Electrolyte – Definition, List of Electrolytes and Examples with FAQs

What are Electrolytes?

An electrolyte is a substance that dissociates in water into charged particles called ions. Positively charged ions are called cations. Negatively charged ions are called anions. Simply, an electrolyte is a substance that can conduct an electric current when melted or dissolved in water.

Electrolysis is the process of passing an electric current through a substance in the molten or aqueous state thereby decomposing it. Glucose and urea do not dissociate in water because they have no electric charge. Therefore, these substances are called nonelectrolytes. The electrolyte is a compound which conducts electricity in the molten state or when dissolved in water.

Electrolytes Explanation

An ionic compound for example, sodium chloride dissolved in water is called an electrolyte because it conducts electricity. Electrolytes are important body constituents because they,

  • Conduct electricity, essential for muscle and nerve function.
  • Exert osmotic pressure, keeping body fluids in their own compartments.
  • Act as before to resist pH changes in body fluids.

Many biological compounds, for example, carbohydrates are not ionic and therefore have no electrical properties when dissolved in water. Important electrolytes other than sodium and chloride include potassium, calcium, bicarbonate and phosphate.

List of Electrolytes

1. Major Electrolytes Outside the Cell

Sodium and chloride, the major electrolytes in extracellular fluid, exert most of their influence outside the cell. Sodium concentration affects serum osmolality and extracellular fluid volume. Sodium also helps nerve and muscle cells interact. Chloride helps maintaining osmotic pressure. Gastric mucosal cells need chloride to produce hydrochloric acid, which breaks down food into absorbable components.

Calcium and bicarbonate are two other electrolytes found in extracellular fluid. Calcium is the major cation involved in the structure and function of bones and teeth. Calcium is needed to

  • stabilize the cell membrane and reduce its permeability to sodium transmit nerve impulses
  • contract muscles
  • coagulate blood
  • form bone and teeth
  • bicarbonate plays a vital role in acid base balance.

2. Major Electrolytes Inside the Cell

Potassium, phosphate and magnesium are among the most abundant electrolytes inside the cell.

Potent potassium

  • Potassium plays an important role in
  • cell excitability regulation
  • nerve impulse conduction
  • resting membrane potential
  • muscle contraction and myocardial membrane responsiveness
  • intracellular osmolality control

Fundamental phosphorus

The body contains phosphorus in the form of phosphate salts. Sometime the word phosphorus in the form of phosphate salts. Sometimes the words phosphorus and phosphate are used interchangeably. Phosphate is essential for energy metabolism. Combined with calcium, phosphate plays a key role in bone and tooth mineralization. It also helps maintain acid-base balance.

Magnesium acts as a catalyst for enzyme reactions. It regulates neuromuscular contraction promotes normal functioning of the nervous and cardiovascular systems, and cardiovascular systems and aids in protein synthesis and sodium and potassium ion transportation.

Understanding Electrolytes

Electrolytes help to regulate water distribution, govern acid base balance and transmit nerve impulses. They also contribute to energy generation and blood clotting. This table summarizes the functions of each of the body’s major electrolytes.

Potassium (K)Main intracellular fluid (ICF) cation. Regulate cell excitability. Permeates cell membranes, thereby affecting the cells electrical status. Helps to control ICF osmolality and consequently ICF osmotic pressure.
Magnesium (Mg)A leading ICF cation. Contributes to many enzymatic and metabolic processes particularly protein synthesis. Modifies nerve impulse transmission and skeletal muscle response.
Phosphorus (P)Main ICF anion Promotes energy storage and carbohydrate, protein and fat metabolism. Acts as a hydrogen buffer.
Sodium (Na)Main extracellular fluid (ECF) cation. Helps govern normal ECF osmolality. Helps maintain acid-base balance Activate nerve and muscle cells Influence water distribution.
Chloride (Cl)Main ECF anion. Helps maintain normal ECF osmolality. Affects body pH. Plays a vital role in maintaining acid-base balance and combines with hydrogen ions to produce hydrochloric acid.
Calcium (Ca)A major cation in teeth and bones is found in fairly equal concentrations in ICF and ECF. Also found in cell membranes, where it helps cells adhere to one another and maintain their shape. Acts as an enzyme activator within cells. Aids coagulation Affects cell membrane permeability and firing level.

Electrochemical Cells

Electrochemical cells are of three basic types. The electrolytic cell, the galvanic cell, and the concentration cell. All such cells are similar in that they have four basic components. These components are

  • The electrolyte is the current-carrying medium between the anode and cathode. It usually is homogeneous in an aqueous solution, but in moist soil, it may vary locally as to concentration or kind of dissolved chemicals.
  • The anode is a metal or substance in contact with the electrolyte capable of conducting an electric current and corrodes by combining with chemicals in the electrolytes.
  • The cathode is also a metal contacting the electrolyte. It is not corroded but receives protection against corrosion.
  • The conductor extremely connects the anode and cathode and completes the circuit for current flow.

Electrolyte Movement

When cells die their contents spill into the extracellular area and upset the electrolyte balance. In this case, elevated levels of intracellular electrolytes are found in plasma.

Although electrolytes are generally concentrated in a specific compartment, they aren’t confined to these areas. Like fluids, they move around trying to maintain balance and electroneutrality.

Electrolyte Balance

Fluid and output acid-base balance hormone secretion and normal cell function can influence electrolyte balance. Because electrolytes and individual imbalances in one electrolyte can affect balance in others.

The body fluids contain a variety of dissolved chemicals that may be categorized as either nonelectrolytes or electrolytes. Nonelectrolytes are those compounds with covalent bonds that therefore do not dissociate when dissolved in water. Electrolytes are those compounds with at least one ionic bond that dissociate freely when dissolved in water.

Even though electrolytes exist inside and outside only the levels outside the cell in the bloodstream are measured. Although serum levels remain fairly stable throughout a person’s life span, understanding which levels are normal and which are abnormal is critical to decide quickly and appropriately to a patient’s electrolyte imbalance.

Frequently Asked Questions on Electrolytes

Q1

What are electrolytes in the body?

All electrolytes are sodium, calcium, potassium, chlorine, phosphate, and magnesium; You get them from the food you consume and your drinking fluids. Electrolyte levels can become too small or too high in your body. This can happen when the body changes its amount of water.

Q2

Why are electrolytes important?

Electrolytes are compounds in body fluids that make up electrically charged particles (ions). These ions hold the required electrical energy for many functions including muscle contractions and nerve impulse transmission. Numerous body functions depend on electrolytes.

Q3

What are common electrolytes?

Electrolytes are found in the human body, and the electrolyte balance in our bodies is necessary for our cells and our organs to function normally. Common electrolytes tested by blood-testing physicians include sodium, potassium, chloride, and bicarbonate.

Q4

Is Salt an electrolyte?

Placing a salt in a liquid (such as water) often contributes to an electrolyte solution, as the salt components dissociate in a process called liquid. Electrolytes can also be smelted salts. Molten sodium chloride, for example, is a liquid that can conduct electricity.

Q5

Is water an electrolyte?

Simple water, which has a very low ion content, can’t conduct electricity. When a solvent dissociates to form ions in water, it is called an electrolyte, since the solution is a strong electrical conductor.

Q6

Is sugar a Nonelectrolyte?

Glucose, or C6H12O6, is a typical example of a nonelectrolyte Glucose (sugar) dissolves readily in water, but because it does not dissociate in solution into ions, it is called a nonelectrolyte; glucose-containing solutions, therefore, do not conduct electricity. “Nonelectrolyte” says.

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

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.