20sec4
•Download as PPT, PDF•
0 likes•250 views
This document discusses the strengths of acids and bases. It defines strong acids and bases as being completely ionized in aqueous solution, while weak acids and bases only ionize slightly. Strength refers to the degree of ionization, not concentration. Strong acids and bases have a higher dissociation constant (Ka for acids, Kb for bases) because they produce more ions. Concentration is different and refers to the number of moles dissolved in a given volume. A concentrated weak acid is possible.
Report
Share
Report
Share
Recommended
Unit 3
This document discusses acids and bases, including their properties and reactions. It defines acids as substances that release hydrogen ions in water and bases as those that release hydroxide ions. Acids and bases neutralize one another in a reaction that produces salt and water. The document also discusses acid-base theories, strong vs. weak acids/bases, pH, electrolytes, self-ionization of water, and acid-base indicators. Buffers are introduced as solutions that resist changes in pH when small amounts of acid or base are added.
Acids andbases cheat sheet
This document provides an overview of key concepts related to acids and bases in chemistry. It defines different types of acids and bases according to several theories. It also discusses properties of acids and bases such as tastes and colors of litmus paper. Strong and weak acids and bases are compared. Buffers are described as mixtures of weak acids and bases that resist pH change. The pH scale is introduced and methods for solving pH problems are outlined, including using Ka, Kb, and Kw values and ICE charts. Acid-base properties of salts and the principles of titrations are also summarized.
Mec chapter 8
This document provides an overview of acids and bases including:
1) It describes the Arrhenius and Brønsted-Lowry theories of acids and bases, defining acids as proton donors and bases as proton acceptors.
2) It discusses strong vs. weak acids and bases based on their degree of dissociation in water, and introduces conjugate acid-base pairs.
3) It explains that water can act as both an acid and base, and discusses the autoionization of water and the definition of pH in terms of the hydronium ion concentration.
Acid base disorders by Dr. Aslam
This document discusses four patient cases presenting with acid-base disorders.
Patient A has a metabolic acidosis caused by salicylate ingestion, shown by a low pH and bicarbonate level with respiratory compensation of an increased PCO2.
Patient B has a respiratory acidosis from chronic obstructive pulmonary disease, shown by a low pH and high PCO2 with metabolic compensation of an increased bicarbonate level.
Patient C has a metabolic acidosis likely from diabetic ketoacidosis, shown by a low pH and bicarbonate level with respiratory compensation of a low PCO2.
Patient D has a respiratory alkalosis from hysterical overbreathing, shown by
Acid base homeostasis
This presentation is clarifying how blood changes its medium from normal or neutral to either acidic or to alkaline medium depending on variable metabolic or respiratory circumstances.
Ap chem unit 14 presentation part 1
[H+] = 2.7x10-2 M
pH = 1.57
The calculated [H+] is within ±5% of Ka, so the
approximation is valid. The pH is 1.57.
Hard soft acid_base
Pearson's Hard Soft Lewis Acid Base (HSAB) principle classifies Lewis acids and bases as hard, soft or borderline based on their ability to form ionic or covalent complexes. According to the principle, hard acids prefer hard bases and form ionic complexes, while soft acids prefer soft bases and form covalent complexes. However, the HSAB model oversimplifies reactions and introduces ambiguities, as no single physical parameter determines hardness. A more nuanced analysis is needed to understand complex Lewis acid-base interactions.
Chapter 18.1 : The Nature of Chemical Equilibrium
This document provides information about chemical equilibrium, including definitions, concepts, and examples. It defines chemical equilibrium as a state where the rates of the forward and reverse reactions are equal and the concentrations of reactants and products remain constant. The equilibrium constant, K, is introduced as a ratio of product concentrations over reactant concentrations raised to their stoichiometric coefficients. Examples are provided to demonstrate how to write equilibrium expressions and calculate K values or concentrations at equilibrium.
Recommended
Unit 3
This document discusses acids and bases, including their properties and reactions. It defines acids as substances that release hydrogen ions in water and bases as those that release hydroxide ions. Acids and bases neutralize one another in a reaction that produces salt and water. The document also discusses acid-base theories, strong vs. weak acids/bases, pH, electrolytes, self-ionization of water, and acid-base indicators. Buffers are introduced as solutions that resist changes in pH when small amounts of acid or base are added.
Acids andbases cheat sheet
This document provides an overview of key concepts related to acids and bases in chemistry. It defines different types of acids and bases according to several theories. It also discusses properties of acids and bases such as tastes and colors of litmus paper. Strong and weak acids and bases are compared. Buffers are described as mixtures of weak acids and bases that resist pH change. The pH scale is introduced and methods for solving pH problems are outlined, including using Ka, Kb, and Kw values and ICE charts. Acid-base properties of salts and the principles of titrations are also summarized.
Mec chapter 8
This document provides an overview of acids and bases including:
1) It describes the Arrhenius and Brønsted-Lowry theories of acids and bases, defining acids as proton donors and bases as proton acceptors.
2) It discusses strong vs. weak acids and bases based on their degree of dissociation in water, and introduces conjugate acid-base pairs.
3) It explains that water can act as both an acid and base, and discusses the autoionization of water and the definition of pH in terms of the hydronium ion concentration.
Acid base disorders by Dr. Aslam
This document discusses four patient cases presenting with acid-base disorders.
Patient A has a metabolic acidosis caused by salicylate ingestion, shown by a low pH and bicarbonate level with respiratory compensation of an increased PCO2.
Patient B has a respiratory acidosis from chronic obstructive pulmonary disease, shown by a low pH and high PCO2 with metabolic compensation of an increased bicarbonate level.
Patient C has a metabolic acidosis likely from diabetic ketoacidosis, shown by a low pH and bicarbonate level with respiratory compensation of a low PCO2.
Patient D has a respiratory alkalosis from hysterical overbreathing, shown by
Acid base homeostasis
This presentation is clarifying how blood changes its medium from normal or neutral to either acidic or to alkaline medium depending on variable metabolic or respiratory circumstances.
Ap chem unit 14 presentation part 1
[H+] = 2.7x10-2 M
pH = 1.57
The calculated [H+] is within ±5% of Ka, so the
approximation is valid. The pH is 1.57.
Hard soft acid_base
Pearson's Hard Soft Lewis Acid Base (HSAB) principle classifies Lewis acids and bases as hard, soft or borderline based on their ability to form ionic or covalent complexes. According to the principle, hard acids prefer hard bases and form ionic complexes, while soft acids prefer soft bases and form covalent complexes. However, the HSAB model oversimplifies reactions and introduces ambiguities, as no single physical parameter determines hardness. A more nuanced analysis is needed to understand complex Lewis acid-base interactions.
Chapter 18.1 : The Nature of Chemical Equilibrium
This document provides information about chemical equilibrium, including definitions, concepts, and examples. It defines chemical equilibrium as a state where the rates of the forward and reverse reactions are equal and the concentrations of reactants and products remain constant. The equilibrium constant, K, is introduced as a ratio of product concentrations over reactant concentrations raised to their stoichiometric coefficients. Examples are provided to demonstrate how to write equilibrium expressions and calculate K values or concentrations at equilibrium.
Strength Of Acid And Alkali
Strong acids and bases ionize completely in water, producing high concentrations of hydrogen or hydroxide ions. Weak acids and bases only partially ionize in water, resulting in lower concentrations of ions. Specifically, hydrochloric acid and sodium hydroxide fully dissociate whereas ethanoic acid and ammonia only partially dissociate, making the latter acids and bases weaker. Strong acids and bases have higher pH values and degrees of ionization compared to their weaker counterparts.
HSAB Theory
The document discusses Pearson's Hard and Soft Acid and Base (HSAB) theory, which states that hard acids prefer to bond with hard bases and soft acids prefer to bond with soft bases. It provides examples of hard and soft ligands and metal ions. Key points include:
- Hard metals have high charge, small size, and are not easily polarized, while soft metals are the opposite.
- The theory can be used to explain the bonding preferences of ambidentate ligands like thiocyanate based on whether they bond to hard or soft metals through nitrogen or sulfur.
- The theory has applications in explaining reactivity patterns in inorganic reactions, organic reactions involving acids and bases of different hardness, and precipitation reactions.
Chemical Equilibrium
The document discusses chemical equilibrium, including:
1) All physical and chemical changes tend toward a state of equilibrium according to Le Chatelier's principle.
2) At dynamic equilibrium, the rates of the forward and reverse reactions are equal and the reaction quotient equals the equilibrium constant.
3) Equilibrium constants can be calculated using concentration values and reaction quotients can indicate the direction a reaction will proceed to reach equilibrium.
VCE Chemistry Acids & Bases Concentration v Strength
This document discusses the distinction between the strength and concentration of acids and bases. It defines strength as the degree of dissociation, with strong acids and bases completely dissociating in solution and weak ones only partially dissociating. Concentration refers to the number of moles of acid or base per volume of solution. A solution can be highly concentrated but still contain a weak acid or base that only partially dissociates, or be weakly concentrated but contain a strong acid or base that fully dissociates. The document provides examples of calculating dissociation for sulfuric acid and sodium hydroxide to illustrate these concepts.
Module 2: Définir la violence basée sur le genre (VBG)
Définir la violence basée sur le genre (VBG) .
Acids and bases and salts
The document discusses acids and bases. It defines acids as substances that give up hydrogen ions in solution and bases as those that give up hydroxide ions. It then provides examples of common acids like vinegar and lemon juice and bases like baking soda. It explains how to test for acids and bases using litmus paper and red cabbage juice and lists some major acid-base theories. DNA is identified as an acid according to Bronsted's definition.
Chemical equilibrium
This document summarizes key concepts about chemical equilibrium:
1) Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal and the concentrations of reactants and products stop changing. The system appears static but reactions are still occurring in both directions.
2) The equilibrium constant, K, is defined based on the balanced chemical equation and describes the position of equilibrium. It depends only on temperature.
3) The reaction quotient, Q, is similar to K but uses the actual concentrations rather than equilibrium concentrations. Comparing Q to K indicates whether a reaction will proceed in the forward or reverse direction to reach equilibrium.
Chem 2 - Acid-Base Equilibria VIII: The Conjugate See-Saw and Analyzing Ka an...
Chem 2 - Acid-Base Equilibria VIII: The Conjugate See-Saw and Analyzing Ka and Kb for Acid or Base Relative Strength
Hsab theory
The document discusses the hard and soft acid and base (HSAB) theory introduced by Pearson in 1963. It explains that hard acids prefer to coordinate with hard bases, and soft acids prefer soft bases, due to their relative polarizabilities. Hard acids and bases are less polarizable, while soft species are more polarizable and form stronger bonds through electron sharing. The HSAB concept is used to understand stability, reactions, and reaction mechanisms based on qualitative descriptions of predominant factors like polarizability.
Chapter15
This document provides an overview of chapter 15 on acids and bases. It begins with an outline of the key concepts and sections to be covered, including the Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases. It then discusses acid and base strengths, factors that influence strength, and the concepts of conjugate acid-base pairs and amphiprotic species. Another section covers self-ionization of water and how pH is defined and calculated. Learning objectives are provided for each major topic.
4 concentration vs strength of acid bases
1) When acids or bases dissolve in water, they dissociate or break apart into ions. For acids, this takes the form HA + H2O ⇌ A- + H3O+.
2) Strong acids and bases dissociate completely in water, forming a high concentration of ions. Weak acids and bases only partially dissociate, forming a low concentration of ions.
3) A titration experiment determines the concentration of an unknown solution by neutralizing it with a solution of known concentration and tracking the equivalence point where [H+] = [OH-].
acid base indicators
The student conducted an experiment to determine which juices could serve as acid-base indicators by boiling various vegetables and fruits in water and observing color changes when vinegar or baking soda were added. Key findings were that rose, black bean, and spinach juices changed color noticeably, indicating they were good acid-base indicators, while carrot and white rice juices did not change color. The student learned that anthocyanin is often responsible for the color changes observed in acid-base indicators.
Chemical Equilibrium
The document discusses chemical equilibrium, including:
- When equilibrium is reached, concentrations of reactants and products remain constant, with the forward and reverse reaction rates being equal.
- Le Chatelier's principle states that applying stress (changing temperature, concentration, volume, or pressure) causes a system at equilibrium to shift in a way that reduces the stress.
- For example, increasing temperature shifts exothermic reactions toward reactants and endothermic reactions toward products.
Cmc chapter 17
This document provides an overview of three sections on chemical equilibrium from a chemistry textbook. Section 17.1 discusses the definition of chemical equilibrium as a state where forward and reverse reactions occur at equal rates. It also defines equilibrium constants and expressions. Section 17.2 explains how temperature, pressure, and concentration changes affect equilibrium based on Le Châtelier's principle. Section 17.3 discusses using equilibrium constants to determine concentrations and solubility products, and how the common ion effect impacts solubility.
Chemistryppt chemical equilibrium
The document discusses chemical equilibrium. It defines equilibrium as a state where the rates of the forward and reverse reactions of a chemical process are equal, resulting in no net change in the concentrations or properties of the system. It provides examples of physical and chemical equilibrium processes. It describes key characteristics of equilibrium like dynamic nature, constant concentrations and temperatures, and the relationship between reaction rates and equilibrium constants.
Acid base equilibria
This document discusses acid-base equilibria and titrations. It defines pH and pOH and their relationships to hydrogen and hydroxide ion concentrations. It describes the differences between strong acids, weak acids, and buffer solutions. It provides examples of preparing acidic and basic buffer solutions, such as an acetic acid-sodium acetate buffer. It also discusses acid-base indicators and their use in titrations, giving examples like methyl orange and phenolphthalein. Finally, it mentions the use of metallochromic indicators like Eriochrome Black T in titrations involving EDTA.
Chemical equillibrium
Equilibrium is a state in which there are no observable changes over time in a chemical system. At equilibrium, the concentrations of reactants and products remain constant. An equilibrium constant (K) can be defined based on the concentrations or pressures of reactants and products at equilibrium. The value of K is independent of initial concentrations and depends only on temperature. A change in concentration, pressure, volume, or temperature will shift the equilibrium in the direction that counteracts the applied stress according to Le Chatelier's principle.
Acid Etching of Enamel and Bond Strength
This document discusses acid etching of dental surfaces. It describes how acid etching was first proposed in 1955 to increase bond strength between composite resin and enamel. Acid etching removes enamel and creates an irregular porous surface that allows resin to penetrate through micromechanical interlocking, improving bond strength. Factors like acid type/concentration, etching duration, and fluoride levels can affect bonding. While acid etching is effective, some alternatives under investigation include crystal growth solutions, air abrasion, and lasers, but they have not achieved bond strengths as high as acid etching.
Chapter 15 Lecture- Chemical Equilibrium
1. The document discusses chemical equilibrium, including the concepts of equilibrium, depicting equilibrium reactions with equations, the equilibrium constant K, and how the value of K relates to whether a reaction favors reactants or products.
2. It also covers heterogeneous equilibria involving solids or liquids, how the concentrations of solids and liquids do not appear in equilibrium expressions, and examples of heterogeneous equilibrium reactions like the decomposition of calcium carbonate.
3. The key aspects covered are the definition of chemical equilibrium as when forward and reverse reactions proceed at the same rate, the use of concentration ratios and partial pressures to define equilibrium constants Kc and Kp, and how heterogeneous reactions involve gases in equilibrium with solids or liquids.
Chemical Equilibrium
The fundamentals of chemical equilibrium including Le Chatier's Principle and solved problems for heterogeneous and homogeneous equilibrium.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Metric system (1)
The document provides information about the metric system, including:
1) It is known as the SI system and is based on units of 10 with prefixes indicating multiples of 10.
2) It establishes standards for exact quantities of length, volume, mass, and time that people agree to use for comparison.
3) Derived units are obtained by combining SI units, like density which is mass divided by volume.
26sec3
The document discusses different types of carbonyl compounds including aldehydes, ketones, carboxylic acids, and esters. It covers their structures, naming conventions, properties, examples and how they are related through oxidation-reduction reactions. Aldehydes contain a carbonyl group bonded to at least one hydrogen, while ketones have the carbonyl group bonded to two carbon groups. Carboxylic acids contain both a carbonyl and hydroxyl group. Esters are derivatives of carboxylic acids where the hydroxyl is replaced by an alkoxy group from an alcohol.
More Related Content
Viewers also liked
Strength Of Acid And Alkali
Strong acids and bases ionize completely in water, producing high concentrations of hydrogen or hydroxide ions. Weak acids and bases only partially ionize in water, resulting in lower concentrations of ions. Specifically, hydrochloric acid and sodium hydroxide fully dissociate whereas ethanoic acid and ammonia only partially dissociate, making the latter acids and bases weaker. Strong acids and bases have higher pH values and degrees of ionization compared to their weaker counterparts.
HSAB Theory
The document discusses Pearson's Hard and Soft Acid and Base (HSAB) theory, which states that hard acids prefer to bond with hard bases and soft acids prefer to bond with soft bases. It provides examples of hard and soft ligands and metal ions. Key points include:
- Hard metals have high charge, small size, and are not easily polarized, while soft metals are the opposite.
- The theory can be used to explain the bonding preferences of ambidentate ligands like thiocyanate based on whether they bond to hard or soft metals through nitrogen or sulfur.
- The theory has applications in explaining reactivity patterns in inorganic reactions, organic reactions involving acids and bases of different hardness, and precipitation reactions.
Chemical Equilibrium
The document discusses chemical equilibrium, including:
1) All physical and chemical changes tend toward a state of equilibrium according to Le Chatelier's principle.
2) At dynamic equilibrium, the rates of the forward and reverse reactions are equal and the reaction quotient equals the equilibrium constant.
3) Equilibrium constants can be calculated using concentration values and reaction quotients can indicate the direction a reaction will proceed to reach equilibrium.
VCE Chemistry Acids & Bases Concentration v Strength
This document discusses the distinction between the strength and concentration of acids and bases. It defines strength as the degree of dissociation, with strong acids and bases completely dissociating in solution and weak ones only partially dissociating. Concentration refers to the number of moles of acid or base per volume of solution. A solution can be highly concentrated but still contain a weak acid or base that only partially dissociates, or be weakly concentrated but contain a strong acid or base that fully dissociates. The document provides examples of calculating dissociation for sulfuric acid and sodium hydroxide to illustrate these concepts.
Module 2: Définir la violence basée sur le genre (VBG)
Définir la violence basée sur le genre (VBG) .
Acids and bases and salts
The document discusses acids and bases. It defines acids as substances that give up hydrogen ions in solution and bases as those that give up hydroxide ions. It then provides examples of common acids like vinegar and lemon juice and bases like baking soda. It explains how to test for acids and bases using litmus paper and red cabbage juice and lists some major acid-base theories. DNA is identified as an acid according to Bronsted's definition.
Chemical equilibrium
This document summarizes key concepts about chemical equilibrium:
1) Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal and the concentrations of reactants and products stop changing. The system appears static but reactions are still occurring in both directions.
2) The equilibrium constant, K, is defined based on the balanced chemical equation and describes the position of equilibrium. It depends only on temperature.
3) The reaction quotient, Q, is similar to K but uses the actual concentrations rather than equilibrium concentrations. Comparing Q to K indicates whether a reaction will proceed in the forward or reverse direction to reach equilibrium.
Chem 2 - Acid-Base Equilibria VIII: The Conjugate See-Saw and Analyzing Ka an...
Chem 2 - Acid-Base Equilibria VIII: The Conjugate See-Saw and Analyzing Ka and Kb for Acid or Base Relative Strength
Hsab theory
The document discusses the hard and soft acid and base (HSAB) theory introduced by Pearson in 1963. It explains that hard acids prefer to coordinate with hard bases, and soft acids prefer soft bases, due to their relative polarizabilities. Hard acids and bases are less polarizable, while soft species are more polarizable and form stronger bonds through electron sharing. The HSAB concept is used to understand stability, reactions, and reaction mechanisms based on qualitative descriptions of predominant factors like polarizability.
Chapter15
This document provides an overview of chapter 15 on acids and bases. It begins with an outline of the key concepts and sections to be covered, including the Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases. It then discusses acid and base strengths, factors that influence strength, and the concepts of conjugate acid-base pairs and amphiprotic species. Another section covers self-ionization of water and how pH is defined and calculated. Learning objectives are provided for each major topic.
4 concentration vs strength of acid bases
1) When acids or bases dissolve in water, they dissociate or break apart into ions. For acids, this takes the form HA + H2O ⇌ A- + H3O+.
2) Strong acids and bases dissociate completely in water, forming a high concentration of ions. Weak acids and bases only partially dissociate, forming a low concentration of ions.
3) A titration experiment determines the concentration of an unknown solution by neutralizing it with a solution of known concentration and tracking the equivalence point where [H+] = [OH-].
acid base indicators
The student conducted an experiment to determine which juices could serve as acid-base indicators by boiling various vegetables and fruits in water and observing color changes when vinegar or baking soda were added. Key findings were that rose, black bean, and spinach juices changed color noticeably, indicating they were good acid-base indicators, while carrot and white rice juices did not change color. The student learned that anthocyanin is often responsible for the color changes observed in acid-base indicators.
Chemical Equilibrium
The document discusses chemical equilibrium, including:
- When equilibrium is reached, concentrations of reactants and products remain constant, with the forward and reverse reaction rates being equal.
- Le Chatelier's principle states that applying stress (changing temperature, concentration, volume, or pressure) causes a system at equilibrium to shift in a way that reduces the stress.
- For example, increasing temperature shifts exothermic reactions toward reactants and endothermic reactions toward products.
Cmc chapter 17
This document provides an overview of three sections on chemical equilibrium from a chemistry textbook. Section 17.1 discusses the definition of chemical equilibrium as a state where forward and reverse reactions occur at equal rates. It also defines equilibrium constants and expressions. Section 17.2 explains how temperature, pressure, and concentration changes affect equilibrium based on Le Châtelier's principle. Section 17.3 discusses using equilibrium constants to determine concentrations and solubility products, and how the common ion effect impacts solubility.
Chemistryppt chemical equilibrium
The document discusses chemical equilibrium. It defines equilibrium as a state where the rates of the forward and reverse reactions of a chemical process are equal, resulting in no net change in the concentrations or properties of the system. It provides examples of physical and chemical equilibrium processes. It describes key characteristics of equilibrium like dynamic nature, constant concentrations and temperatures, and the relationship between reaction rates and equilibrium constants.
Acid base equilibria
This document discusses acid-base equilibria and titrations. It defines pH and pOH and their relationships to hydrogen and hydroxide ion concentrations. It describes the differences between strong acids, weak acids, and buffer solutions. It provides examples of preparing acidic and basic buffer solutions, such as an acetic acid-sodium acetate buffer. It also discusses acid-base indicators and their use in titrations, giving examples like methyl orange and phenolphthalein. Finally, it mentions the use of metallochromic indicators like Eriochrome Black T in titrations involving EDTA.
Chemical equillibrium
Equilibrium is a state in which there are no observable changes over time in a chemical system. At equilibrium, the concentrations of reactants and products remain constant. An equilibrium constant (K) can be defined based on the concentrations or pressures of reactants and products at equilibrium. The value of K is independent of initial concentrations and depends only on temperature. A change in concentration, pressure, volume, or temperature will shift the equilibrium in the direction that counteracts the applied stress according to Le Chatelier's principle.
Acid Etching of Enamel and Bond Strength
This document discusses acid etching of dental surfaces. It describes how acid etching was first proposed in 1955 to increase bond strength between composite resin and enamel. Acid etching removes enamel and creates an irregular porous surface that allows resin to penetrate through micromechanical interlocking, improving bond strength. Factors like acid type/concentration, etching duration, and fluoride levels can affect bonding. While acid etching is effective, some alternatives under investigation include crystal growth solutions, air abrasion, and lasers, but they have not achieved bond strengths as high as acid etching.
Chapter 15 Lecture- Chemical Equilibrium
1. The document discusses chemical equilibrium, including the concepts of equilibrium, depicting equilibrium reactions with equations, the equilibrium constant K, and how the value of K relates to whether a reaction favors reactants or products.
2. It also covers heterogeneous equilibria involving solids or liquids, how the concentrations of solids and liquids do not appear in equilibrium expressions, and examples of heterogeneous equilibrium reactions like the decomposition of calcium carbonate.
3. The key aspects covered are the definition of chemical equilibrium as when forward and reverse reactions proceed at the same rate, the use of concentration ratios and partial pressures to define equilibrium constants Kc and Kp, and how heterogeneous reactions involve gases in equilibrium with solids or liquids.
Chemical Equilibrium
The fundamentals of chemical equilibrium including Le Chatier's Principle and solved problems for heterogeneous and homogeneous equilibrium.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Viewers also liked (20)
VCE Chemistry Acids & Bases Concentration v Strength
VCE Chemistry Acids & Bases Concentration v Strength
Module 2: Définir la violence basée sur le genre (VBG)
Module 2: Définir la violence basée sur le genre (VBG)
Chem 2 - Acid-Base Equilibria VIII: The Conjugate See-Saw and Analyzing Ka an...
Chem 2 - Acid-Base Equilibria VIII: The Conjugate See-Saw and Analyzing Ka an...
More from St. Mary's HS
Metric system (1)
The document provides information about the metric system, including:
1) It is known as the SI system and is based on units of 10 with prefixes indicating multiples of 10.
2) It establishes standards for exact quantities of length, volume, mass, and time that people agree to use for comparison.
3) Derived units are obtained by combining SI units, like density which is mass divided by volume.
26sec3
The document discusses different types of carbonyl compounds including aldehydes, ketones, carboxylic acids, and esters. It covers their structures, naming conventions, properties, examples and how they are related through oxidation-reduction reactions. Aldehydes contain a carbonyl group bonded to at least one hydrogen, while ketones have the carbonyl group bonded to two carbon groups. Carboxylic acids contain both a carbonyl and hydroxyl group. Esters are derivatives of carboxylic acids where the hydroxyl is replaced by an alkoxy group from an alcohol.
26sec2
Alcohols contain an -OH functional group called a hydroxyl group. They are classified based on the number of carbon groups attached to the carbon bearing the hydroxyl. Alcohols exhibit hydrogen bonding and solubility in water. Common alcohols include isopropyl alcohol, ethylene glycol, glycerol, and ethanol. Ethers have the general formula R-O-R and are named by alphabetizing the two carbon groups. Examples include diethyl ether, which was historically used as an anesthetic.
26sec4
Polymers are large molecules formed from smaller molecules called monomers. There are two main types of polymers: addition polymers and condensation polymers. Addition polymers are formed when unsaturated monomers react through addition reactions, examples include polyethylene, polypropylene, polystyrene, and polyvinyl chloride. Condensation polymers are formed through condensation reactions with the loss of water or another small molecule, examples include polyethylene terephthalate, nylon, and Kevlar. Plastics are identified by code numbers that indicate the type of polymer resin used, such as PETE for polyethylene terephthalate in water bottles.
Ch 17 alternative energy sources
Solar energy is the sun's energy that is harnessed and can be used as an alternative to fossil fuels. The sun's energy comes from nuclear fusion reactions, with a small amount of mass converted to a large amount of energy. Only a tiny fraction of the sun's energy reaches Earth, mostly as infrared and visible light. This solar energy can be converted into thermal or electrical energy through the use of solar panels and collectors. While solar energy is clean and free, its intermittent nature and high costs have limited its widespread adoption. New technologies aim to improve solar energy storage to increase its viability as a renewable alternative energy source.
26sec3
The document discusses different types of carbonyl compounds including aldehydes, ketones, carboxylic acids, and esters. It provides their definitions and functional groups. Aldehydes have a carbonyl group bonded to at least one hydrogen, while ketones have the carbonyl group bonded to two carbons. Carboxylic acids contain both a carbonyl and hydroxyl group. Esters are derivatives of carboxylic acids where the hydroxyl is replaced by an alkoxy group from an alcohol. Oxidation and reduction reactions are also discussed, where oxidation involves a loss of hydrogen or gain of oxygen.
26sec2
Alcohols contain an -OH functional group called a hydroxyl group. They are classified based on the number of carbon groups attached to the carbon bearing the hydroxyl. Alcohols exhibit hydrogen bonding and solubility in water. Common alcohols include isopropyl alcohol, ethylene glycol, glycerol, and ethanol. Ethers have the general formula R-O-R and are named by alphabetizing the two carbon groups. Examples include diethyl ether, which was historically used as an anesthetic.
26sec1
The document discusses functional groups and substitution reactions in organic chemistry. It defines functional groups as specific arrangements of atoms that are capable of characteristic chemical reactions. It notes that organic compounds are best classified by their functional groups. It provides examples of common functional groups like alkyl groups and halogen substituents. It also describes substitution reactions where one atom or group replaces another, such as a halogen replacing hydrogen to form a halocarbon.
26sec4
Polymers are large molecules formed from smaller molecules called monomers. There are two main types of polymers: addition polymers and condensation polymers. Addition polymers are formed when unsaturated monomers react through addition reactions, examples include polyethylene, polypropylene, polystyrene, and polyvinyl chloride. Condensation polymers are formed through condensation reactions with the loss of water or another small molecule, examples include polyethylene terephthalate, nylon, and Kevlar. Plastics are identified by code numbers that indicate the type of polymer resin used, such as PETE for polyethylene terephthalate in water bottles.
16.2
Nuclear reactors are designed to generate electricity through nuclear fission. The core holds nuclear fuel rods and control rods, and uses coolant to generate steam that turns turbines to produce electricity. When uranium-239 is split in the active reactor zone, it produces plutonium-239 through a fission reaction harness by Einstein's equation relating mass and energy. Cooling towers then cool the steam for recycling in the process.
Ch 16
Nuclear energy involves subatomic particles like protons, neutrons and electrons that make up atoms. Atoms of the same element have the same number of protons but can have different numbers of neutrons, forming isotopes. Unstable isotopes become stable through radioactive emissions like alpha, beta, and gamma radiation of varying penetrating power that can be stopped by materials like skin, foil or concrete.
Ch 16 notes env.bio
This document contains questions about atomic structure, radioactivity, nuclear fission reactions, nuclear reactors, and nuclear waste. It asks about the subatomic particles that make up atoms, isotopes, radioactive decay, and the three types of radiation. It also asks about the process of nuclear fission, including what it is, what it produces, and how it can be depicted in a diagram. Finally, it addresses nuclear waste storage and disposal issues, as well as some historical nuclear accidents and their causes and impacts.
28.3
Fission and fusion are two types of nuclear reactions. Fission involves splitting heavy nuclei like U-235, releasing energy. It can be uncontrolled, as in atomic bombs, or controlled in nuclear power plants using moderators and control rods. Fusion combines light nuclei like hydrogen into heavier elements like helium and releases even more energy, but requires extremely high temperatures found in stars like the sun or experimental facilities on Earth.
28.2
Stable nuclei exist in the "band of stability" based on their neutron to proton ratio. Those with too many neutrons undergo beta decay to become more stable, while those with too many protons either capture electrons or emit positrons to become more stable. All nuclei above atomic number 83 are radioactive and undergo alpha decay. The half-life of a radioactive isotope is the time for half of it to decay, and varies greatly between isotopes. Nuclear transformations can occur naturally through radioactivity or artificially by bombarding nuclei with particles, allowing one element to be transformed into another.
28.1
This document summarizes key aspects of nuclear radiation and radioactive decay:
1) Radioactive decay occurs as unstable radioactive isotopes spontaneously emit radiation and decay into stable isotopes, releasing large amounts of energy in the process.
2) There are three main types of radiation emitted - alpha, beta, and gamma rays - which differ in their penetrating abilities and what they are composed of.
3) Radioactive decay challenges Dalton's atomic theory, which stated atoms are indivisible, as it involves atomic nuclei breaking down and emitting particles.
28.4
Ionizing radiation such as X-rays and radiation from radioisotopes can knock electrons off atoms and produce ions, but cannot be detected by human senses. Devices like Geiger counters, scintillation counters, and film badges can be used to detect and measure different types of ionizing radiation. Radiation has many uses including detecting trace elements, diagnosing and treating diseases like cancer, and tracing chemical reactions and the movement of substances in the body using radioactive tracers.
25sec4
This document discusses different types of hydrocarbon compounds. Cyclic hydrocarbons contain carbon chains attached to form rings, and are called "cyclo-" compounds. Aromatic hydrocarbons contain unsaturated carbon rings called arenes, with the simplest being benzene. Benzene has a six-carbon ring with alternating single and double bonds, and exhibits resonance due to the location of these bonds. Benzene derivatives are possible by substituting the ring with other groups like methyl, ethyl, or multiple groups including ortho, meta, and para positions.
25sec5
Natural gas and petroleum are fossil fuels formed from marine life buried in ocean sediments millions of years ago. Natural gas is primarily methane but also contains other alkanes like ethane and propane. It burns cleanly and is used widely for energy. Petroleum contains more complex hydrocarbons and must be refined to separate useful fractions like gasoline. Coal was formed from decaying plants over millions of years and ranges from peat to anthracite based on carbon content and other properties. It releases pollutants when burned but provides an important source of fuel.
25sec3
There are different types of isomerism including structural isomers, stereoisomers, geometric isomers, and optical isomers. Structural isomers have the same molecular formula but different structures. Stereoisomers have the same molecular structure but different arrangements of atoms in space. Geometric isomers differ in the geometry of substituted groups around a double bond, which can be in trans or cis configurations. Optical isomers contain asymmetric carbons and exist as left or right-handed stereoisomers.
25sec2
Alkenes and alkynes are types of unsaturated hydrocarbons. Alkenes contain carbon-carbon double bonds and have the general formula CnH2n. They are named with the suffix -ene and the double bond is given the lowest possible number. Alkynes contain carbon-carbon triple bonds and have the formula CnH2n-2. Acetylene is the simplest alkyne and is commonly used as fuel in torches.
More from St. Mary's HS (20)
Recently uploaded
مصحف القراءات العشر أعد أحرف الخلاف سمير بسيوني.pdf
مصحف أحرف الخلاف للقراء العشرةأعد أحرف الخلاف بالتلوين وصلا سمير بسيوني غفر الله له
HYPERTENSION - SLIDE SHARE PRESENTATION.
IT WILL BE HELPFULL FOR THE NUSING STUDENTS
IT FOCUSED ON MEDICAL MANAGEMENT AND NURSING MANAGEMENT.
HIGHLIGHTS ON HEALTH EDUCATION.
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as discipline
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...Nguyen Thanh Tu Collection
https://app.box.com/s/qhtvq32h4ybf9t49ku85x0n3xl4jhr15Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
Temple of Asclepius in Thrace. Excavation results
The temple and the sanctuary around were dedicated to Asklepios Zmidrenus. This name has been known since 1875 when an inscription dedicated to him was discovered in Rome. The inscription is dated in 227 AD and was left by soldiers originating from the city of Philippopolis (modern Plovdiv).
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...Nguyen Thanh Tu Collection
https://app.box.com/s/tacvl9ekroe9hqupdnjruiypvm9rdaneStack Memory Organization of 8086 Microprocessor
The stack memory organization of 8086 microprocessor.
How to deliver Powerpoint Presentations.pptx
"How to make and deliver dynamic presentations by making it more interactive to captivate your audience attention"
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Physical pharmaceutics notes for B.pharm students
Benner "Expanding Pathways to Publishing Careers"
This presentation was provided by Rebecca Benner, Ph.D., of the American Society of Anesthesiologists, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
Recently uploaded (20)
مصحف القراءات العشر أعد أحرف الخلاف سمير بسيوني.pdf
مصحف القراءات العشر أعد أحرف الخلاف سمير بسيوني.pdf
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
Juneteenth Freedom Day 2024 David Douglas School District
Juneteenth Freedom Day 2024 David Douglas School District
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
REASIGNACION 2024 UGEL CHUPACA 2024 UGEL CHUPACA.pdf
REASIGNACION 2024 UGEL CHUPACA 2024 UGEL CHUPACA.pdf
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
20sec4
- 1. 20.4 Strengths of Acids and Bases
- 2. Strength • Acids and Bases are classified according to the degree to which they ionize in water: –Strong are completely ionized in aqueous solution; this means they ionize 100 % –Weak ionize only slightly in aqueous solution • Strength is different from concentration
- 3. Strength • Strong – means it forms many ions when dissolved (100 % ionization) • Mg(OH)2 is a strong base- it falls completely apart when dissolved. –But, not much dissolves- so it is not concentrated
- 6. Measuring strength • Ionization is reversible. • HA ↔ H+ + A- • This makes an equilibrium • Acid dissociation constant = Ka • Ka = [H+ ][A- ] (water is constant) [HA] • Stronger acid = more products (ions), thus a larger Ka (Table 20.8, page 602)
- 7. What about bases? • Strong bases dissociate completely. • MOH ↔ M+ + OH- (M = a metal) • Base dissociation constant = Kb • Kb = [M+ ][OH- ] [MOH] • Stronger base = more dissociated ions are produced, thus a larger Kb.
- 8. Strength vs. Concentration • The words concentrated and dilute tell how much of an acid or base is dissolved in solution - refers to the number of moles of acid or base in a given volume • The words strong and weak refer to the extent of ionization of an acid or base • Is a concentrated weak acid possible?
- 9. Practice • Write the expression for HNO2 • Write the Kb for NH3 (as NH4OH)
- 10. - Page 610