An oxide is a compound formed from oxygen and another element. There are four main types of oxides: acidic, basic, amphoteric, and neutral. Acidic oxides dissolve in water to form acids, basic oxides are insoluble in water and react with acids to form salts, amphoteric oxides react with both acids and bases, and neutral oxides do not react with acids or bases. Common examples of each type and their reactions are provided.
19.1 acids, base and salts By Hamdy KarimHamdy Karim
Students will be able to compare between Arrhenius, Bronsted-Lowry, and Lewis theories to identify the acids and bases concept. They also will study the conjugated acids and bases in addition to the Amphoteric Substances as well!
An acid is a substance that produces hydrogen ions in water and has a pH less than 7. Strong acids, like hydrochloric acid, are completely ionized in water, while weak acids like acetic acid only partially ionize. Acids react with metals to produce salts and hydrogen gas, with carbonates to produce salts, water and carbon dioxide gas, and with bases to produce salts and water. They have sour tastes and are corrosive.
This document discusses three main types of chemical bonding: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between metals and nonmetals through the transfer of electrons from one atom to another, producing charged ions. Covalent bonds form between nonmetals of similar electronegativity through the sharing of electron pairs. Metallic bonds form between metallic elements through a shared "electron cloud" that holds the atoms together strongly.
This document defines acids and bases, describing their properties and common uses. Acids have a pH below 7 and taste sour, while bases have a pH above 7 and feel soapy. The document explains that acids and bases react through neutralization, forming less acidic or basic salt mixtures. Common acids include acetic, citric, and sulfuric acids, which are found in vinegar, fruits, and industrial chemicals, while bases are found in soaps, cleaners, and the human body.
Acids, bases and salts according to the syllabus of CAIE and IGCSEjaveriakhan123
This document provides information about acids and bases:
- Acids are substances that produce hydrogen ions in water and have properties like a sour taste and turning litmus paper red. Strong acids fully ionize in water while weak acids only partially ionize.
- Bases include metal oxides and hydroxides. Soluble bases are called alkalis. Bases react with acids to produce salt and water in a neutralization reaction.
- Important acids and bases have many applications from batteries to cleaning to food preservation. Processes like the Contact Process are used industrially to produce acids like sulfuric acid.
This document discusses different types of oxides based on their reactions with water and acids or bases. It defines acidic, basic, amphoteric, and neutral oxides. Acidic oxides react with water to form acids, while basic oxides react with acids to form salts and water. Amphoteric oxides can behave as either acidic or basic oxides depending on the reaction. Neutral oxides show no acidic or basic properties and are insoluble in water. The document provides examples of common oxides that fall into each category and an decision tree for classifying an unknown oxide based on its solubility properties.
The three main categories of chemical compounds are acids, bases and salts. These compounds are always part of our daily lives in terms of what we eat and use. The human body contains some very common acids like dilute hydrochloric acid in the stomach, which aids in digestion of food. If the contents of our stomach become too acidic, it results to a burning sensation in the stomach. Acids and bases also regulate metabolic activities in the human body through equilibrium processes. Acids contain hydrogen ions (H+). A base is a substance, which on dissolving in water yields hydroxyl ions (OH-) as the only negative ions. Salts are formed by the combination of an acid and base.
An oxide is a compound formed from oxygen and another element. There are four main types of oxides: acidic, basic, amphoteric, and neutral. Acidic oxides dissolve in water to form acids, basic oxides are insoluble in water and react with acids to form salts, amphoteric oxides react with both acids and bases, and neutral oxides do not react with acids or bases. Common examples of each type and their reactions are provided.
19.1 acids, base and salts By Hamdy KarimHamdy Karim
Students will be able to compare between Arrhenius, Bronsted-Lowry, and Lewis theories to identify the acids and bases concept. They also will study the conjugated acids and bases in addition to the Amphoteric Substances as well!
An acid is a substance that produces hydrogen ions in water and has a pH less than 7. Strong acids, like hydrochloric acid, are completely ionized in water, while weak acids like acetic acid only partially ionize. Acids react with metals to produce salts and hydrogen gas, with carbonates to produce salts, water and carbon dioxide gas, and with bases to produce salts and water. They have sour tastes and are corrosive.
This document discusses three main types of chemical bonding: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between metals and nonmetals through the transfer of electrons from one atom to another, producing charged ions. Covalent bonds form between nonmetals of similar electronegativity through the sharing of electron pairs. Metallic bonds form between metallic elements through a shared "electron cloud" that holds the atoms together strongly.
This document defines acids and bases, describing their properties and common uses. Acids have a pH below 7 and taste sour, while bases have a pH above 7 and feel soapy. The document explains that acids and bases react through neutralization, forming less acidic or basic salt mixtures. Common acids include acetic, citric, and sulfuric acids, which are found in vinegar, fruits, and industrial chemicals, while bases are found in soaps, cleaners, and the human body.
Acids, bases and salts according to the syllabus of CAIE and IGCSEjaveriakhan123
This document provides information about acids and bases:
- Acids are substances that produce hydrogen ions in water and have properties like a sour taste and turning litmus paper red. Strong acids fully ionize in water while weak acids only partially ionize.
- Bases include metal oxides and hydroxides. Soluble bases are called alkalis. Bases react with acids to produce salt and water in a neutralization reaction.
- Important acids and bases have many applications from batteries to cleaning to food preservation. Processes like the Contact Process are used industrially to produce acids like sulfuric acid.
This document discusses different types of oxides based on their reactions with water and acids or bases. It defines acidic, basic, amphoteric, and neutral oxides. Acidic oxides react with water to form acids, while basic oxides react with acids to form salts and water. Amphoteric oxides can behave as either acidic or basic oxides depending on the reaction. Neutral oxides show no acidic or basic properties and are insoluble in water. The document provides examples of common oxides that fall into each category and an decision tree for classifying an unknown oxide based on its solubility properties.
The three main categories of chemical compounds are acids, bases and salts. These compounds are always part of our daily lives in terms of what we eat and use. The human body contains some very common acids like dilute hydrochloric acid in the stomach, which aids in digestion of food. If the contents of our stomach become too acidic, it results to a burning sensation in the stomach. Acids and bases also regulate metabolic activities in the human body through equilibrium processes. Acids contain hydrogen ions (H+). A base is a substance, which on dissolving in water yields hydroxyl ions (OH-) as the only negative ions. Salts are formed by the combination of an acid and base.
Acids produce hydrogen ions (H+) in aqueous solutions, have a pH below 7, taste sour, and react with bases. Examples include citric acid and hydrochloric acid. Bases produce hydroxide ions (OH-) in water, have a pH above 7, taste bitter, and feel soapy. Examples include sodium hydroxide and potassium hydroxide. The strength of acids and bases is determined by their level of ionization, with strong acids and bases having near complete ionization and weak ones having little ionization. The pH scale is used to measure acidity and alkalinity.
Chapter 15.1 : Properties of Acids and BasesChris Foltz
This document discusses the properties and nomenclature of acids and bases. It defines acids as substances that increase the hydrogen ion concentration in aqueous solutions, and bases as substances that increase the hydroxide ion concentration. Strong acids fully ionize in water, producing hydronium ions, while weak acids only partially ionize. Common strong acids include sulfuric acid and nitric acid. Common bases, such as sodium hydroxide, fully dissociate in water to produce hydroxide ions. The document also provides examples of uses for several acids in industry and food processing.
6.3 (a) electrolysis of an aqueous solutionAzieda Dot
The document discusses the electrolysis of aqueous solutions. It explains that during electrolysis, only one ion is selectively discharged at each electrode based on its position in the electrochemical series, the nature of the electrode, and the concentration of ions. The ion discharged at the anode depends on which is easier to oxidize, while the ion discharged at the cathode depends on which is easier to reduce. Different products are formed depending on these factors and the specific electrolyte used.
This document discusses the properties and reactions of acids and bases. It states that acids have a sour taste and cause color changes in indicators like litmus. Acids react with metals to produce hydrogen gas and with carbonates to produce carbon dioxide gas. Bases have a bitter taste and feel slippery. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Water can act as both an acid and a base depending on the reaction.
Strong acids and strong bases always react in the same format since the dissociate nearly 100% in water.
Solutions of hydrochloric acid and sodium hydroxide are mixed the reaction occurs as follows:
Weak acids dissociate only slightly in water, and therefore should be left combined and not written as its ions. When weak acids react with strong bases, the H+ from the weak acid is transferred to the OH- from the strong base to form water and a salt. The salt formed, however, will most likely be soluble, and should be written as its respective ions. Remember also, to cancel out any spectator ions.
This document discusses acids, bases, salts, and indicators. It defines acids as sour substances that produce hydrogen ions in solution and have a pH below 7. Bases are defined as having a pH above 7 and forming hydroxide ions in solution. Examples of common acids and bases are provided. Indicators are substances that change color in acidic versus basic solutions, allowing the pH to be determined. Strong acids and bases fully ionize in solution, while weak ones only partially ionize. Neutralization occurs when an acid and base react to form a salt and water. Salts are neutral compounds composed of acid anions and base cations.
This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and have a pH less than 7. Acids have properties such as turning litmus red and reacting with metals. Bases are defined as substances that produce OH- ions in water and have a pH greater than 7. They have properties such as turning litmus blue and reacting with acids to form salt and water. Strong acids and bases are fully dissociated in water while weak acids and bases are only partially dissociated. The document also discusses Bronsted-Lowry and Lewis acid-base theories.
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7 and describes their properties such as neutralizing bases and forming hydrogen ions in solution. Strong acids like hydrochloric acid are described as ionizing completely, while weak acids only partially ionize. Common acids are also listed such as hydrochloric acid found in stomachs. Bases are defined as having a pH greater than 7 and their properties are outlined. The document further discusses pH scales, indicators, buffers, and examples of acid-base reactions. Digestion and pH levels in different parts of the digestive system are briefly covered.
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Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases completely ionize in water, while weak acids and bases only partially ionize. Common strong acids include sulfuric acid and hydrochloric acid, while strong bases include lithium hydroxide and sodium hydroxide. When acids and bases are mixed, they neutralize each other through a reaction that produces water and a salt. Indicators change color depending on whether the solution is acidic or basic, and can be used to measure the pH of a solution.
In this slide you can get about ,what are oxides and how they classify. In this slides I classify the oxides with respect to nature of oxides as well as the oxygen content in it.
THIS PPT WILL EXPLAIN YOU ALL ABOUT ACID AND BASE AND THEORIES OF ACID AND BASE . THIS IS VERY HELPFUL FOR THE STUDENTS FROM DIPLOMA AND BACHELOR PHARMACY STUDENTS.
This document discusses the preparation of salts. It describes two methods for preparing soluble salts: 1) Adding an acid to a solid metal, base, or carbonate and 2) Reacting a dilute acid and alkali through neutralization. It also describes preparing insoluble salts through precipitation reactions. The key steps for each method are outlined, including dissolving reactants, filtering, evaporating solutions, and drying crystals. Examples are provided for preparing copper (II) sulfate using method 1 and lead (II) sulfate using a precipitation reaction between lead (II) nitrate and potassium sulfate solutions.
This document defines acids, bases, and salts according to three theories:
1) Arrhenius defines acids as substances that yield hydrogen ions in water and bases as substances that yield hydroxide ions in water. Neutralization produces salt and water.
2) Bronsted-Lowry defines acids as proton donors and bases as proton acceptors. Neutralization involves the transfer of a proton from an acid to a base.
3) Lewis defines acids as electron pair acceptors and bases as electron pair donors. Neutralization involves the sharing of an electron pair between an acid and base.
This document provides an introduction to acids, bases, and salts for GCSE chemistry students. It discusses key topics like acidity and alkalinity, indicators, the pH scale, types of acids including strong and weak acids, and various methods for making salts through reactions between acids and metals, metal oxides, metal carbonates, metal hydroxides, and ammonia. The document is intended to help students understand and revise these core chemistry concepts in preparation for their exams.
A solution is a homogeneous mixture of two or more substances where a solute is dissolved in a solvent. The concentration of a solution refers to the amount of solute dissolved in a fixed amount of solvent. Solutions can be dilute, containing a small amount of solute, or concentrated, containing a large amount of solute. Soft drinks are considered solutions but contain many unhealthy additives like sugar, artificial sweeteners, caffeine, carbon dioxide, preservatives, artificial flavors, colorings, and sodium. Long term consumption of soft drinks can increase risks of diseases, cancer, and other health issues.
This document discusses haloalkanes and haloarenes. It begins by classifying haloalkanes based on the number of halogen atoms attached to the carbon. It then discusses IUPAC and common naming of these compounds. It describes the nature of C-X bonds and how bond length, enthalpy, stability, and reactivity vary based on the halogen atom. Methods of preparing haloalkanes from alcohols and hydrocarbons are presented. The document discusses physical properties, nucleophilic substitution reactions, elimination reactions, and reactions of haloarenes such as with Grignard reagents and the Wurtz reaction. Health effects of some common haloalkanes like dichloromethane and trich
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
- 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 discusses the Brønsted-Lowry theory of acids and bases. It defines acids as proton donors and bases as proton acceptors. An acid-base pair consists of a conjugate acid and conjugate base, where the acid donates a proton to form the conjugate base, or the base accepts a proton to form the conjugate acid. Water is described as amphiprotic because it can act as both an acid and a base. Examples of acid-base reactions and identification of conjugate species are provided.
Acids produce hydrogen ions (H+) in aqueous solutions, have a pH below 7, taste sour, and react with bases. Examples include citric acid and hydrochloric acid. Bases produce hydroxide ions (OH-) in water, have a pH above 7, taste bitter, and feel soapy. Examples include sodium hydroxide and potassium hydroxide. The strength of acids and bases is determined by their level of ionization, with strong acids and bases having near complete ionization and weak ones having little ionization. The pH scale is used to measure acidity and alkalinity.
Chapter 15.1 : Properties of Acids and BasesChris Foltz
This document discusses the properties and nomenclature of acids and bases. It defines acids as substances that increase the hydrogen ion concentration in aqueous solutions, and bases as substances that increase the hydroxide ion concentration. Strong acids fully ionize in water, producing hydronium ions, while weak acids only partially ionize. Common strong acids include sulfuric acid and nitric acid. Common bases, such as sodium hydroxide, fully dissociate in water to produce hydroxide ions. The document also provides examples of uses for several acids in industry and food processing.
6.3 (a) electrolysis of an aqueous solutionAzieda Dot
The document discusses the electrolysis of aqueous solutions. It explains that during electrolysis, only one ion is selectively discharged at each electrode based on its position in the electrochemical series, the nature of the electrode, and the concentration of ions. The ion discharged at the anode depends on which is easier to oxidize, while the ion discharged at the cathode depends on which is easier to reduce. Different products are formed depending on these factors and the specific electrolyte used.
This document discusses the properties and reactions of acids and bases. It states that acids have a sour taste and cause color changes in indicators like litmus. Acids react with metals to produce hydrogen gas and with carbonates to produce carbon dioxide gas. Bases have a bitter taste and feel slippery. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Water can act as both an acid and a base depending on the reaction.
Strong acids and strong bases always react in the same format since the dissociate nearly 100% in water.
Solutions of hydrochloric acid and sodium hydroxide are mixed the reaction occurs as follows:
Weak acids dissociate only slightly in water, and therefore should be left combined and not written as its ions. When weak acids react with strong bases, the H+ from the weak acid is transferred to the OH- from the strong base to form water and a salt. The salt formed, however, will most likely be soluble, and should be written as its respective ions. Remember also, to cancel out any spectator ions.
This document discusses acids, bases, salts, and indicators. It defines acids as sour substances that produce hydrogen ions in solution and have a pH below 7. Bases are defined as having a pH above 7 and forming hydroxide ions in solution. Examples of common acids and bases are provided. Indicators are substances that change color in acidic versus basic solutions, allowing the pH to be determined. Strong acids and bases fully ionize in solution, while weak ones only partially ionize. Neutralization occurs when an acid and base react to form a salt and water. Salts are neutral compounds composed of acid anions and base cations.
This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and have a pH less than 7. Acids have properties such as turning litmus red and reacting with metals. Bases are defined as substances that produce OH- ions in water and have a pH greater than 7. They have properties such as turning litmus blue and reacting with acids to form salt and water. Strong acids and bases are fully dissociated in water while weak acids and bases are only partially dissociated. The document also discusses Bronsted-Lowry and Lewis acid-base theories.
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7 and describes their properties such as neutralizing bases and forming hydrogen ions in solution. Strong acids like hydrochloric acid are described as ionizing completely, while weak acids only partially ionize. Common acids are also listed such as hydrochloric acid found in stomachs. Bases are defined as having a pH greater than 7 and their properties are outlined. The document further discusses pH scales, indicators, buffers, and examples of acid-base reactions. Digestion and pH levels in different parts of the digestive system are briefly covered.
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Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases completely ionize in water, while weak acids and bases only partially ionize. Common strong acids include sulfuric acid and hydrochloric acid, while strong bases include lithium hydroxide and sodium hydroxide. When acids and bases are mixed, they neutralize each other through a reaction that produces water and a salt. Indicators change color depending on whether the solution is acidic or basic, and can be used to measure the pH of a solution.
In this slide you can get about ,what are oxides and how they classify. In this slides I classify the oxides with respect to nature of oxides as well as the oxygen content in it.
THIS PPT WILL EXPLAIN YOU ALL ABOUT ACID AND BASE AND THEORIES OF ACID AND BASE . THIS IS VERY HELPFUL FOR THE STUDENTS FROM DIPLOMA AND BACHELOR PHARMACY STUDENTS.
This document discusses the preparation of salts. It describes two methods for preparing soluble salts: 1) Adding an acid to a solid metal, base, or carbonate and 2) Reacting a dilute acid and alkali through neutralization. It also describes preparing insoluble salts through precipitation reactions. The key steps for each method are outlined, including dissolving reactants, filtering, evaporating solutions, and drying crystals. Examples are provided for preparing copper (II) sulfate using method 1 and lead (II) sulfate using a precipitation reaction between lead (II) nitrate and potassium sulfate solutions.
This document defines acids, bases, and salts according to three theories:
1) Arrhenius defines acids as substances that yield hydrogen ions in water and bases as substances that yield hydroxide ions in water. Neutralization produces salt and water.
2) Bronsted-Lowry defines acids as proton donors and bases as proton acceptors. Neutralization involves the transfer of a proton from an acid to a base.
3) Lewis defines acids as electron pair acceptors and bases as electron pair donors. Neutralization involves the sharing of an electron pair between an acid and base.
This document provides an introduction to acids, bases, and salts for GCSE chemistry students. It discusses key topics like acidity and alkalinity, indicators, the pH scale, types of acids including strong and weak acids, and various methods for making salts through reactions between acids and metals, metal oxides, metal carbonates, metal hydroxides, and ammonia. The document is intended to help students understand and revise these core chemistry concepts in preparation for their exams.
A solution is a homogeneous mixture of two or more substances where a solute is dissolved in a solvent. The concentration of a solution refers to the amount of solute dissolved in a fixed amount of solvent. Solutions can be dilute, containing a small amount of solute, or concentrated, containing a large amount of solute. Soft drinks are considered solutions but contain many unhealthy additives like sugar, artificial sweeteners, caffeine, carbon dioxide, preservatives, artificial flavors, colorings, and sodium. Long term consumption of soft drinks can increase risks of diseases, cancer, and other health issues.
This document discusses haloalkanes and haloarenes. It begins by classifying haloalkanes based on the number of halogen atoms attached to the carbon. It then discusses IUPAC and common naming of these compounds. It describes the nature of C-X bonds and how bond length, enthalpy, stability, and reactivity vary based on the halogen atom. Methods of preparing haloalkanes from alcohols and hydrocarbons are presented. The document discusses physical properties, nucleophilic substitution reactions, elimination reactions, and reactions of haloarenes such as with Grignard reagents and the Wurtz reaction. Health effects of some common haloalkanes like dichloromethane and trich
This document discusses different types of oxides:
- Acidic oxides are formed from nonmetals and produce acidic solutions. Basic oxides are formed from metals and produce basic solutions.
- Neutral oxides do not react with acids or bases. Amphoteric oxides can behave as either acids or bases depending on the other reactants.
- Common acidic oxides include SO2 and SiO2. Sodium oxide (Na2O) and calcium oxide (CaO) are examples of basic oxides. Zinc oxide and aluminum oxide are amphoteric oxides that can react as either acids or bases.
- 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 discusses the Brønsted-Lowry theory of acids and bases. It defines acids as proton donors and bases as proton acceptors. An acid-base pair consists of a conjugate acid and conjugate base, where the acid donates a proton to form the conjugate base, or the base accepts a proton to form the conjugate acid. Water is described as amphiprotic because it can act as both an acid and a base. Examples of acid-base reactions and identification of conjugate species are provided.
Acid base Theories
Role of the solvents
Acid base dissociation constant,
Relative strength of acids and bases
Distribution of acid base species with pH
Buffer solution
Henderson Hasselbalch equation,
Indicators, Mixed indicators
Different type of titrations (Neutralization curves)
Polyprotic systems,
Phosphoric acid system,
Polyamine and amino acid systems.
Titration of sodium carbonate
Lavoisier definition
Liebig definition
Arrhenius Acids and Bases
Bronsted-Lowry Acid and Base
Lewis Acid and Base
Solvent-system Concept
Lux-Flood Concept
Pearson’s Concept
Historically, the first of the scientific concepts of acids and bases was provided by the French chemist Antoine Lavoisier, circa 1776.
Lavoisier's knowledge of strong acids was mainly restricted to oxyacids, which tend to contain central atoms in high oxidation states surrounded by oxygen, such as HNO3 and H2SO4, and he was not aware of the true composition of the hydrohalic acids, HCl, HBr, and HI. From his limited knowledge,
He defined acids in terms of their content of oxygen, and he named oxygen from Greek words meaning "acid-former"
PHYSICAL CHEMISTRY 1.2- ACIDS,BASES AND SALTSshahzadebaujiti
This document discusses acids, bases, and pH. It defines acids and bases according to Arrhenius, Bronsted-Lowry, and Lewis theories. The key points are:
1) Arrhenius defined acids as producing H+ ions in water and bases as producing OH- ions. Bronsted-Lowry expanded this to include proton donors and acceptors in any solvent.
2) Lewis defined acids and bases in terms of electron pair acceptance and donation.
3) Conjugate acid-base pairs are related - the conjugate base of an acid is its corresponding base, and vice versa.
4) pH measures hydrogen ion concentration on a logarithmic scale from 0-14.
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 and bases buffers ARRHENIUS CONCEPT
THE LEWIS CONCEPT-THE ELECTRON DONOR ACCEPTOR SYSTEM
BRONSTED-LOWRY CONCEPT (PROTON TRANSFER
THEORY
buffer action
ph scale
buffer capacity
acid base balance
isotonicity method
isotonic soltions
buffer solutions in pharmaceutical preparations
This document provides an overview of acid-base titration including definitions, concepts, and procedures. It discusses the Arrhenius, Bronsted-Lowry, and Lewis definitions of acids and bases. It explains the process of ionization and factors that influence it such as relative permittivity. Key aspects of acid-base titration covered include types of reactions that can occur, use of indicators, and standards. The document also discusses acid and base ionization constants and how they relate to strength. Examples are provided to illustrate acid strength calculations and indicator color changes corresponding to pH.
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 summarizes acids and bases according to two theories - Arrhenius and Bronsted-Lowry. According to Arrhenius, an acid is a substance that ionizes in water to produce hydrogen ions, while a base produces hydroxide ions. Bronsted-Lowry defined acids as proton donors and bases as proton acceptors, with no requirement for aqueous solutions. Conjugate acid-base pairs are also discussed, where a conjugate acid is a base that accepts a proton, and a conjugate base is an acid that donates a proton.
The document discusses different concepts of acids and bases including:
1. Arrhenius concept which defines acids as substances that produce H+ ions in water and bases as substances that produce OH- ions.
2. Bronsted-Lowry concept which defines acids as proton donors and bases as proton acceptors.
3. Lewis concept which defines acids as electron pair acceptors and bases as electron pair donors and can explain acid-base reactions not involving proton transfer.
Hydrogen bonding is also discussed as the electrostatic attraction between hydrogen atoms covalently bonded to electronegative atoms. Hydrogen bonding influences properties like melting/boiling points and aggregation of molecules.
This document discusses different concepts of acids and bases, including:
1) The Arrhenius concept defines an acid as a substance that produces hydrogen ions (H+) in aqueous solution, and a base as a substance that produces hydroxide ions (OH-).
2) The Brønsted-Lowry concept defines acids as proton donors and bases as proton acceptors. This allows any hydrogen-containing compound to act as an acid through proton transfer.
3) The Lewis concept further expands the definition of acids and bases to include compounds without hydrogen, such as AlCl3 acting as an acid and Na2CO3 acting as a base by accepting or donating electron pairs.
Diploma_I_Applied science(chemistry)U-III Acid & bases Rai University
1) Acids cause substances like lemons and food to be sour and can damage materials like teeth and sculptures. Acids have positively charged hydrogen ions and turn litmus red.
2) Bases have negatively charged hydroxide ions, feel slippery, and turn litmus blue. Common bases include hand soaps and drain cleaners.
3) The Brønsted-Lowry concept defines acids as proton donors and bases as proton acceptors in reversible acid-base reactions. Both acids and bases can act as conjugates of each other by gaining or losing protons.
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
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.
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 Lewis acids and bases, strong acids and bases, pH and pOH scales, autoionization of water, and buffer solutions. It provides definitions and examples of Arrhenius acids and bases, Bronsted-Lowry acids and bases, and Lewis acids and bases. It also discusses properties of strong acids and bases, calculating pH and pOH, and how buffer solutions resist changes in pH through acid-base equilibriums.
This document discusses various concepts of acids and bases. It begins by describing the early definitions of acids and bases based on their observable properties. It then discusses the Arrhenius theory which defined acids as substances that produce H+ ions in aqueous solution and bases as those that produce OH- ions. The Bronsted-Lowry and Lewis theories expanded these definitions to include proton transfer and electron pair donation/acceptance respectively. The document also discusses hard/soft acids and bases, buffers, and methods for adjusting tonicity and pH.
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
1. The document discusses concepts related to chemistry including pH, pOH, buffer solutions, acid-base theories, and applications of pH.
2. It defines pH as a measurement of acidity or basicity and explains pOH and the ionic product of water. Buffer solutions are described as preventing changes in pH when acids or bases are added.
3. Acid-base theories of Arrhenius, Brønsted-Lowry, and Lewis are outlined along with examples. Applications of pH in industries such as textiles, sugar production, and leather tanning are highlighted.
1. The document discusses various properties of matter and how they are used to classify and identify different types of matter. It describes extensive properties that depend on amount and intensive properties that depend on type.
2. Mixtures and pure substances are introduced. Heterogeneous mixtures are non-uniform while homogeneous mixtures are uniform throughout. Elements have a unique set of properties while compounds contain two or more elements.
3. The three states of matter are defined as solid, liquid, and gas. Physical and chemical changes are distinguished based on whether the composition changes. Chemical symbols and formulas are used to represent elements and compounds in chemical reactions.
1. Matter is everything that has mass and takes up space, and is composed of atoms. There are three main states of matter: solids, liquids, and gases.
2. Solids have a definite shape and volume, with molecules close together. Liquids take the shape of their container but maintain a constant volume. Gases fill their container and have no definite shape or volume.
3. Physical properties can be observed without changing the identity of the substance, such as density, melting point, and boiling point. Changes in state are physical changes. Chemical changes alter the chemical composition.
This document describes the four spheres that make up Earth's systems - the hydrosphere, atmosphere, geosphere, and biosphere. It provides details on each sphere, including that the hydrosphere is made up of 71% of Earth's surface as oceans and saltwater, while the atmosphere is a thin gaseous envelope composed of nitrogen, oxygen, water vapor and aerosols. The document also notes that the geosphere encompasses Earth's solid interior from the crust to the core, and the biosphere incorporates all living things on the planet.
This document discusses various topics in Euclidean geometry for Grade 10 including angles, triangles, congruency, similarity, Pythagoras' theorem, quadrilaterals, parallelograms, rectangles, rhombuses, squares, trapezoids, kites, and the mid-point theorem. It provides definitions and properties for each shape. The mid-point theorem states that the line joining the mid-points of two sides of a triangle is parallel to the third side and equal to half its length.
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This document discusses projectile motion, including:
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This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
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LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
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9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
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2. OBJECTIVES:
a) Define an acid and the base according
to Bronsted-Lowry definition.
b) Explain using the chemical equation
how a proton transfer occur.
c) Identify an conjugate acid-base pairs.
3. Bronsted-lowry definition of
acids and bases
Bronsted and Lowry explain
acid and base based on their
actions in a chemical reaction.
Their theory is the
development of Arrhenius
theory or simply an expansion
of Arrhenius acid definition.
4. The Brønsted-Lowry Model
Definition:
The Brønsted-Lowry Model of
acids and bases states that an
acid is a hydrogen ion donor,
and a base is a hydrogen ion
acceptor.
5. The Brønsted-Lowry Model
Example on proton transfer
Acids are proton donors, hence acids
release protons in the presence of bases
Bases are proton accepters, hence bases
take up protons in the presence of acids
𝐻𝐶𝑙 𝑔 → 𝐻+
𝑎𝑞 + 𝐶𝑙−
𝑎𝑞 𝑁𝐻3 𝑔 + 𝐻+ →. 𝑁𝐻4
+
.
6. The Brønsted-Lowry Model
As the results Brønsted and Lowry rectify Arrhenius Model Limitations that:
Acid-base reaction only occurs in aqueous medium.
The bases are substances that only produce hydroxide ions 𝑂𝐻−
.
A Base without Hydroxide ions
7. The Brønsted-Lowry Model
examples:
– NH3(aq) + H2O(l) ↔ NH4
+(aq) + OH–(aq)
– NH3 = base, H2O(l) = acid, NH4
+ = conjugate
acid, OH– = conjugate base
NB: ‘’The examples above implies that water can act both as an acid and a base
depending on whether is acid or base among the reactants’’
8. The Brønsted-Lowry Model
water among reactants:
When an acid is dissolved in water, the reaction involves the transfer of a proton
from the acid to the water.
Also, when a base is dissolved in water, the reaction involves proton transfer
from water to the base.
NB: As a proton is small and unstable, and when present in water, the
water and the proton react to form a hydronium or oxonium ion,
represented as
9. The Brønsted-Lowry Model
conjugate acid-base pair
When an acid donates its proton, the remaining part of the acid is called the
conjugate base of that acid.
10. The Brønsted-Lowry Model
conjugate acid-base pair
Also, when a base accepts a proton, the remaining part of the base is called the
conjugate acid of that base.
11. The Brønsted-Lowry Model
conjugate acid-base pair
Hence, together the acid and its conjugate base are known as an
conjugate acid-base pair. The same thing apply on a base and its
conjugate acid.
12. HENCE, a reaction must have
an acid, a base, a conjugate
acid and a conjugate base
13. The Brønsted-Lowry Model
summary
1) An acid donates a proton and becomes a
conjugate base.
2) A base accepts a proton and becomes a
conjugate acid.
3) Ampholytes are substances that can behave
either as an acid or a base
15. Determine the acid, base, conjugate
acid and conjugate base!
1). 𝐻𝐶𝑙 𝑎𝑞 + 𝑁𝑎𝑂𝐻 𝑎𝑞 → 𝑁𝑎𝐶𝑙 𝑎𝑞 + 𝐻2 𝑂 𝑎𝑞
2). 𝐻2 𝑆𝑂4 + 𝐻2 𝑂 → 𝐻3 𝑂+
+ 𝐻𝑆𝑂−
4
3). The hydrogen sulfite ion, HSO3-, is amphoteric. Write
its equations with water, acting as both acid and base.
16. The Brønsted-Lowry Model
REFERENCES
Bookstaver, JD. chapter 16 Acids and Bases. Available from Slideshare at
https://www.slideshare.net/jhamze/ap-chemistry-chapter-16-
outline?qid=2304d113-e70f-4cc2-bb2f-1821a377f48d&v=&b=&from_search=42
(Accessed 18 September 2017).
Joshi, M. (2010), Acids, Bases and Salt. A Guide for GCSE Students. Available from
Slideshare at https://www.slideshare.net/maitreyeej3/acids-bases-and-salts-igcse-
chemistry?qid=225b168e-a754-420f-8423-7b02ee3599a5&v=&b=&from_search=7
(Accessed 18 September 2017).
17. The Brønsted-Lowry Model
REFERENCES
Mani, PK. Acid-Base Titration. Available from Slideshare at
https://www.slideshare.net/pabitramani/titrimetrey-as-analytical-
tool?qid=2304d113-e70f-4cc2-bb2f-1821a377f48d&v=&b=&from_search=4
(Accessed 18 September 2017).
Muñoa, R. Acids and Bases: Theory. Available from Slideshare at
https://www.slideshare.net/rafamunoa/theories-5865342?qid=2304d113-e70f-
4cc2-bb2f-1821a377f48d&v=&b=&from_search=5 (Accessed 18 September 2017).
18. The Brønsted-Lowry Model
REFERENCES
Vania and michelle. (2011). Brønsted-Lowry Acids and Bases. Available from
Slideshare at https://www.slideshare.net/vanialundina/acid-base-
7323554?qid=2304d113-e70f-4cc2-bb2f-1821a377f48d&v=&b=&from_search=17
(Accessed 18 September 2017).