Grade 10
  1. Matter and its properties  1.1. States of matter  1.2. Physical and chemical properties of matter  1.3. Classification of substances (elements, compounds, mixtures)  1.4. Changes in Matter (Physical and Chemical Changes)  1.5. Law of conservation of mass and law of definite proportions
  2. Atomic Structure  2.1. Historical development of the atomic model  2.2. Subatomic particles (protons, neutrons, electrons)  2.3. Atomic number, mass number and isotopes  2.4. Electronic Configuration and Energy Levels  2.5. Valency, ion formation and oxidation state
  3. Periodic table  3.1. History and Development of the Periodic Table  3.2. Modern Periodic Law and Periodic Trends  3.3. Groups and Periods in the Periodic Table  3.4. Trends in the Periodic Table  3.5. Metals, non-metals, metalloids and their properties  3.6. Noble gases and their chemical inertness
  4. Chemical bond  4.1. Formation of Chemical Bonds (Octet Rule)  4.2. Ionic Bonding and Properties of Ionic Compounds  4.3. Covalent Bond and Properties of Covalent Compounds  4.4. Metallic bond and its properties  4.5. Molecular geometry and VSEPR theory  4.6. Polarity and dipole moment of molecules  4.7. Intermolecular forces
  5. Chemical Reactions and Equations  5.1. Types of Chemical Reactions  5.2. Writing and balancing chemical equations  5.3. Law of conservation of mass in chemical reactions  5.4. Factors Affecting Chemical Reactions  5.5. Catalysts and their role in chemical reactions  5.6. Exothermic and Endothermic Reactions
  6. Stoichiometry and Chemical Calculations  6.1. Mole concept and Avogadro number  6.2. Molar Mass and Gram-Mole Conversions  6.3. Empirical and molecular formula  6.4. Stoichiometric calculations and chemical yield  6.5. Limiting and Excess Reactants
  7. Acids, Bases and Salts  7.1. Properties and Definitions of Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)  7.2. pH Scale, pOH, and Indicators  7.3. Neutralization reactions and salt formation  7.4. Strength of Acids and Bases (Strong vs. Weak Acids and Bases)  7.5. Common Acids and Bases in Daily Life  7.6. Salts, their solubility and applications
  8. Metals and Nonmetals  8.1. Physical and chemical properties of metals  8.2. Physical and Chemical Properties of Non-Metals  8.3. Reactivity Series of Metals and Displacement Reactions  8.4. Extraction of metals from ores  8.5. Corrosion, its causes and prevention  8.6. Alloys, their composition and uses
  9. Carbon and its compounds  9.1. Allotropes of Carbon  9.2. Hydrocarbons and their classification (alkanes, alkenes, alkynes)  9.3. Functional groups in organic compounds  9.4. Nomenclature of organic compounds (IUPAC system)  9.5. Isomerism in organic chemistry (structural and geometrical)  9.6. Important organic reactions (combustion, addition, substitution, polymerization)  9.7. Applications of organic compounds in industry and daily life
  10. Environmental Chemistry  10.1. Air Pollution (Sources, Effects and Control)  10.2. Water Pollution (Causes, Effects and Remedies)  10.3. Greenhouse effect and global warming  10.4. Ozone layer depletion and its effects  10.5. Green Chemistry and Its Applications  10.6. sustainable chemistry practice
  11. Thermochemistry  11.1. Heat and Energy Changes in Chemical Reactions  11.2. Exothermic and Endothermic Reactions  11.3. Enthalpy, enthalpy change, and heat of reaction  11.4. Specific heat capacity and calorimetry  11.5. Energy Changes in Combustion Reactions
  12. Electrochemistry  12.1. Electrolytes and non-electrolytes  12.2. Electrolysis and its applications (electroplating, extraction of metals)  12.3. Redox reactions (oxidation and reduction)  12.4. Galvanic cell and electrochemical series  12.5. Corrosion and electrochemical prevention methods
  13. Chemical kinetics and equilibrium  13.1. Rate of chemical reactions and its measurement  13.2. Factors affecting the reaction rate (catalyst, temperature, concentration)  13.3. Reversible and irreversible reactions  13.4. Dynamic equilibrium and equilibrium constant  13.5. Le Chatelier's principle and its applications
  14. Gases and Gas Laws  14.1. Properties of gases and kinetic molecular theory  14.2. Boyle's Law (Pressure-Volume Relation)  14.3. Charles's Law  14.4. Gay-Lussac's Law  14.5. Combined Gas Law and Ideal Gas Law  14.6. Real Gases vs Ideal Gases
  15. Nuclear Chemistry  15.1. Introduction to Radioactivity and Nuclear Reactions  15.2. Types of radioactive decay (alpha, beta, gamma)  15.3. Half-life and applications of radioactive isotopes  15.4. Nuclear fission and fusion reactions  15.5. Nuclear power generation and its environmental impact

Grade 10 → Electrochemistry ↓


Electrolytes and non-electrolytes


Chemistry is a fascinating subject that helps us understand the structure and behavior of the substances around us. One area of chemistry is electrochemistry, which involves the study of chemical processes that involve the movement of electrons. In this field, it is important to understand electrolytes and non-electrolytes. By the end of this explanation, you will have a better understanding of what these substances are, their roles in chemistry, and their importance in everyday life.

What are electrolytes?

Electrolytes are substances that dissociate into ions when dissolved in water and are able to conduct electricity. This property is important for many biological and chemical systems. When electrolytes are mixed with water, they break down into positive and negative ions. This division allows the solution to carry an electrical current, as the ions can move freely in the liquid, facilitating the flow of electricity.

NaCl (s) → Na⁺ (aq) + Cl⁻ (aq)

In the example above, table salt (common sodium chloride) is an electrolyte. When it dissolves in water, it dissociates into Na⁺ (sodium) and Cl⁻ (chloride) ions.

Types of electrolytes

There are generally two types of electrolytes depending on the degree of dissociation in water:

Strong electrolytes

Strong electrolytes completely dissociate into ions in water. These solutions conduct electricity very well because there are many ions present to carry the current. Examples include:

  •  HCl
    (hydrochloric acid): 
     HCl → H⁺ + Cl⁻
  •  NaOH
    (sodium hydroxide): 
     NaOH → Na⁺ + OH⁻
  •  NaCl
    (sodium chloride): 
     NaCl → Na⁺ + Cl⁻

Weak electrolytes

Weak electrolytes only partially dissociate into ions in water, which means fewer ions are available to conduct electricity. This results in a weaker electrical current. Examples include:

  •  CH₃COOH
    (acetic acid): 
     CH₃COOH ⇌ CH₃COO⁻ + H⁺
  •  NH₄OH
    (ammonium hydroxide): 
     NH₄OH ⇌ NH₄⁺ + OH⁻

Visual example of electrolytes

Consider a beaker of water with a compound such as NaCl dissolved in it:

Na⁺ Cl⁻

Here, Na⁺ ions are shown in blue, and Cl⁻ ions are shown in green. Both ions are dispersed in solution, allowing them to conduct electricity when a voltage is applied.

Applications of electrolytes

There are many applications of electrolytes:

  • Biological systems: Electrolytes are important in biological systems. For example, in the human body, electrolytes such as sodium and potassium help regulate nerve and muscle function, hydrate the body, balance blood acidity and pressure, and regenerate damaged tissue.
  • Electrolysis: This is a process in which electricity is used to break down electrolytes into their components. It is used to extract metals such as aluminium and in processes such as electroplating.
  • Batteries: In batteries, electrolytes move ions between positive and negative electrodes, allowing electricity to flow.

What are non-electrolytes?

Non-electrolytes are substances that do not break down into ions when dissolved in water and therefore do not conduct electricity in solution. These molecules remain whole and no electric current can flow through the solution.

C₆H₁₂O₆ (s) → C₆H₁₂O₆ (aq)

In the above equation, glucose dissolves in water. However, it does not dissociate into ions, so it is a non-electrolyte.

Examples of non-electrolytes

  • Sugar (e.g., C₆H₁₂O₆) dissolves in water but does not break down into ions.
  • Urea (CO(NH₂)₂) also does not dissociate into ions in water.
  • Many organic compounds, such as alcohols (C₂H₅OH), are non-electrolytes.

Visual example of non-electrolytes

Consider a beaker of water with a compound such as sugar dissolved in it:

C₆H₁₂O₆

In this diagram, the red circle represents the glucose molecule in solution. Note that no new charges or ions are created; the molecule remains uncombined.

Identifying electrolytes and non-electrolytes

To identify whether a substance is an electrolyte or a non-electrolyte, observe its behavior in water:

  1. Conductivity test: If a solution conducts electricity, it means there are ions in it, which indicates an electrolyte.
  2. Solubility: If a compound dissolves, but the solution does not conduct electricity, it is a non-electrolyte.

Importance of electrolytes and non-electrolytes

Understanding electrolytes and non-electrolytes is important in fields ranging from biology to industrial processes. Here's why they're important:

  • Health and Medicine: Electrolyte imbalances can lead to serious health problems. In medicine, solutions such as saline that contain electrolytes are used intravenously to provide patients with the necessary ions.
  • Industrial processes: Electrolytes are integral in electroplating, electrorefining, and battery design. Understanding their properties allows for efficient and effective applications.
  • Research: Investigating the properties of these substances can lead to the development of new materials and technologies.

The role of electrolytes and non-electrolytes in everyday life

Electrolytes and non-electrolytes are frequently encountered in everyday life, often in ways we cannot directly perceive:

Sports drink

When we sweat, we lose electrolytes. Sports drinks contain electrolytes, such as sodium and potassium, which help replenish the body's balance, aiding in athletic performance and recovery.

Homemade products

Common products such as table salt, baking soda or vinegar contain electrolytes that aid in a variety of household tasks, from cleaning to cooking.

Energy storage

Batteries, whether in a car or a phone, rely on electrolytes. These substances are necessary to store and distribute energy efficiently.

Academic implications and future prospects

The study of electrolytes and non-electrolytes continues to influence academic research and industrial advancement. As we explore renewable energy solutions, better battery technology, and medical advancements, our understanding of these substances plays a vital role.

Recent advances have seen the creation of new electrolytes to increase the life and efficiency of batteries, making them safer and more powerful. Similarly, in biological research, understanding electrolytes can lead to advances in medical treatments and healthcare formulations, which can directly benefit society.

Conclusion

Electrolytes and non-electrolytes are not just scientific concepts – they are vital components of life processes, from the human body to industry. Understanding their properties, applications, and implications can provide profound insights into how we interact with the world and use its resources efficiently. Whether you are just studying chemistry or applying it to a variety of fields, the insights gained from electrolytes and non-electrolytes prove invaluable, enhancing both personal understanding and technological advancement.


Grade 10 → 12.1


U
username
0%
completed in Grade 10

← Prev (12)
Electrochemistry
Next (12.2) →
Electrolysis and its applications (electroplating, extraction of metals)

Comments 



Electrolytes and non-electrolytes

https://www.chemistryelite.com/g10/12.1?ceal=en