NCERT Solutions for Class 10 Science Chapter 2 - Acids, Bases And Salts

Intext exercise 1

1. You Have Been Provided With Three Test Tubes. One of Them Contains Distilled Water and the Other Two Contain an Acidic Solution and a Basic Solution, Respectively. If You Are Given Only Red Litmus Paper, How Will You Identify the Contents of Each  Test Tube? 

Ans: Red litmus paper is an indicator for bases and can turn blue in the presence of a base. 

Let us mark the given three test tubes as A, B, and C. Put the given red litmus paper in each solution. If the colour of red litmus paper changes to blue (suppose in test tube A), then it is a base and if there is no colour change, then it is either acidic or neutral. 

Now, a drop of the solution from test tube A is put on the red litmus paper. Same process is repeated with solution B and C. If either of them changes colour to blue, then it is basic (let’s suppose B) Therefore, out of three, one is eliminated as a base.

Out of the remaining two (A and C), any solution can be acidic or neutral. To test them for acidic or neutral, a drop of basic solution is mixed with a drop of each of the remaining two solutions separately and then the nature of the drops of the mixtures is checked. If the colour of red litmus turns blue, then the second solution is neutral (C) and if there is no change in colour, then the second solution is acidic (A). This is because acidic and basic solutions neutralise each other. In this way the contents of each test tube can be identified. 

Intext Exercise 2 

1. Why Should Curd and Sour Substances Not Be Kept in Brass and Copper Vessels?

Ans: Curd contains lactic acid and other sour substances also contain some acids. So, when they are kept in brass and copper vessels, the acid present in curd and sour substances react with the metal to liberate hydrogen gas and harmful products which spoil the food. 

2. Which Gas is Usually Liberated When an Acid Reacts With a Metal? Illustrate With an Example. How Will You Test for the Presence of This Gas?

Ans: Hydrogen gas is liberated when an acid reacts with a metal. 

For example:

-Take some pieces of zinc granules in a test tube and add ${{H}_{2}}S{{O}_{4}}$ to it. 

-Shake it and pass the gas produced into a soap solution. 

-Bubbles are formed in the soap solution. 

-These soap bubbles contain hydrogen gas. 

-The chemical equation of the reaction is: 

${{H}_{2}}S{{O}_{4}}+Zn\to ZnS{{O}_{4}}+{{H}_{2}}\uparrow $ 

Identification test: 

Hydrogen gas is identified by bringing a burning candle near the soap bubbles. The candle will burn with a pop sound. 

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3. Metal Compound a Reacts With Dilute Hydrochloric Acid To Produce Effervescence. The Gas Evolved Extinguishes a Burning Candle. Write a Balanced Chemical Equation for the Reaction if One of the Compounds Formed is Calcium Chloride.

Ans: Calcium carbonate is a metal compound that reacts with dilute hydrochloric acid to produce calcium chloride, carbon dioxide and water. Carbon dioxide produced has the ability to extinguish a burning candle as it will remove the oxygen supply. The balanced chemical equation for the reaction is:

\[\underset{calcium\,carbonate}{\mathop{CaC{{O}_{3(s)}}}}\,+\underset{hydrochloric\,acid}{\mathop{2HC{{l}_{(aq)}}}}\,\to \underset{calcium\,chloride}{\mathop{CaC{{l}_{2(aq)}}}}\,+\underset{carbon\,dioxide}{\mathop{C{{O}_{2(g)}}}}\,+\underset{water}{\mathop{{{H}_{2}}{{O}_{(l)}}}}\,\]

Intext Exercise 3

1. Why do $\text{HCl,}\,\text{HN}{{\text{O}}_{\text{3}}}\text{,}$ etc., Show Acidic Characters in Aqueous Solutions While Solutions of Compounds Like Alcohol and Glucose Do Not Show Acidic Character?

Ans: The acidic character of any compound is due to the presence of the hydronium ions $\left( {{H}_{3}}{{O}^{+}} \right)$ or hydrogen ions $\left( {{H}^{+}} \right)$ in any solution.  In an aqueous solution $HCl$ and $HN{{O}_{3}}$ gets dissociated and forms hydrogen ions. The hydrogen ions combine with ${{H}_{2}}O$ to form hydronium ions. The reaction is as follows: 

\[HC{{l}_{(aq)}}\to {{H}^{+}}+C{{l}^{-}}\] 

\[{{H}^{+}}+{{H}_{2}}O\to {{H}_{3}}{{O}^{+}}\] 

Due to the presence of hydronium ions $HCl,\,HN{{O}_{3}},$ etc., show acidic characters. However, the aqueous solutions of glucose and alcohol contain hydrogen, but it cannot dissociate in water to form hydrogen ions. Therefore, they do not show acidic character. 

2. Why Does an Aqueous Solution of an Acid Conduct Electricity?

Ans:  Acids have the tendency to dissociate into hydronium ions $\left( {{H}_{3}}{{O}^{+}} \right)$ or hydrogen ions $\left( {{H}^{+}} \right)$ in an aqueous solution. Due to the movement of these ions , the solution can conduct electricity. Hence, an aqueous solution of an acid can conduct electricity. 

3. Why Does Dry HCl Gas Not Change the Colour of the Dry Litmus Paper?

Ans: The acidic nature is due to the presence of hydronium $\left( {{H}_{3}}{{O}^{+}} \right)$ or hydrogen $\left( {{H}^{+}} \right)$ ions in aqueous solution.  Dry HCl gas does not contain hydronium or hydrogen ions as only in aqueous solution an acid can dissociate to give ions. The colour of the litmus paper is changed by the hydrogen ions. So, in this case there will be no colour change due to dryness of the HCl gas and the litmus paper. 

4. While Diluting an Acid, Why is It Recommended That the Acid Should Be Added to Water and Not Water to the Acid?

Ans:  It is always recommended that acid should be added to water in order to dilute the acid; because the process of dissolving an acid in water is exothermic that releases heat. If water is added to the acid, then a large amount of heat is generated due to which the mixture spills out and causes burns and injuries that may cause accidents. 

5. How is the Concentration of Hydronium ions $\left( {{\text{H}}_{\text{3}}}{{\text{O}}^{\text{+}}} \right)$ Affected When a solution of an acid is Diluted? 

Ans: When a solution of an acid is diluted, then water is added to that solution. Dilution results in the concentration of hydronium ions $\left( {{H}_{3}}{{O}^{+}} \right)$ per unit volume to get decreased and thus the strength of the acid also decreases.

6. How is the Concentration of Hydroxide ions $\left( \text{O}{{\text{H}}^{\text{-}}} \right)$  Affected When Excess Base is Dissolved in a Solution of Sodium Hydroxide? 

Ans: When an excess of a base is dissolved in a solution, the solution becomes concentrated. This would result in the increase in the concentration of hydroxide ions $\left( O{{H}^{-}} \right)$ per unit volume and the strength of the base will increase.

Intext Exercise 4 

1. You Have Two Solutions, A and B. the pH of Solution A is 6 and pH of Solution B is 8. Which Solution Has More Hydrogen Ion Concentration? Which of These is Acidic and Which One is Basic?

Ans: The pH less than 7 (pH < 7 ) indicates an acidic solution, while pH greater than 7 (pH > 7) indicates a basic solution. Therefore, the solution with pH = 6 will be acidic and it has more hydrogen ion $\left( {{H}^{+}} \right)$ concentration than the solution of pH = 8 that will be a basic solution. The solution of pH = 8 has more hydroxide ion $\left( O{{H}^{-}} \right)$ concentration. 

2. What Effect Does the Concentration of $\left( {{\text{H}}^{\text{+}}}_{\text{(aq)}} \right)$ Ions Have on the Nature of the Solution? 

Ans: When the hydrogen ion$\left( {{H}^{+}} \right)$concentration increases, the solution becomes more acidic. While a decrease of hydrogen ion in the solution makes the solution less acidic and increases the basicity of the solution. 

3. Do Basic Solutions Also Have $\left( {{\text{H}}^{\text{+}}}_{\text{(aq)}} \right)$ ions? If yes, Then Why are These Basic? 

Ans: Yes, the basic solution also contains $\left( {{H}^{+}}_{(aq)} \right)$ ions. However, their concentration is less as compared to the concentration of hydroxide $\left( O{{H}^{-}} \right)$ ions that makes the solution basic. 

4. Under What Soil Condition Do You Think a Farmer Would Treat the Soil of His Fields With Quick Lime (Calcium Oxide) or Slaked Lime (Calcium Hydroxide) or Chalk (Calcium Carbonate)?

Ans: Quick lime (calcium oxide) or slaked lime (calcium hydroxide) or chalk (calcium carbonate) is considered a good base. If the soil is acidic which is improper for cultivation, then to increase the basicity of soil, the farmer would treat the soil with these compounds.

Intext Exercise 5

1. What is the common name of the compound $\text{CaOC}{{\text{l}}_{\text{2}}}$ ? 

Ans: The common name of the given compound $CaOC{{l}_{2}}$ is bleaching powder. 

2. Name the Substance Which on Treatment With Chlorine Yields Bleaching Powder?

Ans: The compound called calcium hydroxide $Ca{{(OH)}_{2}}$ on treatment with chlorine, yields bleaching powder. 

3. Name the Sodium Compound Which is Used for Softening Hard Water.

Ans: Washing soda $\left( N{{a}_{2}}C{{O}_{3}}.10{{H}_{2}}O \right)$ is the sodium compound that is used for softening hard water. 

4. What Will Happen if a Solution of Sodium Hydrocarbonate Is Heated? Give the Equation of the Reaction Involved.

Ans: When a solution of sodium hydrocarbonate or sodium hydrogen carbonate is heated then sodium carbonate and water are formed with the evolution of carbon dioxide gas. 

The Equation is as follows:

\[\underset{sodium\,hydrogen\,carbonate}{\mathop{2NaHC{{O}_{3}}}}\,\xrightarrow{\Delta }\underset{sodium\,carbonate}{\mathop{N{{a}_{2}}C{{O}_{3}}}}\,+\underset{water}{\mathop{{{H}_{2}}O}}\,+\underset{carbon\,dioxide}{\mathop{C{{O}_{2}}\uparrow }}\,\] 

5. Write an Equation To Show the Reaction Between Plaster of Paris and Water.

Ans: The chemical equation can be represented as:

\[\underset{plaster\,of\,paris}{\mathop{CaS{{O}_{4}}.\frac{1}{2}{{H}_{2}}O}}\,+\underset{water}{\mathop{1\frac{1}{2}{{H}_{2}}O}}\,\to \underset{gypsum}{\mathop{CaS{{O}_{4}}.2{{H}_{2}}O}}\,\] 

NCERT Exercises

1. A Solution Turns Red Litmus Blue, Its pH Is Likely To Be

a) 1 

b) 4 

c) 5 

d) 10 

Ans: (d). Bases turn red litmus blue. Basic solution has a pH > 7. Since, the solution turns red litmus blue, its pH would likely be 10. 

2. A Solution Reacts With Crushed Egg-Shells To Give a Gas That Turns Lime-Water Milky. The Solution Contains

a) NaCl 

b) HCl

c) LiCl 

d) KCl 

Ans: (b). The solution contains HCl (acid) which reacts with crushed egg-shells to give a gas (carbon dioxide) that turns lime-water milky. Egg shells contain calcium carbonate (base). 

\[\underset{calcium\,carbonate}{\mathop{CaC{{O}_{3(s)}}}}\,+\underset{hydrochloric\,acid}{\mathop{2HC{{l}_{(aq)}}}}\,\to \underset{calcium\,chloride}{\mathop{CaC{{l}_{2(aq)}}}}\,+\underset{carbon\,dioxide}{\mathop{C{{O}_{2(g)}}}}\,+\underset{water}{\mathop{{{H}_{2}}{{O}_{(l)}}}}\,\] 

3. 10 mL of a Solution of NaOH Is Found To Be Completely Neutralised by 8 mL of a Given Solution of HCl. If We Take 20 mL of the Same Solution of NaOH, the Amount of HCl Solution (the Same Solution As Before) Required To Neutralise It Will Be

a) 4 mL 

b) 8mL 

c) 12 mL 

d) 16 mL 

Ans: (d) 16 mL

10 mL of a solution of NaOH neutralises 8 mL of a solution of HCl. Thus, 20 mL of a solution of NaOH neutralises,$\frac{10}{8}\times \frac{20}{?}$ mL =16 mL of HCl solution.

4. Which one of the following types of medicines is used for treating indigestion? 

a) Antibiotic 

b) Analgesic 

c) Antacid 

d) Antiseptic 

Ans:  (c) Antacid is commonly used for treating indigestion.

5. Write Word Equations and Then Balanced Equations for the Reaction Taking Place When −

a) Dilute Sulphuric Acid Reacts with Zinc Granules. 

b) Dilute Hydrochloric Acid Reacts with Magnesium Ribbon.

Ans: Word equation: Hydrochloric acid + Magnesium → Magnesium chloride + Hydrogen 

c) Dilute Sulphuric Acid Reacts with Aluminium Powder. 

Ans: Word equation: Sulphuric acid + Aluminium → Aluminium sulphate + Hydrogen 

d) Dilute Hydrochloric Acid Reacts with iron Filings.

Ans:  Word equation: Hydrochloric acid + Iron → Ferric chloride + Hydrogen 

6. Compounds Such As Alcohols and Glucose Also Contain Hydrogen but Are Not Categorized As Acids. Describe an Activity To Prove It.

Ans: 

Activity: 

a. Two nails are fitted on a cork kept in a 100 mL beaker. 

b. The nails are then connected to the terminals of a 6-volt battery through a bulb and a switch. 

c. Some dilute HCl is poured in the beaker and the current is switched on. 

d. The same experiment is then performed with glucose solution and alcohol  solution. 

Observations: 

The bulb glows in the HCl solution and does not glow in the glucose or alcohol solution. 

Result: 

In aqueous solution, HCl dissociates into ${{H}^{+}}$ and $C{{l}^{-}}$ ions. These ions conduct electricity in the solution resulting in the glowing of the bulb. On the other hand, the glucose or alcohol solution does not dissociate into ions. Therefore, the bulb does not glow. 

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Conclusion: 

All acids contain hydrogen but not all compounds containing hydrogen are acids. 

So, alcohols and glucose contain hydrogen, but they are not categorised as acids. 

7. Why Does Distilled Water Not Conduct Electricity, Whereas Rain Water Does?

Ans: Distilled water is a pure form of water which is free from ionic species. Therefore, it does not conduct electricity. Rain water is an impure form of water that contains many ionic species like acids and thus, it conducts electricity.

8. Why Do Acids not Show Acidic behaviour in the Absence of Water? 

Ans: Acids can only dissociate in aqueous solution to liberate hydrogen ions which are responsible for the acidic behaviour. Acids do not show acidic behaviour in the absence of water because the dissociation of hydrogen ions from an acid occurs in the presence of water only.

9. Five solutions A, B, C, D and E when tested with universal indicators showed pH as 4, 1,11, 7 and 9, respectively. Which solution is 

a) Neutral 

Ans: Solution D with pH=7 

b) Strongly Alkaline

Ans: Solution C with pH=11

c) Strongly Acidic

Ans: Solution B with pH=1

d) Weakly Acidic

Ans: Solution A with pH=4

e) Weakly Alkaline

Ans: Solution E with pH=9 

f) Arrange the pH in Increasing Order of Hydrogen-ion Concentration. 

Ans: The pH can be arranged in the increasing order of the concentration of hydrogen ions as: 

\[11<9<7<4<1\] 

10. Equal Lengths of Magnesium Ribbons are Taken in Test Tubes A and B. Hydrochloric acid (HCl) is Added to Test tube A, While Acetic Acid $\text{(C}{{\text{H}}_{\text{3}}}\text{COOH)}$  is Added to Test Tube B. In Which Test Tube will the Fizzing Occur More vigorously and why? 

Ans: The fizzing occurs strongly in test tube A, in which hydrochloric acid (HCl) is added. This is because HCl is a stronger acid than acetic acid $(C{{H}_{3}}COOH)$and generates more hydrogen $({{H}^{+}})$ ions. Therefore, HCl produces hydrogen gas at a faster rate due to which fizzing occurs. 

11. Fresh Milk Has a pH of 6. How Do You Think the pH Will Change As It Turns Into Curd? Explain Your Answer.

Ans: The pH of fresh milk is 6. As it changes into curd, the pH will decrease because curd contains lactic acid which reduces the pH. 

12. A Milkman Adds a Very Small Amount of Baking Soda to Fresh Milk.

a) Why does he shift the pH of the fresh milk from 6 to slightly alkaline? 

Ans: In alkaline condition, milk does not set as curd easily due to the formation of lactic acid as in the acidic condition.

b) Why Does This Milk Take a Long Time To Set As Curd?

Ans: Since, this milk is slightly basic than normal milk, acids produced to set the curd are neutralised by the base added to the milk. Thus, it takes a longer time for the curd to set. 

13. Plaster of Paris Should Be Stored in a Moisture-Proof Container. Explain Why?

Ans: Plaster of Paris (POP) should be stored in a moisture-proof container because it is a powdery mass that can absorb water or moisture to form a hard solid mass known as gypsum. The reaction takes place as follows:

\[\underset{plaster\,of\,paris}{\mathop{CaS{{O}_{4}}.\frac{1}{2}{{H}_{2}}O}}\,+\underset{water}{\mathop{1\frac{1}{2}{{H}_{2}}O}}\,\to \underset{gypsum(hard\,solid)}{\mathop{CaS{{O}_{4}}.2{{H}_{2}}O}}\,\]

14. What is a Neutralisation Reaction? Give Two Examples.

Ans: Neutralisation reaction: A reaction in which an acid and base react with each other to form a salt and water is known as a neutralization reaction. For example: 1.$\underset{base}{\mathop{NaOH}}\,+\underset{acid}{\mathop{HCl}}\,\to \underset{salt}{\mathop{NaCl}}\,+\underset{water}{\mathop{{{H}_{2}}O}}\,$ 

2. During indigestion (caused due to the production of excess acid in the stomach), we take an antacid (milk of magnesia, $Mg{{(OH)}_{2}}$ which is basic in nature). The antacid neutralises the excess of acids and thus gives relief from indigestion. 

\[Mg{{(OH)}_{2}}+2HCl\to MgC{{l}_{2}}+2{{H}_{2}}O\] 

15. Give Two Important Uses of Washing Soda and Baking Soda.

Ans:  Uses of Washing Soda are: 

a) It is used to remove permanent hardness of water. 

b) It is used in glass, soap, and paper industries. 

Uses of Baking Soda are: 

a) It is used as baking powder. Baking powder is a mixture of baking soda and tartaric acid. Baking powder makes bread or cake fluffy. 

b) It is used in soda-acid fire extinguishers.

MCQs for NCERT Solutions for Class 10 Science Chapter 2

MCQs based on the chapter Acids, Bases and Salts for Class 10 are given below:

1. Equal pieces of zinc granules are dropped in four test tubes. Following substances are poured into all four test tubes. The reaction will be vigorous with:

1. CH3COOH

2. HCl

3. Lemon juice

4. Sodium bicarbonate solution

Answer: (B)

Zinc (Zn) is an active metal which reacts vigorously with strong acids like HCl. So, the correct answer is (B).

2. A drop of a liquid sample was put on the pH paper. It was observed that the colour of the pH paper turns blue. The liquid sample is:

1. Distilled water

2. Lemon juice

3. Sodium bicarbonate solution

4. Hydrochloric acid

Answer: (C)

Basic solutions turn litmus paper blue. From the above-given options, sodium bicarbonate i.e., NaHCo3 is a basic solution. So, the correct option is (C).

3. A student was asked to collect apparatus from the lab store, for doing an experiment on the pH of the given sample. Identify the article that he is not supposed to pick. 

1. pH paper

2. Petri dish

3. Litmus paper

4. Dropper

Answer: (B)

In the above-given options, all are used for doing an experiment on the pH, except Petri Dish.

4. A solution has a pH value of 5. On adding 10 mL of NaCl to it, what will be the pH of the new solution?

1. Only seven

2. More than 5

3. Less than 5

4. No change in pH

5. Can not be determined

Answer: (D)

NaCl has a pH value of 7 as it is a neutral solution. Therefore adding any amount of NaCl to the solution with a pH value of 5 will not affect its pH value. So, the correct option is (D).

5. A salt is dissolved in water. The pH of this salt solution was found to be 7 by measuring the pH with a universal indicator paper. The salt is most likely to be:

1. KCl

2. CH3COONa

3. NH4Cl

4. Na2CO3

Answer: (A)

In the above options, KCl would be that salt as it is completely ionisable:

KCl→K+ + Cl-

Mind Map of Acid, Bases and Salts Class 10 NCERT Science Chapter 2

Here, we have listed some important points and chemical equations that you must remember.

Types of Salts

What are the Different Types of Indicators and How Do They React in Different Mediums?

List of Common Salts, their Formation and Uses

NCERT Solutions for Class 10 Science Chapter 2 - Acids, Bases and Salts

NCERT Solutions for Class 10 Science

• Chapter 1 - Chemical Reactions and Equations

• Chapter 2 -  Acids, Bases and Salts

• Chapter 3 - Metals and Non-metals

• Chapter 4 - Carbon and Its Compounds

• Chapter 5 - Periodic Classification of Elements

• Chapter 6 - Life Processes

• Chapter 7 - Control and Coordination

• Chapter 8 - How do Organisms Reproduce?

• Chapter 9 - Heredity and Evolution

• Chapter 10 - Light Reflection and Refraction

• Chapter 11 - Human Eye and Colourful World

• Chapter 12 - Electricity

• Chapter 13 - Magnetic Effects of Electric Current

• Chapter 14 - Sources of Energy

• Chapter 15 - Our Environment

• Chapter 16 - Management of Natural Resources

NCERT Solutions for Class 10 Science Chapter 10 Acid Bases and Salts - Free PDF Download

Having legitimate information on the hypotheses, the adequate practice of the reactions, conditions, and equations, and question-solving ability from the NCERT Chemistry books are very significant for prospects and increase the possibility of bagging a good score. The Ch 2 Science Class 10 NCERT solutions provide step by step explanation to the questions provided in the NCERT. This helps students to gain a better understanding of the chapter's concepts through these easy and comprehensive solutions. The Class 10 Science Chapter 2 PDF contains solutions to every question in Class 10 Science Chapter 2.

NCERT Solutions for Science Class 10 - Acids Bases and Salts

Class 10th science chapter 2 is part of unit 1, Chemical Substances - Nature and Behaviours. This chapter portrays acid and base reactions and depicts how acid and base generally cancel out each other.

Acid, base and salt class 10 includes topics such as How do Acids and Bases react with each other or metals, Reaction of acid with Hydrogen carbonates and Metallic oxides, Reaction of bases with oxides, etc. to make students understand the basic concepts. In addition to this, the Class 10th Science Chapter 2 includes various interactive activities and interesting topics such as similarities between acid and base and acid or base in a water solution to make the learning process straightforward and easy to understand.

This chapter will also help students learn about salts, their nature, pH, the chemicals that are derived from salt, and the nature and characteristics of salt crystals.

All the aforementioned information is thoroughly explained through step by step process in the Ch 2 Science Class 10 Solutions that are designed by India's expert Science teachers to help you in understanding the meaning of basic concepts of acids, bases, and salts class 10 towards performing well in examinations as well as their relation to interesting things that we observe in our daily life.

Class 10 Science Chapter 2 Weightage Marks

The Acid, base and salt class 10 is one of the most important chapters as it provides you maximum chances to score high marks in your exams. The unit consisting of the chapter comes for a weightage of 33 marks and the chapter itself for 5 marks in the examination. Through the Class 10 Science Chapter 2 solutions, you will be able to solve questions based on this chapter easily and strengthen the basic concepts of the subject chemistry.

Following are the main headings that are covered under Chapter 2 Science Class 10 acids bases and salts:

• Understanding the properties of bases and acids.

• How do acids and bases respond with metals? 

• How metal carbonates and metal hydrogen carbonates respond with acids?

• How do acids and bases respond with one another?

• The response of metallic oxides with acids.

• The response of non – metallic oxide with base.

• What do all acids and bases share for all intents and purposes?

• Significance of pH in regular day to day existence.

• More about Salts.

• Group of salts.

• pH of salts.

• Synthetic substances from regular salt.

Benefits of Acids Bases and Salts Class 10 NCERT Solutions

NCERT solutions for class 10 science chapter 2 acids bases and salts help students to have a decent comprehension of the concepts of this chapter. This chapter is appropriately explained by class 10 science ch 2 NCERT solutions. The fundamental advantages of these solutions are:

• The solutions are not at all muddled and clarify bit by bit completely to assist you with having a solid comprehension of the important concepts of this chapter.

• Acid bases and salts class 10 solutions are given by teachers who are pros in this field and have an astounding experience. The arrangements made by them are precise and will help you in ensuring that you secure great marks in the tests.

• These solutions are planned and made remembering one of the principal targets towards helping you in acquiring excellent grades.

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