Sulfuric Acid or Sulphuric Acid is a mineral acid consisting of one Sulfur, four Oxygen, and two Hydrogen atoms. The chemical or molecular formula of Sulfuric Acid is H2SO4. Sulfuric Acid is one most important commercially used chemicals. It is also known as Mattling acid or Hydrogen Sulfate or Vitriol. Sulphuric acid is a very strong acid and viscous liquid. It is a colorless, odorless, oily liquid, and corrosive in nature. Sulfuric acid is a component of acid rain as it is soluble in water.
Sulfuric acid is a highly acidic liquid. As a result, it is used for the cleaning of metals, the extraction of impurities from oil, the production of chemicals such as nitric acid and hydrochloric acid, and the manufacture of dye, medicines, detergents, and explosives, among other processes. The molar mass of Sulfuric Acid is 98.079 g/mol. The density of Sulfuric acid is 1.83 g/cm3. The H2SO4 molecule is covalent and has a tetrahedral structure and monoclinic crystal structure.
Table of Contents
What is Sulfuric Acid?
Sulfuric acid is a highly reactive chemical. Sulfuric acid is used in many industries like lead-based automobile batteries, the production of various chemicals, glue, and explosives, the refinement of petroleum, the curing of metal, etc. Hence, due to these wide applications, it is referred to as the “King of Chemicals“. The chemical formula for Sulfuric or Sulphuric Acid is H2SO4.
As shown below, Sulfuric Acid (H2SO4) is a covalent compound that consists of a Sulfur atom, which is attached to two Oxygen atoms and two Hydroxyl molecules (-OH).
Properties of Sulfuric Acid (H2SO4)
Physical Properties of Sulfuric Acid
H2SO4 is a viscous, thick, colorless, and oily liquid
Sulfuric acid has a density of 1.84 g/mL, a boiling point of 337 °C, and a melting point of 10 °C.
Concentrated sulfuric acid is 98% in water, and is the most stable form. Many other concentrations, with different names, are available for various purposes like Battery acid which is 29–32%, chamber acid which is 62-70%, and tower acid which is 78-80%.
It has a specific gravity of 1.84 at 298 K.
It turns blue litmus red and the pH values of sulphuric acid in mmol/l are mentioned in the table below,
pH values
1 mM
10 mM
100 mM
Sulphuric acid (in mmol/l)
2.75
1.87
1.01
It is highly corrosive, making it dangerous to touch.
Chemical Properties of Sulfuric Acid
H2SO4 is a strong acid that completely dissociates into ions in its aqueous solution as,
H2SO4 ⇢ H2+ + SO4-2
Sulphuric Acid is a good oxidizing agent, as it oxidizes other substances by donating its oxygen atoms, in a chemical reaction. As shown below, it oxidizes carbon and sulphur.
2H2SO4 + C ⇢ 2H2O + 2SO2 + CO2
2H2SO4 + S ⇢ 2H2O + 3SO2
Sulfuric acid reacts vigorously with water in a highly exothermic reaction (i.e., releases heat).
Sulphuric Acid is a dibasic acid and releases two hydrogen ions per molecule.
Sulphuric Acid has hygroscopic properties, which implies that H2SO4 can draw and control moisture from its surroundings. This effect makes it a good dehydrating agent.
It is less volatile. This is why it contributes to preparing more volatile acids from their complementary salts.
Structure of Sulphuric Acid
Two oxygen atoms form double bonds with the Sulphur atom, while two hydroxyl groups (OH) form single bonds with the Sulphur atom. Due to its ability to release two protons, it is a diprotic acid. As shown below, the molecule has a tetrahedral structure and is covalent.
Preparation of Sulfuric Acid
Sulfuric Acid is generally prepared and manufactured by the following two methods, which are widely used.
Contact Process
Lead Chamber Process
Contact Process for manufacturing of Sulfuric Acid
The Contact Process comprises three phases in the production of sulphuric acid:
Preparation of Sulphur dioxide by burning sulphur or sulphide ores in the air.
S (s) + O2 (g) → SO2 (g)
Reaction between sulphur dioxide with oxygen in the presence of V2O5 catalyst to produce Sulphur trioxide (SO3) as,
2SO2 (g) + O2 (g) → 2SO3 (g)
SO3 + H2SO4 (Oleum) → H2S2O7
H2S2O7 (l) + H2O (l) → 2H2SO4 (Sulfuric Acid)
The sulphuric acid obtained by the Contact process is 96–98% pure.
Lead Chamber Process
One of the most popular manufacturing processes is the lead Chamber method. It produces around 50 to 60 B-grade acids. Wet SO2 in the presence of nitrogenous oxides is used in this procedure (dynamic impetus). As a result, it undergoes oxidation with airborne oxygen to produce sulphur trioxide. This reaction is stated as,
2SO2 + O2 → 2SO3
Then, water and sulphur trioxide are allowed to interact, resulting in H2SO4. This reaction is stated as,
SO3 + H2O → H2SO4
Molecular Mass of Sulphuric Acid
Sulphuric acid has the chemical formula H2SO4. According to this formula, one molecule of sulphuric acid (H2SO4) comprises 2 moles of hydrogen, 1 mole of sulfur, and 4 moles of oxygen atoms. As a result, the molecular mass of H2SO4 will be equal to the sum of the masses of two moles of hydrogen, one mole of sulfur, and four moles of oxygen. Because hydrogen has an atomic mass of 1u, sulfur has an atomic mass of 32u, and oxygen has an atomic mass of 16u, the molecular mass of sulphuric acid may be computed as follows:
The molecular mass of H2SO4 = Mass of 2 moles of hydrogen atoms + Mass of 1 mole of sulphur + Mass of 4 moles of oxygen atoms
= 2 × 1 + 32 + 4 × 16
= 2 + 32 + 64
= 98 u
Thus, the molecular mass of sulphuric acid is 98u and the molecular weight of sulphuric acid is 98 g/mol.
Reactions of Sulfuric Acid
Dissociation- When pure water-free sulphuric acid is cooked, sulfur trioxide and water are formed.
H2SO4 → SO3 + H2O
Acidic Character of Sulphuric Acid- It’s a common dibasic acid that turns blue litmus crimson when exposed to it. It divides into two groups of salts.
NaOH + H2SO4 → NaHSO4 + H2O
2NaOH + H2SO4 → Na2SO4 + 2H2O
Sulphonating Action of Sulphuric Acid- Concentrated sulphuric acid combines with a variety of organic molecules, such as benzene, toluene, and others, to form sulphonic acids, as an example.
C6H6 + H2SO4 → C6H5SO3H + H2O
Precipitation Reactions with Sulphuric Acid- It creates insoluble sulfates that precipitate when handled with aqueous solutions of barium, lead, and other salts, for example.
H2SO4 + BaCl2 → BaSO4↓ + 2HCl
Reaction with Sulphur Trioxide- Oleum, commonly known as fuming sulphuric acid, is formed when it dissolves sulfur trioxide.
H2SO4 + SO3 → H2S2O7
Uses of Sulfuric Acid
Sulfuric acid is known as one of the most essential reagents, and it has several industrial uses. Several instances include:
Fertilizers such as ammonium sulfate, lime superphosphate, and others are made in this way.
In the production of colors, explosives, and pharmaceuticals.
H2SO4 is used in the production of acids such as HCl and HNO3.
In the production of pigments, paints, and polymers, for example.
In the paper and textile industries, for example.
Nitrocellulose is used in the production of goods.
Applications in metallurgy (Example: Cleaning metals before enameling, electroplating, and galvanizing).
In the leather business.
In storage compartments.
In the oil and gas sector.
In the detergent business.
It works as a dehydrator.
As a reagent in the laboratory.
FAQs on Sulfuric Acid
Question 1: What are the uses of sulphuric acid?
Answer:
Fertilizers, dyestuffs, explosives, and pharmaceuticals are all made with sulphuric acid. It is also used to make acids such as HCl and HNO3. It’s frequently utilised in the metallurgical industry (Example: Cleaning metals before enamelling, electroplating and galvanising).
Question 2: Why is Sulphuric acid called the king of chemicals?
Answer:
Sulphuric acid, sometimes known as the “king of chemicals,” is one of the most significant substances. It’s also known as vitriol oil since it used to be made from green vitriol back in the day. It is very corrosive and more reactive than other acids. As a result, it has a wide range of uses, including usage in laboratories, batteries, detergents, and the manufacture of numerous medications.
Question 3: What will happen when Sulphuric Acid reacts with aqueous solutions of the salts of barium?
Answer:
It generates insoluble sulphates that precipitate when handled with aqueous solutions of barium salts.
H2SO4 + BaCl2 → BaSO4↓ + 2HCl
Question 4: What will happen when Sulphuric Acid reacts with Sulphur Trioxide?
Answer:
Sulphuric acid dissolves sulphur trioxide to generate oleum, often known as fuming sulphuric acid.
H2SO4 + SO3 → H2S2O7
Question 5: What is the structure of sulphuric acid?
Answer:
In sulphuric acid, two hydrogen atoms are firmly bonded to two oxygen atoms, resulting in two-OH groups. The molecule is covalent and has a tetrahedral structure.
Question 6: Which acid is the strongest in the world?
Answer:
Fluoroantimonic acid is a superacid mixture of Antimony Pentafluoride and Hydrofluoric Acid, which is the strongest in the world.
Neeraj Anand, Param Anand
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.
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 Scheme
Marks
Volumetric Analysis
08
Salt Analysis
08
Content Based Experiment
06
Project Work
04
Class record and viva
04
Total
30
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 theapproval 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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