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.
Acids have a sour taste, are electrolytes, turn indicators red, and have a pH less than 7. They donate protons and can neutralize bases to form salts and water. Bases have a bitter taste, are electrolytes, turn indicators blue or yellow, and have a pH greater than 7. They accept protons and can neutralize acids to form salts and water. Common acids include nitric acid, hydrochloric acid, acetic acid, sulfuric acid, and phosphoric acid. Common bases include lithium hydroxide, sodium hydroxide, potassium hydroxide, magnesium hydroxide, and calcium hydroxide.
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.
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.
The document discusses acids, bases, and the ion product constant of water. It defines acids as substances that produce hydrogen ions (H+) in water and bases as those that produce hydroxide ions (OH-). Water undergoes self-ionization in solution, producing a small concentration of H+ and OH- ions such that their product is 1 x 10-14 at 25°C. Solutions with higher [H+] than [OH-] are acidic, while those with higher [OH-] are basic.
This document provides an overview of acid-base theories and properties. It covers the Bronsted-Lowry and Lewis theories of acids and bases. It defines strong and weak acids and bases, and how their strength affects properties like conductivity and reaction rate. It also introduces the pH scale and explains how pH is determined by the concentration of hydrogen ions in solution.
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 provides information on acids and bases, including:
- The Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases.
- Classification of acids and bases as strong or weak based on degree of ionization.
- Conjugate acid-base pairs and how they are involved in acid-base reactions.
- The pH scale and relationships between [H+], [OH-], pH, pOH, and pKw.
- Key acid-base concepts such as autoionization of water, amphoteric nature of water, and using Ka/pKa values to determine acid strength.
This document discusses different definitions of acids and bases that were proposed over time:
1. Lavoisier defined acids as containing oxygen. Liebig later defined acids as containing hydrogen that can be replaced by a metal.
2. Arrhenius defined acids as substances that produce hydrogen ions (H+) in aqueous solution and bases as substances that produce hydroxide (OH-) ions.
3. Brønsted and Lowry defined acids as proton donors and bases as proton acceptors in acid-base reactions, forming conjugate acid-base pairs.
4. Lewis expanded the definition to include electron pair donors and acceptors in both aqueous and non-aqueous reactions.
It also discusses
Acids have a sour taste, are electrolytes, turn indicators red, and have a pH less than 7. They donate protons and can neutralize bases to form salts and water. Bases have a bitter taste, are electrolytes, turn indicators blue or yellow, and have a pH greater than 7. They accept protons and can neutralize acids to form salts and water. Common acids include nitric acid, hydrochloric acid, acetic acid, sulfuric acid, and phosphoric acid. Common bases include lithium hydroxide, sodium hydroxide, potassium hydroxide, magnesium hydroxide, and calcium hydroxide.
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.
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.
The document discusses acids, bases, and the ion product constant of water. It defines acids as substances that produce hydrogen ions (H+) in water and bases as those that produce hydroxide ions (OH-). Water undergoes self-ionization in solution, producing a small concentration of H+ and OH- ions such that their product is 1 x 10-14 at 25°C. Solutions with higher [H+] than [OH-] are acidic, while those with higher [OH-] are basic.
This document provides an overview of acid-base theories and properties. It covers the Bronsted-Lowry and Lewis theories of acids and bases. It defines strong and weak acids and bases, and how their strength affects properties like conductivity and reaction rate. It also introduces the pH scale and explains how pH is determined by the concentration of hydrogen ions in solution.
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 provides information on acids and bases, including:
- The Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases.
- Classification of acids and bases as strong or weak based on degree of ionization.
- Conjugate acid-base pairs and how they are involved in acid-base reactions.
- The pH scale and relationships between [H+], [OH-], pH, pOH, and pKw.
- Key acid-base concepts such as autoionization of water, amphoteric nature of water, and using Ka/pKa values to determine acid strength.
This document discusses different definitions of acids and bases that were proposed over time:
1. Lavoisier defined acids as containing oxygen. Liebig later defined acids as containing hydrogen that can be replaced by a metal.
2. Arrhenius defined acids as substances that produce hydrogen ions (H+) in aqueous solution and bases as substances that produce hydroxide (OH-) ions.
3. Brønsted and Lowry defined acids as proton donors and bases as proton acceptors in acid-base reactions, forming conjugate acid-base pairs.
4. Lewis expanded the definition to include electron pair donors and acceptors in both aqueous and non-aqueous reactions.
It also discusses
The document provides an overview of key topics in biochemistry including energy from food, proteins, carbohydrates, lipids, and nucleic acids. Specifically, it discusses how calorimetry can be used to determine the energy content of foods, the structures and functions of amino acids, proteins, carbohydrates like glucose and starch, and lipid molecules like triglycerides. It also briefly outlines analysis techniques for proteins like chromatography and electrophoresis. The document serves as an introductory guide to understanding the basic building blocks and energy sources in living organisms.
Ionic equilibrium chapter 3(12th HSC Maharashtra state board)Freya Cardozo
The document discusses ionic equilibrium and acid-base theories. It provides examples of different types of salts based on the strength of acids and bases involved:
1) Salts of strong acids and bases, like NaCl, are neutral as they do not undergo hydrolysis.
2) Salts of strong acids and weak bases, like CuSO4, are acidic due to hydrolysis of the metal cation.
3) Salts of weak acids and strong bases, like CH3COONa, are basic due to hydrolysis of the anion.
4) Salts of weak acids and weak bases can be acidic, basic or neutral depending on whether the Ka or Kb is greater and the extent of hydro
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
- Hard and soft acids and bases (HSAB) can be classified based on their polarizability - hard species have tightly held electron clouds while soft species have loosely held, easily polarized electron clouds.
- Hard acids prefer to interact with hard bases that have donor atoms like N, O, F, while soft acids prefer soft bases with donor atoms like P, S, Se, Cl, Br.
- Examples of hard acids are H+, Li+, Na+, K+ and hard bases are OH-, F-. Soft acids include Cu+, Ag+, Au+ and soft bases include S2-, Se2-.
This document provides an overview of acids, bases, and salts. It discusses several acid-base theories including:
- Arrhenius theory which defines acids as producing H+ ions and bases as producing OH- ions.
- Brønsted-Lowry theory which defines acids as proton donors and bases as proton acceptors.
It also describes properties such as:
- Strong vs weak acids and bases based on extent of ionization.
- Mono-, di-, and triprotic acids based on the number of protons donated.
- pH and pKa scales for representing acidity and acid strength.
- Hydrolysis of salt solutions and how it affects pH depending on
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.
1. The document discusses ionic equilibria, including acids and bases, and how to identify strong and weak acids/bases. It also discusses calculating pH and pOH values.
2. It explains how to determine if a salt is neutral, acidic, or basic based on whether the cation or anion comes from a strong or weak acid/base.
3. For sparingly soluble salts, it discusses using Ksp expressions and concentrations to determine if a precipitate will form from mixing solutions of ions.
This document discusses weak bases and how they react with water to form the conjugate acid and hydroxide ions. It defines the base dissociation constant Kb and explains how it refers to the equilibrium of a base reacting with water. It provides examples of calculating the concentration of hydroxide ions produced from a weak base solution and calculating Kb or Ka values for conjugate acid-base pairs using known constants. The document also discusses how the properties of salt solutions are determined by the constituent ions and how buffers resist changes in pH upon addition of acids or bases.
This document defines and describes the characteristics of acids and bases according to three concepts:
Arrhenius, Bronsted-Lowry, and Lewis. According to the Arrhenius concept, acids increase the concentration of hydronium ions (H3O+) in water, while bases increase the concentration of hydroxide ions (OH-). The Bronsted-Lowry concept defines acids as proton donors and bases as proton acceptors. The Lewis concept defines acids as electron pair acceptors and bases as electron pair donors. The document lists characteristics of acids as having a sour taste, changing dye colors, and reacting with metals to produce hydrogen gas. Bases are described as having a bitter taste, changing dye colors,
This document provides an overview of Chapter 22 from a chemistry textbook, which covers topics related to ionic equilibria including:
- pH, Ka, pKa and Kw values and their use in calculations involving strong and weak acids and bases.
- Acid-base titration curves and how they differ for strong-strong, strong-weak, weak-strong, and weak-weak acid-base titrations.
- How acid-base indicators work and their use in determining the endpoint of a titration.
It also lists learning outcomes for understanding these concepts and performing related calculations.
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 discusses various concepts related to ionic equilibrium in solution including strong and weak electrolytes, acid-base theories of Arrhenius, Bronsted-Lowry, and Lewis. It defines strong electrolytes as completely dissociating in water and weak electrolytes as achieving an equilibrium between dissociated and undissociated molecules. Acids are defined as proton donors and bases as proton acceptors under the Bronsted-Lowry theory. The Lewis theory further defines acids as electron pair acceptors and bases as electron pair donors. Dissociation constants and factors affecting acid strength are also covered.
The document discusses several theories of acids and bases that developed over time:
- Lavoisier's original oxygen theory defined acids as containing oxygen (1776). This was disproven by Davy in 1810.
- Liebig proposed in 1838 that acids contain replaceable hydrogen.
- Arrhenius' 1884 definition defined acids as producing hydrogen ions (H+) and bases as producing hydroxide ions (OH-) in aqueous solutions, which became the standard definition.
- Lewis in 1923 expanded the definition to electron pair transfers between any acids and bases, not just involving hydrogen.
- Other theories such as Lux-Flood's oxygen theory of 1939 and Pearson's hard/soft acid base principle
IB Chemistry on Arrhenius, Bronsted Lowry Conjugate Acid Base Pair and Lewis ...Lawrence kok
The document defines different types of acids and bases. Brønsted-Lowry acids are proton donors that donate a proton to a Brønsted-Lowry base, which accepts the proton. Every acid has a conjugate base and every base has a conjugate acid. The conjugate acid has one more hydrogen ion than the conjugate base. Strong acids form weak conjugate bases that do not readily accept protons back, while weak acids form strong conjugate bases that can accept protons. Strong bases form weak conjugate acids that do not readily donate protons, while weak bases form strong conjugate acids that can donate protons. Some substances can act as both acids and bases depending on conditions and are called amphiprotic or amphoteric. Lewis acids are
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.
This document discusses pH and acid-base chemistry concepts. It defines pH as the negative logarithm of the hydrogen ion concentration, and pOH as the negative logarithm of the hydroxide ion concentration. The key relationships discussed are that pH + pOH = 14 for any solution, and pH and pOH can be used to rank acid and base strength based on ion concentration.
El agua es la molécula más abundante en los seres vivos y constituye entre un 60-90% de su composición. Es esencial para todos los tipos de vida y cumple funciones vitales como disolvente biológico, en procesos metabólicos y estructurales, en la regulación de la temperatura, el transporte de nutrientes y como amortiguador mecánico. Sus propiedades físico-químicas como su poder disolvente, fuerza de cohesión y calor específico la hacen indispensable para la vida.
El documento explica el concepto de pH y el equilibrio ácido-base en el cuerpo. Las soluciones biológicas mantienen un estrecho rango de concentración de iones de hidrógeno para permitir funciones vitales. El pH mide la concentración de iones de hidrógeno y se regula a través de amortiguadores, la ventilación pulmonar y la filtración renal para contrarrestar la acidosis o alcalosis.
El documento describe las propiedades y la importancia del agua para la vida. El agua es esencial para todos los seres vivos y constituye entre el 50-95% del peso de cualquier sistema vivo. Sus propiedades como su alta capacidad calorífica, tensión superficial y capacidad como solvente la hacen ideal para regular la temperatura corporal y permitir reacciones químicas necesarias para la vida.
Tema que describe la organización de la materia. También expone la composición molecular así como las propiedades del agua y las sales minerales (principios inmediatos inorgánicos)
The leading digital commerce company in Latin America, Paymentez, provides one-stop shop payment solutions for online and offline transactions across mobile, products, and services. It helps customers increase their user base, conversion rates, and minimize taxes and fees in the region. Paymentez has 4 million registered users and an optimized system to reduce fraud and chargebacks. It offers comprehensive marketing strategies along with ways for customers to monetize applications and games through an easy-to-use interface.
This document provides information about inplant training programs offered by Expert Systems and Solutions (ESS) in Chennai, Tamil Nadu, India. The 5-day training programs in November and December 2012 cost Rs. 5500 per student and have a maximum of 5 students per batch. The training syllabus covers topics like electronics circuits, PCB design and fabrication, MATLAB software, microcontroller fundamentals and programming, and power electronics circuit design using simulation software. It also lists products and services offered like embedded systems, online tutoring, electrical works, and electronics servicing. Contact information including the email ID, address and phone numbers is provided at the end.
The document provides an overview of key topics in biochemistry including energy from food, proteins, carbohydrates, lipids, and nucleic acids. Specifically, it discusses how calorimetry can be used to determine the energy content of foods, the structures and functions of amino acids, proteins, carbohydrates like glucose and starch, and lipid molecules like triglycerides. It also briefly outlines analysis techniques for proteins like chromatography and electrophoresis. The document serves as an introductory guide to understanding the basic building blocks and energy sources in living organisms.
Ionic equilibrium chapter 3(12th HSC Maharashtra state board)Freya Cardozo
The document discusses ionic equilibrium and acid-base theories. It provides examples of different types of salts based on the strength of acids and bases involved:
1) Salts of strong acids and bases, like NaCl, are neutral as they do not undergo hydrolysis.
2) Salts of strong acids and weak bases, like CuSO4, are acidic due to hydrolysis of the metal cation.
3) Salts of weak acids and strong bases, like CH3COONa, are basic due to hydrolysis of the anion.
4) Salts of weak acids and weak bases can be acidic, basic or neutral depending on whether the Ka or Kb is greater and the extent of hydro
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
- Hard and soft acids and bases (HSAB) can be classified based on their polarizability - hard species have tightly held electron clouds while soft species have loosely held, easily polarized electron clouds.
- Hard acids prefer to interact with hard bases that have donor atoms like N, O, F, while soft acids prefer soft bases with donor atoms like P, S, Se, Cl, Br.
- Examples of hard acids are H+, Li+, Na+, K+ and hard bases are OH-, F-. Soft acids include Cu+, Ag+, Au+ and soft bases include S2-, Se2-.
This document provides an overview of acids, bases, and salts. It discusses several acid-base theories including:
- Arrhenius theory which defines acids as producing H+ ions and bases as producing OH- ions.
- Brønsted-Lowry theory which defines acids as proton donors and bases as proton acceptors.
It also describes properties such as:
- Strong vs weak acids and bases based on extent of ionization.
- Mono-, di-, and triprotic acids based on the number of protons donated.
- pH and pKa scales for representing acidity and acid strength.
- Hydrolysis of salt solutions and how it affects pH depending on
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.
1. The document discusses ionic equilibria, including acids and bases, and how to identify strong and weak acids/bases. It also discusses calculating pH and pOH values.
2. It explains how to determine if a salt is neutral, acidic, or basic based on whether the cation or anion comes from a strong or weak acid/base.
3. For sparingly soluble salts, it discusses using Ksp expressions and concentrations to determine if a precipitate will form from mixing solutions of ions.
This document discusses weak bases and how they react with water to form the conjugate acid and hydroxide ions. It defines the base dissociation constant Kb and explains how it refers to the equilibrium of a base reacting with water. It provides examples of calculating the concentration of hydroxide ions produced from a weak base solution and calculating Kb or Ka values for conjugate acid-base pairs using known constants. The document also discusses how the properties of salt solutions are determined by the constituent ions and how buffers resist changes in pH upon addition of acids or bases.
This document defines and describes the characteristics of acids and bases according to three concepts:
Arrhenius, Bronsted-Lowry, and Lewis. According to the Arrhenius concept, acids increase the concentration of hydronium ions (H3O+) in water, while bases increase the concentration of hydroxide ions (OH-). The Bronsted-Lowry concept defines acids as proton donors and bases as proton acceptors. The Lewis concept defines acids as electron pair acceptors and bases as electron pair donors. The document lists characteristics of acids as having a sour taste, changing dye colors, and reacting with metals to produce hydrogen gas. Bases are described as having a bitter taste, changing dye colors,
This document provides an overview of Chapter 22 from a chemistry textbook, which covers topics related to ionic equilibria including:
- pH, Ka, pKa and Kw values and their use in calculations involving strong and weak acids and bases.
- Acid-base titration curves and how they differ for strong-strong, strong-weak, weak-strong, and weak-weak acid-base titrations.
- How acid-base indicators work and their use in determining the endpoint of a titration.
It also lists learning outcomes for understanding these concepts and performing related calculations.
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 discusses various concepts related to ionic equilibrium in solution including strong and weak electrolytes, acid-base theories of Arrhenius, Bronsted-Lowry, and Lewis. It defines strong electrolytes as completely dissociating in water and weak electrolytes as achieving an equilibrium between dissociated and undissociated molecules. Acids are defined as proton donors and bases as proton acceptors under the Bronsted-Lowry theory. The Lewis theory further defines acids as electron pair acceptors and bases as electron pair donors. Dissociation constants and factors affecting acid strength are also covered.
The document discusses several theories of acids and bases that developed over time:
- Lavoisier's original oxygen theory defined acids as containing oxygen (1776). This was disproven by Davy in 1810.
- Liebig proposed in 1838 that acids contain replaceable hydrogen.
- Arrhenius' 1884 definition defined acids as producing hydrogen ions (H+) and bases as producing hydroxide ions (OH-) in aqueous solutions, which became the standard definition.
- Lewis in 1923 expanded the definition to electron pair transfers between any acids and bases, not just involving hydrogen.
- Other theories such as Lux-Flood's oxygen theory of 1939 and Pearson's hard/soft acid base principle
IB Chemistry on Arrhenius, Bronsted Lowry Conjugate Acid Base Pair and Lewis ...Lawrence kok
The document defines different types of acids and bases. Brønsted-Lowry acids are proton donors that donate a proton to a Brønsted-Lowry base, which accepts the proton. Every acid has a conjugate base and every base has a conjugate acid. The conjugate acid has one more hydrogen ion than the conjugate base. Strong acids form weak conjugate bases that do not readily accept protons back, while weak acids form strong conjugate bases that can accept protons. Strong bases form weak conjugate acids that do not readily donate protons, while weak bases form strong conjugate acids that can donate protons. Some substances can act as both acids and bases depending on conditions and are called amphiprotic or amphoteric. Lewis acids are
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.
This document discusses pH and acid-base chemistry concepts. It defines pH as the negative logarithm of the hydrogen ion concentration, and pOH as the negative logarithm of the hydroxide ion concentration. The key relationships discussed are that pH + pOH = 14 for any solution, and pH and pOH can be used to rank acid and base strength based on ion concentration.
El agua es la molécula más abundante en los seres vivos y constituye entre un 60-90% de su composición. Es esencial para todos los tipos de vida y cumple funciones vitales como disolvente biológico, en procesos metabólicos y estructurales, en la regulación de la temperatura, el transporte de nutrientes y como amortiguador mecánico. Sus propiedades físico-químicas como su poder disolvente, fuerza de cohesión y calor específico la hacen indispensable para la vida.
El documento explica el concepto de pH y el equilibrio ácido-base en el cuerpo. Las soluciones biológicas mantienen un estrecho rango de concentración de iones de hidrógeno para permitir funciones vitales. El pH mide la concentración de iones de hidrógeno y se regula a través de amortiguadores, la ventilación pulmonar y la filtración renal para contrarrestar la acidosis o alcalosis.
El documento describe las propiedades y la importancia del agua para la vida. El agua es esencial para todos los seres vivos y constituye entre el 50-95% del peso de cualquier sistema vivo. Sus propiedades como su alta capacidad calorífica, tensión superficial y capacidad como solvente la hacen ideal para regular la temperatura corporal y permitir reacciones químicas necesarias para la vida.
Tema que describe la organización de la materia. También expone la composición molecular así como las propiedades del agua y las sales minerales (principios inmediatos inorgánicos)
The leading digital commerce company in Latin America, Paymentez, provides one-stop shop payment solutions for online and offline transactions across mobile, products, and services. It helps customers increase their user base, conversion rates, and minimize taxes and fees in the region. Paymentez has 4 million registered users and an optimized system to reduce fraud and chargebacks. It offers comprehensive marketing strategies along with ways for customers to monetize applications and games through an easy-to-use interface.
This document provides information about inplant training programs offered by Expert Systems and Solutions (ESS) in Chennai, Tamil Nadu, India. The 5-day training programs in November and December 2012 cost Rs. 5500 per student and have a maximum of 5 students per batch. The training syllabus covers topics like electronics circuits, PCB design and fabrication, MATLAB software, microcontroller fundamentals and programming, and power electronics circuit design using simulation software. It also lists products and services offered like embedded systems, online tutoring, electrical works, and electronics servicing. Contact information including the email ID, address and phone numbers is provided at the end.
Podcasts can improve the learning experience by allowing students to access audio and video files on various devices that provide guidance on class activities. Instructors can assign podcasts to students, who can subscribe and download the files to gain a better understanding of course material. This project estimates the costs to implement podcasts over 10 years and expects the savings to exceed the costs within 4 years, providing financial benefits in addition to improving learning.
This document outlines an assessment task for a social media profile that is worth 25% of the grade. The task involves building an online presence through social media and demonstrating interaction and communication skills. The document provides the name and student number of the person completing the assessment.
This presentation discussed the genealogy research tool Find-A-Grave. It explained how to search for cemeteries and individuals, request photos, and contribute photos and information to entries. The presenter showed how they used Find-A-Grave to research the Deats family, finding burial plots, monuments, and individuals in Cherryville Baptist Cemetery. They tracked research findings in a spreadsheet and posted photos to Find-A-Grave, Family Tree Maker, and a genealogy blog. The presentation demonstrated how Find-A-Grave can aid family history research.
PolyU Design I MAKE Initiative (2015-10-31)Clifford Choy
This is for promoting the I MAKE initiative from PolyU Design (School of Design, the Hong Kong Polytechnic University) to local teachers. This initiative is aiming at promoting the importance of making and the maker culture to students, parents and teachers in local primary and secondary schools. This is relevant to teaches from the following subjects/disciplines: visual arts, design and technology, information technology, science and mathematics.
This document provides an overview of the Indian steel industry. It discusses the industry's size, major players, growth over time, and acquisitions that have occurred. Some key points:
- India is now one of the largest steel producers in the world, with both public and private sector companies involved. Major players include SAIL, Tata Steel, Essar Steel, and JSW Steel.
- The industry has grown significantly since the 1990s with increased investment and production capacity. India's crude steel production grows over 10% annually.
- Notable acquisitions include ArcelorMittal's purchase of Arcelor and Tata Steel's acquisition of Corus, demonstrating the industry's dynamic nature.
The document discusses various aspects of communication including:
1) Communication is like the blood vessels of the body and is essential for business.
2) Communication provides information and feedback to help businesses set goals and adapt.
3) Memory, perception, psychological inertia, language and personality all impact communication. Effective communication involves clarity of purpose, preparation, using familiar language, relevance, and obtaining feedback.
The Social Challenge of 1.5°C Webinar: Frank Biermanntewksjj
Karen O'Brien, Susanne Moser, Ioan Fazey and others from Future Earth's Transformations Knowledge-Action Network discuss mobilising research around the social challenge of a 1.5°C target for climate action.
Este documento describe varias virosis cutáneas. Menciona la epidermodisplasia verruciforme, el herpes simple, el herpes zoster, el molusco contagioso, el nódulo de los ordeñadores y Orf, la rubéola, el sarampión, el dengue grave, la varicela y las verrugas y condilomas virales. Describe los agentes causales, características clínicas y tratamiento de cada una.
The document provides information about a research project opportunity for students in electrical engineering fields. It includes contact information for Experts Systems and Solutions including email, cell phone, and website. It states that students can assemble hardware projects in their research labs and experts will provide guidance.
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 values, Kb values, and the Kw expression. Acid-base properties of salts are addressed. The concepts of titrations and indicators are defined.
Acids and bases can be defined operationally based on experimental observations or conceptually based on theories. Operationally, acids are sour electrolytes that turn litmus red and react with metals, while bases are bitter electrolytes that turn litmus blue. Conceptually, acids are proton donors according to Arrhenius and Bronsted-Lowry, or electron pair acceptors according to Lewis. Conjugate acid-base pairs involve the transfer of a proton between an acid and its conjugate base. The strength of an acid or base depends on its tendency to donate or accept protons.
This document discusses acid-base theories and reactions. It begins with a brief history of acids and bases, noting they were originally defined based on their sour taste. It then focuses on three main acid-base theories:
1) Arrhenius theory defines acids as producing H+ ions in water and bases as producing OH- ions.
2) Brønsted-Lowry theory provides a more general definition, with acids as proton donors and bases as proton acceptors that form conjugate acid-base pairs.
3) Lewis theory defines acids and bases based on their ability to accept or donate electron pairs in chemical bonds.
The document goes on to discuss the properties of acids and bases, ion
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.
This chapter discusses acids and bases according to the Arrhenius and Brønsted-Lowry definitions. The Arrhenius definition states that acids are substances that produce hydronium ions (H3O+) in water and bases produce hydroxide ions (OH-). Brønsted-Lowry defines acids as proton donors and bases as proton acceptors. Both definitions are discussed along with their advantages and limitations. Strong and weak acids/bases are compared based on their extent of ionization in water. Neutralization reactions between acids and bases are outlined. Conjugate acid-base pairs are introduced in the context of Brønsted-Lowry acid-base reactions. Certain substances, called
Acid base information in daily life of people,the theory regarding it in scie...JayeshChavarkar
This document discusses acids, bases, and salts. It covers the key properties of acids and bases, as well as three major theories of acids and bases: Arrhenius, Bronsted-Lowry, and Lewis. It also discusses acid and base strength in terms of acid dissociation constants, as well as neutralization reactions between acids and bases and the use of titrations.
1. The document summarizes key concepts about acids and bases from Chapter 8, including the Arrhenius and Brønsted-Lowry theories of acids and bases. It defines acids as proton donors and bases as proton acceptors.
2. The pH scale is introduced as a measurement from 0 to 14 that indicates the acidity or basicity of a solution. The pH is defined as the negative log of the hydronium ion concentration.
3. Neutralization reactions between acids and bases are discussed, producing a salt and water. The net ionic equation is written as the reaction between hydronium and hydroxide ions.
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,
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.
1. The document discusses different definitions of acids and bases including Arrhenius, Brønsted-Lowry, and Lewis models.
2. Under the Brønsted-Lowry definition, acids donate protons and bases accept protons to form conjugate acid-base pairs.
3. The Brønsted-Lowry model is more inclusive than the Arrhenius model because it classifies ammonia as a base since it can accept protons, even though it does not produce OH-.
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 discusses acids and bases. It defines acids as compounds that increase the concentration of hydrogen ions (H+) in aqueous solution, and bases as compounds that increase the concentration of hydroxide ions (OH-). Strong acids and bases completely ionize in water, while weak acids and bases only partially ionize. Different acid theories are also introduced, including Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases. Common strong and weak acids and bases are listed.
The document defines acids and bases according to three theories:
1) Arrhenius theory defines acids as substances that produce H+ ions in water and bases as substances that produce OH- ions in water.
2) Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors in any solvent.
3) Lewis theory uses electron pair donors and acceptors to define acids and bases and applies to a wider range of substances.
The document also discusses pH scales, strong vs. weak acids and bases, and factors that contribute to acid rain in certain regions.
Acid base reactions BY MUHAMMAD FAHAD ANSARI 12IEEM 14fahadansari131
This document discusses acid-base chemistry, including:
1) Theories of acids and bases including those proposed by Arrhenius and Bronsted-Lowry that expanded the definition of acids and bases.
2) Properties and composition of acids, bases, and salts. Acids are proton donors and can be inorganic or organic substances. Bases accept protons. Salts are formed through neutralization reactions between acids and bases.
3) Important acid-base reactions in aqueous solutions including acid-base neutralization and conjugate acid-base pairs. Acid-base balance is critical for biological functions like in human blood.
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases are defined by Four main theories,
1.Traditional theory / concept
2.Arrhenius theory
3.Bronsted and Lowry theory
4.Lewis theory
Importance of acids and bases in pharmacy
Buffers: Buffer action
Buffer capacity Buffers system
Types of Buffers : Generally buffers are of two types:
1. Acidic buffers
2. Basic buffers
There are some other buffer system:
3. Two salts acts as acid-base pair. Ex- Potassium hydrogen phosphate and potassium dihydrogen phosphate.
4. Amphoteric electrolyte. Ex- Solution of glycine.
5. Solution of strong acid and solution of strong base. Ex- Strong HCl with KCl Mechanism of Buffer action: Mechanism of Action of acidic buffers: Buffer equation-Henderson-Hasselbalch equation:
Standard Buffer Solutions Preparation of Buffer Solutions: Buffers in pharmaceutical systems or Application of buffer: Stability of buffers Buffered isotonic solution Types of Buffer Isotonic solution
1. Isotonic Solutions:
2. Hypertonic Solutions:
3. Hypotonic Solution:
Measurement of Tonicity: 1. Hemolytic method: 2. Cryoscopic method or depression of freezing point:
Methods of adjusting the tonicity:
Class I methods:
In this type, sodium chloride or other substances are added to the solution in sufficient quantity to make it isotonic. Then the preparation is brought to its final volume withan isotonic or a buffered isotonic diluting solution.
These methods are of two types:
Cryoscopic method
Sodium chloride equivalent method.
Class II methods:
In this type, water is added in sufficient quantity make the preparation isotonic. Then the preparation is brought to its volume with an isotonic or a buffered isotonic diluting solution.
These methods are of two types:
White-Vincent method
Sprowls method.
The document provides information about acids and bases including:
1) It defines acids and bases according to the Arrhenius, Bronsted-Lowry, and Lewis theories. Acids are proton donors and bases are proton acceptors.
2) It discusses acid-base reactions such as neutralization reactions between acids and bases which form water, and reactions between acids and carbonates/bicarbonates which form gases.
3) It explains concepts such as pH, pOH, strong vs weak acids/bases, and buffers which resist changes in pH through neutralizing both added acids and bases.
This document provides information about acids and bases. It defines acids and bases according to the Arrhenius and Bronstead-Lowry theories. The Arrhenius definition states that acids release hydrogen ions and bases release hydroxide ions in water. The Bronstead-Lowry definition expands this by defining acids as proton donors and bases as proton acceptors. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate, establishing an equilibrium. The acid dissociation constant and base dissociation constant describe the strength of acids and bases respectively.
This document defines bases and discusses their properties and uses. It states that bases are also called alkalis, act as proton acceptors and electron pair donors, and produce OH- ions in water. Common bases mentioned include sodium hydroxide, potassium hydroxide, and barium hydroxide. Bases are used to make soaps, cleaners, and other products. The document also discusses the Arrhenius, Bronsted-Lowry, and Lewis theories of bases and distinguishes between strong and weak bases based on their degree of dissociation in water.
This document discusses the structure, nomenclature, properties, and synthesis of hydrocarbons. It defines hydrocarbons as compounds composed of only carbon and hydrogen. Alkanes are saturated hydrocarbons with an open chain structure. Alkanes have the general formula CnH2n+2. Constitutional isomers have the same molecular formula but different connectivity of atoms. Higher molecular weight alkanes are liquids or solids at room temperature due to dispersion forces between molecules. Alkanes are important energy sources due to their high heat of combustion when oxidized. Natural gas, petroleum, and coal are major natural sources of alkanes.
The document discusses radioactivity and nuclear medicine, including defining nuclear symbols, describing different types of radiation like alpha and beta particles and gamma rays, properties of radioisotopes such as half-life, and medical applications of radioactivity including using isotopes for cancer therapy and nuclear medicine procedures like tracer studies.
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.
Spontaneous processes occur naturally without an external stimulus, while nonspontaneous processes require something to be done to occur. Whether a reaction is spontaneous can be determined using thermodynamics by calculating the enthalpy and entropy. Energy exists in various forms including thermal, electrical, chemical, and kinetic, and it can be transferred or changed between objects and forms. During chemical reactions, energy is either absorbed or released as bonds break and form.
Spontaneous processes occur naturally without an external stimulus, while nonspontaneous processes require something to be done to occur. Whether a reaction is spontaneous can be determined using thermodynamics by calculating the enthalpy and entropy. Energy exists in various forms including thermal, electrical, chemical, and kinetic, and it can be transferred or changed between objects and forms. During chemical reactions, energy is either absorbed or released as bonds break and form.
This chapter discusses the three states of matter - gases, liquids, and solids. It focuses on the differences in their physical properties. The key gas laws - Boyle's law, Charles's law, and the combined gas law - are introduced. Boyle's law relates the inverse relationship between pressure and volume of a gas at constant temperature. Charles's law describes how the volume of a gas increases directly with temperature at constant pressure. Examples are provided to demonstrate how to apply these gas laws to calculate changes in volume or pressure of a gas under different conditions.
1) The document provides an overview of key concepts in chemistry including the mole concept, chemical formulas and equations, and different types of chemical reactions.
2) It explains that the mole is a unit used to measure amounts of substances and is equal to 6.022x1023 particles. Molar mass refers to the mass of one mole of a substance.
3) Chemical equations are used to represent chemical reactions and must satisfy the law of conservation of mass by being balanced with the same number and type of atoms on each side of the reaction arrow.
This document provides an overview of chemical bonding and the properties of ionic and covalent compounds. It discusses the following key points:
1. Chemical bonds form due to the attraction between atoms and involve the transfer or sharing of valence electrons. Ionic bonds form through electron transfer between metals and nonmetals, while covalent bonds involve electron sharing.
2. Lewis symbols represent atoms and their valence electrons and are used to predict bonding patterns. Electronegativity determines bond polarity.
3. Ionic compounds have high melting and boiling points due to strong electrostatic attractions in the crystal lattice. Covalent compounds can be solids, liquids or gases.
This document provides an overview of atomic structure and the development of atomic theory. It discusses the basic composition of atoms, including electrons, protons, and neutrons. It describes Dalton's atomic theory and the key postulates. It also discusses subatomic particles like isotopes, ions, and the discovery of electrons, protons, and neutrons through experiments. The document is divided into sections on the composition of atoms, atomic calculations, isotopes, ions, atomic mass, and the development of atomic theory from Dalton to the discovery of subatomic particles.
This document provides an overview of key concepts in chemistry, including:
1. Chemistry is the study of matter, its properties, and the changes it undergoes. The scientific method is used to systematically study matter through observation, questioning, experimentation and summarization.
2. Matter can exist in three physical states - solid, liquid, and gas. It also has physical and chemical properties and can undergo physical or chemical changes.
3. The metric system is the standard system of measurement in chemistry. It relates units decimally and is easier for conversion than the English system. Careful measurement and use of appropriate units is important in chemistry.
The document summarizes key concepts about solutions from chapter 6, including:
1) It defines solutions, solutes, solvents, and aqueous solutions.
2) It describes general properties of solutions like transparency, electrolytes vs nonelectrolytes, and how volumes are non-additive.
3) It discusses concentration units like molarity, calculates concentrations from masses and volumes, and explains dilution.
4) It covers colligative properties like vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure that depend on solute concentration.
At Techbox Square, in Singapore, we're not just creative web designers and developers, we're the driving force behind your brand identity. Contact us today.
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2. 8.1 Acids and Bases
• Acids: Taste sour, dissolve some metals,
cause plant dye to change color
• Bases: Taste bitter, are slippery, are
corrosive
• Two theories that help us to understand
the chemistry of acids and bases
1. Arrhenius Theory
2. Brønsted-Lowry Theory
3. Arrhenius Theory of Acids
and Bases
8.1 Acids and Bases
• Acid - a substance, when dissolved in
water, dissociates to produce hydrogen
ions
– Hydrogen ion: H+ also called “protons”
HCl is an acid:
HCl(aq) → H+(aq) + Cl-(aq)
4. Arrhenius Theory of Acids
and Bases
8.1 Acids and Bases
• Base - a substance, when dissolved in
water, dissociates to produce hydroxide
ions
NaOH is a base
NaOH(aq) → Na+(aq) + OH-(aq)
5. Arrhenius Theory of Acids
and Bases
8.1 Acids and Bases
• Where does NH3 fit?
• When it dissolves in water it has basic
properties but it does not have OH- ions in
it
• The next acid-base theory gives us a
broader view of acids and bases
6. Brønsted-Lowry Theory of
Acids and Bases
8.1 Acids and Bases
• Acid - proton donor
• Base - proton acceptor
– Notice that acid and base are not defined
using water
– When writing the reactions, both accepting
and donation are evident
7. Brønsted-Lowry Theory of
Acids and Bases
8.1 Acids and Bases
HCl(aq) + H2O(l) → Cl-(aq) + H3O+(aq)
acid base
What donated the proton? HCl
Is it an acid or base? Acid
What accepted the proton? H2O
Is it an acid or base? Base
8. .Brønsted-Lowry Theory of
Acids and Bases
8.1 Acids and Bases
NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)
base acid
Now, let us look at NH3 and see why it is a
base.
Did NH3 donate or accept a proton? Accept
Is it an acid or base? Base
What is water in this reaction? Acid
9. 8.1 Acids and Bases Acid-Base Properties of Water
• Water possesses both acid and base
properties
– Amphiprotic - a substance possessing both acid
and base properties
– Water is the most commonly used solvent for
both acids and bases
– Solute-solvent interactions between water and
both acids and bases promote solubility and
dissociation
10. 8.1 Acids and Bases Acid and Base Strength
• Acid and base strength – degree of
dissociation
– Not a measure of concentration
– Strong acids and bases – reaction with water is
virtually 100% (Strong electrolytes)
11. 8.1 Acids and Bases Strong Acids and Bases
• Strong Acids:
– HCl, HBr, HI Hydrochloric Acid, etc.
– HNO3 Nitric Acid
– H2SO4 Sulfuric Acid
– HClO4 Perchloric Acid
• Strong Bases:
– NaOH, KOH, Ba(OH)2
– All metal hydroxides
12. 8.1 Acids and Bases Weak Acids
• Weak acids and bases – only a small
percent dissociates (Weak electrolytes)
• Weak acid examples:
– Acetic acid:
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
– Carbonic Acid:
H2CO3(aq) + H2O(l) HCO3-(aq) + H3O+(aq)
14. 8.1 Acids and Bases Conjugate Acids and Bases
• The acid base reaction can be written in
the general form:
HA + B A– + HB+
acid base
• Notice the reversible arrows
• The products are also an acid and base
called the conjugate acid and base
15. 8.1 Acids and Bases
HA + B A- + HB+
acid base base acid
• Conjugate acid - what the base becomes
after it accepts a proton
• Conjugate base - what the acid becomes
after it donates its proton
• Conjugate acid-base pair - the acid and
base on the opposite sides of the
equation
16. 8.1 Acids and Bases Acid-Base Dissociation
HA + B A– + HB+
• The reversible arrow isn’t always written
– Some acids or bases essentially dissociate 100%
– One way arrow is used
• HCl + H2O → Cl- + H3O+
– All of the HCl is converted to Cl-
– HCl is called a strong acid – an acid that
dissociates 100%
• Weak acid - one which does not dissociate
100%
17. 8.1 Acids and Bases Conjugate Acid-Base Pairs
• Which acid is
stronger:
HF or HCN? HF
• Which base is
stronger:
CN- or H2O? CN -
18. 8.1 Acids and Bases Acid-Base Practice
• Write the chemical reaction for the following
acids or bases in water
• Identify the conjugate acid-base pairs
1. HF (a weak acid)
2. H2S (a weak acid)
3. HNO3 (a strong acid)
4. CH3NH2 (a weak base)
Note: The degree of dissociation also defines weak
and strong bases
19. 8.1 Acids and Bases The Dissociation of Water
• Pure water is virtually 100% molecular
• Very small number of molecules dissociate
– Dissociation of acids and bases is often called
ionization
H2O(l) + H2O(l) H3O+(aq) + OH-(aq)
• Called autoionization
• Very weak electrolyte
20. 8.1 Acids and Bases Hydronium Ion
• H3O+ is called the hydronium ion
• In pure water at room temperature:
– [H3O+] = 1 x 10-7 M
– [OH-] = 1 x 10-7 M
• What is the equilibrium expression for:
H2O(l) + H2O(l) H3O+(aq) + OH-(aq)
+
K eq = [H 3O ][OH ] -
Remember, liquids are not included in equilibrium
expressions
21. 8.1 Acids and Bases Ion Product of Water
• This constant is called the ion product for
water and has the symbol Kw
+
K w = [H 3O ][OH ] -
• Since [H3O+] = [OH-] = 1.0 x 10-7 M, what is
the value for Kw?
– 1.0 x 10-14
– It is unitless
22. 8.2 pH: A Measurement Scale
for Acids and Bases
• pH scale - a scale that indicates the acidity
or basicity of a solution
– Ranges from 0 (very acidic) to 14 (very basic)
• The pH scale is rather similar to the
temperature scale assigning relative values
of hot and cold
• The pH of a solution is defined as:
pH = -log[H3O+]
23. A Definition of pH
Scale for Acids and Bases
8.2 pH: A Measurement
• Use these observations to develop a concept
of pH
– if know one concentration, can calculate the
other
– if add an acid, [H3O+] ↑ and [OH-] ↓
– if add a base, [OH-] ↑ and [H3O+] ↓
– [H3O+] = [OH-] when equal amounts of acid
and base are present
• In each of these cases 1 x 10-14 = [H3O+][OH-]
24. Measuring pH
Scale for Acids and Bases
8.2 pH: A Measurement
• pH of a solution can be:
– Calculated if the concentration of either is
known
• [H3O+]
• [OH-]
– Approximated using indicator / pH paper
that develops a color related to the solution
pH
– Measured using a pH meter whose sensor
measures an electrical property of the
solution that is proportional to pH
25. Calculating pH
Scale for Acids and Bases
8.2 pH: A Measurement
• How do we calculate the pH of a solution
when either the hydronium or hydroxide
ion concentration is known?
• How do we calculate the hydronium or
hydroxide ion concentration when the pH
is known?
• Use two facts:
pH = -log[H3O+]
1 x 10-14 = [H3O+][OH-]
26. Calculating pH from
Scale for Acids and Bases
8.2 pH: A Measurement
Acid Molarity
What is the pH of a 1.0 x 10-4 M HCl solution?
– HCl is a strong acid and dissociates in water
– If 1 mol HCl is placed in 1 L of aqueous
solution it produces 1 mol [H3O+]
– 1.0 x 10-4 M HCl solution has [H3O+]=1.0x10-4M
pH = -log[H3O+]
= -log [H3O+]
= -log [1.0 x 10-4]
= -[-4.00] = 4.00
27. Calculating [H3O+] From pH
Scale for Acids and Bases
8.2 pH: A Measurement
What is the [H3O+] of a solution with pH = 6.00?
pH = -log[H3O+]
• 4.00 = -log [H3O+]
• Multiply both sides of equation by –1
• -4.00 = log [H3O+]
• Take the antilog of both sides
• Antilog -4.00 = [H3O+]
• Antilog is the exponent of 10
• 1.0 x 10-4 M = [H3O+]
28. Calculating the pH of a Base
Scale for Acids and Bases
8.2 pH: A Measurement
What is the pH of a 1.0 x 10-3 M KOH solution?
• KOH is a strong base (as are any metal hydroxides)
• 1 mol KOH dissolved and dissociated in aqueous
solution produces 1 mol OH-
• 1.0 x 10-3 M KOH solution has [OH-] = 1.0 x 10-3 M
1 x 10-14 = [H3O+][OH-]
• Solve equation for [H3O+] = 1 x 10-14 / [OH-]
• [H3O+] = 1 x 10-14 / 1.0 x 10-3 = 1 x 10-11
• pH = -log [1 x 10-11]
pH = -log[H3O+]
= 11.00
29. Calculating pH from Acid
Scale for Acids and Bases
8.2 pH: A Measurement
Molarity
What is the pH of a 2.5 x 10-4 M HNO3 solution?
• We know that as a strong acid HNO3 dissociates
to produce 2.5 x 10-4 M [H3O+]
pH = -log[H3O+]
• pH = -log [2.5 x 10-4]
• = 3.60
30. Calculating [OH-] From pH
Scale for Acids and Bases
8.2 pH: A Measurement
What is the [OH-] of a solution with pH = 4.95?
• First find [H3O+] pH = -log[H O+] 3
• 4.95 = -log [H3O+]
• [H3O+] = 10-4.95
• [H3O+] = 1.12 x 10-5 1 x 10-14 = [H3O+][OH-]
• Now solve for [OH-]
• [OH-] = 1 x 10-14 / 1.12 x 10-5
= 1.0 x 10-9
31. 8.2 pH: A Measurement
Scale for Acids and Bases
The pH Scale
32. For a strong acid For a strong base
Scale for Acids and Bases
HCl molarity pH
8.2 pH: A Measurement
NaOH molarity pH
1.0 x 100 0.00 1.0 x 100 14.00
1.0 x 10-1 1.00 1.0 x 10-1 13.00
More basic
1.0 x 10-2 2.00 1.0 x 10-2 12.00
1.0 x 10-3 3.00 1.0 x 10-3 11.00
1.0 x 10-4 4.00 1.0 x 10-4 10.00
1.0 x 10-5 5.00 1.0 x 10-5 9.00
1.0 x 10-6 6.00 1.0 x 10-6 8.00
ci d c Aer o M
1.0 x 10-7 7.00 1.0 x 10-7 7.00
Each 10 fold change in concentration
i
changes the pH by one unit
33. The Importance of pH and
Scale for Acids and Bases
8.2 pH: A Measurement
pH Control
Any change that takes place in aqueous solution
generally has at least some pH dependence
– Agriculture - crops grow best in soil with proper
pH
– Physiology - blood pH shift of 1 pH is fatal
– Acid Rain - lowers pH of water in aquatic
systems causing problems for native fishes
– Municipal services - sewage treatment and water
purification require optimal pH
– Industry - many processes require strict pH
control for cost-effective production
34. 8.3 Reactions Between Acids
and Bases
• Neutralization reaction - the reaction of an acid
with a base to produce a salt and water
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Acid Base Salt Water
• Break apart into ions:
H+ + Cl- + Na+ + OH- →Na+ + Cl- + H2O
• Net ionic equation
– Show only the changed components
– Omit any ions appearing the same on both sides of
equation = Spectator ions
H+ + OH- → H2O
35. Net Ionic Neutralization Reaction
8.3 Reactions Between
• The net ionic neutralization reaction is more
Acids and Bases
accurately written:
H3O+(aq) + OH-(aq) → 2H2O(l)
• This equation applies to any strong acid / strong
base neutralization reaction
• An analytical technique to determine the
concentration of an acid or base is titration
• Titration involves the addition of measured
amount of a standard solution to neutralize the
second, unknown solution
• Standard solution - solution of known
concentration
36. 8.3 Reactions Between Acid – Base Titration
Buret – long glass
Standard solution
tube calibrated in mL
is slowly added
Acids and Bases
which contains the
until the color
standard solution
changes
The equivalence Indicator – a
point is when the substance which
moles of H3O+ changes color as
pH changes
and OH- are equal
Flask contains a
solution of unknown
concentration plus
indicator
37. 8.4 Acid-Base Buffers
• Buffer solution - solution which resists large
changes in pH when either acids or bases are
added
• These solutions are frequently prepared in
laboratories to maintain optimum conditions
for chemical reactions
• Buffers are also used routinely in
commercial products to maintain optimum
conditions for product behavior
38. 8.4 Acid-Base Buffers The Buffer Process
• Buffers act to establish an equilibrium between a
conjugate acid – base pair
• Buffers consist of either
– a weak acid and its salt (conjugate base)
– a weak base and its salt (conjugate acid)
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
– Acetic acid (CH3COOH) with sodium acetate
(CH3COONa)
• An equilibrium is established in solution
between the acid and the salt anion
• A buffer is Le Chatelier’s principle in action
39. Addition of Base (OH-) to a
Buffer Solution
8.4 Acid-Base Buffers
• Adding a basic substance to a buffer causes
changes
– The OH- will react with the H3O+ producing water
– Acid in the buffer system dissociates to replace
the H3O+ consumed by the added base
– Net result is to maintain the pH close to the initial
level
• The loss of H3O+ (the stress) is compensated
by the dissociation of the acid to produce
more H3O+
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
40. Addition of Acid (H3O+) to a
Buffer Solution
8.4 Acid-Base Buffers
• Adding an acidic substance to a buffer causes
changes
– The H3O+ from the acid will increase the overall
H3O+
– Conjugate base in the buffer system reacts with
the H3O+ to form more acid
– Net result is to maintain the H3O+ concentration
and the pH close to the initial level
• The gain of H3O+ (the stress) is compensated
by the reaction of the conjugate base to
produce more acid
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
41. 8.4 Acid-Base Buffers Buffer Capacity
• Buffer capacity - a measure of the ability
of a solution to resist large changes in
pH when a strong acid or strong base is
added
• Also described as the amount of strong
acid or strong base that a buffer can
neutralize without significantly changing
pH