll put an (aq) here to let you know that it's actually just floating around in solution.0818

Right now, we're writing the molecular formula; this whole molecular, total ionic, net ionic--it applies to acid-base reactions, as well.0826

Plus sodium hydroxide: again, (aq); well, let's switch partners: HOH (well, actually, let me do the Na and the Cl first).0834

NaCl +HOH (I hope it doesn't bother you that I write HOH; it just helps me to think about it like this, instead of writing H2O): well, this is the molecular equation, so let me write "molecular" here.0848

Let's see what is going on.0865

Well, HCl is fully dissociated; it's a strong electrolyte: HCl, minus...oh, I'm sorry; let's make sure it's balanced...it is; yes, not a problem.0867

Sodium hydroxide, a strong electrolyte, fully dissociates; so I have sodium and hydroxide floating around.0877

Remember, everything on the left hand of the arrow is everything before something happens; it's a description of the system before a reaction takes place.0884

Everything on the right hand side of the arrow is a description of the reaction after something has taken place; really, really important.0892

Nothing is going on over here; it's kind of nice--everything is just freely floating.0899

Well, like we said, any time H and OH are in the vicinity of each other, they bind to form water--liquid water.0903

Plus the NaCl...well, NaCl is...again, back to the Solubility Guidelines--you're always checking that--NaCl is fully soluble.0912

Therefore, it doesn't precipitate out; it just stays, sodium ion and chloride ion, floating around in solution.0921

This is our total ionic equation.0928

Now, we write our net ionic; we cancel the things on the right that are the same on the left; what we are left with is H+ + OH-.0930

Those two...HOH, liquid.0943

Molecular formula; total ionic formula; net ionic; and remember, the net ionic is the actual chemistry that takes place; the chemistry that took place here was the hydrogen ion from the acid, and the hydroxide ion from the base, came together to form liquid water in a neutralization reaction.0946

In other words, the two ions neutralized each other--a profoundly important reaction.0968

Let's do another example here.0978

We'll call this one Example 1, because it's our formal example.0982

All right, molecular, total ionic, and net ionic equations for the reaction of (let's see...) carbonic acid, H2CO3, and potassium hydroxide, KOH.0987

So, we want molecular, total ionic, and net ionic equations for the reaction of carbonic acid and potassium hydroxide.1029

Carbonic acid: the other important acid in biological systems--it is how the blood...basically, the fluid outside of your cells regulates the acid content of your blood.1035

Your normal blood pH hovers around 7.3 or 7.4, or somewhere in that range.1050

Well, it needs to stay in that range, and carbonic acid--the carbonate buffer system--is what controls it; that is why you exhale CO2, because if you didn't exhale CO2, your blood would start to get very acidic, and some very bad things would start to happen.1055

So, outside the cell--carbonate buffer system; inside the cell, phosphate buffer system.1070

Let's see; well, let's just write it out!1075

We have H2CO3, carbonic acid, plus potassium hydroxide, and we are doing a molecular here.1082

So, we'll switch partners: we have H and OH; we know that we have an acid and a base--we know that we're going to get salt and water, always; it always happens.1092

We have HOH (actually, you know what--I think I'll put my water second; so I'll do potassium carbonate); I'll do K2CO3 first--it's just more traditional; we tend to put...HOH.1104

Now, let's balance it: 2 potassium on the right; I put a 2 there; I have 2 hydroxide--let me put a 2 here; that is 2 hydroxide, and now I have 2 H's; 2 H's.1121

This is one of the reasons why I write it as HOH instead of H2O; when I'm dealing with polyatomic ions and balancing, I like to balance polyatomic ions completely; hydroxide on the left, hydroxide on the right.1131

Think of water as hydrogen hydroxide--how is that?1142

OK...well, let's see what we can do.1146

H2CO3; now, we have to check solubility; H2CO3, carbonic acid, is one of those acids that is actually a weak electrolyte; it does not dissociate completely--in fact, it's not very soluble at all.1151

It's soluble in the sense that, if you dropped carbonic acid in water, you wouldn't be able to tell the difference; you would get a homogeneous mixture, so it dissolves, but it doesn't dissociate--meaning the H2CO3...the H doesn't really leave.1164

A little bit of it does, but most of it does not.1179

So, we actually don't write it as free ionic species; we leave it as H2CO3.1182

Does that make sense?--I hope that makes sense; so just because something dissolves, like sugar (let's just say glucose, C6H12O6), you can drop glucose in water, and it will dissolve--you won't be able to see the difference between the glucose and the water--but the carbons, the hydrogens, and the oxygens that make up sugar don't come apart.1191

That is different; that is dissociation--it dissolves, so carbonic acid, H2CO3, dissolves in water, but it doesn't dissociate in water the way that, say, hydrogen chloride does.1212

OK, so I leave it like this, and I put a little (aq) here to let me know that it's dissolved.1223

Well, potassium hydroxide--absolutely, it is a strong electrolyte, so it comes apart completely into free hydroxide and free potassium.1228

And now, potassium carbonate: let's see, what is potassium carbonate?1237

Potassium carbonate, actually, is an alkali metal with a carbonate, so it is soluble; therefore, I do get 2K+ + CO32-.1242

Water, of course, is, well...water is water.1253

So, let's cancel this; so the second one is your total ionic; now, let's cancel on the left and right--the only thing that cancels is the potassium.1257

Now, I have to write what is left over.1269

H2CO3, plus 2 hydroxide ions, goes to CO32- + 2 waters.1272

That is my total ionic; this is my chemistry, right here.1284

The total ionic represents the chemistry.1287

One molecule of carbonic acid reacts with two molecules, if you will, of hydroxide ion, to produce one carbonate ion and two molecules of water.1290

That is kind of extraordinary, when you think about it; it happens just like this.1302

And, with a 2- charge on the right and a 2- charge on the left, charge balances; mass balances; everything is good.1306

OK, let's do another one; let's do Example 2.1315

This time, I'll just go ahead and write down what it is that we're mixing; we are going to mix lead (2) hydroxide plus (oops, I'll balance it in a minute) hydrochloric acid, and I want to know what happens.1321

Well, OK; I know that I have lead hydroxide, which is a base; and I have HCl, which is an acid; I switch partners--I know I'm going to get a salt plus water.1340

Well, the water comes from the HOH; the only salt left over to make is the PbCl.1352

So, I write PbCl2, because this is lead (2), and I write HOH, and now I have to balance it.1357

2 hydroxides; 2 hydroxides gives me 2 H's; I put 2 H's; 2Cl, 2Cl; I'm balanced.1365

Now, I check for solubility; that is my next step--that's how I come up with my total ionic equation.1372

Lead hydroxide is not soluble; it stays as a solid.1377

Lead hydroxide, lead (2) hydroxide, is a solid; it does not come apart.1384

Very, very little of it dissociates, which is why the reaction actually proceeds (we'll talk about that later, when we talk about Le Chatelier Principle, solubility equilibria, things like that).1389

But, for right now, it is a solid; it does not break up into free ions; but HCl does: 2H+ + Cl-1399

PbCl2...now notice, this is a product; this is something that is formed.1410

Well, lead chloride is also insoluble; therefore, I'm going to put a little down arrow, showing that it falls out of solution as a solid, a precipitate.1414

That stays the same (oops, I have all those stray lines showing up again): PbCl2, down arrow, is a solid, and then of course water is just water: 2HOH.1422

Notice, there is nothing on the left and nothing on the right that is the same; therefore, this total ionic is the same; or I should say, the net ionic is the same as the total ionic.1438

This is the chemistry, right here; in this particular case, we have a mixture of what we talked about before and now--there is an acid-base reaction going on, in the sense that hydrogen ion and hydroxide ion form water.1451

But, there is also a precipitation reaction going on; there is lead ion and chloride ion, come together to form the solid, lead chloride.1464

So, that is also a possibility; and again, you just kind of deal with it systematically--deal with each thing that comes up.1475

It's not a problem if you have an acid-base reaction together with a precipitation reaction; there is no law that says they have to be separate things.1480

They can happen together.1487

Now, I want to introduce a concept called molarity, and it is used to discuss aqueous solutions.1494

After I introduce it really briefly, I'm going to actually do a stoichiometry problem, because we are talking about stoichiometry, and it's going to be a mixture: it's going to be an acid-base neutralization, and it's going to basically just take us through a pretty standard stoichiometry problem, so you get an idea of what it is that we're looking for--how to handle the equations.1505

That is the really important part of the stoichiometry here: Which equations do I use?1524

If you understand the chemistry, I promise, the math is easy; very, very easy; so let's get started.1528

Molarity: it is defined as the moles of solute (the thing that you're dissolving) over the liters of solution (the thing you're dissolving in).1536

And, since most of the time we'll be talking about water, normally our solute will be an acid or a salt dissolved in some kind of water.1554

Now, the symbol for molarity--I'm going to use two symbols: the common symbol, that has been popular for about the last 15 or 20 years, is the capital M, Molarity.1561

I learned it as an m with a line over it; so I'm going to...I'll use both, but in your book, you'll see, of course, the capital M; but just know that an m with a line over it is also another symbol for molarity.1576

You'll see it in the older literature.1586

OK, so moles of solute, liters of solution: the unit is moles per liter--that's it.1589

So, molarity is moles per liter--very, very important--that is a new unit; you have already had grams per mole; you had particles per mole (Avogadro's number); now, you have moles per liter.1595

So, three units that involve mole; clearly, the mole is very important.1606

Let's just do an example here.1611

We'll call it Example 3: I have 14.6 grams of potassium chloride, and it is dissolved in 400 milliliters of water.1618

What is the molarity of this solution?1638

Molarity--another word for concentration: what is the concentration of this solution in moles per liter--what is the molarity?1642

Well, what is our definition of molarity?1649

Molarity is equal to the moles of solute (which, in this case, is KCl) divided by the liters of solution (which, in this case, is water).1654

So, all I need to do is find a denominator, find a numerator, do my division, and I'm done!1664

Well, I know that the volume is the easiest one--it's 400 milliliters--but since the unit is in liters, I'll just convert that to liters, which is 0.400 liters.1671

Now, I need to find how many moles of potassium chloride.1680

I wasn't given moles--I was given grams--but of course, I can convert by using the molar mass.1686

Let's do that: 14.6 grams of KCl times (1 mole of it happens to weigh) 74.55 grams, and when you do that division, you end up with 0.1958 mol of KCl.1691

This is the number that goes up there: 0.1958 mol of KCl, dissolved in .4 liters.1711

I do the division, and I end up with (what is my number?) 0.49; 0.49 moles per liter, or I can put 0.49 Molar (we often say Molar solution).1721

That's it; molarity is just a way of talking about how many moles of something there are floating around in liquid, in a solution (more often than not, water).1741

Because when I drop something in water, more often than not, it will dissolve, I want to know how many moles are actually floating around.1752

If I keep the volume the same, but I dump in five times as many moles, now I'm five times as concentrated--which is why they also refer to molarity as concentration.1759

How concentrated is this particular solution?1768

This .49 tells me that, in 1 liter of solution, I have .49 moles of potassium chloride floating around.1772

"Potassium chloride floating around"--potassium chloride is made of one atom of potassium, one atom of chloride, so I have one mole of potassium floating around and one mole of chloride floating around.1781

So, stoichiometry is really, really important.1795

Again, this dissolves.1798

So, let's jump into a problem here.1803

This will be Example #4.1806

How many grams of PbCl2 will precipitate when 10 grams of lead (2) hydroxide is dropped into 50 milliliters of a 0.50 Molar HCl solution?1815

Wow, it seems like there is a lot going on here; don't worry about it--we'll deal with it systematically.1864

I have a 50-milliliter beaker; actually, I have 100--let's say a 100-milliliter beaker, about half full--50 milliliters; and it is a hydrochloric acid solution, .5 Molar hydrochloric acid solution.1869

That means, for every liter, there is .5 moles of hydrochloric acid floating around.1883

That's reasonably strong--it will certainly do some damage if you allow it to; not terribly strong, but certainly there is enough acid floating around.1888

So, what we do is: we take 10 grams of lead hydroxide; we drop it into this acid solution; and we know, from the example that we just did when we did lead hydroxide plus the hydrochloric acid, that we're going to get lead chloride plus water.1897

Lead chloride is insoluble, so some of it is just going to drop to the bottom like a stone.1909

We want to know how much lead chloride is actually going to fall out, based on this.1914

So, we have an acid-base reaction; we have a precipitation reaction; this is a stoichiometry problem that involves limiting reactant.1918

All of these things come together now: limiting reactant, acid-base, precipitation.1928

Fortunately, in this case, we're not worried about the water; we're not worried about the acid-base portion; we're worried about the precipitation, so we can narrow our focus.1932

Let's write our equation again, so we know what we're dealing with.1941

That is the most important--always start your chemistry with an equation; that is what chemistry is--it's about things that come together and change.1945

If you don't have an equation, you might be able to do the math, but it's not really going to make much sense; you need an equation.1951

Start with the equation.1956

Pb(OH)2 + 2HCl goes to PbCl2 as a precipitate +2HOH.1959

Now, I have my equation that I'm working with; let's get started.1974

Since I'm talking about (let me do this in red) lead chloride, and that is what I'm looking for here--lead chloride--let me take a look at that reaction individually.1979

Lead chloride comes from the following (and again, this is what you're going to be doing in the stoichiometry--write out all of the equations that you need; this is what it's all about--the equations will guide your mathematics).1990

We have lead ion; it comes together with 2 chloride ions to form PbCl2 as a precipitate; that is my equation for the formation of lead chloride.2001

Well, this says that one mole of lead produces one mole of lead chloride.2014

Two moles of chloride ion produces one mole of lead chloride.2021

Again, it's basic stoichiometry.2024

The first thing we want to do is: we want to find out how many moles of lead ion there are.2028

Then, we're going to find out how many moles of chloride ion there are, because it's a solution of HCl; and then it's going to be a limiting reactant problem.2032

Whichever is the limiting reactant--that is going to control how much PbCl2 precipitates.2041

So, we have extracted the important information; this equation right here--this is the equation we're dealing with, because we want to know the PbCl2.2046

Moles of Pb(OH)2; well, we have 10 grams of the Pb(OH)2, and one mole of it is 241.2 grams; therefore, we have 0.0414 mol of Pb(OH)2.2055

Again, in stoichiometry, you're going to always be working in moles; so immediately, if you do nothing else, just convert it to moles.2086

Well, each molecule of lead hydroxide is made up of one atom of lead; therefore, one mole of lead hydroxide produces 1 mole of lead of ion; so .0414 mol of lead hydroxide produces (I'll do a little double arrow)--it implies 0.0414 mol of lead ion, which is what we were interested in; this is our equation.2093

Do you see what I did?--I hope you do.2127

I started with a whole molecule, but each one of these molecules--one molecule releases one molecule of lead, so .0414 mol of the molecule releases .0414 mol of lead ion.2129

That is what is going to react with the chloride to give me the PbCl.2143

Let me put a little bracket around that; I'm going to use that in a minute.2148

Now, let's see...well, let's just go ahead and do the moles of...now, I need to know the number of moles of chloride ion I'm dealing with.2154

Well, the moles of HCl--I have liters, and I have moles per liter.2167

That is why molarity is used, because we often deal with solutions; so we need to know the number of moles to be able to extract it from solutions.2172

For a solid, you use molar mass; but for solutions, you have to use molarity.2182

So, here we go: I have 0.050 liters of solution, and the molarity is 0.5 moles per liter.2187

The units cancel, and I end up with 0.025 mol of HCl floating around.2201

Well, HCl is not floating around; it's dissociated; but every molecule of HCl produces one molecule of H+ ion and one molecule of Cl-.2208

Therefore, I have 0.025 mol of Cl- floating around; that is my other thing.2217

I hope that made sense; again (oops, these lines just show up out of nowhere, don't they)...2228

Now that I have .0414 mol of Pb, and .025 mol of Cl, now I can find out which one is the limiting reactant.2239

So, let me draw a little bit of a line here; let me go back to blue ink; and I'm going to do the limiting reactant part.2247

I hope I have enough room here; yes, I think I do; actually, you know what--that is fine; let me just move forward.2260

So, let me write that again; this is going to be the limiting reactant part of the calculation.2269

Now, I can choose either one; I can either choose the .025 moles of chloride to start with, or I can choose the .0414 moles of lead ion to start with--it doesn't matter which one.2278

I'm just deciding which one is going to run out first.2289

I'm going to choose the lead.2292

.0414 moles of lead ion (let me rewrite the equation, by the way, so we have a reference here: Pb2+ + 2Cl- goes to PbCl2 as a precipitate.2295

PbCl2...there we go.2316

.0414 moles of Pb, moles of lead; moles of chloride; the mole ratio of lead and chloride is 2:1; that is 2:1; that is what I'm doing here.2320

This tells me that, if I have .0414 moles of lead, .0818 moles of chloride are required to react with it.2336

That is what this equation tells me: for every mole of lead, I need 2 moles of chloride to produce a molecule of lead chloride.2350

Well, if I have .0414 moles, and the mole ratio is 2, I multiply by 2; I get .0818--that is moles of Cl- required.2357

Do I have .0818 moles of Cl-? No.2365

I only have 0.025 moles of Cl-; that is what I just calculated; so therefore, Cl- is limiting.2373

So, the Cl- is going to control how much lead chloride I have; I'm going to end up with excess lead ion floating around.2386

This is my limiting reactant; now that I have my limiting reactant, I can go ahead and perform my actual reaction.2394

This is the reaction part.2402

Well, I have 0.025 moles of Cl- (it's my limiting reactant, so I start with that--that is what is going to control it).2409

Now, the relationship--the mole relationship--between Cl- and PbCl2 is 2:1.2420

I have mol of Cl- on the bottom, because it's on top here; mol of PbCl2, so it is going to be 2:1; that cancels, and I get 0.0125 mol of PbCl2 produced.2427

Now, I take 0.0125 mol of PbCl2, and I multiply by its molar mass, which happens to be 278.1, and I end up with 3.48 grams of PbCl2 that have precipitated.2451

That is my final answer.2473

Let's see what I did: I had 10 grams of lead hydroxide that I dropped into (how many milliliters was it?--I forgot the actual volume amount; let me double-check here; how much was my volume? Yes, it was 50 milliliters) 50 milliliters of a .5 Molar hydrochloric acid solution.2476

I asked for lead chloride; lead chloride precipitates; therefore, I dealt with that equation: one lead ion plus two chloride ions gives me one molecule of lead chloride.2501

I first found the number of moles of lead ion, and then I found the number of moles of chloride ion.2511

Then, it became a limiting reactant problem; I found out that chloride was my limiting reactant--it's the one that is going to run out first--therefore, it is going to control the reaction.2517

I used chloride and the mole ratio of chloride to lead chloride to find out that I'm going to end up producing .0125 moles of lead chloride, which I then convert to grams, and I end up with 3.48 grams of PbCl2.2526

So, as you see, everything is starting to come together.2543

Stoichiometry, acid-base, precipitation, all of these things are going to play into the problems that you solve on the AP exam.2546

Yes, both in the multiple-choice section, which are going to be no calculator--but you will have to still do the math; the math mostly simple numbers; but particularly in the free response section.2557

It isn't going to be just "Give me this, give me this, give me this"; it's going to be a whole slew of things happening.2567

As long as you understand the chemistry, these other things are just techniques; that is what is going on here.2572

This is a very, very characteristic problem that you will see on the AP exam.2579

You have an acid-base, a precipitation reaction, and you have some stoichiometric calculations.2583

This is the heart and soul of chemistry.2588

Everything happens simultaneously.2590

OK, thank you for joining us here at Educator.com for our discussion of acid-base and solution stoichiometry.2592

Next time, we'll talk about oxidation-reduction; take good care--goodbye.2598

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