acids basis and salts
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Acids have a pH below 7 and donate hydrogen ions in solution. They react with bases and metals. Common acids include hydrochloric acid and citric acid. Bases have a pH above 7 and accept hydrogen ions, feeling slippery. Common bases are sodium hydroxide and ammonia. When an acid and base react, they form a salt and water. Salts are neutral and composed of the ions of the original acid and base. The digestive system uses acids and bases to break down foods, with acid in the stomach and bases in the intestines.
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Acids and bases
This document discusses acids and bases, including their properties and uses. It defines acids as compounds that increase hydronium ions in water and bases as compounds that increase hydroxide ions in water. Examples of acids include H2SO4 and HCl, while examples of bases include NaOH and Ca(OH)2. Acids and bases have similar properties such as being corrosive or changing the color of litmus paper. They have many industrial and household uses like making paper, detergents, and antacids. The document also explains how strong acids and bases fully dissociate in water and the neutralization reaction between acids and bases.
Acid bases
Acid is a chemical substance that ionises in water to produce hydrogen ions (H+). Acids only show their acidic properties when water is present. In water, hydrochloric acid turns litmus paper red and allows electricity to conduct, but in dry methylbenzene it does not change litmus color or allow conductivity. Similarly, alkalis like ammonia only demonstrate their alkaline properties in water, not in dry solvents.
Acids Bases and Salts
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.
Chapter 19 acids, bases, and salts probe
Acids have a pH below 7 and react with bases to form salts and water. Common acids include hydrochloric acid, sulfuric acid, and acetic acid. Bases have a pH above 7 and react with acids in neutralization reactions. Common bases are sodium hydroxide, calcium hydroxide, and potassium hydroxide. Indicators are used to test whether a solution is acidic or basic by changing color in different pH ranges.
Acid base titration
This document discusses acids, bases, and acid-base titration. It defines acids as substances that can donate protons and bases as substances that can accept protons. It explains that acids are sour and turn litmus red, while bases are bitter and slippery and turn litmus blue. Acid-base indicators are then discussed, including how they change color with pH. Two theories of acid-base indicators are described: Ostwald's theory involving ionization equilibrium, and the quinonoid theory involving tautomeric forms. Finally, different types of acid-base titrations are listed along with the typical indicators used for each type.
Acid base concepts Acid Base concepts; Arrhenius, Lowery-Bronsted, Lewis. So...
Acid Base concepts;
Arrhenius,
Lowery-Bronsted,
Lewis.
Soft and hard acid base concept,
Applications of SHAB
5 bishop
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.
Acid –base 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.
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Acids and bases
This document discusses acids and bases, including their properties and uses. It defines acids as compounds that increase hydronium ions in water and bases as compounds that increase hydroxide ions in water. Examples of acids include H2SO4 and HCl, while examples of bases include NaOH and Ca(OH)2. Acids and bases have similar properties such as being corrosive or changing the color of litmus paper. They have many industrial and household uses like making paper, detergents, and antacids. The document also explains how strong acids and bases fully dissociate in water and the neutralization reaction between acids and bases.
Acid bases
Acid is a chemical substance that ionises in water to produce hydrogen ions (H+). Acids only show their acidic properties when water is present. In water, hydrochloric acid turns litmus paper red and allows electricity to conduct, but in dry methylbenzene it does not change litmus color or allow conductivity. Similarly, alkalis like ammonia only demonstrate their alkaline properties in water, not in dry solvents.
Acids Bases and Salts
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.
Chapter 19 acids, bases, and salts probe
Acids have a pH below 7 and react with bases to form salts and water. Common acids include hydrochloric acid, sulfuric acid, and acetic acid. Bases have a pH above 7 and react with acids in neutralization reactions. Common bases are sodium hydroxide, calcium hydroxide, and potassium hydroxide. Indicators are used to test whether a solution is acidic or basic by changing color in different pH ranges.
Acid base titration
This document discusses acids, bases, and acid-base titration. It defines acids as substances that can donate protons and bases as substances that can accept protons. It explains that acids are sour and turn litmus red, while bases are bitter and slippery and turn litmus blue. Acid-base indicators are then discussed, including how they change color with pH. Two theories of acid-base indicators are described: Ostwald's theory involving ionization equilibrium, and the quinonoid theory involving tautomeric forms. Finally, different types of acid-base titrations are listed along with the typical indicators used for each type.
Acid base concepts Acid Base concepts; Arrhenius, Lowery-Bronsted, Lewis. So...
Acid Base concepts;
Arrhenius,
Lowery-Bronsted,
Lewis.
Soft and hard acid base concept,
Applications of SHAB
5 bishop
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.
Acid –base 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.
acids and bases
1) Acids release H+ ions in water and bases release OH- ions. Strong acids and bases dissociate completely while weak acids and bases only partially dissociate.
2) Acids taste sour, turn litmus red, and react with metals and carbonates. Bases taste bitter and feel slippery.
3) The pH scale measures acidity and alkalinity, with values below 7 being acidic and above 7 being basic. Acid-base indicators change color at specific pH values.
ACIDS , BASES AND SALT
The document discusses acids and bases, including their properties, reactions, and pH scales. Acids are sour, conduct electricity, change litmus to red, and give H+ ions. Bases are bitter, change litmus to blue, and give OH- ions. Acids and bases can undergo neutralization reactions, forming salts and water. Examples of common salts include NaCl, CaOCl2, Na2CO3, and NaHCO3. The pH scale measures the concentration of hydrogen ions, with acids having a pH less than 7 and bases greater than 7. Mixing acids or bases with water is an exothermic reaction that results in dilution and decreased ion concentration.
Acid and base
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.
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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.
Acids, Bases, and Salts
This document discusses acids, bases, and salts. It defines acids as substances that increase the concentration of hydrogen ions in water and bases as those that increase hydroxide ions. Salts are formed through the neutralization reaction of acids and bases. Common indicators of acidity and alkalinity include litmus paper, pH meters, and natural indicators like red cabbage juice. Acids have a sour taste, do not feel slippery, and can react with metals. Bases have a bitter taste, feel soapy, and some can react with metals. Safety measures for handling acids and bases include wearing protective equipment and flushing exposed areas with water. The document also provides examples of investigating substances using natural indicators.
Acids bases and salts
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.
Acid base titration
An acid-base titration is used to determine the concentration of an acid or base. The equivalence point is reached when there are equal moles of H3O+ and OH- ions, resulting in a neutral pH of 7. The titration endpoint is indicated by a color change in the indicator, which should change sharply at the equivalence point. Different types of acid-base reactions result in different pH values at the equivalence point, determined by whether the acid and base are strong or weak.
Acid & Base - Physical Chemistry Presentation
Slide show of the topic Acid & Base as a part of the assignment in our Physical Chemistry course.
Created by: Annisa Hayatunnufus
Bachelor of Pharmacy
Management & Science University
Theories
The document discusses several theories of acids and bases:
1. According to Arrhenius, acids are compounds that produce H+ ions in water and bases produce OH- ions. Strong acids fully dissociate while weak acids only partially dissociate.
2. Bronsted and Lowry defined acids as proton donors and bases as proton acceptors. An acid and base always work together in a proton transfer reaction. Some substances can act as both an acid and a base depending on the reaction.
3. Lewis defined acids as electron pair acceptors and bases as electron pair donors.
Acid and base arhenius concept
This document discusses acids and bases according to the Arrhenius concept. It defines acids as substances that dissociate in water to produce hydrogen ions and bases as those that dissociate to produce hydroxide ions. Examples of common Arrhenius acids include hydrochloric acid, nitric acid, and sulfuric acid. Examples of common Arrhenius bases include sodium hydroxide, potassium hydroxide, and calcium hydroxide. The document notes limitations of the Arrhenius concept, including that it only applies to aqueous solutions and cannot explain the behavior of compounds like carbon dioxide and ammonia that act as acids and bases yet do not contain hydrogen or hydroxide ions.
Strong weak acids and bases
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
Acid and base theories
This document discusses acids and bases. It begins by defining the objectives of understanding acid and base definitions and theories. It then provides examples of common household and laboratory acids and bases. Next, it explains the Arrhenius theory that acids dissociate in water to form H+ ions and bases dissociate to form OH- ions. It also discusses the Brønsted-Lowry theory that acids donate protons and bases accept protons. Neutralization reactions between acids and bases to form salts and water are then explained. The document concludes by discussing acid-base conjugate pairs and examples.
Acid base titrations and theory in acid base conepts
1) The document discusses Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases. It defines acids as substances that produce H+ ions and bases as those that produce OH- ions.
2) The Brønsted-Lowry theory proposes that acids are proton donors and bases are proton acceptors in acid-base reactions. It also introduces conjugate acid-base pairs.
3) The document discusses acid-base indicators and two theories for how their color changes with pH - Ostwald's theory involving indicator ionization and the quinonoid theory involving structural tautomerism between forms.
Blog.7 2.Acid And Base
The document defines acids and bases according to Arrhenius and Brønsted-Lowry theories. Acids are substances that produce hydrogen (H+) or hydronium (H3O+) ions in water according to Arrhenius, and are proton donors according to Brønsted-Lowry. Bases are substances that produce hydroxide (OH-) ions in water according to Arrhenius, and are proton acceptors according to Brønsted-Lowry. Conjugate acid-base pairs are also defined. Common acids, bases, and salts are listed along with their formulas and IUPAC names.
An Introduction Acids, Bases and pH
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.
Acids, Bases and Salts
This document discusses acids, bases, and salts. It defines acids as hydrogen-containing substances that can donate protons, and bases as substances that can accept protons and produce hydroxide ions in aqueous solutions. Strong acids fully dissociate in water while weak acids only partially dissociate. Common strong acids include sulfuric acid and hydrochloric acid. Common strong bases include sodium hydroxide and calcium hydroxide. Salts are formed when acid protons are replaced by metal ions. Salts have various properties and uses such as in batteries, fertilizers, and medicine. The document also explains the pH scale for measuring acidity and basicity.
Acid Base Notes (H)
This document provides information about acids and bases including:
1) Common acids and their names, acid-base definitions using Arrhenius and Brønsted-Lowry models, and properties of acids and bases.
2) Conjugate acid-base pairs, acid and base strength, pH and pOH calculations.
3) Buffers, neutralization reactions, and examples of pH indicators.
Acid base concepts
This document discusses different theories of acids and bases:
1) Arrhenius theory defines acids as substances that produce H+ ions in aqueous solution and bases as substances that produce OH- ions. Neutralization occurs via reaction of H+ and OH- to form H2O.
2) Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Acid-base reactions involve proton transfer.
3) Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. Lewis acid-base reactions involve sharing of electron pairs to form adducts. Common examples include formation of hydronium ion and metal-ligand complexes.
Acids bases salts for class 7 cbse
The document provides answers to 11 questions about acids, bases and salts. It defines strong and weak acids, and lists differences between acids and bases. It explains that acetic acid is in vinegar, ammonia is basic. Litmus solution comes from lichens and is used as a pH indicator. Distilled water is neutral as shown by litmus. Neutralization reactions form salts and water. Antacids neutralize excess stomach acid; calamine neutralizes ant bites. Factory waste is neutralized before disposal. The last questions discuss indicator color changes with acids and bases.
Acid and base
This document discusses acids and bases according to several theories:
- According to the Arrhenius theory, acids donate H+ ions and bases donate OH- ions in water. This theory does not explain behavior in non-aqueous solutions.
- The Bronsted-Lowry theory states that acids are proton donors and bases are proton acceptors. Conjugate acids and bases are formed in acid-base reactions.
- The Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. Covalent bonds are formed between them.
- Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. Examples of strong and weak acids and bases are provided
Acids, Bases, & Salts.ppt
Acids have a pH below 7 and donate hydrogen ions in solution, forming H+ ions. They react with metals and bases. Bases have a pH above 7 and accept hydrogen ions, forming OH- ions. Common acids include HCl and H2SO4, while common bases include NaOH and Mg(OH)2. A salt is formed during a neutralization reaction between an acid and a base, producing water. The digestive system uses acids and bases to break down foods, with the stomach having a highly acidic pH around 2 to aid in digestion.
Acids, bases, & salts
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 and bases
1) Acids release H+ ions in water and bases release OH- ions. Strong acids and bases dissociate completely while weak acids and bases only partially dissociate.
2) Acids taste sour, turn litmus red, and react with metals and carbonates. Bases taste bitter and feel slippery.
3) The pH scale measures acidity and alkalinity, with values below 7 being acidic and above 7 being basic. Acid-base indicators change color at specific pH values.
ACIDS , BASES AND SALT
The document discusses acids and bases, including their properties, reactions, and pH scales. Acids are sour, conduct electricity, change litmus to red, and give H+ ions. Bases are bitter, change litmus to blue, and give OH- ions. Acids and bases can undergo neutralization reactions, forming salts and water. Examples of common salts include NaCl, CaOCl2, Na2CO3, and NaHCO3. The pH scale measures the concentration of hydrogen ions, with acids having a pH less than 7 and bases greater than 7. Mixing acids or bases with water is an exothermic reaction that results in dilution and decreased ion concentration.
Acid and base
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.
TOPIC 8 : Acids and Bases
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.
Acids, Bases, and Salts
This document discusses acids, bases, and salts. It defines acids as substances that increase the concentration of hydrogen ions in water and bases as those that increase hydroxide ions. Salts are formed through the neutralization reaction of acids and bases. Common indicators of acidity and alkalinity include litmus paper, pH meters, and natural indicators like red cabbage juice. Acids have a sour taste, do not feel slippery, and can react with metals. Bases have a bitter taste, feel soapy, and some can react with metals. Safety measures for handling acids and bases include wearing protective equipment and flushing exposed areas with water. The document also provides examples of investigating substances using natural indicators.
Acids bases and salts
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.
Acid base titration
An acid-base titration is used to determine the concentration of an acid or base. The equivalence point is reached when there are equal moles of H3O+ and OH- ions, resulting in a neutral pH of 7. The titration endpoint is indicated by a color change in the indicator, which should change sharply at the equivalence point. Different types of acid-base reactions result in different pH values at the equivalence point, determined by whether the acid and base are strong or weak.
Acid & Base - Physical Chemistry Presentation
Slide show of the topic Acid & Base as a part of the assignment in our Physical Chemistry course.
Created by: Annisa Hayatunnufus
Bachelor of Pharmacy
Management & Science University
Theories
The document discusses several theories of acids and bases:
1. According to Arrhenius, acids are compounds that produce H+ ions in water and bases produce OH- ions. Strong acids fully dissociate while weak acids only partially dissociate.
2. Bronsted and Lowry defined acids as proton donors and bases as proton acceptors. An acid and base always work together in a proton transfer reaction. Some substances can act as both an acid and a base depending on the reaction.
3. Lewis defined acids as electron pair acceptors and bases as electron pair donors.
Acid and base arhenius concept
This document discusses acids and bases according to the Arrhenius concept. It defines acids as substances that dissociate in water to produce hydrogen ions and bases as those that dissociate to produce hydroxide ions. Examples of common Arrhenius acids include hydrochloric acid, nitric acid, and sulfuric acid. Examples of common Arrhenius bases include sodium hydroxide, potassium hydroxide, and calcium hydroxide. The document notes limitations of the Arrhenius concept, including that it only applies to aqueous solutions and cannot explain the behavior of compounds like carbon dioxide and ammonia that act as acids and bases yet do not contain hydrogen or hydroxide ions.
Strong weak acids and bases
Acids are divided into two categories based on the ease with which they can donate protons to the solvent: i) strong acids and ii) weak acids
Strong acids are acids that completely dissociate in water. The reaction of an acid with its solvent (typically H2O) is called an acid dissociation reaction.
Weak acids are acids that dissociate partially in water. The extent of dissociation is given by the equilibrium constant.
Note:
A measure of the relative strength of an acid is: i) the equilibrium constant ka of the dissociation reaction of the acid in water (depends on temperature) ii) the degree of dissociation α of the acid in water (depends on the concentration of the acid an on temperature).
Acid and base theories
This document discusses acids and bases. It begins by defining the objectives of understanding acid and base definitions and theories. It then provides examples of common household and laboratory acids and bases. Next, it explains the Arrhenius theory that acids dissociate in water to form H+ ions and bases dissociate to form OH- ions. It also discusses the Brønsted-Lowry theory that acids donate protons and bases accept protons. Neutralization reactions between acids and bases to form salts and water are then explained. The document concludes by discussing acid-base conjugate pairs and examples.
Acid base titrations and theory in acid base conepts
1) The document discusses Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases. It defines acids as substances that produce H+ ions and bases as those that produce OH- ions.
2) The Brønsted-Lowry theory proposes that acids are proton donors and bases are proton acceptors in acid-base reactions. It also introduces conjugate acid-base pairs.
3) The document discusses acid-base indicators and two theories for how their color changes with pH - Ostwald's theory involving indicator ionization and the quinonoid theory involving structural tautomerism between forms.
Blog.7 2.Acid And Base
The document defines acids and bases according to Arrhenius and Brønsted-Lowry theories. Acids are substances that produce hydrogen (H+) or hydronium (H3O+) ions in water according to Arrhenius, and are proton donors according to Brønsted-Lowry. Bases are substances that produce hydroxide (OH-) ions in water according to Arrhenius, and are proton acceptors according to Brønsted-Lowry. Conjugate acid-base pairs are also defined. Common acids, bases, and salts are listed along with their formulas and IUPAC names.
An Introduction Acids, Bases and pH
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.
Acids, Bases and Salts
This document discusses acids, bases, and salts. It defines acids as hydrogen-containing substances that can donate protons, and bases as substances that can accept protons and produce hydroxide ions in aqueous solutions. Strong acids fully dissociate in water while weak acids only partially dissociate. Common strong acids include sulfuric acid and hydrochloric acid. Common strong bases include sodium hydroxide and calcium hydroxide. Salts are formed when acid protons are replaced by metal ions. Salts have various properties and uses such as in batteries, fertilizers, and medicine. The document also explains the pH scale for measuring acidity and basicity.
Acid Base Notes (H)
This document provides information about acids and bases including:
1) Common acids and their names, acid-base definitions using Arrhenius and Brønsted-Lowry models, and properties of acids and bases.
2) Conjugate acid-base pairs, acid and base strength, pH and pOH calculations.
3) Buffers, neutralization reactions, and examples of pH indicators.
Acid base concepts
This document discusses different theories of acids and bases:
1) Arrhenius theory defines acids as substances that produce H+ ions in aqueous solution and bases as substances that produce OH- ions. Neutralization occurs via reaction of H+ and OH- to form H2O.
2) Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Acid-base reactions involve proton transfer.
3) Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. Lewis acid-base reactions involve sharing of electron pairs to form adducts. Common examples include formation of hydronium ion and metal-ligand complexes.
Acids bases salts for class 7 cbse
The document provides answers to 11 questions about acids, bases and salts. It defines strong and weak acids, and lists differences between acids and bases. It explains that acetic acid is in vinegar, ammonia is basic. Litmus solution comes from lichens and is used as a pH indicator. Distilled water is neutral as shown by litmus. Neutralization reactions form salts and water. Antacids neutralize excess stomach acid; calamine neutralizes ant bites. Factory waste is neutralized before disposal. The last questions discuss indicator color changes with acids and bases.
Acid and base
This document discusses acids and bases according to several theories:
- According to the Arrhenius theory, acids donate H+ ions and bases donate OH- ions in water. This theory does not explain behavior in non-aqueous solutions.
- The Bronsted-Lowry theory states that acids are proton donors and bases are proton acceptors. Conjugate acids and bases are formed in acid-base reactions.
- The Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. Covalent bonds are formed between them.
- Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. Examples of strong and weak acids and bases are provided
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Acid base titrations and theory in acid base conepts
Acid base titrations and theory in acid base conepts
Similar to acids basis and salts
Acids, Bases, & Salts.ppt
Acids have a pH below 7 and donate hydrogen ions in solution, forming H+ ions. They react with metals and bases. Bases have a pH above 7 and accept hydrogen ions, forming OH- ions. Common acids include HCl and H2SO4, while common bases include NaOH and Mg(OH)2. A salt is formed during a neutralization reaction between an acid and a base, producing water. The digestive system uses acids and bases to break down foods, with the stomach having a highly acidic pH around 2 to aid in digestion.
Acids, bases, & salts
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.
PPT on Acids, Bases & Salts submitted by Bhavneet Singh.ppt
This document discusses acids, bases, and salts. It defines acids as substances with a pH below 7 that produce hydrogen ions and notes common acids include hydrochloric acid in stomachs and sulfuric acid in car batteries. Bases are defined as having a pH above 7 and producing hydroxide ions, with examples being sodium hydroxide in drains and magnesium hydroxide in antacids. Salts are neutral substances formed from acid-base reactions, composed of an acid's anion and a base's cation. The document also outlines acid-base reactions and how pH is controlled in various systems like ponds, blood, and swimming pools.
Acids, bases, and salts
This document defines acids, bases, and salts. It explains that acids have a pH below 7 and donate hydrogen ions in solution, forming H+ ions. Bases have a pH above 7 and donate hydroxide ions in solution, feeling slippery. Salts are neutral compounds formed from the reaction of acids and bases, containing the positive ion from the base and negative ion from the acid. Common acids include hydrochloric, sulfuric, nitric, acetic, carbonic, and phosphoric acids. Common bases include sodium hydroxide, magnesium hydroxide, and aluminum hydroxide.
Acids, bases, & 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.
Acids Bases and Salts ppt.ppt
This document defines acids, bases, and salts. It states that acids have a pH below 7 and contain hydrogen ions (H+) in solution. They neutralize bases and are corrosive. Bases have a pH above 7, feel slippery, taste bitter, contain hydroxide (OH-) ions in solution, and neutralize acids. Common acids and bases are listed. Salts are formed from the positive ion of a base and negative ion of an acid during a neutralization reaction between an acid and base, producing water. Examples of salts include NaCl and MgSO4.
Acids, bases, & salts
This document discusses acids, bases, and salts. It defines acids as having a pH less than 7 and forming H+ ions in solution, and bases as having a pH greater than 7 and forming OH- ions in solution. Acids are classified as weak or strong depending on how completely they ionize in water. Common acids include hydrochloric acid, sulfuric acid, and acetic acid. Bases are also classified as weak or strong. Common bases include sodium hydroxide, magnesium hydroxide, and ammonium hydroxide. A salt is formed when an acid and base react, consisting of the negative ion from the acid and positive ion from the base.
Acids, bases, & salts by sugam raghav
Acids have a pH less than 7 and neutralize bases by donating hydrogen ions in solution. Common acids include hydrochloric acid in stomachs, sulfuric acid in car batteries, and acetic acid in vinegar. Strong acids like hydrochloric and nitric acids fully ionize in water, while weak acids like acetic and phosphoric acids only partially ionize. Bases accept hydrogen ions and include sodium hydroxide, calcium hydroxide, and ammonium hydroxide. The pH scale measures hydrogen ion concentration from 0 to 14, with acids having a lower pH and bases a higher pH. A neutralization reaction occurs when an acid and base react, producing a salt and water.
Science acids, bases and salts1
Acids are sour, turn litmus red, and react with bases to form salts and water. Bases are bitter, feel soapy, turn litmus blue, and react with acids to form salts and water. Common acids include lemon juice and battery acid. Common bases include soap and drain cleaner. Acids and bases can be identified using indicators like litmus paper or red cabbage juice which change color.
najmjamelh.pptx
Acids and bases are fundamental compounds found everywhere in nature and in daily life. They are responsible for many natural processes and used in many products. An acid is a compound that increases the hydrogen ion (H+) concentration in water, donating protons. A base is a compound that increases the hydroxide ion (OH-) concentration in water, accepting protons. Common acids include hydrochloric acid and citric acid, while common bases include sodium hydroxide and ammonia. The pH scale measures how acidic or basic a solution is on a scale from 0 to 14. Acid-base reactions result in neutralization and salt formation.
Acids, bases, & salts
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7, forming H+ ions in solution, and neutralizing bases. Common acids include hydrochloric, sulfuric, nitric, acetic, carbonic, and phosphoric acids. Bases are defined as having a pH greater than 7, feeling slippery, and dissolving fats and oils. Common bases include sodium hydroxide, magnesium hydroxide, aluminum hydroxide, and ammonium hydroxide. Salts are formed from the reaction of acids and bases and are composed of the negative ion of an acid and positive ion of a base. A neutralization reaction produces a salt and water when an acid re
ACIDS AND BASES
Acids and bases are defined by their properties in aqueous solutions. Acids release hydrogen ions (H+) and have a sour taste, while bases release hydroxide ions (OH-) and feel slippery. The pH scale measures acidity and basicity, with values from 0-14 and neutral substances having a pH of 7. Acid-base indicators change color with pH and can test whether a solution is acidic or basic. When acids and bases are mixed, a neutralization reaction occurs where they cancel out each other's properties and form a salt and water.
ACIDS and BASES.
Properties/characteristics of Acid and Base.
Understanding the pH scale.
Acid-Base Indicator.
Neutralization.
Example of acids and bases
Acid Base And Salt.pdf
1) Acids are compounds that form hydrogen (H+) ions in solution and have a pH less than 7. Common strong acids include hydrochloric acid, nitric acid, and sulfuric acid.
2) Bases are compounds that form hydroxide (OH-) ions in solution and have a pH greater than 7. Common bases include sodium hydroxide, calcium hydroxide, and ammonium hydroxide.
3) A salt is formed through a neutralization reaction between an acid and a base, producing water and an ionic compound composed of the cation from the base and the anion from the acid. Examples of salts include sodium chloride, magnesium sulfate, and ammonium nitrate.
Acid, Base and Salt. Science Plus one NIOS
This document discusses acids, bases, and salts. It defines acids as substances that release hydrogen ions (H+) in water, and bases as substances that release hydroxide ions (OH-). Strong acids and bases fully dissociate in water, while weak ones only partially dissociate. Acids react with metals and bases to produce salts and either water or hydrogen gas. The pH scale is used to measure acidity, with acidic solutions having a pH below 7 and basic solutions above 7. Common examples of acids, bases, and salts are also provided.
Acids and bases and salts
The document discusses acids and bases. It defines acids as substances that give up hydrogen ions in solution and bases as those that give up hydroxide ions. It then provides examples of common acids like vinegar and lemon juice and bases like baking soda. It explains how to test for acids and bases using litmus paper and red cabbage juice and lists some major acid-base theories. DNA is identified as an acid according to Bronsted's definition.
Lesson 9 acids and bases
Acids and bases are defined by whether they release H+ or OH- ions in water. Strong acids and bases dissociate completely, while weak ones only partially dissociate. Acids taste sour, react with carbonates and metals to produce gas, and contain hydrogen. Bases taste bitter, feel slippery, and contain hydroxide ions. The pH scale measures acidity and alkalinity, with values below 7 indicating acids and above 7 indicating bases. Acid-base indicators change color at specific pH levels, allowing identification of acids and bases. When acids and bases neutralize, they form water and salts.
acids, bases and salts
This document defines acids, bases, and salts. It states that acids are sour, turn litmus red, and release H+ ions, while bases are bitter, soapy, turn litmus blue and release OH- ions. Salts are formed through neutralization reactions between acids and bases. It provides examples of common acids, bases, and salts. It also discusses acid-base indicators and their color changes. The document further details chemical properties of acids and bases, the pH scale, and provides additional information on salt.
Shake your acids, bases and salts
This document discusses acids, bases, and salts. It defines acids as substances that give H+ ions in water and have a sour taste, react with metals, and have a pH less than 7. Bases are defined as substances that give OH- ions in water, usually taste bitter, feel slippery, and have a pH greater than 7. Salts are formed when acids and bases react, combining H+ and OH- ions to form water. Common examples of acids include vinegar and cola, bases include drain cleaner and baking powder, and salts include table salt and toothpaste. The document provides characteristics, examples, and a brief activity to identify household substances as acids, bases or salts.
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Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
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Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
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1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
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acids basis and salts
- 2. What is an ACID? • pH less than 7 • Neutralizes bases • Forms H + ions in solution • Corrosive-reacts with most metals to form hydrogen gas • Good conductors of electricity
- 3. Acids Generate Ions HNO3 + H2O H3O+ + NO3
- 4. Weak vs. Strong Acids • Weak Acids do not ionize completely: Acetic, Boric, Nitrous, Phosphoric, Sulfurous • Strong Acids ionize completely: Hydrochloric, Nitric; Sulfuric, Hydriodic
- 5. Common Acids • HCl- hydrochloric- stomach acid • H2SO4- sulfuric acid - car batteries • HNO3 – nitric acid - explosives • HC2H3O2- acetic acid - vinegar • H2CO3-carbonic acid – sodas • H3PO4- phosphoric acid -flavorings
- 7. What is a BASE? • pH greater than 7 • Feels slippery • Dissolves fats and oils • Usually forms OH - ions in solution • Neutralizes acids
- 8. Weak vs. Strong Bases • Weak Bases: ammonia; potassium carbonate, sodium carbonate • Strong Bases: sodium hydroxide; sodium phosphate; barium hydroxide; calcium hydroxide
- 9. Common Bases • NaOH- sodium hydroxide (LYE) soaps, drain cleaner • Mg (OH)2 - magnesium hydroxide-antacids • Al(OH)3-aluminum hydroxide-antacids, deodorants • NH4OH-ammonium hydroxide- “ammonia”
- 10. Types of Acids and Bases • In the 1800’s chemical concepts were based on the reactions of aqueous solutions. • Svante Arrhenius developed a concept of acids and bases relevant to reactions in H2O. • Arrhenius acid – produces hydrogen ions in water. • Arrhenius base – produce hydroxide ions in water.
- 11. A broader ,more modern concept of acids and bases was developed later. Bronsted-Lowry acid- donates a hydrogen ion in a reaction. Bronsted – Lowry base – accepts a hydrogen in a reaction.
- 12. • Conjugate acid- compound formed when an base gains a hydrogen ion. • Conjugate base – compound formed when an acid loses a hydrogen ion.
- 13. pH Scale
- 14. pH of Common Substances Timberlake, Chemistry 7th Edition, page 335
- 15. Reactions with indicators Indicator Acid color Neutral color Base color Phenolphthalein Colorless Faint pink Dark pink Bromthymol blue Yellow Green Blue Litmus Red ----- Blue
- 16. pH paper • pH paper changes color to indicate a specific pH value.
- 17. Buffers • A buffer is a solution that resists changes in pH when small amounts of acids and bases are added.
- 18. Situations in which pH is controlled • “Heartburn” • Planting vegetables and flowers • Fish Tanks and Ponds • Blood • Swimming pools
- 19. Acids and Bases in Solution • HCl + H20 H3O + + Cl- (more hydronium ions, more acidic) • NaOH in water Na+ + OH- (more hydroxide ions, more basic) • NaOH + HCl NaCl + HOH Acid + Base yields type of salt and water • NH3 + H20 NH4 + + OH- ammonia gas + water yields ammonium and hydroxide ions
- 20. Acid Rain Pollution in the air (sulfur dioxide, carbon dioxide, nitrogen dioxide) combines with water to form various acids. .
- 21. Rapid changes in pH can kill fish and other organisms in lakes and streams. Soil pH is affected and can kill plants and create sinkholes
- 25. What is a SALT? • A salt is a neutral substance produced from the reaction of an acid and a base. • Composed of the negative ion of an acid and the positive ion of a base. • One of the products of a Neutralization Reaction • Examples: KCl, MgSO4, Na3PO4
- 26. Neutralization Reaction • A neutralization reaction is the reaction of an acid with a base to produce salt and water. • Example H2SO4 + NaOH NaHSO4 + H2O
- 27. Digestion and pH • Digestion-process by which foods are broken down into simpler substances. • Mechanical digestion-physical process in which food is torn apart (mouth) • Chemical digestion- chemical reactions in which large molecules are broken down into smaller molecules. (stomach and small intestines)
- 28. pH in the Digestive System • Mouth-pH around 7. Saliva contains amylase, an enzyme which begins to break carbohydrates into sugars. • Stomach- pH around 2. Proteins are broken down into amino acids by the enzyme pepsin. • Small intestine-pH around 8. Most digestion ends. Small molecules move to bloodstream toward cells that use them
- 30. Acids, Bases, and Salts The End