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 are substances that donate protons and turn litmus paper red, while bases are substances that accept protons and turn litmus paper blue. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate. The reaction between acids and bases produces salts and water. Common examples of salts produced for various uses include sodium chloride, calcium oxychloride (bleaching powder), sodium bicarbonate (baking soda), sodium carbonate (washing soda), and calcium sulfate hemihydrate (Plaster of Paris).
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This document provides an introduction to acids, bases and salts. It defines acids and bases according to Arrhenius and Bronsted-Lowry theories. Examples of common acids and bases are given. Physical properties of acids and bases like taste and effect on indicators are described. Key acid-base reactions like those with metals, metal carbonates and the neutralization reaction are outlined. The document also discusses water's role in dissociating acids and bases, as well as concepts like pH, strength of acids and bases, and dilution. Methods for manufacturing important acids and bases are summarized. Finally, the properties and uses of some common salts are mentioned.
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 and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Strong acids and bases completely ionize, while weak ones only partially ionize. Neutral substances have equal concentrations of hydrogen and hydroxide ions. When acids and bases are mixed, they neutralize to form salts and water through balanced chemical reactions. pH indicators can be used to determine if a solution is acidic, basic, or neutral.
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.
Acids are substances that donate protons and turn litmus paper red, while bases are substances that accept protons and turn litmus paper blue. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate. The reaction between acids and bases produces salts and water. Common examples of salts produced for various uses include sodium chloride, calcium oxychloride (bleaching powder), sodium bicarbonate (baking soda), sodium carbonate (washing soda), and calcium sulfate hemihydrate (Plaster of Paris).
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This document provides an introduction to acids, bases and salts. It defines acids and bases according to Arrhenius and Bronsted-Lowry theories. Examples of common acids and bases are given. Physical properties of acids and bases like taste and effect on indicators are described. Key acid-base reactions like those with metals, metal carbonates and the neutralization reaction are outlined. The document also discusses water's role in dissociating acids and bases, as well as concepts like pH, strength of acids and bases, and dilution. Methods for manufacturing important acids and bases are summarized. Finally, the properties and uses of some common salts are mentioned.
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 and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Strong acids and bases completely ionize, while weak ones only partially ionize. Neutral substances have equal concentrations of hydrogen and hydroxide ions. When acids and bases are mixed, they neutralize to form salts and water through balanced chemical reactions. pH indicators can be used to determine if a solution is acidic, basic, or neutral.
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 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, bases, and salts. It defines acids as substances that release hydrogen ions in water and bases as substances that produce hydroxide ions in water. It explains that acids and bases neutralize through a reaction that produces a salt and water. Salts are usually solid crystals formed through neutralization reactions between acids and bases or other reactions like those between acid/base oxides or metals and acids. Common examples of acids, bases, and their properties are provided.
The document discusses acids, bases and salts. It defines these substances and classifies them based on various properties such as origin, strength and concentration. Acids are classified as organic or mineral, strong or weak, and dilute or concentrated. Bases are called alkalies and are also classified as strong or weak, and dilute or concentrated. Indicators are substances that change color in acidic vs basic solutions and help identify their nature. The document also discusses the reactions of acids and bases with water, metals, metal carbonates, bicarbonates, and each other. It describes pH and the pH scale for measuring acidity and alkalinity. Living organisms are sensitive to pH and maintaining the proper pH is important.
The document discusses acids, bases and salts. It defines these substances and classifies them based on various properties such as origin, strength and concentration. Acids are classified as organic or mineral, strong or weak, and dilute or concentrated. Bases are called alkalies and are also classified as strong or weak, and dilute or concentrated. Indicators are substances that change color in acidic vs basic solutions and help determine the pH. The pH scale measures the concentration of hydrogen ions (H+) or hydroxyl ions (OH-) to determine if a solution is acidic, basic or neutral. Living organisms and processes like digestion require specific pH ranges to function properly.
The document discusses acids, bases and salts. It defines acids as substances that have a sour taste and turn litmus paper red, while bases have a bitter taste and soapy texture and turn litmus paper blue. Examples of common acids include citric acid in lemons and lactic acid in curd. The document also covers the reactions of acids and bases, such as acids reacting with metals to produce salts and hydrogen gas. A neutralization reaction occurs when an acid and base react and form water and a salt.
PowerPoint Presentation on the topic - 'Acids, Bases and Salts'. For Class - 10th.
Created By - 'Neha Rohtagi'
I hope that you will found this presentation useful and it will help you out for your concept understanding.
Thank You!
The document discusses acids, bases and their properties. It defines acids as substances that release hydrogen ions (H+) in water, forming hydronium ions (H3O+). Bases release hydroxyl ions (OH-) in water. Acids and bases conduct electricity when dissolved in water due to the ions released. Indicators like litmus are used to test if a substance is acidic or basic. Acids and bases react through neutralization reactions to form salts and water. The pH scale is used to measure acidity and alkalinity. Examples of acid-base reactions and their applications are also provided.
ACIDS, BASES AND SALTS ppt-converted.pptxSurabhi Gupta
This document provides information about acids, bases and salts. It defines acids as substances that produce hydrogen (H+) ions in water and have a pH less than 7. Examples of acids include vinegar, lemon juice and stomach acid. Bases are defined as substances that produce hydroxide (OH-) ions in water and have a pH greater than 7. Examples include ammonia, sodium hydroxide and calcium hydroxide. The document also discusses the reactions of acids and bases with metals, metal carbonates, and each other. It provides information on salts, pH scale, and the importance of pH in everyday life.
1. Acids are substances that liberate hydrogen ions (H+) when dissolved in water. Common acids include hydrochloric acid, nitric acid, and sulfuric acid.
2. Bases are substances that form hydroxide ions (OH-) when dissolved in water, such as sodium hydroxide and potassium hydroxide.
3. Acids and bases react through neutralization reactions, where hydrogen and hydroxide ions exchange partners to form water and a salt. This is illustrated by the reaction of sulfuric acid and calcium hydroxide to form calcium sulfate and water.
This document provides information about acid-base chemistry including:
1. Acids and bases are defined, and indicators like litmus paper are described for testing acidity and basicity.
2. The pH scale is introduced to measure acidity and alkalinity, and examples of strong and weak acids and bases are given.
3. Common acids, bases, and salts are described including their properties and reactions. Processes like neutralization, ionization, and the formation of soap as a salt are explained.
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,
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
Chemistry - Chp 19 - Acids, Bases, and Salt - PowerPointsMr. Walajtys
This document provides an overview of acids and bases according to different theories:
1. Arrhenius theory defines acids as producing hydrogen ions in water and bases as producing hydroxide ions.
2. Brønsted-Lowry theory defines acids as hydrogen ion donors and bases as hydrogen ion acceptors.
3. Lewis theory focuses on electron pair donation and acceptance between reactants.
It also discusses the pH scale, ion product constant of water, and using indicators to determine if a solution is acidic, basic, or neutral.
This document discusses indicators, acids, bases, and the reactions between them. It provides examples of natural and synthetic acid-base indicators and how they change color with pH. Acids are defined as sour substances that turn litmus red and donate hydrogen ions in water, while bases are defined as bitter substances that turn litmus blue and accept hydrogen ions in water. Common strong acids and bases are listed. The document also summarizes several acid-base reactions including neutralization and reactions with metals, carbonates, and oxides. It discusses the pH scale and importance of pH in everyday life. In the end, it briefly discusses the preparation and uses of several common salts.
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.
PPT on Acids, Bases & Salts submitted by Bhavneet Singh.pptAbhyDeepSingh
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.
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.
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, bases, and salts. It defines acids as substances that release hydrogen ions in water and bases as substances that produce hydroxide ions in water. It explains that acids and bases neutralize through a reaction that produces a salt and water. Salts are usually solid crystals formed through neutralization reactions between acids and bases or other reactions like those between acid/base oxides or metals and acids. Common examples of acids, bases, and their properties are provided.
The document discusses acids, bases and salts. It defines these substances and classifies them based on various properties such as origin, strength and concentration. Acids are classified as organic or mineral, strong or weak, and dilute or concentrated. Bases are called alkalies and are also classified as strong or weak, and dilute or concentrated. Indicators are substances that change color in acidic vs basic solutions and help identify their nature. The document also discusses the reactions of acids and bases with water, metals, metal carbonates, bicarbonates, and each other. It describes pH and the pH scale for measuring acidity and alkalinity. Living organisms are sensitive to pH and maintaining the proper pH is important.
The document discusses acids, bases and salts. It defines these substances and classifies them based on various properties such as origin, strength and concentration. Acids are classified as organic or mineral, strong or weak, and dilute or concentrated. Bases are called alkalies and are also classified as strong or weak, and dilute or concentrated. Indicators are substances that change color in acidic vs basic solutions and help determine the pH. The pH scale measures the concentration of hydrogen ions (H+) or hydroxyl ions (OH-) to determine if a solution is acidic, basic or neutral. Living organisms and processes like digestion require specific pH ranges to function properly.
The document discusses acids, bases and salts. It defines acids as substances that have a sour taste and turn litmus paper red, while bases have a bitter taste and soapy texture and turn litmus paper blue. Examples of common acids include citric acid in lemons and lactic acid in curd. The document also covers the reactions of acids and bases, such as acids reacting with metals to produce salts and hydrogen gas. A neutralization reaction occurs when an acid and base react and form water and a salt.
PowerPoint Presentation on the topic - 'Acids, Bases and Salts'. For Class - 10th.
Created By - 'Neha Rohtagi'
I hope that you will found this presentation useful and it will help you out for your concept understanding.
Thank You!
The document discusses acids, bases and their properties. It defines acids as substances that release hydrogen ions (H+) in water, forming hydronium ions (H3O+). Bases release hydroxyl ions (OH-) in water. Acids and bases conduct electricity when dissolved in water due to the ions released. Indicators like litmus are used to test if a substance is acidic or basic. Acids and bases react through neutralization reactions to form salts and water. The pH scale is used to measure acidity and alkalinity. Examples of acid-base reactions and their applications are also provided.
ACIDS, BASES AND SALTS ppt-converted.pptxSurabhi Gupta
This document provides information about acids, bases and salts. It defines acids as substances that produce hydrogen (H+) ions in water and have a pH less than 7. Examples of acids include vinegar, lemon juice and stomach acid. Bases are defined as substances that produce hydroxide (OH-) ions in water and have a pH greater than 7. Examples include ammonia, sodium hydroxide and calcium hydroxide. The document also discusses the reactions of acids and bases with metals, metal carbonates, and each other. It provides information on salts, pH scale, and the importance of pH in everyday life.
1. Acids are substances that liberate hydrogen ions (H+) when dissolved in water. Common acids include hydrochloric acid, nitric acid, and sulfuric acid.
2. Bases are substances that form hydroxide ions (OH-) when dissolved in water, such as sodium hydroxide and potassium hydroxide.
3. Acids and bases react through neutralization reactions, where hydrogen and hydroxide ions exchange partners to form water and a salt. This is illustrated by the reaction of sulfuric acid and calcium hydroxide to form calcium sulfate and water.
This document provides information about acid-base chemistry including:
1. Acids and bases are defined, and indicators like litmus paper are described for testing acidity and basicity.
2. The pH scale is introduced to measure acidity and alkalinity, and examples of strong and weak acids and bases are given.
3. Common acids, bases, and salts are described including their properties and reactions. Processes like neutralization, ionization, and the formation of soap as a salt are explained.
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,
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
Chemistry - Chp 19 - Acids, Bases, and Salt - PowerPointsMr. Walajtys
This document provides an overview of acids and bases according to different theories:
1. Arrhenius theory defines acids as producing hydrogen ions in water and bases as producing hydroxide ions.
2. Brønsted-Lowry theory defines acids as hydrogen ion donors and bases as hydrogen ion acceptors.
3. Lewis theory focuses on electron pair donation and acceptance between reactants.
It also discusses the pH scale, ion product constant of water, and using indicators to determine if a solution is acidic, basic, or neutral.
This document discusses indicators, acids, bases, and the reactions between them. It provides examples of natural and synthetic acid-base indicators and how they change color with pH. Acids are defined as sour substances that turn litmus red and donate hydrogen ions in water, while bases are defined as bitter substances that turn litmus blue and accept hydrogen ions in water. Common strong acids and bases are listed. The document also summarizes several acid-base reactions including neutralization and reactions with metals, carbonates, and oxides. It discusses the pH scale and importance of pH in everyday life. In the end, it briefly discusses the preparation and uses of several common salts.
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.
PPT on Acids, Bases & Salts submitted by Bhavneet Singh.pptAbhyDeepSingh
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.
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.
Similar a Acid, Base and Salt. Science Plus one NIOS (20)
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
বিসিএস ও ব্যাংক এর লিখিত পরীক্ষা ...+এছাড়া মাধ্যমিক ও উচ্চমাধ্যমিকের স্টুডেন্টদের জন্য অনেক কাজে আসবে ...
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
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Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
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.
2. ACID
❏ Latin term ‘accre’ means sour
❏ Used by Robert Boyle in 17th century
❏ It’s a substance which release hydrogen ions (H+) when dissolved in water.
❏ (H+) does not exist alone, it combines with water molecule (H2O) and forms
(H3O+) (Hydronium ion)
Eg:- HCl — H++Cl-
3. BASES
● The substances which hydroxide ions (OH-) when dissolved in water.
● Bases soluble in water called Alkalis
Eg: NaOH, KOH
➔ Neutralization is the chemical reaction in which acid and base quantitatively
react together to form a salt and water as products.
4. Properties
ACID
● Taste sour
● Feel like water
● Corrosive to metals
● Change blue litmus to red
● React with metals and forms H2 & Salt
● React with Base to form water and salt
(Neutralization)
● Conduct electricity when dissolved in
water
● Colorless in phenolphthalein.
BASE
● Taste bitter
● Feel soapy
● Non- reactive with metals
● React with acid to form water and salt
(Neutralization)
● Change red litmus to blue
● Pink color in phenolphthalein
● Conducts electricity when dissolved in
water
6. Strength of Acids/ Bases
● Strong acid releases more H+ ions like
HCL
● Weak acid releases less H+ ions like acetic
acid
● Strong base releases more OH- ions like
NaOH
● Weak base releases less OH- ions like
Ammonium Hydroxide (NH4OH)
8. Mineral & Organic acids
➔ Mineral acids are those acids that are man-made and derived from one or
more inorganic compounds.
➔ Organic acids are the acids found naturally in plants and animals. They are
weak acids and do not dissociate completely in water.
10. Indicators
● Substances that tell us whether a substance is acidic or basic by change in
color, smell etc…
Types of indicators:
Olfactory indicator: Substances that changes its odour in acidic or basic
media like Vanilla, Onion etc…
Natural indicator: turmeric, Litmus (Obtained from lichen, hibiscus etc..)
Synthetic indicator: Methyl Orange, Phenolphthalein.
11. Indicators
Indicator Natural color Acids Bases
Red litmus Red Remains red Turns Blue
Blue litmus Blue Turns red Remains blue
Phenolphthalein Colorless Colorless Pink
Methyl Orange Reddish Orange Red Yellow
14. Properties of Acid
1. Taste
2. Action on indicators
3. Conduction of electricity and dissociation of acids
4. Reaction of acids with metals
5. Reaction with metal carbonates and hydrogen carbonates
6. Reaction with metal oxides
7. Reaction with bases
8. Corrosive nature
15. 3. Conduction of electricity and dissociation of acids
Dissociation: Process of producing ions which help conducting electricity when
acid dissolved in water.
H+ + H2O H3O+ H+(aq)
Hydrogen ion Hydronium ion
16. 3.1 Strong & weak acids
Strong acid
Acid which completely dissociate in water are
called strong acids.
Eg:- Nitric acid
HNO3 H+ + NO3
Strong acids :- Mineral acids like Hydrochloric
acid (HCl), Hydrobromic acid (HBr), Hydroiodic
acid (HI) etc..
Weak acid
Acid which partially dissociate in water are
called weak acids.
HF ⇌ H+ + F-
Weak acids:- Organic acids like citric acid,
Oxalic acid etc..
17. 4 Reaction of acid with metal
Acid + Metal Salt + Hydrogen gas
Eg:- Zn + H2SO4 ZnSO4 + H2
Zinc
metal Diluted sulphuric acid Zinc sulphate salt Hydrogen gas
18. 5. Reaction of acid with metal carbonate & Hydrogen Carbonate
Acid + Metal Carbonate Salt + CO2+ H2O
Eg:- 2HCl + MgCO3 MgCl2 +CO2 + H2O
Acid + Hydrogen Carbonate Salt + CO2+ H2O
Eg:- HCl + Na2CO3 NaCl + H2O + CO2
19. 6. Reaction of acid with metal oxides
Acid + Metal Oxide Salt + Water
Eg:- CuO + 2HCl CuCl2 + H2O
Copper Oxide Diluted Hydrochloric
acid Copper Chloride
Water
20. 7. Reaction of acid with bases
Acid + Base Salt + Water
Eg:- HCl + NaOH NaCl + H2O
Hydrochloric acid Sodium Hydroxide Sodium Chloride
Water
22. Properties of Base
1. Taste and touch
2. Action on indicators
3. Conduction of electricity & dissociation of ions
4. Reaction with metals
5. Reaction with non-metal oxides
6. Reaction with acids
23. Conduction of electricity & dissociation of ions
★ The bases which are soluble in water and give OH- ions in their aqueous
solution are called alkalis.
24. 3.1 Strong & weak bases
Strong base
Base which completely dissociate in water and
form OH- are called strong bases.
Eg:- KOH K+ + OH-
Strong bases :- Lithium hydroxide (LiOH),
Sodium hydroxide (NaOH), Rubidium hydroxide
(RbOH) etc
Weak base
bases which seldomly produce OH- ions when
dissolved in water are called weak bases.
NH3+ H2O ⇌ NH4
+ + OH-
Weak bases: Ammonium hydroxide(NH4OH),
Copper hydroxide (Cu(OH)2)
25. Reaction of base with metal
Metal + Base Salt + Hydrogen gas
Eg:- 2NaOH + Zn Na2ZnO2 + H2
Sodium Hydroxide
Zinc Metal Sodium zincate
Hydrogen
26. Reaction of base with non-metal Oxides
Non-metal Oxide + Base Salt + Water
Eg:- Ca(OH)2 + CO2 CaCO3 + H2O
Calcium Hydroxide
Carbon dioxide Calcium carbonate
Water
27. Reaction of base with acid
Acid + Base Salt + Water (Neutralization)
Eg:- HCl + KOH KCl + H2O
➢ Neutralization is the process in which acid react with base each other to
produce salt and water.
➢ Salt is obtained when hydrogen of acids is replaced by the metal.
Eg:- HCl NaCl, H2SO4 Na2SO4
Common Salt:- NaCl is Obtained from sea
28. Fact Checking
➔ Metallic Oxides are Basic Oxides:
Because metallic oxides react with acids to give salt and water, similar to the
reaction of a base with an acid
➔ Non-metallic oxides are Acidic oxides:
Because non-metallic oxides react with bases to give salt and water, similar
to the reaction of an acid with base.
29. Role of water in dissociation
➔ Most of the acids and bases have no dissociation (furnishing H+ and OH-)
without water.
➔ Dissociation process is highly exothermic.
30. Self dissociation of water
➔ Dissociation of water itself is extremely small and only about 2 out of every billion water
molecules are dissociated in 25oC.
➔ H2O ⇌ H+ +OH-
➔ H+= OH- = 1.0 x 10-7
➔ Pure water or ionic product of water is H+= OH- It’s symbolized as Kw (Ionic Constant
product of water). So we conclude that:
Kw = [H+] [OH-] ie: Kw = (1.0 x 10-7) x (1.0 x 10-7)
Kw = 1.0 x 10-14
34. pH and its importance
➔ pH means the power of hydrogen
➔ It was denoted by Danish biochemist Soren Sorensen in 1909.
pH= log 1/[H+]
➔ Acid rain is 5.6 pH
40. Common acids and bases
Common acids pH Value Common Bases pH Value
HCl 0 Blood Plasma 7.4
Stomach acid 1 Egg white 8
Lemon Juice 2 Sea water 8
Vinegar 3 Baking soda 9
Oranges 3.5 Antacids 10
Soda, Grapes 4 Ammonia water 11
Sour Milk 4.5 Lime water 12
Fresh Milk 5 Drain cleaner 13
Human Saliva 6-8 Caustic soda 14
Pure water 7
42. Use of pH in everyday life
➔ pH in humans and animals: Biochemical reactions in our body are narrow are
in narrow pH range of 7.0 -7.8. Even small change in it disturbs this process.
➔ Acid rain: if rain water falls below pH 5.6 it’s called acid rain.
➔ pH in plants: plants have a healthy growth when a specific pH range is
maintained.
➔ In digestive system: Our stomach produce hydrochloric acid which helps
digestion of food.
➔ Self defence of animals and plants: Bee sting causes severe pain and burning
sensation.it’s due to methanoic acid. Use of mild base can prevent it.
43. Use of pH in everyday life
➔ Self defence of animals and plants: Nettle plant have fine stinging hair which
inject methanoic acid.
➔ Tooth decay: tooth enamel is made of calcium phosphate which hardest
substance in our body. If we didn’t wash our mouth properly after every meal,
the food particles and sugar remaining in mouth produces acids with the help
of bacterias in our mouth. If its pH goes below 5.5 it cause to corrode the
tooth enamel and tooth decay.
44.
45.
46. Formation of salts
1) By neutralization of acids and bases
NaOH + HCl → NaCl + H2O
1) By action of acid on metals
Zn + H2SO4 → ZnSO4 + H2
1) By action of acid on metal carbonates and hydrogen carbonates
CaCO3 + 2HCl → CaCl2 + H2O +
CO2
NaHCO3 + HCl → NaCl + H2O
+ CO2
47. Types of salts
Acid Base Nature of Solution pH (at 25oC)
Strong Strong Neutral pH=7
Weak Strong basic pH>7
Strong Weak acidic pH<7
Weak Weak More information
required
_
48. Some commonly used salts
1. Baking soda
➔ Sodium hydrogen carbonate (NaHCO3)
➔ Manufacturing is through Solvay's process
➔ Raw Materials required: Limestone (CaCO3), Sodium Chloride (NaCl) in the
form of brine, Ammonia (NH3).
➔ Process: A. CaCO3 →(Heating) CaO + CO2
B. NaCl + CO2 + NH3+ H2O → NaHCO3 + NH4Cl
C. 2NaHCO3 →(Heating) Na2CO3+ H2O+ CO2
➔ Uses: Cooking of certain foods, baking powder, medicine,
soda acid fire extinguisher.
49. Some commonly used salts
2. Washing soda
➔ Sodium carbonate decahydrate (Na2CO3 10H2O)
➔ Raw Materials required: Limestone (CaCO3), Sodium Chloride (NaCl)
in the form of brine, Ammonia (NH3).
➔ Manufacture:
2NaHCO3 →(Heating) Na2CO3+ H2O+ CO2
Na2CO3+10H2O → Na2CO3 10H2O
Uses: Caustic soda, glass, soap powder, paper industry, to remove
permanent hardness of water, cleaning agent.
50. Some commonly used salts
3. Plaster of paris
➔ POP- Calcium sulphate hemihydrate (2 CaSO4. ½ H2O)
➔ Raw Materials required: Gypsum(2 CaSO4.2 H2O).
➔ Manufacture:
2 CaSO4.2 H2O →(Heating 100oC) 2 CaSO4. ½ H2O + 3/2 H2O
Uses: making toys, chalk, fire proof materials, ceilings, wall, pillars.
51. Some commonly used salts
4. Bleaching powder
➔ Calcium oxychloride (CaOCl2)
➔ Raw Materials required: Slaked lime (Ca(OH)2), Chlorine gas (Cl2).
➔ Manufacture: Hasenclever process.
(Ca(OH)2 + Cl2 → CaOCl2 + H2O
Uses: textile industry, bleaching of wood pulp, to make wool
unshrinkable.