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.
The document discusses acids and bases. It defines acids as compounds that yield hydrogen ions (H+) when dissolved in water. It provides examples of common acids like hydrochloric acid, nitric acid, sulfuric acid, etc. and describes how each one reacts with water to produce hydrogen ions. The document also classifies acids based on origin, strength, concentration, and number of hydrogen ions produced. Similarly, it defines bases as compounds that yield hydroxide ions (OH-) in water, provides examples, and describes their classification based on strength and concentration.
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,
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.
The answer is C Litmus. Litmus is commonly used as an acid-base indicator that changes color based on whether the solution is acidic or basic. Sodium bicarbonate is a base, vinegar is an acid, and salt is a neutral compound, not an indicator.
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.
1) The document discusses acids and bases, describing their common properties and examples. Acids are defined as compounds that produce hydrogen ions (H+) in water, while bases produce hydroxide ions (OH-).
2) Two theories of acids and bases are described. The Arrhenius theory defines acids as H+ ion producers and bases as OH- ion producers. The Bronsted-Lowry theory expands this to any proton donors as acids and proton acceptors as bases.
3) Acids and bases are classified as strong or weak based on their degree of ionization - strong substances completely ionize while weak ones only partially ionize. Examples of common strong and weak acids and bases are provided.
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.
The document discusses acids and bases. It defines acids as compounds that yield hydrogen ions (H+) when dissolved in water. It provides examples of common acids like hydrochloric acid, nitric acid, sulfuric acid, etc. and describes how each one reacts with water to produce hydrogen ions. The document also classifies acids based on origin, strength, concentration, and number of hydrogen ions produced. Similarly, it defines bases as compounds that yield hydroxide ions (OH-) in water, provides examples, and describes their classification based on strength and concentration.
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,
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.
The answer is C Litmus. Litmus is commonly used as an acid-base indicator that changes color based on whether the solution is acidic or basic. Sodium bicarbonate is a base, vinegar is an acid, and salt is a neutral compound, not an indicator.
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.
1) The document discusses acids and bases, describing their common properties and examples. Acids are defined as compounds that produce hydrogen ions (H+) in water, while bases produce hydroxide ions (OH-).
2) Two theories of acids and bases are described. The Arrhenius theory defines acids as H+ ion producers and bases as OH- ion producers. The Bronsted-Lowry theory expands this to any proton donors as acids and proton acceptors as bases.
3) Acids and bases are classified as strong or weak based on their degree of ionization - strong substances completely ionize while weak ones only partially ionize. Examples of common strong and weak acids and bases are provided.
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.
The document discusses Arrhenius's theory of acids and bases. It defines acids as hydrogen-containing compounds that yield hydrogen ions (H+) in solution, and bases as compounds that yield hydroxide ions (OH-) in solution. It provides examples of common acids like hydrochloric acid and sulfuric acid, as well as bases like sodium hydroxide. It classifies acids based on the number of ionizable hydrogens they contain as mono-, di-, or triprotic. The document also discusses the properties of acids and bases and their reactions in aqueous solutions.
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Acids have a sour taste, turn litmus red, and react with metals and carbonates. Bases have a bitter taste, turn litmus blue, and react with acids to form salts and water. The document also discusses pH scale, uses of acids and bases, and how to classify different types of oxides such as acidic, basic, amphoteric, and neutral oxides based on their chemical properties.
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.
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.
This document provides information about acids and bases, including their properties and reactions. It defines acids as substances that produce hydrogen ions in aqueous solution, and bases as metal oxides or hydroxides. Strong acids are fully ionized in water, while weak acids are only partially ionized. The strength of an acid does not relate to its concentration. Common uses of acids include battery electrolytes, rust removal, and food preservation.
This document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt. Salts are formed when the hydrogen ions in an acid are replaced by metal ions from a base. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction. Common salts have various uses including in fertilizers, batteries, soap making, and more.
The document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt through a neutralization reaction. Salts are formed when hydrogen ions in an acid are replaced by metal ions. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction that forms them. Common salts have various uses including in fertilizers, drying agents, medicines, and other applications.
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 acids, bases, and salts. It defines acids as substances that produce hydrogen ions (H+) in aqueous solution, making them sour and able to turn litmus red. Bases are defined as substances that produce hydroxide ions (OH-) in solution, making them soapy and able to turn litmus blue. Salts are formed by the reaction of acids and bases and can be acidic, basic, or neutral depending on the reactants. Common natural and synthetic acid-base indicators are also described. The document then discusses the properties and reactions of acids, bases, and salts and how pH is used to measure acidity. Finally, several industrial chemicals derived from sodium chloride (common salt) are summarized, including
Acids are substances that increase the concentration of hydrogen ions in water and have a pH below 7. They have a sour taste and can turn litmus paper red. Bases are the opposite and have a bitter taste, turning litmus paper blue. Bases produce hydroxide ions in water. When acids and bases react, they form salts and water through a neutralization reaction. Salts are ionic compounds composed of cations and anions that result from the reaction of acids and bases. They have crystalline structures and come in different varieties depending on if they hydrolyze in water.
Chemistry GCSE Chapter 8 Acid bases and Salts .pptxAnumToqueer
This document discusses acids, bases, and salts. It defines acids as substances that produce hydrogen ions in aqueous solution and bases as substances that produce hydroxide ions in aqueous solution. Examples of strong acids and weak acids are provided. The document also discusses the properties of acids and bases, including their reactions with metals, metal hydroxides, metal carbonates to form salts. It introduces the pH scale for measuring acidity and alkalinity and discusses acid-base indicators. Various types of oxides such as basic, acidic, amphoteric, and neutral oxides are also defined.
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.
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.
This document provides an introduction to acids, bases and salts including:
- The Arrhenius and Bronsted-Lowry theories of acids and bases which define acids as substances that produce H+ ions in water and bases as those that produce OH- ions.
- Common acids like hydrochloric acid and common bases like sodium hydroxide.
- Acid-base reactions include neutralization reactions and reactions with metals and carbonates that produce salts, water and other products.
- Properties of salts like pH, families based on cations and anions, and methods of preparation for common salts.
This document discusses acids, bases, and salts. It defines acids as compounds that produce hydrogen ions (H+) in water, have a pH below 7, and react with metals. Bases are defined as compounds that produce hydroxide ions (OH-) in water and have a pH above 7. Salts are neutral compounds formed by the reaction of acids and bases. Common acids and bases are listed, along with their uses. The pH scale and indicators are also explained.
This document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt through a neutralization reaction. Salts are formed when hydrogen ions in an acid are replaced by metal ions. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction that forms them. Salts have various uses such as in fertilizers, drying agents, medicines, and gunpowder.
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Strong acids and bases completely dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures hydrogen ion concentration and indicates whether a substance is acidic, basic, or neutral. Acid rain occurs when atmospheric pollutants like sulfur and nitrogen oxides dissolve in water to form strong acids. Some substances can act as both acids and bases and are called amphoteric or amphiprotic.
This document provides information about acids, bases, salts, and pH scale. It defines acids and bases, describes their properties and classifications. It discusses the preparation and uses of acids, bases, and salts. It also explains what the pH scale measures, how it indicates acidity and basicity, and how pH values correspond to acids and bases.
The document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt. Salts are formed when the hydrogen ions in an acid are replaced by metal ions from a base. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction. Common salts have various uses including in fertilizers, batteries, drying agents, and soap making.
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Similar to properties of acids base and the law given by scientists
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.
The document discusses Arrhenius's theory of acids and bases. It defines acids as hydrogen-containing compounds that yield hydrogen ions (H+) in solution, and bases as compounds that yield hydroxide ions (OH-) in solution. It provides examples of common acids like hydrochloric acid and sulfuric acid, as well as bases like sodium hydroxide. It classifies acids based on the number of ionizable hydrogens they contain as mono-, di-, or triprotic. The document also discusses the properties of acids and bases and their reactions in aqueous solutions.
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Acids have a sour taste, turn litmus red, and react with metals and carbonates. Bases have a bitter taste, turn litmus blue, and react with acids to form salts and water. The document also discusses pH scale, uses of acids and bases, and how to classify different types of oxides such as acidic, basic, amphoteric, and neutral oxides based on their chemical properties.
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.
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.
This document provides information about acids and bases, including their properties and reactions. It defines acids as substances that produce hydrogen ions in aqueous solution, and bases as metal oxides or hydroxides. Strong acids are fully ionized in water, while weak acids are only partially ionized. The strength of an acid does not relate to its concentration. Common uses of acids include battery electrolytes, rust removal, and food preservation.
This document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt. Salts are formed when the hydrogen ions in an acid are replaced by metal ions from a base. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction. Common salts have various uses including in fertilizers, batteries, soap making, and more.
The document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt through a neutralization reaction. Salts are formed when hydrogen ions in an acid are replaced by metal ions. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction that forms them. Common salts have various uses including in fertilizers, drying agents, medicines, and other applications.
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 acids, bases, and salts. It defines acids as substances that produce hydrogen ions (H+) in aqueous solution, making them sour and able to turn litmus red. Bases are defined as substances that produce hydroxide ions (OH-) in solution, making them soapy and able to turn litmus blue. Salts are formed by the reaction of acids and bases and can be acidic, basic, or neutral depending on the reactants. Common natural and synthetic acid-base indicators are also described. The document then discusses the properties and reactions of acids, bases, and salts and how pH is used to measure acidity. Finally, several industrial chemicals derived from sodium chloride (common salt) are summarized, including
Acids are substances that increase the concentration of hydrogen ions in water and have a pH below 7. They have a sour taste and can turn litmus paper red. Bases are the opposite and have a bitter taste, turning litmus paper blue. Bases produce hydroxide ions in water. When acids and bases react, they form salts and water through a neutralization reaction. Salts are ionic compounds composed of cations and anions that result from the reaction of acids and bases. They have crystalline structures and come in different varieties depending on if they hydrolyze in water.
Chemistry GCSE Chapter 8 Acid bases and Salts .pptxAnumToqueer
This document discusses acids, bases, and salts. It defines acids as substances that produce hydrogen ions in aqueous solution and bases as substances that produce hydroxide ions in aqueous solution. Examples of strong acids and weak acids are provided. The document also discusses the properties of acids and bases, including their reactions with metals, metal hydroxides, metal carbonates to form salts. It introduces the pH scale for measuring acidity and alkalinity and discusses acid-base indicators. Various types of oxides such as basic, acidic, amphoteric, and neutral oxides are also defined.
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.
Chemistry - Chp 19 - Acids, Bases, and Salt - PowerPointsMel Anthony Pepito
This document provides an overview of acids and bases including:
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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.
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This document provides an introduction to acids, bases and salts including:
- The Arrhenius and Bronsted-Lowry theories of acids and bases which define acids as substances that produce H+ ions in water and bases as those that produce OH- ions.
- Common acids like hydrochloric acid and common bases like sodium hydroxide.
- Acid-base reactions include neutralization reactions and reactions with metals and carbonates that produce salts, water and other products.
- Properties of salts like pH, families based on cations and anions, and methods of preparation for common salts.
This document discusses acids, bases, and salts. It defines acids as compounds that produce hydrogen ions (H+) in water, have a pH below 7, and react with metals. Bases are defined as compounds that produce hydroxide ions (OH-) in water and have a pH above 7. Salts are neutral compounds formed by the reaction of acids and bases. Common acids and bases are listed, along with their uses. The pH scale and indicators are also explained.
This document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt through a neutralization reaction. Salts are formed when hydrogen ions in an acid are replaced by metal ions. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction that forms them. Salts have various uses such as in fertilizers, drying agents, medicines, and gunpowder.
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Strong acids and bases completely dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures hydrogen ion concentration and indicates whether a substance is acidic, basic, or neutral. Acid rain occurs when atmospheric pollutants like sulfur and nitrogen oxides dissolve in water to form strong acids. Some substances can act as both acids and bases and are called amphoteric or amphiprotic.
This document provides information about acids, bases, salts, and pH scale. It defines acids and bases, describes their properties and classifications. It discusses the preparation and uses of acids, bases, and salts. It also explains what the pH scale measures, how it indicates acidity and basicity, and how pH values correspond to acids and bases.
The document discusses acids, bases, and salts. It explains that acids contain hydrogen ions and bases contain hydroxide ions. When an acid and base react, they form water and a salt. Salts are formed when the hydrogen ions in an acid are replaced by metal ions from a base. There are different types of salts including normal salts, acid salts, and basic salts depending on the reaction. Common salts have various uses including in fertilizers, batteries, drying agents, and soap making.
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2. Acids
Produce H+ ions in water
Have a sour taste
Break down metals
Formula starts with H
Poisonous and corrosive to skin
pH less than 7
3. Acid
turn blue litmus red
Dissolve in water to form solution which conduct electricity
React with reactive metal metals to form salt and hydrogen (explained)
Acids react with carbonates and hydrogen carbonates to form a salt,
water and carbon dioxide (explained)
Acids react with metal oxides and hydroxides to form a salt and water
only(explained)
4. Alkalis
Produce OH- ions in water
Have a bitter taste and a slippery feel
Break down fats and oils
Formula ends with OH
Poisonous and corrosive to skin
pH greater than 7
5. Alkalis
turn red litmus blue
React with acids to form salt and water only.(explained)
Heated with ammonium salts gives off ammonia gas.(explained)
React with a solution of one metal salt to give another metal salt
and metal hydroxide.(explained)
8. Arrhenius Concept of Acids and Bases
According to the Arrhenius concept of acids and bases, an acid is
a substance that, when dissolved in water, increases the
concentration of hydronium ion (H3O+).
Remember, however, that the aqueous hydrogen ion is actually
chemically bonded to water, that is, H3O+.
9. Arrhenius Concept of Acids and Bases
A base, in the Arrhenius concept, is a substance
that, when dissolved in water, increases the
concentration of hydroxide ion, OH-(aq).
10. Bronsted-Lowry Acid and Bases
Bronsted-Lowry Acid can donate a proton
Bronsted-Lowry Base can accept a proton
Must contain a non-bonding pair of electrons
Conjugate base of an acid is the species remaining after
the acid has lost a proton
11. Bronsted-Lowry Acid and Bases
Conjugate acid is the species formed after the base has
accepted a proton
HCl + H2O ↔ H3O+ + Cl-
Water is conjugate base of H3O+ and Cl- is conjugate
base of HCl
12. Bronsted-Lowry Acid and Bases
Water can act both as acid and base. Amphiprotic
Strong acids have weak conjugate base
Weak acids have strong conjugate base
ACID: Ethanol (C2H5OH) =>weak
CONJUGATE BASE: Ethoxide ion (C2H5O-) => strong
13. Lewis Acids and Bases
Bases can donate a pair of electrons
Acids can accept a pair of electrons
Covalent bond is formed
Many Lewis Acids don’t contain hydrogen
15. Properties of Acids and Bases
Neutralization reaction with bases
With hydroxides to form salt and water
CH3COOH + NaOH NaCH3COO + H2O
With metal oxides to form a salt and water
H2SO4 + CuO CuSO4 + H2O
With ammonia to form salt
HCl + NH3 NH4Cl
16. Properties of Acids and Bases
With reactive metals to form salt and hydrogen
2HCl + Mg MgCl2 + H2
With carbonates to form salt, CO2, water
2HCl + CaCO3 CaCl2 + CO2 + H2O
With hydrogen carbonates to form salt, CO2, water
HCl + NaHCO3 NaCl + CO2 + H2O
17. Strong Acids and Bases
Strong acid and base is completely dissociated (ionized) into its
ions in aqueous solutions
Strong acids
HCl (Hydrochloric acid)
HNO3 (Nitric Acid)
H2SO4 (Sulfuric Acid)
19. Weak Acids and Bases
Weak acids and bases is slightly dissociated into their ions in
aqueous solution
Weak acids
CH3COOH (Ethanoic Acid)
H2CO3(Carbonic acid)
21. Acidic oxides
Acidic oxides are the oxides of non-metals. When combined with
water, they produce acids, e.g.,
Acidic oxides are, therefore, known as acid anhydrides, e.g.,
Sulphur dioxide is sulphurous anhydride; Sulphur trioxide is
sulphuric anhydride.
22. Basic oxides
Basic oxides are the oxides of metals. If soluble in water they react with
water to produce hydroxides (alkalis).
Basic oxides do not reacts with alkalis.
Examples:
CaO + H2O Ca(OH)2
MgO + H2O Mg(OH)2
23. Amphoteric oxides
Amphoteric oxides are metallic oxides, which show both basic as
well as acidic properties. When they react with an acid, they
produce salt and water, showing basic properties. While reacting
with alkalis they form salt and water showing acidic properties
24. Neutral oxides
These are the oxides, which show neither basic nor acidic
properties, that is, they do not form salts when reacted with acids
or bases, e.g., carbon monoxide (CO); nitrous oxide (N2O); nitric
oxide (NO), etc., are neutral oxides.