This document discusses acids and bases according to different definitions:
- Arrhenius definition: acids produce H+ ions in water, bases produce OH- ions. Limited to aqueous solutions.
- Bronsted-Lowry definition: acids are proton donors, bases are proton acceptors. Acids and bases always come in pairs when reacting. This definition includes both aqueous and gas phase reactions.
- Amphoteric substances can act as both acids and bases through autoionization in water. The ion product constant Kw relates concentrations of H+ and OH- in water. The pH scale describes acidity and ranges from 0 to 14, with 7 being neutral.
This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.
This document discusses acids and bases, including:
- The Arrhenius definition of acids and bases as substances that increase H+ or OH- ions in water.
- The Brønsted-Lowry definition of acids as proton donors and bases as proton acceptors.
- Conjugate acid-base pairs that differ by the presence or absence of a proton.
- Amphoteric substances that can act as both acids and bases, such as water.
- The pH scale for measuring the concentration of hydrogen ions in a solution.
- Strong acids and bases that fully dissociate in water versus weak acids and bases that only partially dissociate.
This document outlines the key concepts and learning objectives for Chapter 16 on acid-base equilibria. It covers the acid-base properties of weak acids and bases in solution, including acid-ionization equilibria, polyprotic acids, and base-ionization equilibria. It also discusses acid-base properties of salt solutions, the common ion effect, buffers, and acid-base titration curves. The chapter provides the necessary background for students to write and balance acid-base reactions, determine equilibrium constants and concentrations of species, and perform acid-base calculations.
The document discusses different definitions of acids and bases, including:
1) Arrhenius definitions - acids produce H+ ions in water, bases produce OH- ions. Limited to aqueous solutions.
2) Bronsted-Lowry definitions - acids are H+ donors, bases are H+ acceptors. Acids and bases always come in pairs when reacting.
3) pH scale is used to express acidity because [H+] is usually very small. pH decreases as [H+] increases exponentially. Common substances are classified as acidic, basic, or neutral based on their pH.
The document discusses the properties and definitions of acids and bases. It defines acids as substances that produce hydrogen (H+) ions or hydronium (H3O+) ions in water. Acids taste sour and react with metals and carbonates. Bases produce hydroxide (OH-) ions in water, taste bitter and slippery, and feel soapy. Common strong acids include HNO3, HCl, and H2SO4. Strong acids and bases ionize completely in water. Weak acids and bases only partially ionize. pH is a measure of hydrogen ion concentration in solutions. The autoionization of water and the pH scale are also explained.
This document provides an overview of acid-base theories and key concepts such as:
[1] Arrhenius and Brønsted-Lowry definitions of acids and bases. Acids donate protons while bases accept protons.
[2] Water can act as both an acid and a base in different reactions due to its amphiprotic nature.
[3] Equilibria involving proton transfers favor the reaction where the proton moves to the stronger base. The position of equilibrium is determined by relative acid and base strengths.
This document covers Bronsted-Lowry acids and bases, conjugate acids and bases, and acid-base equilibrium. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. Conjugate acids are formed when a base gains a proton, and conjugate bases are formed when an acid loses a proton. Several examples of conjugate acid-base pairs are given. The document also discusses how the strength of an acid or base determines the position of acid-base equilibrium and the autoionization process and ion product constant for water.
Here are the ratios [HA]/[A-] required for each system to yield a pH of 4.30:
Acetic acid (pKa = 4.76): [HA]/[A-] = 1
Benzoic acid (pKa = 4.19): [HA]/[A-] = 1
Phthalic acid (pKa = 2.89): [HA]/[A-] is not possible since the pKa is too low.
The optimal system is acetic acid/sodium acetate since it has a pKa closest to the desired pH of 4.30. This system allows a ratio of [HA]/[A-] = 1, which provides maximum buffering
This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.
This document discusses acids and bases, including:
- The Arrhenius definition of acids and bases as substances that increase H+ or OH- ions in water.
- The Brønsted-Lowry definition of acids as proton donors and bases as proton acceptors.
- Conjugate acid-base pairs that differ by the presence or absence of a proton.
- Amphoteric substances that can act as both acids and bases, such as water.
- The pH scale for measuring the concentration of hydrogen ions in a solution.
- Strong acids and bases that fully dissociate in water versus weak acids and bases that only partially dissociate.
This document outlines the key concepts and learning objectives for Chapter 16 on acid-base equilibria. It covers the acid-base properties of weak acids and bases in solution, including acid-ionization equilibria, polyprotic acids, and base-ionization equilibria. It also discusses acid-base properties of salt solutions, the common ion effect, buffers, and acid-base titration curves. The chapter provides the necessary background for students to write and balance acid-base reactions, determine equilibrium constants and concentrations of species, and perform acid-base calculations.
The document discusses different definitions of acids and bases, including:
1) Arrhenius definitions - acids produce H+ ions in water, bases produce OH- ions. Limited to aqueous solutions.
2) Bronsted-Lowry definitions - acids are H+ donors, bases are H+ acceptors. Acids and bases always come in pairs when reacting.
3) pH scale is used to express acidity because [H+] is usually very small. pH decreases as [H+] increases exponentially. Common substances are classified as acidic, basic, or neutral based on their pH.
The document discusses the properties and definitions of acids and bases. It defines acids as substances that produce hydrogen (H+) ions or hydronium (H3O+) ions in water. Acids taste sour and react with metals and carbonates. Bases produce hydroxide (OH-) ions in water, taste bitter and slippery, and feel soapy. Common strong acids include HNO3, HCl, and H2SO4. Strong acids and bases ionize completely in water. Weak acids and bases only partially ionize. pH is a measure of hydrogen ion concentration in solutions. The autoionization of water and the pH scale are also explained.
This document provides an overview of acid-base theories and key concepts such as:
[1] Arrhenius and Brønsted-Lowry definitions of acids and bases. Acids donate protons while bases accept protons.
[2] Water can act as both an acid and a base in different reactions due to its amphiprotic nature.
[3] Equilibria involving proton transfers favor the reaction where the proton moves to the stronger base. The position of equilibrium is determined by relative acid and base strengths.
This document covers Bronsted-Lowry acids and bases, conjugate acids and bases, and acid-base equilibrium. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. Conjugate acids are formed when a base gains a proton, and conjugate bases are formed when an acid loses a proton. Several examples of conjugate acid-base pairs are given. The document also discusses how the strength of an acid or base determines the position of acid-base equilibrium and the autoionization process and ion product constant for water.
Here are the ratios [HA]/[A-] required for each system to yield a pH of 4.30:
Acetic acid (pKa = 4.76): [HA]/[A-] = 1
Benzoic acid (pKa = 4.19): [HA]/[A-] = 1
Phthalic acid (pKa = 2.89): [HA]/[A-] is not possible since the pKa is too low.
The optimal system is acetic acid/sodium acetate since it has a pKa closest to the desired pH of 4.30. This system allows a ratio of [HA]/[A-] = 1, which provides maximum buffering
This document outlines the key concepts and learning objectives for Chapter 17, which covers solubility equilibria and complex-ion equilibria. The chapter will examine how to determine solubility product constants (Ksp) and use them to calculate solubility. It will also explore how the common ion effect and pH can impact solubility. The chapter will then discuss the formation of complex ions and how they relate to solubility and precipitation. It concludes by looking at applications to qualitative metal ion analysis.
The document discusses various concepts related to aqueous equilibria including:
1) The common ion effect where adding a strong electrolyte containing a common ion with a weak electrolyte decreases the ionization of the weak electrolyte.
2) Buffers and how they resist pH changes through reactions of the weak acid/base with added strong acid or base.
3) Solubility products (Ksp) and how solubility is affected by factors like common ions, pH, and complex ion formation.
The document provides information about acids and bases, including:
1) It defines acids as proton donors and bases as proton acceptors. It lists the formulas and dissociation equations of common acids like sulfuric acid, nitric acid, and ethanoic acid as well as bases like potassium hydroxide and calcium hydroxide.
2) It defines terms like acid, base, alkali and explains that alkalis are soluble bases that release hydroxide ions in water.
3) It discusses acid-base reactions and neutralization reactions where acids and bases react to form water and a salt. It also introduces the concept of conjugate acid-base pairs.
B sc_I_General chemistry U-II Ionic equilibria in aqueous solution Rai University
This document provides an overview of acids, bases, and pH. It defines acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. Acids are substances that produce H+ ions in water or donate protons in reactions, while bases produce OH- ions or accept protons. The document also discusses acid and base strength, pH, self-ionization of water, and using pH to calculate hydrogen or hydroxide ion concentrations. Common examples like acids in orange juice and blood pH are provided.
This document discusses several key topics regarding bases:
1. The hydroxides of Group 1 and 2 elements are strong bases, with NaOH and KOH being common laboratory reagents. The alkaline earth hydroxides have low solubility.
2. Calculating the pH of a solution involves determining the hydroxide ion concentration from any reacting species. A 5.0x10-2 M NaOH solution has a pH of 12.70.
3. Many bases other than hydroxides can produce hydroxide ions through reaction with water, such as ammonia. Calculations for weak bases are similar to weak acids.
4. Salts can behave as acids or bases depending on
This document provides definitions and explanations of key concepts related to acids and bases:
- Arrhenius and Brønsted-Lowry definitions of acids and bases are introduced. Acids donate protons while bases accept protons.
- When an acid dissolves in water, it donates a proton to form the conjugate base and hydronium ion. Strong acids fully dissociate while weak acids only partially dissociate.
- pH is defined as the negative log of the hydronium ion concentration. A solution's pH depends on whether it has a higher or lower hydronium ion concentration than pure water.
- Dissociation constants (Ka for acids and Kb for bases) describe the
1. This document discusses acid-base theories including Arrhenius, Bronsted-Lowry, and acid-base equilibria.
2. It explains the ion product constant of water (Kw) and how pH and pOH scales are used to measure hydrogen and hydroxide ion concentrations.
3. Weak acids and bases only partially dissociate in water and their equilibria are expressed using acid (Ka) and base (Kb) dissociation constants.
The document discusses naming acids. It divides acids into binary and oxyacids. Binary acids contain two elements, while oxyacids contain three elements including oxygen. Oxyacids are named based on their "-ate" ion, with variations indicating one more, one less, or two less oxygen atoms than the reference "-ic" acid. Common "-ate" ions include sulfate, nitrate, chlorate, and phosphate.
This document discusses acid-base chemistry and provides information on different acid-base theories, acid and base strength, pH calculations, and polyprotic acids. It includes definitions, examples, and practice problems related to these topics. Key points covered include the Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases, definitions of strong and weak acids/bases, calculations for pH and pOH, and the stepwise dissociation of polyprotic acids. Practice problems are provided throughout for calculating pH, pOH, and acid/base ionization constants.
This document provides an overview of acids and bases according to different theories:
1) Arrhenius concept defines acids and bases as compounds that release H+ and OH- ions in water.
2) Bronsted-Lowry concept defines acids as proton donors and bases as proton acceptors in any reaction.
3) Lewis concept defines acids as electron pair acceptors and bases as electron pair donors, forming coordinate covalent bonds.
Buffer solutions maintain pH upon addition of small amounts of acid or base and are important in biological systems like blood plasma.
This document discusses acid-base theories and concepts such as:
1) Arrhenius, Brønsted-Lowry, and Lewis acid-base theories. It also discusses acid-base behavior in water and provides examples of strong acids and weak acids.
2) Key concepts like pH, pKa, dissociation constants (Ka and Kb), and relationships between Ka, Kb, and Kw.
3) Calculations involving Ka, Kb, pH, and pKa including determining concentrations and dissociation constants from initial concentrations and pH/pOH values.
4) The concepts of hydrolysis, polyprotic acids, and titration of weak acids vs bases.
Lect w7 152_abbrev_ intro to acids and bases_algchelss
This document provides an overview of acids and bases, including:
- Water can act as both an acid and a base in chemical reactions.
- The autoionization of water establishes an equilibrium expression relating [H3O+] and [OH-].
- Adding acids or bases shifts the equilibrium by changing [H3O+] or [OH-] while maintaining the same Kw expression.
- pH is a measure of acidity and is defined as -log[H3O+], with lower pH indicating higher acidity.
The document discusses key concepts regarding acids and bases including: Bronsted-Lowery acids and bases, conjugate acid-base pairs, the pH scale, strong and weak acids and bases, acid-base properties of salts, and Lewis acids and bases. Key equations discussed include the ionization of water and the autoionization constant Kw. Sample problems are provided for calculating pH, percentage of ionization, and acid and base dissociation constants.
This document provides an overview of acids and bases for a high school chemistry rapid learning series. It defines acids and bases based on Arrhenius, Brønsted-Lowry, and Lewis theories. It discusses strong versus weak acids and bases, and how concentrated or dilute solutions affect strength. Conjugate acids and bases are defined. Common strong acids and bases are listed. Properties of acids and bases like taste and effect on litmus are covered. The pH scale is introduced and calculating pH of strong acids and bases is demonstrated. How salts can have acidic, basic, or neutral properties is explained. Finally, buffers and how they resist pH change are described.
This document discusses various topics relating to aqueous equilibria, including the common ion effect, buffers, titrations, solubility products, and factors that affect solubility. It provides examples of calculations for concentrations and pH involving these concepts and explains how precipitation of ions from solution can be used to separate mixtures.
This document provides an overview of acids and bases for an AP Chemistry course. It begins with definitions of acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. It then distinguishes between strong and weak acids/bases, as well as concentrated and dilute solutions. Conjugate acids and bases are defined. Equilibrium concepts such as acid dissociation constants (Ka) and base dissociation constants (Kb) are introduced, and their relationships to strength are explained. The autoionization of water and the water dissociation constant (Kw) are covered. Finally, the logarithmic pH scale is defined.
1. The document discusses acid-base concepts including the Brønsted-Lowry theory of acids and bases. It defines Arrhenius, Brønsted-Lowry acids and bases, and conjugate acid-base pairs.
2. Factors that influence acid strength are examined, including bond polarity, bond strength, and structural features of oxoacids and carboxylic acids.
3. The autoionization of water is discussed, including the ion product constant Kw and its implications for solutions being acidic, basic, or neutral.
This document summarizes key concepts about acids and bases from a chemistry textbook chapter:
1. It defines acids as substances that produce H+ ions in aqueous solution and bases as substances that produce OH- ions. Strong acids and bases dissociate completely while weak acids and bases dissociate partially.
2. The pH scale is introduced and used to classify solutions as acidic, basic or neutral. Common acid-base reactions like neutralization and self-ionization of water are described.
3. Key acid-base concepts are explained like Brønsted-Lowry acids and bases, conjugate acid-base pairs, acid-base equilibria, and the importance of pH buffers in biological systems like
This document summarizes key concepts about acids and bases from a chemistry textbook chapter:
1. It defines acids as substances that produce H+ ions in aqueous solution and bases as substances that produce OH- ions. Strong acids and bases fully dissociate while weak ones partially dissociate.
2. The pH scale is introduced and used to classify solutions as acidic, basic or neutral. Henderson-Hasselbalch equation relates pH, pKa, and concentrations of weak acids and their conjugate bases in buffer solutions.
3. Key acid-base concepts covered include Brønsted-Lowry definitions, conjugate acid-base pairs, acid-base equilibria, self-ionization of water,
This document outlines the key concepts and learning objectives for Chapter 17, which covers solubility equilibria and complex-ion equilibria. The chapter will examine how to determine solubility product constants (Ksp) and use them to calculate solubility. It will also explore how the common ion effect and pH can impact solubility. The chapter will then discuss the formation of complex ions and how they relate to solubility and precipitation. It concludes by looking at applications to qualitative metal ion analysis.
The document discusses various concepts related to aqueous equilibria including:
1) The common ion effect where adding a strong electrolyte containing a common ion with a weak electrolyte decreases the ionization of the weak electrolyte.
2) Buffers and how they resist pH changes through reactions of the weak acid/base with added strong acid or base.
3) Solubility products (Ksp) and how solubility is affected by factors like common ions, pH, and complex ion formation.
The document provides information about acids and bases, including:
1) It defines acids as proton donors and bases as proton acceptors. It lists the formulas and dissociation equations of common acids like sulfuric acid, nitric acid, and ethanoic acid as well as bases like potassium hydroxide and calcium hydroxide.
2) It defines terms like acid, base, alkali and explains that alkalis are soluble bases that release hydroxide ions in water.
3) It discusses acid-base reactions and neutralization reactions where acids and bases react to form water and a salt. It also introduces the concept of conjugate acid-base pairs.
B sc_I_General chemistry U-II Ionic equilibria in aqueous solution Rai University
This document provides an overview of acids, bases, and pH. It defines acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. Acids are substances that produce H+ ions in water or donate protons in reactions, while bases produce OH- ions or accept protons. The document also discusses acid and base strength, pH, self-ionization of water, and using pH to calculate hydrogen or hydroxide ion concentrations. Common examples like acids in orange juice and blood pH are provided.
This document discusses several key topics regarding bases:
1. The hydroxides of Group 1 and 2 elements are strong bases, with NaOH and KOH being common laboratory reagents. The alkaline earth hydroxides have low solubility.
2. Calculating the pH of a solution involves determining the hydroxide ion concentration from any reacting species. A 5.0x10-2 M NaOH solution has a pH of 12.70.
3. Many bases other than hydroxides can produce hydroxide ions through reaction with water, such as ammonia. Calculations for weak bases are similar to weak acids.
4. Salts can behave as acids or bases depending on
This document provides definitions and explanations of key concepts related to acids and bases:
- Arrhenius and Brønsted-Lowry definitions of acids and bases are introduced. Acids donate protons while bases accept protons.
- When an acid dissolves in water, it donates a proton to form the conjugate base and hydronium ion. Strong acids fully dissociate while weak acids only partially dissociate.
- pH is defined as the negative log of the hydronium ion concentration. A solution's pH depends on whether it has a higher or lower hydronium ion concentration than pure water.
- Dissociation constants (Ka for acids and Kb for bases) describe the
1. This document discusses acid-base theories including Arrhenius, Bronsted-Lowry, and acid-base equilibria.
2. It explains the ion product constant of water (Kw) and how pH and pOH scales are used to measure hydrogen and hydroxide ion concentrations.
3. Weak acids and bases only partially dissociate in water and their equilibria are expressed using acid (Ka) and base (Kb) dissociation constants.
The document discusses naming acids. It divides acids into binary and oxyacids. Binary acids contain two elements, while oxyacids contain three elements including oxygen. Oxyacids are named based on their "-ate" ion, with variations indicating one more, one less, or two less oxygen atoms than the reference "-ic" acid. Common "-ate" ions include sulfate, nitrate, chlorate, and phosphate.
This document discusses acid-base chemistry and provides information on different acid-base theories, acid and base strength, pH calculations, and polyprotic acids. It includes definitions, examples, and practice problems related to these topics. Key points covered include the Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases, definitions of strong and weak acids/bases, calculations for pH and pOH, and the stepwise dissociation of polyprotic acids. Practice problems are provided throughout for calculating pH, pOH, and acid/base ionization constants.
This document provides an overview of acids and bases according to different theories:
1) Arrhenius concept defines acids and bases as compounds that release H+ and OH- ions in water.
2) Bronsted-Lowry concept defines acids as proton donors and bases as proton acceptors in any reaction.
3) Lewis concept defines acids as electron pair acceptors and bases as electron pair donors, forming coordinate covalent bonds.
Buffer solutions maintain pH upon addition of small amounts of acid or base and are important in biological systems like blood plasma.
This document discusses acid-base theories and concepts such as:
1) Arrhenius, Brønsted-Lowry, and Lewis acid-base theories. It also discusses acid-base behavior in water and provides examples of strong acids and weak acids.
2) Key concepts like pH, pKa, dissociation constants (Ka and Kb), and relationships between Ka, Kb, and Kw.
3) Calculations involving Ka, Kb, pH, and pKa including determining concentrations and dissociation constants from initial concentrations and pH/pOH values.
4) The concepts of hydrolysis, polyprotic acids, and titration of weak acids vs bases.
Lect w7 152_abbrev_ intro to acids and bases_algchelss
This document provides an overview of acids and bases, including:
- Water can act as both an acid and a base in chemical reactions.
- The autoionization of water establishes an equilibrium expression relating [H3O+] and [OH-].
- Adding acids or bases shifts the equilibrium by changing [H3O+] or [OH-] while maintaining the same Kw expression.
- pH is a measure of acidity and is defined as -log[H3O+], with lower pH indicating higher acidity.
The document discusses key concepts regarding acids and bases including: Bronsted-Lowery acids and bases, conjugate acid-base pairs, the pH scale, strong and weak acids and bases, acid-base properties of salts, and Lewis acids and bases. Key equations discussed include the ionization of water and the autoionization constant Kw. Sample problems are provided for calculating pH, percentage of ionization, and acid and base dissociation constants.
This document provides an overview of acids and bases for a high school chemistry rapid learning series. It defines acids and bases based on Arrhenius, Brønsted-Lowry, and Lewis theories. It discusses strong versus weak acids and bases, and how concentrated or dilute solutions affect strength. Conjugate acids and bases are defined. Common strong acids and bases are listed. Properties of acids and bases like taste and effect on litmus are covered. The pH scale is introduced and calculating pH of strong acids and bases is demonstrated. How salts can have acidic, basic, or neutral properties is explained. Finally, buffers and how they resist pH change are described.
This document discusses various topics relating to aqueous equilibria, including the common ion effect, buffers, titrations, solubility products, and factors that affect solubility. It provides examples of calculations for concentrations and pH involving these concepts and explains how precipitation of ions from solution can be used to separate mixtures.
This document provides an overview of acids and bases for an AP Chemistry course. It begins with definitions of acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. It then distinguishes between strong and weak acids/bases, as well as concentrated and dilute solutions. Conjugate acids and bases are defined. Equilibrium concepts such as acid dissociation constants (Ka) and base dissociation constants (Kb) are introduced, and their relationships to strength are explained. The autoionization of water and the water dissociation constant (Kw) are covered. Finally, the logarithmic pH scale is defined.
1. The document discusses acid-base concepts including the Brønsted-Lowry theory of acids and bases. It defines Arrhenius, Brønsted-Lowry acids and bases, and conjugate acid-base pairs.
2. Factors that influence acid strength are examined, including bond polarity, bond strength, and structural features of oxoacids and carboxylic acids.
3. The autoionization of water is discussed, including the ion product constant Kw and its implications for solutions being acidic, basic, or neutral.
This document summarizes key concepts about acids and bases from a chemistry textbook chapter:
1. It defines acids as substances that produce H+ ions in aqueous solution and bases as substances that produce OH- ions. Strong acids and bases dissociate completely while weak acids and bases dissociate partially.
2. The pH scale is introduced and used to classify solutions as acidic, basic or neutral. Common acid-base reactions like neutralization and self-ionization of water are described.
3. Key acid-base concepts are explained like Brønsted-Lowry acids and bases, conjugate acid-base pairs, acid-base equilibria, and the importance of pH buffers in biological systems like
This document summarizes key concepts about acids and bases from a chemistry textbook chapter:
1. It defines acids as substances that produce H+ ions in aqueous solution and bases as substances that produce OH- ions. Strong acids and bases fully dissociate while weak ones partially dissociate.
2. The pH scale is introduced and used to classify solutions as acidic, basic or neutral. Henderson-Hasselbalch equation relates pH, pKa, and concentrations of weak acids and their conjugate bases in buffer solutions.
3. Key acid-base concepts covered include Brønsted-Lowry definitions, conjugate acid-base pairs, acid-base equilibria, self-ionization of water,
This document provides an overview of acid-base theories and chemistry. It defines acids and bases according to three main theories:
1) Arrhenius theory defines acids as substances that donate H+ ions in water and bases as those that donate OH- ions.
2) Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors, providing a better explanation of substances like ammonia.
3) Lewis theory defines acids as electron pair acceptors and bases as electron pair donors, explaining both traditional acids/bases and coordination compounds.
The document then discusses acid/base reactions and equilibrium expressions, relative acid/base strengths, and the differences between strong vs. weak acids and
AP Chemistry The Chemistry Of Acids And BasesLeonard Goudy
This document provides an overview of acids and bases including:
- Definitions of acids and bases according to Arrhenius, Bronsted-Lowry, and Lewis theories. The Bronsted-Lowry theory is the main one used.
- Explanations of strong vs weak acids and bases, and how acid/base strength relates to conjugate acid-base pairs.
- A discussion of water's autoionization and how it relates to the pH scale, which is used to measure hydrogen ion concentration.
- Examples of calculating hydrogen and hydroxide ion concentrations and pH for various acid and base solutions.
This document discusses acid-base equilibria, including weak acids, weak bases, and water. It explains how weak acids and bases form equilibrium reactions in water, and defines the equilibrium constants KA and KB. It also describes how water forms an equilibrium with a constant of KW. Additionally, it introduces conjugate acids and bases and how acid-base reactions can produce new materials with acidic or basic properties. Finally, it provides an example of calculating the pH of a sodium acetate solution through considering its hydrolysis equilibrium.
Chem 2 - Acid-Base Equilibria I: The Basics of Acids and BasesLumen Learning
This document discusses the basics of acids and bases according to three definitions:
1) Arrhenius definition - acids produce H3O+ in water and bases produce OH- in water.
2) Brønsted-Lowry definition - acids donate protons and bases accept protons.
3) Lewis definition - acids accept electron pairs and bases donate electron pairs.
It also covers the pH scale, differences between strong and weak acids/bases, and conjugate acid-base pairs. Neutralization reactions between acids and bases are described.
This document provides an overview of acids and bases including:
- The Arrhenius, Bronsted-Lowry, and Lewis models of acids and bases
- Key concepts such as conjugate acid-base pairs, acid dissociation constants, and the pH scale
- How to calculate the pH of strong acid solutions, weak acid solutions, and solutions involving conjugate acid-base pairs
- Common strong/weak acids and bases and their properties
The document explains acid and base chemistry concepts thoroughly and provides practice problems to illustrate applications of these concepts.
This document provides definitions and information about acids and bases:
- It defines acids and bases according to Arrhenius and Brønsted-Lowry theories. Acids donate protons while bases accept protons.
- When an acid dissolves in water, it donates a proton to form its conjugate base and hydronium ion. Reactions between acids and bases yield conjugate acid-base pairs.
- Strong acids fully dissociate in water while weak acids only partially dissociate. The strength of an acid or base determines which direction a proton transfer equilibrium will favor.
- Water autoionizes to a small extent, forming hydronium and hydroxide ions. The ion
B sc i chemistry i u ii ionic equilibria in aqueous solution aRai University
This document provides an overview of acids, bases, and pH. It defines acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. Acids are substances that produce H+ ions in water or donate protons in reactions, while bases produce OH- ions or accept protons. The document also discusses acid and base strength, pH, self-ionization of water, and examples of calculating pH from H+ concentration and vice versa. Common acids, bases, and pH indicators are listed.
This document discusses acids and bases, including:
1) Strong acids like HCl completely dissociate in water, while weak acids like acetic acid only partly dissociate and retain most of their protons.
2) Strong acids have weak conjugate bases, while weak acids have strong conjugate bases. Strong bases have weak conjugate acids, while weak bases have strong conjugate acids.
3) The acid dissociation constant (Ka) describes the equilibrium between an acid and its ions, with weaker acids having smaller Ka values and stronger acids having larger Ka values.
This document discusses strong and weak acids and bases, and their dissociation in water. It provides examples of common strong acids (HCl, H2SO4, HNO3) and weak acids (acetic acid), and indicates that strong acids fully dissociate while weak acids only partially dissociate. It asks which would produce more hydrogen ions, 1M HCl or 1M acetic acid, and indicates HCl is the strong acid. Finally, it discusses conjugate acid-base pairs and their relative strength.
1. There are three classes of strong electrolytes: strong acids, strong bases, and most water soluble salts. Weak acids and bases only partially dissociate in water.
2. pH is a measure of the concentration of hydrogen ions [H+] in a solution. Low pH indicates high [H+] and an acidic solution, while high pH indicates low [H+] and a basic solution. Household substances like coffee, milk, and baking soda have different pH values.
3. The acid dissociation constant Ka and base dissociation constant Kb are equilibrium constants that indicate the strength of an acid or base. Strong acids and bases fully dissociate while weak acids and bases only partially dissociate,
The document discusses strong versus weak acids and bases. Strong acids and bases completely dissociate in water, while weak acids and bases only partially dissociate. Strong acids have a weak conjugate base, while weak acids have a strong conjugate base. The document provides examples of strong and weak acids such as hydrochloric acid (HCl), sulfuric acid (H2SO4), nitric acid (HNO3), and acetic acid (CH3COOH, vinegar).
1. The document discusses acid-base theories including Arrhenius, Brønsted-Lowry, and Lewis theories. It also defines terms related to acid-base titrations such as titration, standard solution, titrant, equivalence point, and indicator.
2. Key concepts around acid-base equilibria are explained, including the autoionization of water and the dissociation constants for weak acids and bases (Ka and Kb). The Henderson-Hasselbalch equation relating pH and the concentrations of conjugate acid-base pairs in a buffer solution is also derived.
3. Methods for determining the endpoint in an acid-base titration are described, including the use of acid-
This document contains information about strong vs weak acids and bases:
1) Strong acids like HCl completely dissociate in water, producing more hydrogen ions (H+), while weak acids like acetic acid only partly dissociate and most remain attached to hydrogen ions.
2) Strong bases like NaOH completely dissociate in water, while weak bases like NH3 only partly dissociate.
3) Acid and base strength is determined by their dissociation constants, Ka for acids and Kb for bases. Strong acids and bases have higher dissociation constants since they dissociate more completely.
This document provides an introduction to acids and bases, including:
1) How acids and bases are defined according to the Arrhenius, Bronsted-Lowry, and Lewis theories. Acids donate protons while bases accept protons.
2) Examples of strong acids like HCl and weak acids like acetic acid. Strong acids fully dissociate in water while weak acids only partially dissociate.
3) The pH scale measures hydrogen ion concentration from 0-14, with lower values being more acidic and higher more basic. Neutral solutions have a pH of 7.
1. The document discusses acids and bases according to the Arrhenius and Brønsted-Lowry definitions. It describes the key characteristics of acids and bases and provides examples of strong and weak acids and bases.
2. Neutralization reactions between acids and bases are discussed as double displacement reactions that produce water and a salt. Examples of reactions between acids and hydroxide or carbonate bases are provided.
3. The document explains why both the Arrhenius and Brønsted-Lowry definitions are useful, noting their relative strengths and limitations. Key concepts like conjugate acid-base pairs and amphoteric substances are also introduced.
This document provides an overview of acid-base equilibria, including:
- Definitions of acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories.
- A discussion of auto-ionization of water and the pH scale. Weak acids only partially dissociate in water according to their acid dissociation constant, Ka.
- Explanations of acid-base terminology like conjugate acid-base pairs and the effect of relative acid strength on the direction of acid-base reactions.
- Examples of calculating quantities like [H3O+], pH, pKa, and determining the direction of acid-base reactions.
The document
Chemistry - Chp 19 - Acids, Bases, and Salt - PowerPointsMel Anthony Pepito
This document provides an overview of acids and bases including:
1) It defines acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories and compares their properties.
2) It explains how hydrogen and hydroxide ion concentrations determine if a solution is neutral, acidic, or basic and how pH and pOH scales relate to these concentrations.
3) It describes how acid strength relates to acid dissociation constants and distinguishes between strong and weak acids.
Similar to Ch14z5eacidbase 110115231543-phpapp01 (20)
This document discusses suffixes and terminology used in medicine. It begins by listing common combining forms used to build medical terms and their meanings. It then defines several noun, adjective, and shorter suffixes and provides their meanings. Examples are given of medical terms built using combining forms and suffixes. The document also examines specific medical concepts in more depth, such as hernias, blood cells, acromegaly, splenomegaly, and laparoscopy.
The document is a chapter from a medical textbook that discusses anatomical terminology pertaining to the body as a whole. It defines the structural organization of the body from cells to tissues to organs to systems. It also describes the body cavities and identifies the major organs contained within each cavity, as well as anatomical divisions of the abdomen and back.
This document is from a textbook on medical terminology. It discusses the basic structure of medical words and how they are built from prefixes, suffixes, and combining forms. Some key points:
- Medical terms are made up of elements including roots, suffixes, prefixes, and combining vowels. Understanding these elements is important for analyzing terms.
- Common prefixes include hypo-, epi-, and cis-. Common suffixes include -itis, -algia, and -ectomy.
- Dozens of combining forms are provided, such as gastro- meaning stomach, cardi- meaning heart, and aden- meaning gland.
- Rules are provided for analyzing terms, such as reading from the suffix backward and dropping combining vowels before suffixes starting with vowels
This document is the copyright information for Chapter 25 on Cancer from the 6th edition of the textbook Molecular Cell Biology published in 2008 by W. H. Freeman and Company. The chapter was authored by a team that includes Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 24 on Immunology from the 6th edition of the textbook Molecular Cell Biology published in 2008 by W. H. Freeman and Company. The chapter was authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
Nerve cells, also known as neurons, are highly specialized cells that process and transmit information through electrical and chemical signals. This chapter discusses the structure and function of neurons, how they communicate with each other via synapses, and how signals are propagated along neurons through changes in their membrane potentials. Neurons play a vital role in the nervous system by allowing organisms to process information and coordinate their responses.
This document is the copyright information for Chapter 22 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "The Molecular Cell Biology of Development" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 21 from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Cell Birth, Lineage, and Death" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright page for Chapter 20 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Regulating the Eukaryotic Cell Cycle" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 19 from the 6th edition textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Integrating Cells into Tissues" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This chapter discusses microtubules and intermediate filaments, which are types of cytoskeletal filaments that help organize and move cellular components. Microtubules are involved in processes like cell division and intracellular transport, while intermediate filaments provide mechanical strength and help integrate the nucleus with the cytoplasm. Together, these filaments play important structural and functional roles in eukaryotic cells.
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This document is the copyright page for Chapter 16 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Signaling Pathways that Control Gene Activity" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This document is the copyright page for Chapter 15 of the 6th edition textbook "Molecular Cell Biology" by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira. It provides the chapter title "Cell Signaling I: Signal Transduction and Short-Term Cellular Responses" and notes the copyright is held by W. H. Freeman and Company in 2008.
This document is the copyright page for Chapter 14 from the 6th edition textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Vesicular Traffic, Secretion, and Endocytosis" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This chapter discusses how proteins are transported into membranes and organelles within cells. Proteins destined for membranes or organelles have targeting signals that are recognized by transport systems. The transport systems then direct the proteins to their proper destinations, such as inserting membrane proteins into membranes or delivering soluble proteins into organelles.
This document is the copyright information for Chapter 12 from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Cellular Energetics" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This chapter discusses the transmembrane transport of ions and small molecules across cell membranes. It covers topics such as passive transport through membrane channels and pumps, as well as active transport using ATP. The chapter is from the 6th edition of the textbook Molecular Cell Biology and is copyrighted by W. H. Freeman and Company in 2008.
This document is the copyright information for Chapter 10, titled "Biomembrane Structure", from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter was written by a team of authors including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This document is the copyright information for Chapter 9 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Visualizing, Fractionating, and Culturing Cells" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
How to Manage Your Lost Opportunities in Odoo 17 CRMCeline George
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
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This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
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You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
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Answers about how you can do more with Walmart!"
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
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LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
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
How to Fix the Import Error in the Odoo 17Celine George
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
2. 2
Z5e 14.1 The Nature of Acids and BasesZ5e 14.1 The Nature of Acids and Bases
Arrhenius DefinitionArrhenius Definition
Acids produce hydrogen ions inAcids produce hydrogen ions in
aqueous solution.aqueous solution.
Bases produce hydroxide ions whenBases produce hydroxide ions when
dissolved in water.dissolved in water.
Limited to aqueous solutions.Limited to aqueous solutions.
Only one kind of base (hydroxide).Only one kind of base (hydroxide).
NHNH33 ammonia could not be anammonia could not be an
Arrhenius base.Arrhenius base.
http://www.youtube.com/watch?v=h2UczzWu-Qs&mode=related&searchhttp://www.youtube.com/watch?v=h2UczzWu-Qs&mode=related&search==
3. 3
Bronsted-Lowry DefinitionsBronsted-Lowry Definitions
AnAn acidacid is an proton (His an proton (H++
)) donordonor and aand a
basebase is a protonis a proton acceptoracceptor..
Acids and bases always come inAcids and bases always come in pairspairs..
HCl is an acid.HCl is an acid.
When it dissolves in water it gives itsWhen it dissolves in water it gives its
proton to water (so Hproton to water (so H22O is a base).O is a base).
HClHCl(g)(g) + H+ H22OO(l)(l) →→ HH33OO++
+ Cl+ Cl--
Water is aWater is a basebase: makes hydronium ion: makes hydronium ion
5. 5
Bronsted-Lowry Acids
Acids are hydrogen ion (H+)
donors
Bases are hydrogen ion (H+
) acceptors
HCl + H2O H3O+
+ Cl-
donor acceptor + -
+ +
6. 6
NH3, A Bronsted-Lowry Base
When NH3 reacts with water, most of the
reactants remain dissolved as molecules, but a
few NH3 reacts with water to form NH4
+
and
hydroxide ion.
NH3 + H2O NH4
+
(aq) + OH-
(aq)
acceptor donor
+ +
7. 7
B. Definitions pp
Brønsted-Lowry
HCl + H2O → Cl–
+ H3O+
• AcidsAcids are proton (H+
) donors.
• BasesBases are proton (H+
) acceptors.
conjugate acid
conjugate base
baseacid
13. 13
PairsPairs pppp
General equationGeneral equation
HA(aq) + HHA(aq) + H22O(l)O(l) HH33OO++
(aq) + A(aq) + A--
(aq)(aq)
Acid + BaseAcid + Base Conjugate acid +Conjugate acid +
Conjugate baseConjugate base
This is an equilibrium.This is an equilibrium.
CompetitionCompetition forfor HH++
betweenbetween HH22O and AO and A--
The stronger base controls direction.The stronger base controls direction.
If HIf H22O is a stronger base it takes the HO is a stronger base it takes the H++
Equilibrium moves to right.Equilibrium moves to right.
14. 14
Acid dissociation constant KAcid dissociation constant Kaa
The equilibrium constant for theThe equilibrium constant for the
general equation.general equation.
HA(aq) + HHA(aq) + H22O(l)O(l) HH33OO1+1+
(aq) + A(aq) + A1-1-
(aq)(aq)
KKaa = [H= [H33OO++
][A][A--
]]
[HA][HA]
HH33OO++
is often written His often written H++
ignoring theignoring the
water in equation (it is implied).water in equation (it is implied).
16. 16
Acid dissociation constant KAcid dissociation constant Kaa
HA(aq)HA(aq) HH++
(aq) + A(aq) + A--
(aq)(aq)
KKaa = [H= [H++
][A][A--
]]
[HA][HA]
We can write the expression for anyWe can write the expression for any
acid.acid.
Strong acids dissociate completely.Strong acids dissociate completely.
Equilibrium far to right.Equilibrium far to right.
Conjugate base must be weak.Conjugate base must be weak.
17. 17
Figure 14.5Figure 14.5
Acid StrengthAcid Strength
Versus ConjugateVersus Conjugate
Base StrengthBase Strength z5e 661z5e 661
18. 18
Z5e 14.2 Acid StrengthZ5e 14.2 Acid Strength
Strong acidsStrong acids
KKaa is largeis large
[H[H++
] is about equal] is about equal
toto originaloriginal [HA][HA]
AA--
is a weaker baseis a weaker base
than waterthan water
Weak acidsWeak acids
KKaa is smallis small
[H[H++
] <<< [HA]] <<< [HA]
AA--
is a stronger baseis a stronger base
than waterthan water
19. 19
Z5e Figure 14.4 p. 661Z5e Figure 14.4 p. 661 pppp
GraphicGraphic
Representation ofRepresentation of
the Behavior ofthe Behavior of
Acids of DifferentAcids of Different
Strengths inStrengths in
Aqueous SolutionAqueous Solution
((a) = strong acid,a) = strong acid,
completecomplete
dissociation.dissociation.
((b) = weak acid,b) = weak acid,
slight dissociationslight dissociation..
20. 20
Which of the following
"molecular" pictures, “A”
or “B”, best represents
a concentrated solution
of the weak acid HA
with Ka = 10-5
? . . .
“B”, because . . .
There are more
molecules of
undissociated form.
“A” represents a strong
acid.
21. 21
Types of AcidsTypes of Acids
Polyprotic AcidsPolyprotic Acids - more than 1 acidic- more than 1 acidic
hydrogen (diprotic, triprotic).hydrogen (diprotic, triprotic).
OxyacidsOxyacids - Proton is attached to the- Proton is attached to the
oxygen of an ion.oxygen of an ion.
Organic acidsOrganic acids contain the Carboxylcontain the Carboxyl
group -COOH with the H attached to Ogroup -COOH with the H attached to O
Polyprotic acids are generally veryPolyprotic acids are generally very
weak (but, Hweak (but, H22SOSO44 is strong with 1is strong with 1stst
HH++
and weak with 2and weak with 2ndnd
).).
22. 22
Relative Base Strength of AcidsRelative Base Strength of Acids pppp
Using Table 14.2 p. 628, arrange theUsing Table 14.2 p. 628, arrange the
following in increasingfollowing in increasing basebase strength.strength.
HH22OO,, FF1-1-
, Cl, Cl1-1-
, NO, NO22
1-1-
, CN, CN1-1-
Steps . . .Steps . . .
Hint: Strongest acid will have weakestHint: Strongest acid will have weakest
base. Which conjugate of the abovebase. Which conjugate of the above
bases would be the strongest acid? . . .bases would be the strongest acid? . . .
That’s right, HCl. So, ClThat’s right, HCl. So, Cl1-1-
must be themust be the
weakestweakest base.base.
23. 23
Relative Base Strength of AcidsRelative Base Strength of Acids pppp
Arrange HArrange H22OO,, FF1-1-
, Cl, Cl1-1-
, NO, NO22
1-1-
, CN, CN1-1-
inin
increasingincreasing basebase strength.strength.
Considering HConsidering H22OO,, the others arethe others are
conjugate bases ofconjugate bases of weakweak acids, so theacids, so the
above bases must beabove bases must be strongerstronger thanthan
water acting as a base. So . . .water acting as a base. So . . .
ClCl--
< water < conjugate bases of weak< water < conjugate bases of weak
acids . . .acids . . .
24. 24
Relative Base Strength of AcidsRelative Base Strength of Acids pppp
Arrange HArrange H22OO,, FF1-1-
, Cl, Cl1-1-
, NO, NO22
1-1-
, CN, CN1-1-
inin
increasingincreasing basebase strength.strength.
ClCl--
< water < conj. bases of weak acids.< water < conj. bases of weak acids.
Now, use Table 14.2 p. 628 to “order”Now, use Table 14.2 p. 628 to “order”
the rest. Your answer is . . .the rest. Your answer is . . .
ClCl--
< H< H22O < FO < F1-1-
< NO< NO22
1-1-
< CN< CN1-1-
25. 25
AmphotericAmphoteric
Behaves as acid & base -- autoionizesBehaves as acid & base -- autoionizes
2H2H22O(l)O(l) HH33OO++
(aq) + OH(aq) + OH--
(aq)(aq)
KKWW= [H= [H33OO++
][OH][OH--
]=[H]=[H++
][OH][OH--
]]
HH22OO(l)(l) drops out of =m expression since itdrops out of =m expression since it
is a pure liquidis a pure liquid
At 25ºC KAt 25ºC KWW = 1.0 x10= 1.0 x10-14-14
inin EVERYEVERY aqueousaqueous
solution.solution.
KKww = ion product constant (or dissociation= ion product constant (or dissociation
constant)constant)
So, we can use it to find [HSo, we can use it to find [H++
] and [OH] and [OH--
]]
27. 27
Autoionization of Water problemAutoionization of Water problem
KKww = 1 x 10= 1 x 10-13-13
at 60ºC. Using Le Chatelier,at 60ºC. Using Le Chatelier,
predict if exo- or endothermicpredict if exo- or endothermic 2H2H22OO(l)(l)
HH33OO1+1+
(aq)(aq) + OH+ OH1-1-
(aq)(aq) Hint:Hint:
compare Kcompare Kww at 25ºC.at 25ºC.
Endothermic since KEndothermic since Kww increases withincreases with
temperature so energy is a reactant.temperature so energy is a reactant.
28. 28
Autoionization of Water problemAutoionization of Water problem
KKww = 1 x 10= 1 x 10-13-13
at 60ºC.at 60ºC.
2H2H22OO(l)(l) HH33OO1+1+
(aq)(aq) + OH+ OH1-1-
(aq)(aq)
Calculate [HCalculate [H++
] & [OH] & [OH--
] in] in neutralneutral soln.soln.
Hint: since neutral, they must be equal.Hint: since neutral, they must be equal.
Answer . . .Answer . . .
3 x 103 x 10-7-7
MM since [Hsince [H++
] [OH] [OH--
] = 1 x 10] = 1 x 10-13-13
29. 29
Figure 14.7Figure 14.7
Two Water Molecules React to FormTwo Water Molecules React to Form
HH33OO++
and OHand OH--
30. 30
Z5e 14.3 The pH ScaleZ5e 14.3 The pH Scale
pH= -log[HpH= -log[H++
]]
Used because [HUsed because [H++
] is usually very small] is usually very small
As pHAs pH decreasesdecreases, [H, [H++
]] increasesincreases
exponentiallyexponentially
Sig figs: Only the digitsSig figs: Only the digits afterafter thethe
decimal place of a pH are significant!decimal place of a pH are significant!
[H[H++
] = 1.0 x 10] = 1.0 x 10-8-8
pH= 8.00pH= 8.00 22 sig figssig figs
pOH= -log[OHpOH= -log[OH--
]]
pKa = -log KpKa = -log Kaa
31. 31
A solution with pH = 5 is 100 times more
acidic than a solution with a pH = ?
A) 7 B) 3 C) 0.05
• 7 because . . .
• 7 is 2 pH units more basic so 100 times
less [H3O1+
] (or 100 x more [OH1-
]
32. 32
RelationshipsRelationships pppp
KKWW = [H= [H++
][OH][OH--
]]
-log K-log KWW = -log([H= -log([H++
][OH][OH--
])])
-log K-log KWW = -log[H= -log[H++
]+ -log[OH]+ -log[OH--
]]
pKpKWW = pH + pOH= pH + pOH
KKWW = 1.0 x10= 1.0 x10-14-14
14.00 = pH + pOH14.00 = pH + pOH
[H[H++
] = 10] = 10-pH-pH
and [OHand [OH--
] = 10] = 10-pOH-pOH
[H[H++
],[OH],[OH--
],pH and pOH: Given any one],pH and pOH: Given any one
33. 33
Figure 14.8Figure 14.8
The pH Scale and pHThe pH Scale and pH
Values of SomeValues of Some
Common SubstancesCommon Substances
35. 35
Calculating pH of SolutionsCalculating pH of Solutions
AlwaysAlways write down the major specieswrite down the major species
in solution. If you forget you’llin solution. If you forget you’ll
probably get a wrong solution!probably get a wrong solution!
Remember, these are equilibria.Remember, these are equilibria.
Remember the chemistry.Remember the chemistry.
Don’t try to memorize, there is no oneDon’t try to memorize, there is no one
way to do this.way to do this.
36. 36
Calculating pH of SolutionsCalculating pH of Solutions
The pH of a blood sample was 7.41 atThe pH of a blood sample was 7.41 at
25ºC. Calculate pOH, [H25ºC. Calculate pOH, [H1+1+
] and [OH] and [OH1-1-
].].
Answers? . . .Answers? . . .
pOH = 6.59pOH = 6.59 (14 - 7.41 = 6.59) [H(14 - 7.41 = 6.59) [H1+1+
] = ?] = ?
[H[H1+1+
] = 3.9 x 10] = 3.9 x 10-8-8
(10(10-7.41-7.41
)) [OH[OH1-1-
] = ?] = ?
[OH[OH1-1-
] = 2.6 x 10] = 2.6 x 10-7-7
Either 10Either 10-6.59-6.59
or since Kor since Kww ==
[H[H1+1+
][OH][OH1-1-
],], [OH[OH1-1-
] = 10] = 10-14-14
/3.9 x 10/3.9 x 10-8-8
37. 37
z5e 14.4 Calculating the pH of Strong Acidsz5e 14.4 Calculating the pH of Strong Acids pppp
HBr, HI, HCl, HNOHBr, HI, HCl, HNO33, H, H22SOSO44, HClO, HClO44
ALWAYS WRITE THE MAJOR SPECIESALWAYS WRITE THE MAJOR SPECIES
Above are completely dissociated (strong acids)Above are completely dissociated (strong acids)
So, [HSo, [H++
] =] = originaloriginal [HA][HA]
[OH[OH--
] is going to be small because of] is going to be small because of
equilibrium (essentially none since shifted so farequilibrium (essentially none since shifted so far
to the right)to the right)
1010-14-14
= [H= [H++
][OH][OH--
]]
If [HA] < 10If [HA] < 10-7-7
thenthen waterwater contributes Hcontributes H++
andand
must be taken into account!!!must be taken into account!!!
38. 38
Strong AcidsStrong Acids pppp
Calculate the pH of 1.0 x 10Calculate the pH of 1.0 x 10-10-10
MM HCl. Ans.?HCl. Ans.?
pH = 7.00. Why? . . .pH = 7.00. Why? . . .
Always write the major species, which are . . .Always write the major species, which are . . .
HH22O, HO, H1+1+
and Cland Cl1-1-
Both contribute HBoth contribute H1+1+
But, the [HCl] is so small thatBut, the [HCl] is so small that it has no effectit has no effect!!
Essentially all the HEssentially all the H1+1+
is coming from water.is coming from water.
So, pH = 7.00.So, pH = 7.00.
39. 39
Z5e 14.5 Calculating the pH of Weak AcidsZ5e 14.5 Calculating the pH of Weak Acids pppp
Ka will be small.Ka will be small.
ALWAYS WRITE THE MAJOR SPECIESALWAYS WRITE THE MAJOR SPECIES..
It will be an equilibrium problemIt will be an equilibrium problem fromfrom
the startthe start (and shifted to the(and shifted to the leftleft).).
Determine whether most of the HDetermine whether most of the H++
willwill
come from the acid or the water!come from the acid or the water!
Compare to Ka or Kw per aboveCompare to Ka or Kw per above
Rest is just like last chapter (see,Rest is just like last chapter (see,
summary next slide)summary next slide)
41. 41
ExampleExample pppp
Calculate the pH of 2.0Calculate the pH of 2.0 MM acetic acid HCacetic acid HC22HH33OO22
with a Ka 1.8 x10with a Ka 1.8 x10-5-5
Steps. . .Steps. . .
Major species are . . .Major species are . . .
HCHC22HH33OO22 & H& H22O. pH answer is . . . (use RICE)O. pH answer is . . . (use RICE)
pH = 2.22pH = 2.22
Calculate pOH, [OHCalculate pOH, [OH--
], [H], [H++
] Ans. are . . .] Ans. are . . .
pOH = 11.78pOH = 11.78
[OH[OH--
] = 1.7 x 10] = 1.7 x 10-12-12
[H[H++
] = 6.0 x 10] = 6.0 x 10-3-3
42. 42
A mixture of Weak AcidsA mixture of Weak Acids pppp
The process is the same.The process is the same.
Determine the major species.Determine the major species.
The stronger will predominate.The stronger will predominate.
So, use bigger Ka if concentrations areSo, use bigger Ka if concentrations are
comparable (comparable (i.e.,i.e., can ignore smaller Ka)can ignore smaller Ka)
43. 43
A mixture of Weak AcidsA mixture of Weak Acids pppp
Calculate the pH of aCalculate the pH of a mixturemixture of 1.20of 1.20 MM
HF (Ka = 7.2 x 10HF (Ka = 7.2 x 10-4-4
) and 3.4) and 3.4 MM HOCHOC66HH55
(Ka = 1.6 x 10(Ka = 1.6 x 10-10-10
))
Major species: HF, HOCMajor species: HF, HOC66HH55, H, H22OO
Since HF is the dominant producer ofSince HF is the dominant producer of
HH++
, use its Ka, use its Ka
Set up “RICE” table, useSet up “RICE” table, use
approximations and 5% rule to get . . .approximations and 5% rule to get . . .
[H[H++
] = .030 & pH = 1.53] = .030 & pH = 1.53
44. 44
A mixture of Weak AcidsA mixture of Weak Acids pppp
Calculate theCalculate the [OC[OC66HH55
1-1-
]] of a mixture ofof a mixture of
1.201.20 MM HF (Ka = 7.2 x 10HF (Ka = 7.2 x 10-4-4
) and 3.4) and 3.4 MM
HOCHOC66HH55 (Ka = 1.6 x 10(Ka = 1.6 x 10-10-10
))
Use Ka and “RICE” for HOCUse Ka and “RICE” for HOC66HH55,, butbut
remember that [Hremember that [H++
] concentration came] concentration came
fromfrom bothboth acidsacids
So, 1.6 x 10So, 1.6 x 10-10-10
= (= (0.0300.030)(x)/(3.4))(x)/(3.4)
[OC[OC66HH55
1-1-
] = . . .] = . . .
45. 45
Percent dissociationPercent dissociation pppp
== amount dissociatedamount dissociated x 100%x 100%
initialinitial concentrationconcentration
For aFor a weakweak acid percent dissociationacid percent dissociation increasesincreases
as acid becomesas acid becomes more dilutemore dilute..
Calculate the % dissociation of 1.00Calculate the % dissociation of 1.00 MM andand
0.1000.100 MM Acetic acid (Ka = 1.8 x 10Acetic acid (Ka = 1.8 x 10-5-5
). Ans. . .). Ans. . .
% diss 1.00% diss 1.00 MM = 0.42%, 0.00100= 0.42%, 0.00100 MM = 1.3%= 1.3%
As [HA]As [HA]00 decreases [Hdecreases [H++
]] decreasesdecreases but %but %
dissociationdissociation increasesincreases..
Le Chatelier’s principle operates hereLe Chatelier’s principle operates here
46. 46
The other wayThe other way pppp
What is the Ka of a weak acid that isWhat is the Ka of a weak acid that is
8.1 % dissociated as 0.1008.1 % dissociated as 0.100 MM solution?solution?
Ans. . .Ans. . .
6.6 x 106.6 x 10-4-4
Solving method . . .Solving method . . .
Since (X/0.100)(100%) = 8.1%,Since (X/0.100)(100%) = 8.1%,
x = 8.1 x 10x = 8.1 x 10-3-3
= [H= [H++
] = [A] = [A--
]]
Then plug into =m to solve for Ka.Then plug into =m to solve for Ka.
(8.1 x 10(8.1 x 10-3-3
))22
÷ 0.100 = 6.6 x 10÷ 0.100 = 6.6 x 10-4-4
(remember, divide by initial [ ])(remember, divide by initial [ ])
47. 47
Figure 14.10Figure 14.10
p. 643.p. 643.
The Effect ofThe Effect of
Dilution onDilution on
the Percentthe Percent
DissociationDissociation
and (H+) of aand (H+) of a
Weak AcidWeak Acid
SolutionSolution
48. 48
Z5e 14.6 BasesZ5e 14.6 Bases
The OHThe OH--
is a strong base.is a strong base.
Hydroxides of theHydroxides of the alkalialkali metals aremetals are
strong bases because they dissociatestrong bases because they dissociate
completely when dissolved.completely when dissolved.
The hydroxides ofThe hydroxides of alkaline earthsalkaline earths
Ca(OH)Ca(OH)22 etc. are strong dibasic bases,etc. are strong dibasic bases,
butbut they don’t dissolve well in water.they don’t dissolve well in water.
So, used as antacids because [OHSo, used as antacids because [OH--
] can’t] can’t
build up with them, which would hurtbuild up with them, which would hurt
the stomach lining..the stomach lining..
49. 49
BasesBases withoutwithout OHOH--
B-L bases are protonB-L bases are proton acceptorsacceptors..
NHNH33 + H+ H22OO NHNH44
++
+ OH+ OH--
It is the lone pair on nitrogen (N:) thatIt is the lone pair on nitrogen (N:) that
accepts the proton.accepts the proton.
Many weak bases contain NMany weak bases contain N
BB(aq)(aq) + H+ H22O(l)O(l) BHBH++
(aq)(aq) + OH+ OH--
(aq)(aq)
KKbb = [= [BHBH++
][][OHOH--
]]
[[BB]]
50. 50
Strength of BasesStrength of Bases
N:
Hydroxides are strong.Hydroxides are strong.
Others are weak.Others are weak.
SmallerSmaller KKbb == weaker base.weaker base.
Calculate the pH of a solution of 4.0Calculate the pH of a solution of 4.0 MM
pyridinepyridine (K(Kbb = 1.7 x 10= 1.7 x 10-9-9
). Answer . . .). Answer . . .
51. 51
Strength of BasesStrength of Bases
Calculate the pH of a solution of 4.0Calculate the pH of a solution of 4.0 MM
pyridine (Kpyridine (Kbb = 1.7 x 10= 1.7 x 10-9-9
)) DidDid
you get pH = 4.08?you get pH = 4.08?
Oops!!!Oops!!!
You got pYou got pOHOH = 4.08 (= 4.08 (from [OHfrom [OH1-1-
] = 1.2 x 10] = 1.2 x 10-10-10
-- you were given K-- you were given Kbb))
pH = 14 - pOH = 9.92pH = 14 - pOH = 9.92
This makes sense since pyridine is aThis makes sense since pyridine is a
weakweak basebase! (so, high pH)! (so, high pH)
52. 52
Z5e 14.7 Polyprotic acidsZ5e 14.7 Polyprotic acids pppp
These always dissociateThese always dissociate stepwisestepwise..
TheThe firstfirst HH++
comes offcomes off muchmuch easiereasier thanthan
the second.the second.
So, the KSo, the Kaa for the first step is muchfor the first step is much
bigger than Ka for the second.bigger than Ka for the second.
Denoted KaDenoted Ka11, Ka, Ka22, Ka, Ka33
Overall K = KaOverall K = Ka11•Ka•Ka22•Ka•Ka33 . . .. . . (AP quest)(AP quest)
For a typical polyprotic acid in HFor a typical polyprotic acid in H220,0,
only the 1st dissociation step isonly the 1st dissociation step is
important in determining the pHimportant in determining the pH
53. 53
Polyprotic acidPolyprotic acid
HH22COCO33 HH++
+ HCO+ HCO33
--
KaKa11= 4.3 x 10= 4.3 x 10-7-7
HCOHCO33
--
HH++
+ CO+ CO33
-2-2
KaKa22= 4.3 x 10= 4.3 x 10-10-10
The base in first step is acid in second.The base in first step is acid in second.
InIn pHpH calculations we cancalculations we can normallynormally
ignore the second dissociation.ignore the second dissociation.
But, you may have to calculate KaBut, you may have to calculate Ka11 andand
KaKa22 in Lab 14, depending on your acid.in Lab 14, depending on your acid.
54. 54
Calculate the ConcentrationCalculate the Concentration pppp
Of all the ions in a solution of 1.00Of all the ions in a solution of 1.00 MM
Arsenic acid HArsenic acid H33AsOAsO44
KaKa11 = 5.0 x 10= 5.0 x 10-3-3
KaKa22 = 8.0 x 10= 8.0 x 10-8-8
KaKa33 = 6.0 x 10= 6.0 x 10-10-10
Steps. . .Steps. . .
What’s the first step? . . .What’s the first step? . . .
Write the major species, which are . . .Write the major species, which are . . .
HH22O and HO and H33AsOAsO44
55. 55
Calculate the ConcentrationCalculate the Concentration pppp
Of all the ions in a solution of 1.00Of all the ions in a solution of 1.00 MM
Arsenic acid HArsenic acid H33AsOAsO44
Write the =m expression for HWrite the =m expression for H33AsOAsO44 . . .. . .
HH33AsOAsO44 HH1+1+
+ H+ H22AsOAsO44
1-1-
xx22
/ [H/ [H33AsOAsO44] = K] = Ka1a1 = 5.0 x 10= 5.0 x 10-3-3
x = 7.1 x 10x = 7.1 x 10-2-2
= [H= [H1+1+
]] andand [H[H22AsOAsO44
1-1-
]]
56. 56
Calculate the ConcentrationCalculate the Concentration pppp
Of all the ions in a solution of 1.00Of all the ions in a solution of 1.00 MM
Arsenic acid HArsenic acid H33AsOAsO44
Now, write =m expression for HNow, write =m expression for H22AsOAsO44
1-1-
HH22AsOAsO44
1-1-
HH1+1+
+ HAsO+ HAsO44
2-2-
We cannot useWe cannot use xx22
/ [H/ [H22AsOAsO44
1-1-
] = K] = Ka2a2
Why?Why?
[H[H1+1+
] ≠ [HAsO] ≠ [HAsO44
2-2-
] because we have [H] because we have [H1+1+
] of] of
7.1 x 107.1 x 10-2-2
from thefrom the firstfirst =m.=m.
57. 57
Calculate the ConcentrationCalculate the Concentration pppp
Of all the ions in a solution of 1.00Of all the ions in a solution of 1.00 MM
Arsenic acid HArsenic acid H33AsOAsO44
HH22AsOAsO44
1-1-
HH1+1+
+ HAsO+ HAsO44
2-2-
[H[H1+1+
][HAsO][HAsO44
2-2-
]/[H]/[H22AsOAsO44
1-1-
] = . . .] = . . .
(7.1 x 10(7.1 x 10-2-2
)(x) = k)(x) = ka2a2 = 8.0 x 10= 8.0 x 10-8-8
7.1 x 107.1 x 10-2-2
So, x = [HAsOSo, x = [HAsO44
2-2-
] = k] = ka2a2
This is important forThis is important for titrationstitrations..
58. 58
Calculate the ConcentrationCalculate the Concentration pppp
Of all the ions in a solution of 1.00 MOf all the ions in a solution of 1.00 M
Arsenic acid HArsenic acid H33AsOAsO44..
You do it for the last KYou do it for the last Ka3a3 = 6.0 x 10= 6.0 x 10-10-10
[AsO[AsO44
3-3-
] = ???] = ???
6.8 x 106.8 x 10-16-16
from (x)(7.1 x 10from (x)(7.1 x 10-2-2
) = 6.0 x 10) = 6.0 x 10-10-10
8.0 x 108.0 x 10-8-8
59. 59
Sulfuric acid is specialSulfuric acid is special
InIn firstfirst step it is astep it is a strongstrong acid.acid.
In the second step, KaIn the second step, Ka22 = 1.2 x 10= 1.2 x 10-2-2
Calculate the [ ]s of theCalculate the [ ]s of the major speciesmajor species in ain a
3.03.0 MM solution of Hsolution of H22SOSO44. Answer . . .. Answer . . .
Both [HBoth [H++
] and [HSO4] and [HSO4--
] are 3.0] are 3.0 MM, since, since
completely dissociated.completely dissociated.
We can neglect the effect of the 2nd stepWe can neglect the effect of the 2nd step
because it is so small (<5%) compared tobecause it is so small (<5%) compared to
the 1st step complete disassociation.the 1st step complete disassociation.
60. 60
Sulfuric acid is specialSulfuric acid is special
In first step it is a strong acid.In first step it is a strong acid.
In the second step, KaIn the second step, Ka22 = 1.2 x 10= 1.2 x 10-2-2
Calculate the concentrations in a 2.0Calculate the concentrations in a 2.0 x 10x 10-3-3
MM solution of Hsolution of H22SOSO44 (tricky: why?)(tricky: why?)
SinceSince dilutedilute, the 2nd step, the 2nd step doesdoes contributecontribute
HH++
, so quadratic expression must be used, so quadratic expression must be used
because Kabecause Ka22 is not small enough tois not small enough to
simplify the expression.simplify the expression.
A pre-test question requires you to use theA pre-test question requires you to use the
quadratic for an Hquadratic for an H22SOSO44 problem.problem.
61. 61
Z5e 14.8 Salts as acids and basesZ5e 14.8 Salts as acids and bases
Salts areSalts are ionicionic compounds.compounds.
Salts of theSalts of the cationcation ofof strongstrong basesbases andand
thethe anionanion ofof strongstrong acidsacids are neutral.are neutral.
for example, NaCl, KNOfor example, NaCl, KNO33
There isThere is no equilibriumno equilibrium forfor strongstrong acidsacids
and bases.and bases.
So, we can ignore the reverse reaction.So, we can ignore the reverse reaction.
62. 62
BasicBasic SaltsSalts
If theIf the anionanion of a salt is the conjugate base of aof a salt is the conjugate base of a
weakweak acidacid →→ basicbasic solution.solution.
In an aqueous solution of NaFIn an aqueous solution of NaF
thethe major speciesmajor species are Naare Na++
, F, F--
, and H, and H22OO
FF--
+ H+ H22OO HF + OHHF + OH--
KKbb =[HF][=[HF][OHOH--
]]
[F[F--
]]
but Kbut Kaa = [= [HH++
][F][F--
]]
[HF][HF]
66. 66
Basic SaltsBasic Salts
KKaa x Kx Kbb = [HF][OH= [HF][OH--
]] x [Hx [H++
][F][F--
]]
[F[F--
]] [HF][HF]
KKaa x Kx Kbb =[OH=[OH--
] [H] [H++
]]
67. 67
Basic SaltsBasic Salts
KKaa x Kx Kbb = [HF][OH= [HF][OH--
]] x [Hx [H++
][F][F--
]]
[F[F--
]] [HF][HF]
KKaa x Kx Kbb = [OH= [OH--
] [H] [H++
]]
Since [OHSince [OH--
] [H] [H++
] = K] = KWW
KKaa x Kx Kbb = K= KWW
68. 68
KKaa tells us Ktells us Kbb pppp
Calculate the pH of 1.00Calculate the pH of 1.00 MM NaCN.NaCN.
KKaa of HCN is 6.2 x 10of HCN is 6.2 x 10-10-10
Answer . . .Answer . . .
Answer: pH = 11.60. Here’s why . . .Answer: pH = 11.60. Here’s why . . .
The anion of a weak acid is a weakThe anion of a weak acid is a weak
base. Why? Consider the above:base. Why? Consider the above:
2 reactions:2 reactions: (1) dissociation of HCN(1) dissociation of HCN
(2) CN(2) CN--
reacting with Hreacting with H22O.O.
The CNThe CN--
ion competes with OHion competes with OH--
for Hfor H++
Base strength = OHBase strength = OH--
> CN> CN--
> H> H22O.O.
69. 69
KKaa tells us Ktells us Kbb pppp
Calculate the pH of a solution of 1.00Calculate the pH of a solution of 1.00 MM NaCN.NaCN.
KKaa of HCN is 6.2 x 10of HCN is 6.2 x 10-10-10
Ans. pH = 11.60Ans. pH = 11.60
Write major species: NaWrite major species: Na1+1+
, CN, CN1-1-
and Hand H22OO
Set up =m betweenSet up =m between anionanion and waterand water
CNCN1-1-
+ HOH+ HOH HCN + OHHCN + OH1-1-
Since product includes hydroxide ion, mustSince product includes hydroxide ion, must
use Kuse Kbb so need to get from Kso need to get from Kaa (using K(using Kww))
Calculate hydroxide concentration, convert toCalculate hydroxide concentration, convert to
pOH,pOH, subtract from 14 to get pHsubtract from 14 to get pH
70. 70
AcidicAcidic saltssalts
A salt with the cation of aA salt with the cation of a weakweak base and thebase and the
anion of aanion of a strongstrong acid will beacid will be acidicacidic..
The same development as bases leads toThe same development as bases leads to
KKaa x Kx Kbb = K= KWW
Other acidic salts are those of highly chargedOther acidic salts are those of highly charged
metal ions (e.g., aluminum ion -- 3+).metal ions (e.g., aluminum ion -- 3+).
More on this later.More on this later.
71. 71
Acidic saltsAcidic salts pppp
Calculate the pH of a solution of 0.40Calculate the pH of a solution of 0.40 MM NHNH44Cl (the KCl (the Kbb
of NHof NH33 1.8 x 101.8 x 10-5-5
). Steps). Steps
How do we know the correct =m rxn to use? . . .How do we know the correct =m rxn to use? . . .
Write the major species! NHWrite the major species! NH44
1+1+
, Cl, Cl1-1-
, H, H22OO
ClCl--
isis notnot conj. base of WA, but of SA (no equilibrium),conj. base of WA, but of SA (no equilibrium),
so look at NHso look at NH44
++
which is the CA of WB.which is the CA of WB.
Since NHSince NH44
++
isis a major species and NHa major species and NH33 isn’t, the =misn’t, the =m
must be: NHmust be: NH44
++
NHNH33 + H+ H++
and use Kand use Kaa
So,So, don’tdon’t use NHuse NH33 + OH+ OH1-1-
NHNH44
1+1+
or Kor Kbb !!!!
Use KUse Kaa x Kx Kbb = K= Kww to calculate Kto calculate Kaa
Answer for pH is . . .Answer for pH is . . .
72. 72
Anion of weak acid, cation of weak baseAnion of weak acid, cation of weak base
KKaa > K> Kbb acidicacidic
KKaa < K< Kbb basicbasic
KKaa = K= Kbb NeutralNeutral
See Table 14.6, p. 660 for summarySee Table 14.6, p. 660 for summary
74. 74
Z5e 14.9 Structure & Acid base PropertiesZ5e 14.9 Structure & Acid base Properties
A molecule with an H in it is aA molecule with an H in it is a potentialpotential acid.acid.
TheThe strongerstronger the X-Hthe X-H bondbond thethe lessless acidicacidic;; i.e.i.e.,,
more basic (compare bond dissociationmore basic (compare bond dissociation
energies).energies).
TheThe more polarmore polar the X-H bond thethe X-H bond the stronger thestronger the
acidacid (use electronegativities).(use electronegativities).
The more polar H-O-X bond - stronger acid.The more polar H-O-X bond - stronger acid.
75. 75
Strength of oxyacidsStrength of oxyacids
The more oxygen hooked to the centralThe more oxygen hooked to the central
atom, the more acidic the hydrogen.atom, the more acidic the hydrogen.
HClOHClO44 > HClO> HClO33 > HClO> HClO22 > HClO> HClO
Remember that the H is attached to anRemember that the H is attached to an
oxygen atom (oxygen atom (notnot the central atom).the central atom).
The oxygens are electronegative.The oxygens are electronegative.
So, they pull electrons away fromSo, they pull electrons away from
hydrogenhydrogen
80. 80
Hydrated metalsHydrated metals
Highly chargedHighly charged
metalmetal ionsions pull thepull the
electrons ofelectrons of
surrounding watersurrounding water
molecules towardmolecules toward
them.them.
Makes it easier forMakes it easier for
HH++
to come off.to come off.
Al+3 O
H
H
82. 82
Z5e 14.10 Acid-Base Properties of OxidesZ5e 14.10 Acid-Base Properties of Oxides
Non-metalNon-metal oxides dissolved in wateroxides dissolved in water
can make acids.can make acids.
SOSO33(g) + H(g) + H22O(l)O(l) HH22SOSO44(aq)(aq)
IonicIonic (e.g., metal) oxides dissolve in(e.g., metal) oxides dissolve in
water to produce bases.water to produce bases.
CaO(s) + HCaO(s) + H22O(l)O(l) Ca(OH)Ca(OH)22(aq)(aq)
83. 83
Z5e 14.11 Lewis Acids and BasesZ5e 14.11 Lewis Acids and Bases
Most general definition.Most general definition.
Acids are electron pair acceptors.Acids are electron pair acceptors.
Bases are electron pair donors.Bases are electron pair donors.
B F
F
F
:N
H
H
H
84. 84
Lewis Acids and BasesLewis Acids and Bases
Boron trifluoride wants more electrons.Boron trifluoride wants more electrons.
B F
F
F
:N
H
H
H
85. 85
Lewis Acids and BasesLewis Acids and Bases
Boron trifluoride wants more electrons.Boron trifluoride wants more electrons.
BFBF33 is Lewis base NHis Lewis base NH33 is a Lewis Acid.is a Lewis Acid.
BF
F
F
N
H
H
H
86. 86
B. Definitions
Lewis
• AcidsAcids are electron pair acceptors.
• BasesBases are electron pair donors.
Lewis
base
Lewis
acid
87. 87
Lewis Acids and BasesLewis Acids and Bases
Al+3
( )
H
H
O
Al
( )6
H
H
O
+ 6
+3
88. 88
Z5e 14.12 Strategy for solving Acid-Z5e 14.12 Strategy for solving Acid-
Base ProblemsBase Problems pppp
What major species are present?What major species are present?
Does a reaction occur that can beDoes a reaction occur that can be
assumed to go to completion?assumed to go to completion?
What equilibriumWhat equilibrium dominatesdominates thethe
solution?solution?
See guide on next slide and page 667.See guide on next slide and page 667.
89. 89
Z5e Solving Acid-Base Problems p. 667Z5e Solving Acid-Base Problems p. 667 pppp
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Editor's Notes
Z5e 14.1 658 The Nature of Acids and Bases
Alternative link if can’t get through to YouTube:
http://dailycackle.com/2007/01/20/science-experiment-gone-wrong/
Z53 Fig. 14.1 659: reaction of HCl and H20
Z5e 660 SE 14.1 a, c, e
Z5e fig. 14.5 p. 661
Z5e 661 14.2 Acid Strength; see Table 14.1
For SE 14.2 -- you need to “remember” that HCl is a strong acid, so Cl- is a weak base (since id does not easily accept a proton (or a H+).
That is, acid strength is inversely proportional to its conjugate base strength.
Z5e 663 SE 14.2
Z5e 663 SE 14.2
Z5e 663 SE 14.2
Rf. Z5e 664
Note: in =m expression, H2O (l) is a pure liquid, so constant and drops out of the expression.
Kw called the ion-product constant (or the dissociation constant)
Rf. Z5e 664
Note: in =m expression, H2O (l) is a pure liquid, so constant and drops out of the expression.
Kw called the ion-product constant (or the dissociation constant)
Z5e 666 SE 14.4
Z5e 664 Fig. 14.7
Z5e 14.3 The pH Scale
Z5e Fig. 14.8 667
Z5e 668. SE 14.6
Z5e 669 Section 14.4: Calculating the pH of Strong Acid Solutions
Z5e 670 SE 14.7b
Z5e 671 Section 14.5: Calculating the pH of Weak Acid Solutions
[H+] = .0060, so pH = 2.22
pOH = 11.78; [OH-] = 1.7 x 10-12 & [H+] = 6.0 x 10-3
Z5e 675
Major species: HF, HOC6H5, H2O
Since HF is dominant producer of H+, use its Ka
Set up “RICE” table, use approximations and 5% rule
[H+] = .030 & pH = 1.53
Z5e 675
Major species: HF, HOC6H5, H2O
Since HF is dominant producer of H+, use its Ka
Set up “RICE” table, use approximations and 5% rule
[H+] = .030 & pH = 1.53
Rf. Z5e 675 SE 14.9
Z5e 677
[H] = 4.24 x 10-3 vs. 1.34 x 10-4
So % dissociation (aka % ionization) = 0.42% vs. 1.3%
Rf. Z5e 680 SE 14.11
Since (X/0.100)(100%) = 8.1%, x = 8.1 x 10-3 = [H+] = [A-], then plug into =m to solve for Ka.
Ans. = 6.6 x 10-4
Z5e 680 fig. 14.10
Z5e 681 Section 14.6 Bases
See next slide for explanation
[hydroxide] = 1.2 x 10-10
Z5e 688 Section 14.7 Polyprotic Acids
[H+] = 7.1 x 10-2
[H2AsO42-] = 7.1 x 10-2 also
[HAsO43-] = 8.0 x 10-8 = Ka2
[AsO43-] = 6.8 x 10-16
Remember: Must consider [H+] from all sources
[H+] = 7.1 x 10-2
[H2AsO42-] = 7.1 x 10-2 also
[HAsO43-] = 8.0 x 10-8 = Ka2
[AsO43-] = 6.8 x 10-16
Remember: Must consider [H+] from all sources
[H+] = 7.1 x 10-2
[H2AsO42-] = 7.1 x 10-2 also
[HAsO43-] = 8.0 x 10-8 = Ka2
[AsO43-] = 6.8 x 10-16
Remember: Must consider [H+] from all sources
[H+] = 7.1 x 10-2
[H2AsO42-] = 7.1 x 10-2 also
[HAsO43-] = 8.0 x 10-8 = Ka2
[AsO43-] = 6.8 x 10-16
Remember: Must consider [H+] from all sources
[H+] = 7.1 x 10-2
[H2AsO42-] = 7.1 x 10-2 also
[HAsO43-] = 8.0 x 10-8 = Ka2
[AsO43-] = 6.8 x 10-16
Remember: Must consider [H+] from all sources
Both [H+] and [HSO4-] are 2 M, since completely dissociated.
Both [H+] and [HSO4-] are 2 M, since completely dissociated.
Z5e 694 Section 14.8 Acid-Base properties of Salts
Z5e 695
Write major species
Set up =m between anion and water
Since product includes hydroxide ion, must use Kb so need to convert from Ka
Calculate hydroxide concentration, convert to pOH, subtract from 14 to get pH
Z5e 695
Write major species
Set up =m between anion and water
Since product includes hydroxide ion, must use Kb so need to convert from Ka
Calculate hydroxide concentration, convert to pOH, subtract from 14 to get pH
Z5e 697
Z5e 697
Z5e 699 Table 14.5
Z5e 701 Section 14.9 The Effect of Structure on Acid-Base Properties
Z5e 702 Figure 14.11
Z5e Section 14.10 Acid-Base Properties of Oxides
Z5e 704 Section 14.11 The Lewis Acid-Base Model
Al ion is Lewis acid and water is Lewis base
Z5e 707 Section 14.12 Strategy for Solving Acid-Base Problems: A Summary