Acids and Bases: Strong and Weak, pH, Chemistry

Acids and Bases: Strong and Weak, pH

XVIII. Acids and Bases: Lecture 1 | 60:41 min

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Acids and Bases: Strong and Weak, pH

Arrhenius acids give H⁺ ; Arrhenius bases give OH^-
Bronsted-Lowry acids are H⁺ donors; B-L bases are H⁺ acceptors
Lewis bases are electron pair donors, like NH₃ ; Lewis acids are electron pair acceptors like BF₃
Common strong acids: HCl, HNO₃ (monoprotic); H₂SO₄ (diprotic)
Common strong bases: NaOH, KOH, Ca(OH)₂
Weak acid: acetic, CH₃COOH
Weak base: NH₃
Water is both weak acid and weak base; K_w = 1.0 x 10^-14
Equilibria of weak acids and bases: K_a and K_b
pH = -log₁₀[H⁺] ; pH = 7.0, neutral; pH < 7, acidic; pH >7, basic

Acids and Bases: Strong and Weak, pH

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I. Introduction
	Introduction to Chemistry	47:38
II. Atoms
	Atomic Theory and Measurement	62:38
	The Chemist's Atom	22:20
III. Significant Figures
	Significant Figures and the Mole	51:06
IV. Equations and Formulas
	Balancing Equations, Limiting Reagents, Percentage Yield	58:17
	Empirical and Molecular Formulas	61:11
V. Chemical Reactions
	Classifying Chemical Reactions	42:43
	Energy in Chemical Reactions	63:47
VI. Electromagnetic Radiation
	Electromagnetic Radiation Quantum Theory	63:35
VII. Periodic Table and Bonding
	Periodic Table, Electronic Configurations, Ionic Bond	73:12
	Covalent Bond, Lewis Structures, Molecular Orbitals	77:27
	Shapes of Molecules and Hybridization	71:19
VIII. States of Matter
	States of Matter, Intermolecular Forces, Gases and Gas laws	61:12
IX. Gases
	Partial Pressure, Real Gases, Atmospheric Pollution	61:12
X. Phases
	Vapor Pressure, Boiling Point, Phase Diagrams	56:58
XI. Solids
	Types of Solids, X-Ray Diffraction, Unit Cells	57:30
XII. Carbon
	Carbon Allotropes, Band Theory of Solids	52:34
XIII. Solutions
	Solutions, Henry's Law, Concentration Equations	65:40
XIV. Colligative Properties
	Colligative Properties, Colloids, Surfactants	70:42
XV. Kinetics
	Kinetics, Rate Laws, Reaction Mechanism	68:48
XVI. Temperature Effects
	Temperature Effects, Reaction Rate Theory, Catalysis	62:56
XVII. Equilibrium
	Physical and Chemical Equilibrium, Equilibrium Law, Le Chatelier's Principle	70:47
XVIII. Acids and Bases
	Acids and Bases: Strong and Weak, pH	60:41
	pH Calculations, Polyprotic Acids	60:09
	Titrations, Indicators, Buffers	66:19
XIX. Solubility
	Solubility Product Constant, Precipitation	59:36
XX. Enthalpy and Entropy
	Enthalpy, Entropy, Second Law of Thermodynamics	53:51
XXI. Gibbs' Function
	Gibbs' Function, Equilibrium	61:10
XXII. Redox Reactions
	Balancing Redox Reactions, Half Reactions	67:26
XXIII. Electrochemistry
	Electrochemical Cells, Half-Cell Potentials	67:52
	Practical Batteries, Electrolysis	62:06
XXIV. Radioactivity
	Radioactivity, Nuclear Equations, Mass Energy Equivalence	40:35
	Radioactive Decay, Half-Life, Nuclear Reactions	56:12
XXV. Miscellaneous
	Organic Structures, Isomers, Functional Groups	68:32
	Chemistry and the Environment	50:13

Advanced Placement Chemistry

I. Introduction
	Introduction to Chemistry			47:38
		Intro		0:00
		What is Chemistry?		0:07
			Experimental Science	0:48
			Changes in Matter	1:18
			Energy and its Redistribution	2:20
			Central Science	2:45
		Properties of Matter		7:10
			Physical	7:45
			Example: Physical Properties	7:58
			Chemical	9:02
			Example: Chemical Properties	9:18
		Physical Changes (Reversible)		11:19
			Melting	11:39
			Boiling (Evaporation and Condensation)	13:21
			Dissolving (Solution)	15:41
		Chemical Changes		18:04
			Example: Balanced Chemical Equation	18:37
		Compositions of Matter		23:15
			Heterogeneous Mixture	23:27
			Example: Milk	23:40
			Example: Dirt	25:07
			Homogenous Mixture	25:40
			Example: Air, Gas, Vinegar	26:20
			Solutions vs Pure Substances	27:06
			Compounds and Elements	29:13
		Additional Example 1		8:52
		Additional Example 2		7:32
II. Atoms
	Atomic Theory and Measurement			62:38
		Intro		0:00
		Dalton's Atomic Theory		0:05
			Law of Multiple Proportions	3:10
		Current Atomic Theory		5:59
			Components: Electrons, Protons, Neutrons	6:51
			Isotopes	8:04
			Complex Molecules	9:35
		Fundamental Definition of an Element		11:27
			Nuclear Charge (Z)	11:35
			Atomic Number	12:37
			Isotopes	13:37
		Atomic Masses		15:53
			Hydrogen, Carbon, Chlorine	16:33
		Measurement		22:35
			SI Units	23:50
		Basic Units		26:39
			Meter, Kilogram, Second, Kelvin, Liter	26:52
		Multiplier Prefixes		33:05
		Measure Quantity		40:50
			Number x Unit	41:05
			Example: Height, Volume	41:16
		Additional Example 1		8:23
		Additional Example 2		4:03
	The Chemist's Atom			22:20
		Intro		0:00
		JJ Thompson and the Electron		1:11
			Cathode Ray Tube	1:19
			Electron Prediction	3:31
			Millikan, Charge of Electron	3:57
			Proton	4:45
		Rutherford and the Nucleus		5:42
			Alpha Particles	6:06
			Nucleus	8:05
		Chadwick and the Neutron		12:35
			Neutron	13:27
		Constitutions of Atoms		17:05
			Example: Hydrogen Isotopes	17:09
			Example: Iodine 127	20:08
III. Significant Figures
	Significant Figures and the Mole			51:06
		Intro		0:00
		Significant Figures: Sphere		0:14
		Example: Cube		7:11
			Example: Weight	10:40
		The Mole		13:36
			Examples: Number of Entities	14:00
			Avogadro's Number	15:10
			Carbon 12	16:16
			Mass of 1 Mol	17:49
			Molar Mass of Oxygen	20:01
		Stoichiometry		25:15
			Example: Molar Masses	26:25
		Molar Mass		26:39
			Example: Cholesterol	27:08
			Example: Insulin	38:38
		Additional Example 1		4:46
		Additional Example 2		5:16
IV. Equations and Formulas
	Balancing Equations, Limiting Reagents, Percentage Yield			58:17
		Intro		0:00
		Balancing Chemical Equations		0:49
			Atoms and Charges	1:50
			Example: Mercury and Oxygen	2:45
			Example: Combustion of a Hydrocarbon	6:19
		Redox: Oxidation and Reduction		12:30
			Example: Sodium and Chlorine	23:55
			Electron Transfer	19:34
		Limiting Reagent		22:25
			Example: Nuts and Bolts	22:45
			Example: Mercury and Oxygen	27:24
		Reaction Formulas		32:03
			Example: Iron Oxide and Carbon	32:11
			Example: Benzene and Chlorine	38:28
		Theoretical Yields, Actual Yields		42:13
			Percentage Yield	42:53
			Example	43:08
			Theoretical Yield from Limiting Reagent	45:11
			Example: Benzene and Chlorine	45:35
		Additional Example 1		3:12
		Additional Example 2		6:02
	Empirical and Molecular Formulas			61:11
		Intro		0:00
			Empirical Formula	0:45
			Molecular Formula	1:22
		Percentage by Mass		1:40
			Elements in Compounds	1:48
			Example: Water	2:44
			Example: Copper Sulfate	7:29
		Empirical Formula		13:02
			Example: Hydrocarbons	13:37
		Calculating Empirical Formula		20:24
			Example: C, H, O	20:32
		Molar Mass and Molecular Formulas		27:54
		Determining Molar Mass		32:21
			Mass Spectrometry	32:38
			Gas Laws	36:28
			Colligative Properties	39:18
		Empirical and Molecular Formulas		39:30
			Example: Ethylene and Chlorine	39:32
		Additional Example 1		5:23
		Additional Example 2		6:45
V. Chemical Reactions
	Classifying Chemical Reactions			42:43
		Intro		0:00
		Combustion Reactions		0:39
			Example: Balancing	2:33
		Exchange Reactions		7:58
			Example: Silver Nitrate + Sodium Chloride	9:11
			Precipitate	10:56
			Example: Sulfuric Acid + Sodium Chloride	13:20
			Naming Ions With Oxygen	16:10
			Example: Benzene and Chlorine	17:26
		Acid Base Reactions		18:50
			Recognizing Acids	19:18
			Recognizing Bases	23:48
			Litmus Test	26:02
			Common Acids	26:31
			Common Bases	28:40
		Redox Reactions		34:13
			Example: Potassium + Fluorine	35:54
			Example: Sodium + Oxygen	39:11
	Energy in Chemical Reactions			63:47
		Intro		0:00
		Forms of Energy		1:30
			Potential Energy and Kinetic Energy	1:32
			Example: Potential	2:53
			Example: Kinetic	4:07
		Units of Energy		5:20
			Example: Kinetic Energy, Joules	6:40
			Calorie	8:02
		Conservation of Energy		11:41
			First Law of Thermodynamics	12:22
		Heat Capacity and Measurement		17:10
			Heat Capacity	17:38
			Calorimeter	19:04
			Examples: Elements and Compounds	20:37
		Enthalpy		25:40
		Enthalpy Changes in Physical/Chemical Processes		31:25
			Exothermic	32:09
			Endothermic	34:16
			Example: Water	36:09
			Reversing a Process	38:21
			Example: Hydrogen + Oxygen	39:06
		Hess's Law		42:38
			Example: Hydrogen + Oxygen	43:46
		Enthalpy of Formation		47:05
			Example: Hydrogen + Oxygen	49:53
		Enthalpy of Formation: Carbon Disulfide		51:13
		Additional Example 1		5:42
VI. Electromagnetic Radiation
	Electromagnetic Radiation Quantum Theory			63:35
		Intro		0:00
		Waves and Their Characteristics		0:32
			Amplitude, Trough, Crest	1:01
			Wavelength	1:40
			Frequency	2:11
			Velocity (Speed of Light)	2:58
		Electromagnetic Radiation		5:10
			Gamma Rays and X-Rays	5:43
			Visible Light	6:19
			Infrared	6:54
			Radio Waves	7:16
		Spectra and Spectroscopy		7:58
		Hydrogen Atom Spectrum		10:13
			Emission Spectrum vs Absorption Spectrum	14:13
			Rydberg Formula	14:51
		Planck's Quantum Theory		16:55
			Black Body Radiation and Quanta	17:30
		Photoelectric Effect		23:29
		Bohr's Theory of the Hydrogen Atom		28:20
			Ground State	29:17
			Excited State	29:26
		Heisenberg and the Uncertainty Principle		34:48
		De Broglie and the Wave Nature of Particles		40:07
		Principle Quantum Number		44:05
		First Quantum Number		45:46
		m1 Quantum Number		51:00
		Spin Quantum Number		54:28
		Pauli Principle		54:58
		Additional Example 1		5:30
VII. Periodic Table and Bonding
	Periodic Table, Electronic Configurations, Ionic Bond			73:12
		Intro		0:00
		Periodic Law of Mendeleev and Meyer		0:43
		Modern Periodic Table		5:09
			Atomic Number	5:51
			Noble Gases	6:46
			Halogens	7:06
			Group Number	7:16
			Metals	8:07
			Groups and Periods	8:30
			Transition Metals	9:18
			Lanthanides	10:23
			Actinides	11:26
		Quantum Numbers and the Shape of the Table		12:06
		Electron Configuration of Atoms		17:59
		Electron Configuration of Neutral Atoms		19:49
			Example: Elements	20:23
			Example: Noble Gases	25:26
		Electron Configuration of Monatomic Ions		28:40
			Example: Elements	29:42
		Atomic Size		37:59
			Larger as Down a Group	38:44
			Smaller as Across a Period	39:34
		Sizes of Monatomic Ions		42:05
			Example: Elements	43:15
		Noble Gas Electron Configurations		45:52
			Example: Elements	46:10
		Electron Affinity		50:20
		Ionization Energy		52:32
			Example: First Ionization Energy	52:43
			Periodic Table Trend	53:37
			Example: Boron	54:22
		Ionic Compounds (NaCl)		57:00
			Ionic Bond (Electrostatic)	57:57
		Additional Example 1		9:08
		Additional Example 2		5:59
	Covalent Bond, Lewis Structures, Molecular Orbitals			77:27
		Intro		0:00
		Covalent Bond		1:05
			Hydrogen Atom	1:38
			Lewis	2:41
			Sharing of Electrons	3:14
		Valence Electrons		4:13
			Example: Lewis Symbols	5:35
		Lewis Structures of Atoms and Ions		10:05
			Example: Ions	10:56
		Octet Rule		13:34
			Noble Gases	14:14
		How to Draw Lewis Structures		17:35
			Single Bond	21:39
			Double Bond	21:54
			Triple Bond	22:02
			Examples: Compounds	22:23
		Formal Charges		32:44
			Example: 3 Structures of FCN	34:01
		Exceptions to the Octet Rule		40:17
			Fewer Than 8 Electrons	41:07
			Example: Boron (Electron Deficiency)	41:53
			More Than 8 Electrons	44:22
			Example: Compounds	45:37
		Electronegativity		48:09
			Example: Values	49:24
			Ionic or Polar Covalent Bond	52:02
		Molecular Orbitals		54:16
		Sigma and Pi Bonding		55:56
		Additional Example 1		11:33
		Additional Example 2		7:14
	Shapes of Molecules and Hybridization			71:19
		Intro		0:00
		VSEPR: Valence Shell Electron Pair Repulsion		0:53
		Counting Electron Sets		4:20
			Example: Methane	4:48
			Example: Ammonia	5:48
			Example: Formaldehyde	7:06
			Example: Hydrogen Cyanide	8:48
		Geometry of 2 and 3 Sets		10:28
			Two Sets: Linear	11:30
			Examples	11:57
			Three Sets: Trigonal and Planar	14:29
			Examples	15:48
		Geometry of 4 Sets		19:46
			Four Sets: Tetrahedral	20:08
			Examples	22:03
		Geometry of 5 and 6 Sets		27:50
			Five Sets: Trigonal Bipyramid	28:12
			Six Sets: Octahedron	30:28
		Hybridization and Hybrid Orbitals		32:07
			Linus Pauling	33:27
			Example: Carbon	33:46
		Orbital Phases		40:14
			Wave Function Phases	40:20
			Example: 2p Orbital	41:09
		Sigma Bonds		42:51
			Example: Ethane	46:37
		Pi Bonds		49:04
			Example: Ethylene	50:15
		Additional Example 1		10:31
		Additional Example 2		5:45
VIII. States of Matter
	States of Matter, Intermolecular Forces, Gases and Gas laws			61:12
		Intro		0:00
		States of Matter: Solid, Liquid, Gas		0:43
			Solid	1:10
			Liquid	2:14
			Gas	3:10
		Phase Transitions		4:36
			Melting, Freezing, Boiling, Condensing	5:09
			Sublimation, Condensation	6:49
			Example: Dry Ice	7:25
		Ionic Forces and Ion Dipole Forces		8:42
			Example: Ionic Forces	11:04
			Example: Ion Dipole Forces (Polar)	12:44
		Dipole-Dipole Forces and Hydrogen Bonding		15:51
			Example: Water Molecules	16:06
			Example: Liquid Hydrogen Chloride	16:46
			Strong Dipole-Dipole, Hydrogen Bonds	17:43
			Boiling Points	19:30
		Dispersion or London Forces		22:36
			Boiling Points of Noble Gases	26:39
		Hydrogen Bonding in Water and Biological Systems		28:17
			Example: Crystalline Water (Open Structure)	28:28
			Example: Protein	29:34
			Example: DNA Double Helix	30:31
		Gaseous State: Kinetic Molecular Model		31:00
		Gases of the Atmosphere		33:31
			Percentage by Volume	33:59
		Pressure		33:15
			Mercury Barometer	36:14
		Units of Pressure		38:33
			Pascal	39:23
			Bar, Torr, Atm	39:49
		Gas Laws and the Ideal Gas Law		41:47
			Boyle's Law	42:01
			Charles' Law	42:45
			Ideal Gas Law (Combined Law)	43:25
			Gas Constant R	44:11
		Example: Gas Law Calculations		45:02
		Molar Mass from Gas Law Calculations		47:21
			Example: Experimental Gas	48:21
		Additional Example 1		5:29
		Additional Example 2		4:03
IX. Gases
	Partial Pressure, Real Gases, Atmospheric Pollution			61:12
		Intro		0:00
		Partial Pressure and Mole Fraction		1:08
			Example: Gases A, B, C	3:00
			Example: Mole Fraction of A, B, C	4:28
		Dalton's Law of Partial Pressures		6:29
			Example: Gases A, B, C	8:14
			Example: Air	11:27
		Applications of Dalton's Law		12:23
			Example: Potassium Chlorate	12:39
		Real Gases		20:16
			Example: Hydrogen and Nitrogen	21:05
			Departure from Ideal Gas Law	23:42
		Van der Waals' Equation		28:52
			Corrective Equation	31:18
		Ozone and the Ozone Hole		34:01
			How Ozone is Formed	35:56
		Effects of Chlorofluorocarbons (CFC)		40:49
			Example: Freon	52:59
		Oxides of Nitrogen		47:15
		Sulfur Dioxide		51:32
		Acid Rain		54:19
		Additional Example 1		3:11
X. Phases
	Vapor Pressure, Boiling Point, Phase Diagrams			56:58
		Intro		0:00
		Vapor Pressure: An Equilibrium Phenomenon		0:55
			Thought Experiment: Water Equilibrium	1:06
		Boiling Point and Normal Boiling Point		6:19
			Reducing Boiling Point	3:10
			Example: Water	9:51
		Surface Tension		14:12
			Example: Water	15:55
		Viscosity		19:53
			Intermolecular Forces	22:22
			Example: Ethanol, Antifreeze, Glycerol	22:52
		Enthalpies of Phase Changes		28:08
			Example: Water	28:22
		Phase Diagrams (Water)		32:22
			Vapor Pressure Curve	35:30
			Melting Point Line	35:54
			Triple Point	36:36
			Critical Point	37:50
		Phase Diagrams (Carbon Dioxide)		38:42
			Sublimation	40:11
			Critical Point	42:56
		Triple Point and Critical Point		44:54
			Example: Carbon Dioxide	46:11
XI. Solids
	Types of Solids, X-Ray Diffraction, Unit Cells			57:30
		Intro		0:00
		Solids: Crystalline and Amorphous		0:59
			X-Ray Diffraction	4:30
		Types of Crystalline Solids: Atomic		5:39
			Example: Metallic Copper	5:50
		Types of Crystalline Solids: Ionic Crystal		7:20
			Example: NaCl	7:37
		Types of Crystalline Solids: Molecular Crystal		11:30
			Example: Ice	11:42
		Types of Crystalline Solids: Network Solid		13:22
			Example: Carbon Allotropes (Diamond and Graphite)	13:36
		X-Ray Diffraction and Bragg's Law		18:26
			Bragg's Law Equation	23:53
		Unit Cell		26:55
			Simple Cubic Unit Cell	27:47
		Face-Centered and Body-Centered Unit Cells		31:06
			Body-Centered Cubic	31:22
			Face-Centered Cubic	32:53
		Unit Cell and Densities of Crystalline Solids		36:13
			Example: Platinum	36:39
		First Law of Thermodynamics and Lattice Energy		42:14
			Example: NaCl	42:33
		Lattice Energies and Constitutions of Ionic Solids		47:33
		Additional Example 1		7:09
XII. Carbon
	Carbon Allotropes, Band Theory of Solids			52:34
		Intro		0:00
		Diamond and Graphite		0:55
			Diamond	1:32
			Graphite	3:25
		C-60: An Unexpected Allotrope		6:59
			Buckyball (R. Buckminster Fuller)	9:30
		Carbon Nanotubes		11:42
			Possible Uses	13:51
		Metals, Semiconductors, and Insulators		15:34
			3 Classes of Conductors	15:41
		Conductivity and Band Theory		20:30
			Example: Valence Band	22:46
		P-Type and N-Type Semiconductors		27:21
			Phosphorus to Silicon	29:21
			Boron to Silicon	31:38
		P/N Junctions		33:48
			Integrated Circuit	38:49
		Glasses and Ceramics		40:26
			Glasses	41:02
			Example: Common Window Glass	44:49
			Ceramics	47:16
XIII. Solutions
	Solutions, Henry's Law, Concentration Equations			65:40
		Intro		0:00
		Types of Solutions		1:43
			Examples: Homogeneous Mixtures	2:37
			Examples: Solid Solutions	6:59
		Saturation Solubility		8:47
			Example: Solvent and Soluten (Salt and Water)	9:15
			Solubility Dependencies	14:54
		Henry's Law		15:36
			Values for Henry's Law Constant (Water)	18:01
			Example: Soda Can	19:27
			Example: SCUBA	21:10
		Solution Concentration Expressions		26:02
			Percentage by Mass	26:16
			Example: Salt and Water	26:52
			Molarity	28:18
			Molality	31:26
		Calculation of Solution Concentrations		32:42
			Example: Sodium Chloride Solution	32:49
		Dilution of Solutions		37:35
			Example: Hydrochloric Acid	38:54
		Effects of Temperature on Solubility (Gases in Liquids)		42:01
			Example: Water	42:40
		Effects of Temperature on Solubility (Solids in Liquids)		45:42
			Examples: Various Salts	46:47
		Entropy: Qualitative Introduction		52:25
		Temperature Effects: Enthalpy, Entropy		55:39
		Additional Example 1		7:20
XIV. Colligative Properties
	Colligative Properties, Colloids, Surfactants			70:42
		Intro		0:00
		Colligative Properties and Raoult's Law		0:43
			Colligative (Collective)	0:46
			Raoult's Law	1:55
			Uses of Raoult's Law (Mole Fraction and Molar Mass)	4:34
		Boiling Point Elevation, Freezing Point Depression		5:47
			Pure Water and Solution in Water	6:17
			Lower Vapor Pressure	6:53
			Higher Boiling Point (Elevation)	7:04
			Lower Freezing Point (Depression)	7:52
			Example: Antifreeze	8:37
			Change in Boiling Point (Molality)	10:55
		Molar Mass from Elevation and Depression		12:49
			Example: Water and Cystine	13:20
		Van der Waals' Alpha Factor		18:59
			Alpha Factor Equation	20:15
			Example: Salt Ions	21:11
		Osmosis		23:02
			Blood (Isotonic, Hypertonic, Hypotonic)	23:47
		Osmotic Pressure		27:40
			Osmotic Pressure Definition (Pi)	30:14
			Van der Waals'	30:57
		Molar Mass from Osmotic Pressure		33:29
			Example: Peptide in Water	34:20
		Colloids and the Tyndall Effect		38:33
			Light Beam (Solution and Colloidal Suspension)	41:05
		Surfactants		44:11
			Example: Sodium Stearate (Soap)	45:10
		Soaps and Detergents		49:24
			Ordinary Soaps Problem	52:36
			Synthetic Soaps	53:57
		Additional Example 1		5:57
		Additional Example 2		6:41
XV. Kinetics
	Kinetics, Rate Laws, Reaction Mechanism			68:48
		Intro		0:00
		Reaction Rate		1:30
			Chemical Reaction Rate	2:36
			Example: Methyl Bromide and Sodium Hydroxide	4:04
		Reaction Rates: Changing Concentrations		10:28
			Example: Double Initial Concentrations	11:33
		Order of Reaction		17:05
			Experimental Rate Law	17:47
			Overall Rate	21:27
		Initial Rate Measurement		23:24
			Example: Methyl Bromide and Sodium Hydroxide	23:44
		Integrated Rate Laws: First Order Reaction		29:54
			Integrated Rate Equation	31:12
			Example: Transitional Metal Complex	33:48
		Integrated Rate Laws: Second Order Reaction		38:12
			Integrated Rate Equation	38:37
		Experimental Rate Laws		39:41
			Example: Transitional Metal Complex	39:55
		Experimental Rate Laws, cont.		42:45
			Example: Nitramide	43:00
		Reaction Mechanism		46:12
			Hypothetical Aspect	47:38
			Predict Outcomes	48:02
		Elementary Reactions and Reaction Mechanisms		49:43
			Example: Methyl Bromide and Hydroxide Ion	51:02
		Rate Limiting Step		54:47
			Example: Rate Limiting Step	55:41
		Additional Example 1		3:00
		Additional Example 2		7:07
XVI. Temperature Effects
	Temperature Effects, Reaction Rate Theory, Catalysis			62:56
		Intro		0:00
		Effects of Temperature on Reaction Rates		1:05
			Common Examples	4:30
		Arrhenius' Equation		6:40
			Activation Energy	9:09
			Example: Nitrogen Pentoxide	11:52
		Reaction Rate Theory		15:20
			Activated Complex and Transition State	17:05
			Example: Methyl Bromide and Hydroxide Ion	19:58
		Calculating Activation Energy		22:32
			Plotting ln K and Inverse T	23:38
		Catalysis in Practice		25:33
			Example: Catalytic Converter	26:43
			Example: Oil Refinery	29:30
		Acid Catalysis of Ehtyl Acetate Hydrolysis		31:48
			Example	32:03
		Industrial Production of Ammonia		35:54
			Haber Bosch Process	36:06
		Industrial Production of Sulfuric Acid		41:02
			Series of Processes	41:38
		Enzymes as Catalysts		45:59
			Example: Amino Acid	47:04
			Example: Protein	47:18
		Additional Example 1		4:15
XVII. Equilibrium
	Physical and Chemical Equilibrium, Equilibrium Law, Le Chatelier's Principle			70:47
		Intro		0:00
		Equilibrium in Physical Processes		1:13
			Example: Water Equilibrium (Vapor Pressure)	1:30
			Example: Water Equilibrium (Melting )	1:58
		Equilibrium in Chemical Processes		3:37
			Example: Acetic Acid and Ethanol	3:51
		The Equilibrium Law and Equilibrium Constant		9:11
			Equilibrium Law	11:32
			Equilibrium Constant K	12:47
		Equilibrium Expressions and Constants		14:11
			Example: Acetic Acid and Ethanol	14:24
			Example: Calcium Carbonate (Lime Burning)	17:23
		Standard Concentration and Activities		21:13
		Kp and Kr		23:56
			Example: Nitric Oxide	24:26
		Calculations of Equilibria		29:06
			Example: Acetic Acid and Ethanol	29:17
		Le Chatelier's Principle		40:47
			Stressors	42:55
			Example: Haber Bosch	49:26
		Additional Example 1		6:48
		Additional Example 2		6:29
XVIII. Acids and Bases
	Acids and Bases: Strong and Weak, pH			60:41
		Intro		0:00
		Acids		0:36
			React with Some Metals	2:25
			Litmus Test (Red)	3:04
		Bases		4:33
			Litmus Test (Blue)	5:52
			Acids and Base Neutralize	6:43
		Classification: Arrhenius and Bronsted-Lowry		8:52
			Arrhenius Classification	9:11
			Example: HCl (Hydronium) and NaOH (Hydroxide)	11:08
			Bronsted-Lowry Classification	12:42
			Example: HCl	13:30
			Conjugate Acid, Conjugate Base	14:08
		Lewis Acids and Bases		16:23
			Lewis Base: Electron Pair Donor	17:24
			Lewis Acid: Electron Pair Acceptor	18:24
			Example: Lewis Acid Base Reaction	20:03
		Common Strong Acids		22:02
		Common Strong Bases		24:39
		Common Weak Acids		26:24
		Common Weak Bases		31:14
		Water as an Acid and Base: Kw		34:01
			K of Water	35:21
		Ionization Constants for Weak Acids		38:11
			Examples: Constants	38:20
		Ionization Constants for Weak Bases		40:30
			Examples: Constants	40:44
		pH and the pH Scale		43:12
			Sorenson pH	43:46
			Neutral Water	44:48
			Acid and Base pH	46:24
			pH Scale (Acid and Alkaline)	47:30
		Additional Example 1		5:53
	pH Calculations, Polyprotic Acids			60:09
		Intro		0:00
		pH in a Solution of a Weak Acid		0:45
			Vinegar (Acetic Acid)	1:00
			Example: pH of Acetic Acid Solution	2:34
		pH in a Solution of a Weak Base		9:42
			Ammonia	9:48
			Example: pH of Pyridine Solution	11:46
		Salts of Weak Acids with Strong Bases		17:15
			Example: Acetic Acid and Sodium Hydroxide	17:55
		Salts of Weak Bases with Strong Acids		20:55
			Example: Ammonia and Hydrochloric Acid	21:13
		Conjugate Acid Base Pairs: Ka and Kb		22:58
			Example: Acetic Acid Ionization	23:06
		Polyprotic Acids: Successive Ka Values		28:50
			Example: Diprotic Acid (Sulfuric Acid)	29:13
			Example: Tripotic Acid (Phosphoric Acid)	29:28
		pH in a Polyprotic Acid Solution		41:02
			Example: Phosphoric Acid Solution pH	41:21
		Salts of Polyprotic Acids		47:32
			Examples: TSP, Tartaric Acid	47:45
		Additional Example 1		6:15
	Titrations, Indicators, Buffers			66:19
		Intro		0:00
		Titration and Analysis		0:43
			Equipment: Burets, Pipet, Stopcock, Volumetric Flask	1:38
			Molarity	4:04
		Strong Acid-Strong Base Titration		6:16
			Example: Sodium Hydroxide and Hydrochloric Acid	7:04
		Weak Acid-Strong Base Titration		16:45
			Example: Acetic Acid and Sodium Hydroxide	17:06
		pH Meter		28:48
			pH Electrode: Logarithmic Change to Hydronium	29:19
		Indicators		32:10
			Example: Indicator and Hydronium	33:21
			Phenolphthalein	34:07
			Methyl Orange	35:12
		Theory and Choice of Indicators		39:19
			Indicator Visibility if Factor of 10	40:45
		Buffers		42:47
			What is a Buffer Solution?	46:08
			Acetate Buffer and Ammonium Buffer	47:16
			Example: Buffer Effects	48:26
		Buffer Regions in Titrations		51:38
			Example: Acetic Acid and Sodium Hydroxide	51:48
		Practical Buffers		55:17
			Example: Acetic Acid and Acetate Ion (pH Range)	55:27
		Additional Example 1		7:51
XIX. Solubility
	Solubility Product Constant, Precipitation			59:36
		Intro		0:00
		Equilibrium in Saturated Salt Solution		1:12
			Example: Silver Chloride	1:50
			Ksp (Solubility Product Constant)	4:12
		Solubility Product Constant		6:19
			Example : Lead Iodide	6:31
		Limitations of the Solubility Product		9:06
			Low Solubility	9:23
			Complexes that are Soluble	11:31
		Ksp Values and Ion Concentrations		13:28
			Example: Silver Chloride	16:06
			Example: Lead Chloride	19:22
		Precipitation of Salts		23:56
			Example: Silver Bromide and Copper Bromide	25:31
		Common Ion Effect		31:52
			Example: Lead Sulfate	32:11
			Le Chatelier's Principle	39:30
		Common Ion Solubility		42:37
			Example: Lead Chloride in Sodium Chloride Solution	42:46
		Acids, Bases, and Solubility Equilibria		48:32
			Example: Lead Carbonate	48:46
			Lle Chatelier's Principle	54:26
		Group Separation and Qualitative Analysis of Metal Ions		55:09
			Examples	56:25
		Additional Example 1		5:42
XX. Enthalpy and Entropy
	Enthalpy, Entropy, Second Law of Thermodynamics			53:51
		Intro		0:00
		Factors Affecting Equilibrium Constants		1:15
			Spontaneous Reaction	2:17
			Temperature Effects	4:50
		State Functions: Enthalpy and Entropy		6:17
			Example: Methane and Chlorine	8:32
			Hess's Law	10:36
			Entropy	10:55
		Statistical Interpretation of Entropy		13:24
			Boltzmann Entropy Equation	13:33
			Reversible Change	16:24
			Example: Water and Ice	16:55
		Third Law of Thermodynamics		20:06
			Nernst	20:31
		Entropies of Gases, Liquids, and Solids		23:16
			Example: Entropy Values	25:17
		Entropy Values from Enthalpy/Temperature		28:55
			Example: Water (Graph)	29:34
		Entropy Changes in Phase Changes		32:33
			Melting (Fusion)	32:41
			Example: Water Melting	33:15
		Second Law of Thermodynamics		34:21
			Example: Hydrogen and Oxygen	37:20
			Statement of Second Law (Spontaneous/Reversible)	39:28
		Reactant Favored and Product Favored Equilibria		41:10
			Reactant or Product Favored	41:48
			Converse	45:15
		Limitations of Applying the Second Law to Equilibria		46:57
			Delta S	47:30
XXI. Gibbs' Function
	Gibbs' Function, Equilibrium			61:10
		Intro		0:00
		The Gibbs' Function		0:35
			Values of Delta G	4:57
		The Gibbs' Function and K		9:11
			Gibbs' Function Change (Free Energy)	11:06
			Values of Gibbs' Function Standard Change	14:17
		Calculation of K from ThermoDynamic Data		15:46
			Example: Nitrogen Dioxide to Dinitrogen Tetroxide	16:01
		Calculation of K		24:32
			Example: Diamond to Graphite	24:46
		Calculation of K		31:33
			Example: Ammonia	31:38
		Temperature Changes: Gibbs' Function and K		38:12
			Estimating Gibbs' Function Values at Temperatures	40:04
		Temperature Changes		42:29
			Example: Oxide of Iron and Carbon	42:49
		Additional Example 1		8:26
XXII. Redox Reactions
	Balancing Redox Reactions, Half Reactions			67:26
		Intro		0:00
		Oxidation and Reduction Review		0:58
			Example: Sodium and Chlorine	1:05
		Determining Oxidation Numbers		5:43
			Rules for Assigning Oxidation Numbers	8:02
		Oxidation Number Assignment		11:25
			Examples: Various	11:42
		Balancing Half Reactions		18:26
			Example: Half Reactions	21:22
			Example: Zinc in Hydrochloric Acid	22:34
		Combining Half Reactions Into Complete Reactions		24:32
			Example: Zinc	24:40
			Spectator Ions	26:10
		Half Reactions in Acidic and Basic Solutions		28:38
			Example: Permanganate	29:18
		Balancing Redox Reactions		36:34
			Example: Determination of Iron	37:22
		Balancing Redox Reactions		45:54
			Example: Lead Dioxide and Chloride Ion	46:12
		Additional Example 1		5:14
		Additional Example 2		9:28
XXIII. Electrochemistry
	Electrochemical Cells, Half-Cell Potentials			67:52
		Intro		0:00
		Electricity from Chemical Reactions		0:29
			Galvani Volta: Current Electricity	0:40
			Voltaic Pile (Battery)	3:33
			Potato Clock	4:35
		Daniell Cell		5:56
			Oxidation of Zinc, Reduction of Copper	6:46
			Spontaneous Overall Reaction	8:25
			Anode and Cathode	9:20
		Current Electricity Fundamentals		11:34
			Electric Charge: Coulomb	11:46
			Electric Current: Ampere	12:33
			Volt	14:43
			Ohm's Law	16:16
		Galvanic Cell		17:41
			Salt Bridge	19:35
		Cell Potential and Work		20:56
			Joules	21:40
			Coulombs	22:27
		Hydrogen Electrode		22:53
			Breakdown	24:12
		Half-Cell Potentials		29:24
			Example: Zinc and Standard Hydrogen Electrode (SHE)	30:50
		Electrochemical Series		35:04
			Example: Aluminum Reducing Iron Ion	38:26
		Nernst Equation		41:46
			Faraday	42:09
			Example: Concentration Cell (Copper Ions)	46:39
		Nernst Equation: pH Meter		52:24
			Example: Potential and pH	53:21
		Nernst Equation: Ion Concentrations		56:11
		Additional Example 1		5:19
		Additional Example 2		5:12
	Practical Batteries, Electrolysis			62:06
		Intro		0:00
		Primary Batteries		0:54
			Leclanche Dry Cell	1:03
			Alkaline Cell	4:34
		Fuel Cell		6:53
			Overall Reaction	8:24
		Secondary Batteries		13:47
			Car Battery	14:04
		Electrolysis		18:41
			Aluminum Plant	19:14
			Chromium Plating	22:42
		Sodium Chloride		24:08
			Example: Metallic Na	24:20
			Example: Bleach	28:38
		Faraday's Laws		32:22
			Example: Aluminum Electrolysis	34:54
		Corrosion of Iron		41:24
			Example: Iron Galvanic Cell	44:34
		Protection of Iron Against Corrosion		46:55
			Coating of Tin Cans	47:18
		Additional Example 1		4:45
XXIV. Radioactivity
	Radioactivity, Nuclear Equations, Mass Energy Equivalence			40:35
		Intro		0:00
		Radioactivity Pioneers		0:36
			Becquerel	2:20
			Curie	1:53
			Rutherford	2:38
			Soddy	2:55
		Alpha, Beta, and Gamma Radiation		3:46
			Three Types of Emission	4:28
		Transmutation and Nuclear Equations		7:01
			Decay of Uranium	8:07
		Balancing Nuclear Equations		13:08
			Example: Chromium	13:19
			Example: Radium	15:56
		Synthesis of New Isotopes and Elements		18:47
			Example: Nitrogen and Alpha Particles	19:44
			Example: Uranium and Carbon Nuclei	21:41
		Mass Changes in Nuclear Transformations		23:55
			Mass and Energy Equivalence (e=mc2, Einstein)	24:39
		Mass-Energy Transformations		28:35
			Example: Uranium	28:38
		Stability of Nuclei and Binding Energy		33:11
			Nucleons	33:34
			Example: Deuterium and Helium	33:51
		Curve of Binding Energy; Fission and Fusion		35:53
	Radioactive Decay, Half-Life, Nuclear Reactions			56:12
		Intro		0:00
		First Order Nuclear Decay		0:41
			Example: Uranium	2:01
			Rate Constant	3:42
			Integrated Rate Equation	3:52
			Half-Life	5:14
		Half-Lives and Rate Constants		6:09
			Examples: Various	6:14
		Radioactive Dating: Rocks		9:18
			Example: Rock with Uranium and Lead	10:53
		Radioactive Dating: Carbon-14		17:27
			Example: Shroud of Turin	20:54
			Example: Wooden Staff	22:31
		Nuclear Fusion in Stars		27:22
			Example: Reaction in Sun	29:21
		Nuclear Weapons		32:24
			Example: Uranium Isotope	34:14
		Nuclear Power		38:52
			Nuclear Power Usage	42:30
		Nuclear Wastes and Their Disposal		45:03
		Additional Example 1		5:33
XXV. Miscellaneous
	Organic Structures, Isomers, Functional Groups			68:32
		Intro		0:00
		Saturated Hydrocarbons C-1 to C-4		1:41
			Acyclic	2:38
			Example: Methane, Ethane, Propane	3:28
			Isomers	7:19
		Acyclic Saturated Hydrocarbons C-5 Isomers		10:27
			Example: Pentanes	10:40
		Alkenes and Ring Compounds		14:56
			Alkenes	15:34
			Example: Ethene, Ethylene	16:25
			Example: Propene Isomers	19:19
		Geometric Isomers of Alkenes		24:13
			Example: 2-Butene	24:34
			Trans and Cis	26:27
		Optical Isomers		28:45
			Example: Carbon Atom	33:49
		Functional Groups: Alcohols and Caboxylic Acids		39:11
			Alcohols	39:27
			Carboxylic Acids	41:41
		Functional Groups: Esters and Ethers		44:10
			Esters (Ethyl Acetate)	44:27
			Ethers (Diethylether)	46:14
		Functional Groups: Aldehydes and Ketones		47:48
			Examples	47:59
		Amines		51:01
		Amide Group		54:24
		Peptides and Proteins		56:02
		Additional Example 1		9:41
	Chemistry and the Environment			50:13
		Intro		0:00
		Global Climate Change		1:41
			Greenhouse Gases	3:49
		Greenhouse Gases and Climate Change		6:53
			Last 100 Years	9:11
		Water Pollution: Eutrophication		12:59
			Example: Fertilizers	15:41
		Water Pollution: Organic Pollutants		9:15
			Chlorinated Hydrocarbons (DDT)	19:30
			Dioxins and Phthalates	20:58
		Water Pollution: Heavy Metal Pollutants		23:58
			Examples: Lead, Chromium, Arsenic	24:17
		Radiation in the Environment		24:35
			Thresholds	39:20

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Acids and Bases: Strong and Weak, pH

Acids and Bases: Strong and Weak, pH

Advanced Placement Chemistry

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