The Ultimate Guide to Lakhmir Singh Chemistry Class 10 Pdf Free 1525l
Lakhmir Singh Chemistry Class 10 Pdf Free 1525l: A Comprehensive Guide for CBSE Students
Introduction
Chemistry is one of the most fascinating and practical subjects that students learn in class 10. It helps them to understand the nature and behavior of matter, its composition, properties, transformations and interactions. Chemistry also connects with many aspects of our daily life, such as food, health, environment, industry, agriculture and technology.
Lakhmir Singh Chemistry Class 10 Pdf Free 1525l
However, chemistry can also be challenging and complex for some students who find it difficult to grasp the concepts and apply them to solve problems. That's why they need a good reference book that can help them to master the subject and score well in their board exams.
One such book is Lakhmir Singh Chemistry Class 10 Pdf Free 1525l, which is a revised edition of the popular textbook by Lakhmir Singh and Manjit Kaur. This book is based on the NCERT syllabus prescribed by the Central Board of Secondary Education (CBSE) for class 10 science. It covers all the topics of chemistry in a simple, concise and comprehensive manner. It also provides ample examples, diagrams, tables, exercises, value-based questions and solutions to help students learn effectively.
If you are looking for a reliable and easy-to-use chemistry book for class 10, then Lakhmir Singh Chemistry Class 10 Pdf Free 1525l is a great choice. You can download it for free from various online sources or buy a hard copy from any bookstore. In this article, we will give you a chapter-wise summary of this book, along with its benefits and FAQs.
Chapter-wise Summary of Lakhmir Singh Chemistry Class 10 Pdf Free 1525l
Lakhmir Singh Chemistry Class 10 Pdf Free 1525l consists of five chapters that cover all the important topics of chemistry for class 10. Here is a brief overview of each chapter:
Chapter 1: Chemical Reactions and Equations
This chapter deals with chemical reactions and equations, as mentioned in the title. The chapter starts with an example of a chemical reaction happening when magnesium ribbon is cleaned when rubbing it with sandpaper before burning it in the air. Then, it talks about the characteristics of chemical reactions and how to balance the equations. Chemical reactions that are applicable and their examples in our day-to-day life are also covered in this chapter.
Key concepts
Chemical reaction: A process in which one or more substances (reactants) are converted into one or more new substances (products).
Chemical equation: A symbolic representation of a chemical reaction, showing the reactants and products along with their physical states and coefficients.
Types of chemical reactions: Combination, decomposition, displacement, double displacement, oxidation, reduction, redox, exothermic, endothermic, etc.
Effects of chemical reactions: Change in state, color, temperature, gas evolution, precipitate formation, etc.
Law of conservation of mass: Mass can neither be created nor destroyed in a chemical reaction.
Law of constant proportions: In a chemical compound, the elements are always present in a fixed ratio by mass.
Balancing of chemical equations: The process of making the number of atoms of each element equal on both sides of a chemical equation by using suitable coefficients.
Important questions and answers
What is the difference between a physical change and a chemical change?
A physical change is a change in which no new substance is formed and the original properties of the substance are retained. A chemical change is a change in which one or more new substances are formed and the original properties of the substance are changed.
Write a balanced chemical equation for the following reaction: Hydrogen gas reacts with oxygen gas to form water.
2H2(g) + O2(g) 2H2O(l)
Identify the type of reaction in the following equation: Zn + CuSO4 ZnSO4 + Cu
This is a displacement reaction, in which zinc displaces copper from copper sulphate solution and forms zinc sulphate and copper metal.
What is meant by oxidation and reduction?
Oxidation is a process in which a substance loses electrons or gains oxygen or loses hydrogen. Reduction is a process in which a substance gains electrons or loses oxygen or gains hydrogen.
Give an example of an exothermic and an endothermic reaction.
An exothermic reaction is a reaction in which heat is released to the surroundings. For example, combustion of fuels. An endothermic reaction is a reaction in which heat is absorbed from the surroundings. For example, decomposition of calcium carbonate by heating.
Chapter 2: Acids, Bases and Salts
This chapter deals with the acids, bases and salts and their definitions in terms of furnishing H+ and OH- ions. The chapter starts with an introduction of indicators for acids and bases. It also includes their general properties, examples, and uses. The concept of pH scales and their importance in everyday life are also covered in the chapter. Then, it clearly explains the preparation and uses of sodium hydroxide, washing soda, baking soda, bleaching powder and plaster of Paris.
Key concepts
Acid: A substance that furnishes hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water.
Base: A substance that furnishes hydroxide ions (OH-) when dissolved in water.
Salt: A substance that is formed by the neutralization of an acid and a base.
pH: A measure of the acidity or alkalinity of a solution on a scale of 0 to 14. pH = -log[H+].
pH indicators: Substances that change their color depending on the pH of the solution. For example, litmus, phenolphthalein, methyl orange, etc.
Sodium hydroxide (NaOH): A strong base that is prepared by the electrolysis of brine (aqueous sodium chloride) solution. It is used for making soap, paper, rayon, etc.
Sodium carbonate (Na2CO3): Commonly known as washing soda. It is prepared by heating baking soda. It is used for washing clothes, softening hard water, making glass, etc.
Sodium hydrogen carbonate (NaH 71b2f0854b