Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

Acids, Bases, and Salts – Definition, Types, Properties, and Uses

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Acids, Bases, and Salts

Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

They are found in various substances including our food. Vinegar or acetic acid is used as a food preservative. Citrus fruits have citric acid and etc.

Other than food they also have a wide variety of uses such as in various industries, manufacturing plants, processing plants, laboratories, and others. In this article, we will learn about Acids, Bases, and Salts, their properties, types, uses, and others in detail. The figure given below shows acid and base which when reacting form salt.

Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

What are Acids?

Acids are a type of chemical substance that is characterized by their ability to donate hydrogen ions (H+) when dissolved in water. Acids can be found naturally in many foods and beverages, including citrus fruits, vinegar, and fermented products, and they are also used in various industrial processes. Here are some key points about acids:

  • Acids can be classified into two categories: organic acids, which are derived from living organisms, and inorganic acids, which are derived from non-living sources.
  • Acids have a sour taste and can cause a tingling or burning sensation on the tongue or skin.
  • The strength of an acid is determined by its pH value, which ranges from 0 to 14. Acids with a pH less than 7 are considered to be acidic, while those with a pH greater than 7 are basic or alkaline.
  • Acids can react with bases to form salts and water in a process called neutralization.
  • Acids are used in a variety of industrial applications, such as the production of fertilizers, dyes, and pharmaceuticals.
  • Some acids can be harmful or corrosive to living tissue, such as hydrochloric acid, which is found in the stomach and is necessary for digestion, but can cause severe burns if it comes into contact with the skin.
  • Acids are also used in various chemical reactions, such as in the production of polymers and plastics, as well as in the cleaning and sterilization of medical equipment.
Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

Physical Properties of Acids

Acids are chemical substances that have unique physical and chemical properties. Here are some of the physical properties of acids:

Acids have a sour taste: Most acids have a distinctly sour taste, such as lemon juice and vinegar.

Acids change the color of indicators: Acids change the color of certain indicators, such as litmus paper, which turns red in the presence of an acid.

Acids are corrosive: Many acids are corrosive and can cause damage to living tissue or corrode metal and other materials.

Acids have a low pH: The pH scale measures the acidity or alkalinity of a solution, with a pH of 7 being neutral, and lower pH values indicating greater acidity. Acids typically have a pH of less than 7.

Acids react with bases to form salts and water: When an acid reacts with a base, the two substances neutralize each other, forming a salt and water.

Acids have a higher boiling point than water: Acids generally have a higher boiling point than water, which means that they require more energy to boil than water.

Acids are good conductors of electricity: In a solution, acids can conduct electricity because they contain charged particles known as ions.

Chemical Properties of Acid

Acid has various chemical properties few of the following chemical properties of acids include, 

Reaction of acids with metal: When an acid reacts with a metal, it produces hydrogen gas and the corresponding salt. 

Metal + Acid → Salt + Hydrogen

Example: When hydrochloride acid combines with zinc metal, it produces hydrogen gas and zinc chloride.

Zn + 2HCl  → ZnCl2 + H2

Reaction of acids with metal carbonate: When acids react with metal carbonates, they produce carbon dioxide gas and salts as well as water.

Metal carbonate + Acid → Salt + Carbon dioxide + Water

Example: When hydrochloric acid combines with sodium carbonate, it produces carbon dioxide gas, sodium chloride, and water.

 Na2CO3 + 2HCl → 2NaCl + H2O + CO2

Reaction of acid with hydrogen carbonates (bicarbonates): When acids react with metal hydrogen carbonates, they produce carbon dioxide gas, salt, and water.

Acid + Metal hydrogen carbonate → Salt + Carbon dioxide + Water

Example: Sulfuric acid gives sodium sulfate, Carbon dioxide gas and water when it reacts with sodium bicarbonate.

2NaHCO3 + H2SO4 → NaCl + CO2 + H2O

Types of Acids

Acids are classified into different categories, the classification of acids is discussed below in the article.

On the basis of their Occurrence 

On the basis of their Occurrence  acid are subdivided into two categories

  • Natural Acid
  • Mineral Acids

Natural Acid

Natural acids, often known as organic acids, are acids derived from natural sources. For example Methanoic acid (HCOOH), Acetic acid (CH3COOH), Oxalic acid (C2H2O4), etc.

Mineral Acids

Mineral acids are acids that are created from minerals. Inorganic acids, man-made acids, and synthetic acids are all examples of Mineral Acids. For example Hydrochloric acid (HCl), Sulphuric acid (H2SO4), Nitric acid (HNO3), Carbonic acid (H2CO3), Phosphoric acid (H3PO4), etc.

On the basis of Concentration

On the basis of Concentration, acids are categorized into two categories

Strong Acids

Strong Acid is an acid that is totally ionized in water and produces (H+). For example Hydrochloric acid (HCl), Sulphuric acid (H2SO4), Nitric acid (HNO3) etc.

Weak Acids

A weak acid is partially ionized in water, creating a tiny amount of hydrogen ions (H+). For example Acetic acid (CH3COOH), Carbonic acid (H2CO3) etc. 

Uses of Acids

Acids have various uses some of the important uses of acid are,

  • Vinegar is a diluted solution of acetic acid that has a variety of uses in the home. It’s mostly utilized in the food industry as a preservative.
  • Orange and lemon juice contain a significant amount of citric acid. It can also be used for food preservation.
  • In batteries, sulfuric acid is commonly utilized. This acid is typically found in the batteries used to start vehicle motors.
  • Sulfuric and nitric acid is used in the industrial production of dyes, explosives, paints, and fertilizers.
  • Many soft drinks contain phosphoric acid as the main ingredient.

What are Bases?

Bases are chemical compounds that react chemically with acids, they produce salts and hydroxide ions (OH–) in water. For example Potassium hydroxide (caustic potash or KOH), Calcium hydroxide (Ca(OH)2), Sodium hydroxide (caustic soda or NaOH) etc. The image given below shows a base in its aqueous medium.

Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

Physical Properties of Base

Bases have specific physical properties and they can easily be distinguished by their physical properties. Some physical properties of bases are:

  • Base has a bitter taste
  • Bases are soapy to touch
  • Base change red litmus to blue
  • Aquous solution of base conducts electricity

Chemical Properties of Base

Bases have various chemical properties few of the following chemical properties of bases are,

Reaction of Base with Metals: When alkali (base) reacts with metal, salt and hydrogen gas is produced.

Alkali + Metal → Salt + Hydrogen

Example: When sodium hydroxide interacts with aluminium metal, sodium aluminate and hydrogen gas are generated.

2NaOH + 2Al + 2H2O → 2NaAlO2 + 2H2

Reaction of Non-Metallic Oxides with Base: Salt and water are formed when non-metallic oxides react with a base.

Non-metallic oxide + Base → Salt + Water

Example: When calcium hydroxide reacts with carbon dioxide calcium carbonate is formed along with water.

Ca(OH)2 + CO2 → CaCO3 + H2O

Action of Alkalis/Base with Ammonium Salts: Ammonia is produced when alkalis react with ammonium salts.

Alkali + Ammonium salt   →   Salt   +  Water  +  Ammonia

Example: When calcium hydroxide reacts with ammonium chloride, calcium chloride, water, and ammonia are produced.

Ca(OH)2 + NH4Cl  →  CaCl2 + H2O + NH3

Types of Bases

Acidity, concentration, and degree of ionization are three variables that can be used to classify bases.

Types of Bases Based on Acidity

The number of hydroxyl ions presents determines acidity in bases. Based on acidity, bases are classified into three categories:

  • Monoacidic
  • Diacidic
  • Triacidic

Monoacidic

Mono-acidic bases are those that contain only one hydroxyl ion and interact with only one hydrogen ion. Mono-acidic bases include NaOH, KOH, and others.

Diacidic

Diacidic base is a base with two hydroxyl ions that interact with two hydrogen ions. Ca(OH)2, Mg(OH)2, and other di-acidic bases are examples.

Triacidic

Triacidic base is a type of base that comprises three hydroxyl ions and three hydrogen ions. Triacidic bases include Al(OH)3, Fe(OH)2, and others.

Types of Bases Based on their Concentration

Based on their concentration in an aqueous solution, bases are divided into two categories:

Concentrated: The concentration of base in these types of bases is higher in the solution. Concentrated NaOH solution, for example.

Diluted: These types of bases have a lower concentration of base in their aqueous solution. For instance, dilute NaOH, dilute KOH, and so on.

Types of Bases Based on their Degree of Ionization

The degree of ionization of bases in solution can be used to classify them. It’s also known as foundation strength. When dissolved in water, it produces a certain quantity of hydroxyl ions. The degree of ionization distinguishes two types of bases.

Strong Base: A strong base is one that dissociates entirely or to a large extent in water. For example, NaOH, KOH, and strong bases.

Weak Base: A weak base is one that does not dissolve entirely or only dissociates to a very little level. For example, NH4OH, and others are weak bases.

Uses of Bases

Base has various uses some of the important uses of the base are,

  • Sodium hydroxide is used in the making of paper and soap. Sodium hydroxide (NaOH) is also utilized in the production of rayon.
  • Bleaching powder is made from Ca(OH)2, commonly known as calcium hydroxide or slaked lime.
  • Calcium hydroxide is used to create dry mixtures for painting and decorating.
  • Magnesium hydroxide, popularly known as milk of magnesia, is a laxative that is extensively used. It is also used as an antacid since it decreases excess acidity in the human stomach.
  • In laboratories, ammonium hydroxide is a critical reagent.
  • Slaked lime can be used to neutralize any excess acidity in soils.

Alkali

Bases that are easily dissolved in water are called Alkali, in other words, water-soluble bases are called Alkali. For example, NaOH is an alkali as it dissolves in water forming Na+ and OH– ions.

Difference between Alkali and Base

The difference between Alkali and Base can easily be understood with the help of the table given below,

Alkali Vs Base
AlkaliBase 
Water soluble bases are called alkaliBases do not dissolve in water
All alkalis are basesNot all bases are alkali
Alkali releases OH– ions on dissolving in water, they also are proton acceptors.Bases neutralize the acid in an acid-base neutralization reaction.
Example: Potassium Hydroxide (KOH), Sodium Hydroxide(NaOH)Example: Zinc hydroxide(ZnOH), Copper Oxide(CuO)

Arrhenius’s Theory of Acid and Base

What is acid, what is base, and what is the difference between acid and base? these questions are nightmares to chemists in the early 15 and 16 centuries. To solve these questions a chemist name Arrhenius came up with a theory called  Arrhenius theory. According to Arrhenius’s theory, a substance that gives H+ ion in its aqueous solution is called acid whereas the substance that ionizes OH– ion in the aqueous solution is called a Base.

HCl(aquaous solution) ⇌ H+ + Cl–

NaOH(aquaous solution) ⇌ Na+ + OH–

Bronsted-Lowry Theory of Acid and Base

Bronsted-Lowry Theory also provides an explanation of acid and base, according to this theory, acid is an H+ ion or a proton donor and it forms its conjugate base whereas the base is a substance that accepts an H+ ion or a proton to form conjugate acid.

Bronsted-Lowry Acid

According to Bronsted-Lowry acids are substances that donate a proton or H+ ion to the other compound.

Acid ⇌ Proton + Conjugate Base

Example: H2SO4 ⇌  H+ + HSO4–

Bronsted-Lowry Base

According to Bronsted-Lowry bases are substances that accept a proton or H+ ion from other compounds.

Base + Proton ⇌ Conjugate Acid

Example: OH– + H+ ⇌  H2O 

Strength of Acids and Bases

The strength of an acid or a base is measured by the amount of H+ ions or OH– ions present in their aqueous solution.

Strong acids have a higher concentration of H+ ions per unit volume in their aqueous solution whereas weaker acids have a lower concentration of H+ ions per unit volume in their aqueous solution. An example of a strong acid is H2SO4 and an example of a weak acid is CH3COOH. 

Similarly, strong bases have a higher concentration of OH– ions per unit volume in their aqueous solution whereas weaker bases have a lower concentration of OH– ions per unit volume in their aqueous solution. An example of a strong base is KOH and an example of a weak acid is CaO.

The strength of Acids and Bases can easily be measured using a pH scale.

pH Scale

pH scale is used to measure the basicity and acidity of a solution. It gives the strength of any solution. pH is determined by the amount of hydrogen ion concentration in the solution.

It is calculated using the formula,

pH = -log[H+]

For an acid, pH ranges from 0 to 7 whereas for a base it ranges between 7 and 14. The lower the pH higher is the strength of the acid and the higher the pH higher the strength of the base.

Note: pH ranges of acids and bases.

  • 0 < Acid < 7
  • 7 < Base< 14

Indicator

Indicators are chemical compounds which help to indicate the presence of acid or base in a chemical reaction. They possess different colours in acidic solutions and different colours in basic solutions. Indicators are made naturally by plants and animals or artificially by humans. The image shows a litmus test of acids and bases.

Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

An indicator indicating the pH

  • The range of 0 to 7 indicates an acidic solution. 
  • The range of 7 to 14 indicates the basic solution.
  • 7 is a neutral solution.

Types of Indicators

There are various types of indicators used for various purposes some of which are,

  • Natural Indicators: Indicators derived from plants, animals or any living organism are natural indicators. Examples, Red Cabbage, Litmus paper and others.
  • Synthetic Indicators:  Indicators made artificially in laboratories and factories are synthetic indicators. Examples, are Phenopthelien, Methyl orange, and others.
  • Olfactory Indicators: Substances that have different smells in acidic or basic mediums are called Olfactory Indicators. Example onions, olives and others.

What are Salts?

When an acid and a base react to neutralize one another, they generate sales, which are ionic substances. Salts do not have an electrical charge. Salts come in a variety of forms, the most common of which is sodium chloride. Table salt and common salt are both terms for sodium chloride. Sodium chloride is used to make dishes taste better. The image given below shows a salt and its cation and anion.

Acids, Bases, and Salts are the main chemical compounds that exist in our surroundings. Acids, Bases, and Salts are compounds that occur naturally and can also be created artificially.

Physical Properties of Salt

Salts have various physical properties and some of following physical properties of salts are,

  • In nature, the bulk of the salts is crystalline.
  • Salts that are transparent or opaque are available.
  • The bulk of salts is soluble in water.
  • Salt solutions, in their molten state, also transmit electricity.
  • The flavour of salt can be salty, sour, sweet, bitter, or umami (savoury).
  • There is no odour to neutral salts.
  • Salts that are colourless or coloured are available.
  • Because it contains ions, salt water is an excellent conductor of electricity.
  • Electrostatic attraction holds the ions together, and a chemical bond is established between them.

Types of Salts

Salts are categorised into various categories some of the important categories are given below

  • Acidic Salt
  • Basic or Alkali Salt
  • Neutral Salts

Acidic Salt

A partial neutralisation of a diprotic or polyprotic acid produces an acidic salt. These salts contain H+ cations or strong cations in their aqueous solution. The ionizable H+ makes up the majority of the ions. Some examples of acidic salts are NaHSO4­, KH2PO4 etc. These salts are formed by the neutralization of strong acids and weak bases.

Ammonium Chloride

Ammonium chloride is formed when hydrochloric acid (a strong acid) interacts with ammonium hydroxide (a weak base).

NH4OH + HCl → NH4Cl + H2O

Ammonium Sulphate

Ammonium sulphate is formed when ammonium hydroxide (a weak base) reacts with sulphuric acid (a strong acid).

2NH4OH + H2SO4 → (NH4)2SO4 + 2H2O

Basic or Alkali Salt

A basic salt is formed when a strong base reacts with a weak acid to partially neutralise it. When they are hydrolyzed, they decompose into a basic solution. This is because when a basic salt is hydrolyzed, it produces the conjugate base of a weak acid in the solution. e.g. Sodium Carbonate (Na2CO3), Sodium Acetate (CH3COONa)

Sodium Carbonate

Sodium carbonate is formed when sodium hydroxide (a strong base) reacts with carbonic acid (a weak acid)

H2CO3 + 2NaOH → Na2CO3 + H2O

Sodium Acetate

Sodium acetate is formed when a strongly basic, sodium hydroxide (a strong base), reacts with acetic acid (a weak acid)

CH3COOH + NaOH → CH3COONa + H2O

Neutral Salts

Salts generated by the reaction of a strong acid with a strong base are neutral in nature. The pH of these salts is 7, which is considered neutral. Potassium Chloride, Sodium Chloride, and others are examples of neutral salts.

Sodium Chloride (NaCl)

Sodium Chloride is formed when hydrochloric acid (a strong acid) mixes with sodium hydroxide (a strong base).

NaOH + HCl → NaCl + H2O

Sodium Sulphate (Na2SO4)

It’s made when sulphuric acid combines with sodium hydroxide (a strong basic) ( a strong acid).

2NaOH + H2SO4 → Na2SO4 + 2H2O

Salts can also be categorised into other categories which include,

Double Salt

Salts with more than one cation or anion are known as double salts. They’re created by mixing two different salts that crystallised in the same ionic lattice. e.g. Potassium Sodium Tartrate (KNaC4H4O6.4H2O) also known as Rochelle salt.

Mixed Salts

Salts which are produced by mixing two salts, which generally share a common cation or anion, are called mixed salt. e..g. Bleaching Powder CaOCl2.

What Causes the Formation of Acidic, Basic, and Neutral Salts?

The causes of the formation of Acidic, Basic, and Neutral Salts are discussed below,

  • When a strong acid reacts with a weak base, the base is unable to completely neutralise the acid. As a result, a salt that is acidic forms.
  • When a strong base is combined with a weak acid, the acid is unable to completely neutralise it. As a result, you get a simple salt.
  • When an equal-strength acid and base react, they totally neutralise each other. A neutral salt is formed as a result of this process.

Some Common Salts

Salts are chemical compounds that are formed as a result of a neutralization reaction between acids and bases. When we hear salt we only think about common salt which is Sodium chloride that we eat in our daily life but there are several other salts also which are widely useful. Here in this article, we will learn about some common salt that is widely used.

  • Baking Soda or Sodium Bicarbonate
  • Washing Soda or Sodium Carbonate
  • Bleaching Powder or Calcium Hypochlorite

Baking Soda

Baking soda also called Sodium Hydrogen Carbonate, is a chemical compound whose chemical formula is NaHCO3. Baking soda has a sodium cation (Na+) and a bicarbonate anion (HCO3–). Sodium bicarbonate is a white, crystalline powder and as the name suggests is used for baking.

Chemical Name: Sodium hydrogen carbonate

Chemical Formula: NaHCO3

Preparation:

Baking soda can be prepared with the help of the reaction given below.

NaCl(aq) + NH3(g) + CO2(g) + H2O(l) → NaHCO3(aq) + NH4Cl(aq)

Uses:

A few of the uses of Baking Soda are,

  • It is used as an antacid in case of acidity.
  • It is used for baking purposes.
  • It is used as a water softener.

Washing Soda

Washing soda also called Sodium Carbonate, is a chemical compound whose chemical formula is Na2CO3. Washing soda has two sodium cations (Na+) and a carbonate anion (CO32-). Sodium carbonate is a white, crystalline powder and as the name suggests is used for washing purposes.

Chemical Name: Sodium Carbonate

Chemical Formula: Na2CO3

Uses:

A few of the uses of Washing Soda are,

  • It is used in the glass, soap and paper industries.
  • It is used as washing powder.

Bleaching Powder

Bleaching Powder also called Calcium Hypochlorite, is a chemical compound whose chemical formula is CaOCl2. Bleaching Powder is used for bleaching purposes. In its aqueous solution bleaching powder releases chlorine which is responsible for the bleaching action.

Chemical Name: Calcium Hypochlorite

Chemical Formula: CaOCl2

Preparation:

Bleaching Powder can be prepared with the help of the reaction given below.

Ca(OH)2(aq) + Cl2(g) → CaOCl2(aq) + H2O(l)

Uses:

A few of the uses of Bleaching Powder are,

  • It is used for bleaching the laundry.
  • It is used as an oxidizer in many industries.
  • It is used as a disinfectant to clean water

Crystals of Salts

Some salts combining with water form crystals and these water molecules which are required to form crystals are called water of crystallisation. Some examples of crystal salts are Table salt (sodium chloride crystals), Sugar (sucrose crystals).

Plaster of Paris

Plaster of Paris is a widely used chemical compound is used for various purposes such as sculpting materials, gauze bandages, building and furnishing houses and others. Plaster of Paris is hydrated calcium sulphate obtained by calcining gypsum. It is a white powdery chemical compound.

Chemical Name: Calcium Sulphate Hemi Hydrate.

Chemical Formula: CaSO4. ½ H2O

Preparation of Plaster of Paris

Plaster of Paris can easily be prepared with the help of the equation given below,

CaSO4.2H2O (s) (heating at 100°C ) —> CaSO4. ½ H2O + 3/2 H2O

Also, Check

FAQs on Acids, Bases, and Salts

What are salts in acids, bases, and, salts?

The neutralization reaction of acids and bases results in a substance called salt. Salts are made of cations and anions. Some examples of salt are NaCl, Na2SO4

What are the two types of acids?

Acids can easily be categorised as,

  • Inorganic Acids: Examples, Sulphuric Acid (H2SO4), Nitric acid (HNO3), and others.
  • Organic Acids: Examples, Acetic acid Citric acid, and others.

What is the difference between an acid and a base?

Acids and bases are two types of corrosive chemicals.  Acids are ionic chemicals that break down in water to create the hydrogen ion (H+) and they have a pH value between 0 and 7, while base are ionic chemicals that break down in water to create the hydronium ion (OH–) and they have a pH value between 7 and 14.

What are the physical properties of bases?

The physical properties of bases are,

  • They have a bitter taste to them.
  • Their aqueous solutions have a soapy quality to them.
  • They change the colour of litmus paper from red to blue.
  • Their aqueous solutions are electrically conductive.
  • In an aqueous solution, they release OH– ions.

What are the physical properties of acids?

The physical properties of the acids are

  • Acids have a sour flavour to them.
  • Blue litmus turns red.
  • Electricity can be conducted through an acidic solution.
  • In an aqueous solution, they release H+ ions.

What happens when hydrochloric acid reacts with sodium carbonate?

When hydrochloric acid combines with sodium carbonate, it produces carbon dioxide gas, sodium chloride, and water.

                                             Na2CO3 + 2HCl → 2NaCl + H2O + CO2

Are salt basic or acidic?

A salt can either be basic or be acidic depending on the types of acid and base that react to form a salt.

Is NH4Cl a basic salt?

No, Ammonium chloride (NH4Cl) is an acidic salt because it is a salt of a strong acid (hydrochloric acid) and a weak base (ammonium hydroxide).

What happens when metal reacts with HCl?

Metal reacting with acid produces salt and hydrogen.

Acid + Metal → Salt + Hydrogen

Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations. In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS". He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.

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CBSE Class 11 Chemistry Syllabus

CBSE Class 11 Chemistry Syllabus is a vast which needs a clear understanding of the concepts and topics. Knowing CBSE Class 11 Chemistry syllabus helps students to understand the course structure of Chemistry.

Unit-wise CBSE Class 11 Syllabus for Chemistry

Below is a list of detailed information on each unit for Class 11 Students.

UNIT I – Some Basic Concepts of Chemistry

General Introduction: Importance and scope of Chemistry.

Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements,
atoms and molecules.

Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.

UNIT II – Structure of Atom

Discovery of Electron, Proton and Neutron, atomic number, isotopes and isobars. Thomson’s model and its limitations. Rutherford’s model and its limitations, Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.

UNIT III – Classification of Elements and Periodicity in Properties

Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.

UNIT IV – Chemical Bonding and Molecular Structure

Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.

UNIT V – Chemical Thermodynamics

Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics – internal energy and enthalpy, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction)
Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes.
Third law of thermodynamics (brief introduction).

UNIT VI – Equilibrium

Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization,
ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).

UNIT VII – Redox Reactions

Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.

UNIT VIII – Organic Chemistry: Some basic Principles and Techniques

General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.

UNIT IX – Hydrocarbons

Classification of Hydrocarbons
Aliphatic Hydrocarbons:
Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions.
Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition.
Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.

Aromatic Hydrocarbons:

Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.

To know the CBSE Syllabus for all the classes from 1 to 12, visit the Syllabus page of CBSE. Meanwhile, to get the Practical Syllabus of Class 11 Chemistry, read on to find out more about the syllabus and related information in this page.

CBSE Class 11 Chemistry Practical Syllabus with Marking Scheme

In Chemistry subject, practical also plays a vital role in improving their academic scores in the subject. The overall weightage of Chemistry practical mentioned in the CBSE Class 11 Chemistry syllabus is 30 marks. So, students must try their best to score well in practicals along with theory. It will help in increasing their overall academic score.

CBSE Class 11 Chemistry Practical Syllabus

The experiments will be conducted under the supervision of subject teacher. CBSE Chemistry Practicals is for 30 marks. This contribute to the overall practical marks for the subject.

The table below consists of evaluation scheme of practical exams.

Evaluation SchemeMarks
Volumetric Analysis08
Salt Analysis08
Content Based Experiment06
Project Work04
Class record and viva04
Total30

CBSE Syllabus for Class 11 Chemistry Practical

Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.

A. Basic Laboratory Techniques
1. Cutting glass tube and glass rod
2. Bending a glass tube
3. Drawing out a glass jet
4. Boring a cork

B. Characterization and Purification of Chemical Substances
1. Determination of melting point of an organic compound.
2. Determination of boiling point of an organic compound.
3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.

C. Experiments based on pH

1. Any one of the following experiments:

  • Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
  • Comparing the pH of solutions of strong and weak acids of same concentration.
  • Study the pH change in the titration of a strong base using universal indicator.

2. Study the pH change by common-ion in case of weak acids and weak bases.

D. Chemical Equilibrium
One of the following experiments:

1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions.
2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.

E. Quantitative Estimation
i. Using a mechanical balance/electronic balance.
ii. Preparation of standard solution of Oxalic acid.
iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid.
iv. Preparation of standard solution of Sodium carbonate.
v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonatesolution.

F. Qualitative Analysis
1) Determination of one anion and one cation in a given salt
Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4 +
Anions – (CO3)2‐ , S2‐, NO2‐ , SO32‐, SO2‐ , NO ‐ , Cl‐ , Br‐, I‐, PO43‐ , C2O2‐ ,CH3COO‐
(Note: Insoluble salts excluded)

2) Detection of ‐ Nitrogen, Sulphur, Chlorine in organic compounds.

G) PROJECTS
Scientific investigations involving laboratory testing and collecting information from other sources.

A few suggested projects are as follows:

  • Checking the bacterial contamination in drinking water by testing sulphide ion
  • Study of the methods of purification of water.
  • Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional
    variation in drinking water and study of causes of presence of these ions above permissible
    limit (if any).
  • Investigation of the foaming capacity of different washing soaps and the effect of addition of
    Sodium carbonate on it.
  • Study the acidity of different samples of tea leaves.
  • Determination of the rate of evaporation of different liquids Study the effect of acids and
    bases on the tensile strength of fibres.
  • Study of acidity of fruit and vegetable juices.

Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with the approval of the teacher.

Practical Examination for Visually Impaired Students of Class 11

Below is a list of practicals for the visually impaired students.

A. List of apparatus for identification for assessment in practicals (All experiments)
Beaker, tripod stand, wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand,
dropper, test tube holder, ignition tube, china dish, tongs, standard flask, pipette, burette, conical flask, clamp
stand, dropper, wash bottle
• Odour detection in qualitative analysis
• Procedure/Setup of the apparatus

B. List of Experiments A. Characterization and Purification of Chemical Substances
1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid
B. Experiments based on pH
1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied
concentrations of acids, bases and salts using pH paper
2. Comparing the pH of solutions of strong and weak acids of same concentration.

C. Chemical Equilibrium
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing
the concentration of eitherions.
2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the
concentration of either of the ions.

D. Quantitative estimation
1. Preparation of standard solution of oxalic acid.
2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard
solution of oxalic acid.

E. Qualitative Analysis
1. Determination of one anion and one cation in a given salt
2. Cations – NH+4
Anions – (CO3)2-, S2-, (SO3)2-, Cl-, CH3COO-
(Note: insoluble salts excluded)
3. Detection of Nitrogen in the given organic compound.
4. Detection of Halogen in the given organic compound.

Note: The above practicals may be carried out in an experiential manner rather than recording observations.

We hope students must have found this information on CBSE Syllabus useful for their studying Chemistry. Learn Maths & Science in interactive and fun loving ways with ANAND CLASSES (A School Of Competitions) App/Tablet.

Frequently Asked Questions on CBSE Class 11 Chemistry Syllabus

Q1

How many units are in the CBSE Class 11 Chemistry Syllabus?

There are 9 units in the CBSE Class 11 Chemistry Syllabus. Students can access various study materials for the chapters mentioned in this article for free at ANAND CLASSES (A School Of Competitions).

Q2

What is the total marks for practicals examination as per the CBSE Class 11 Chemistry Syllabus?

The total marks for the practicals as per the CBSE Class 11 Chemistry Syllabus is 30. It includes volumetric analysis, content-based experiment, salt analysis, class record, project work and viva.

Q3

Which chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry?

The organic chemistry chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry.

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