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Selina solutions for Class 10 Chemistry chapter 3 - Acids, Bases and Salts

Selina ICSE Concise Chemistry for Class 10

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Chapter 3: Acids, Bases and Salts

Chapter 3: Acids, Bases and Salts solutions [Page 0]

What do you understand by the terms, acid and base?

Explain the formation of hydronium ion.

Write the ionization of sulphuric acid showing the formation of hydronium ion.

Water is never added to acid in order to dilute it why?

Define the term ‘basicity’ of an acid.

Give the basicity of: nitric acid, sulphuric acid and phosphoric acid.

Give two examples of the following:

oxy-acid

Give two examples of the following:
hydracids

Give two examples of the following:
monobasic acid

Give two examples of the following:
dibasic acid

Give two examples of the following:
tribasic acid

Name the acidic anhydride of the following acids:
(i) sulphurous acid
(ii) nitric acid
(iii) phosphoric acid
(iv) carbonic acid

Name the acids present in vinegar, grapes and lemon.

Name the ion that turns red litmus blue.

Name the ion that turns blue litmus red.

What do you understand by the statement ‘acetic acid is a monobasic acid?

Give a balanced equation for reaction of nitrogen dioxide with water.

How many types of salts does dibasic acid produce when it reacts with caustic soda solution? Give equation(s)

Carbonic acid gives an acid salt but hydrochloric acid does not. Explain.

What do you understand by the strength of an acid? On which factor does the strength of an acid depend?

Dil. HCl acid is stronger than highly concentrated acetic acid. Explain.

How is an acid prepared from a Non-metal
Give an equation for it.

How is an acid prepared from a Salt?
Give an equation for it.

Name an acid used to flavor and preserve food.

Name an acid used in a drink.

Name an acid used to remove ink spots.

Name an acid used as an eyewash.

Give equation to show how the following is made from their corresponding anhydrides.

 sulphurous acid

Give equation to show how the following is made from their corresponding anhydrides.
phosphoric acid

Give equation to show how the following is made from their corresponding anhydrides.
carbonic acid

Give equation to show how the following is made from their corresponding anhydrides.
sulphuric acid

Chapter 3: Acids, Bases and Salts solutions [Page 0]

What do you understand by an alkali? Give two examples of:
(a) strong alkalis
(b) weak alkalis

What is the difference between an alkali and a base?

What is the difference between an alkali and a metal hydroxide?

Define in term of ionization an acid.

Define in term of ionization an alkali?

Name the ions furnished by bases in solution.

Name the ions furnished by  a weak alkali.

Name the ions furnished by an acid.

Give one example in the following case:
A basic oxide which is soluble in water.

Give one example in the following case:
A hydroxide which is highly soluble in water.

Give one example in the following case:
A basic oxide which is insoluble in water.

Give one example in the following case:
a hydroxide which is insoluble in water.

Give one example in the following case:
A weak mineral acid.

Give one example in the following case:
a base which is not an alkali.

Give one example in the following case:
An oxide which is a base.

Give one example in the following case:
A hydrogen containing compound which is not an acid.

Give one example in the following case:
A base which does not contain a metal ion.

You have been provided with three test tubes. One of them contains distilled water and the other two have 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?

HCl, HNO3, C2H5OH, C6H12O0 all contain H atoms but only HCI and HNO3 show acidic character. Why?

Dry HCI gas does not change the colour of dry litmis paper. Why?

Is PbO2 a base or not? Comment.

what effect does the concentration of [H3O+] ion have on solution?

Do basic solutions also have H+(aq)? Why are they basic?

How would you obtain a base from other base.

How would you obtain an alkali from a base.

How would you obtain salt from another salt?

Write balanced equation to satisfy the following statement:
Acid + Active metal ⟶ Salt + hydrogen

Write balanced equation to satisfy the following statement:
Acid + Base ⟶ Salt + water

Write balanced equation to satisfy the following statement:
Acid + carbonate Or bicarbonate ⟶ Salt + water + carbon dioxide

Write balanced equation to satisfy the following statement:
Acid + sulphite Or bisulphite ⟶ Salt + water + sulphur dioxide

Write balanced equation to satisfy the following statement:
Acid + sulphide ⟶ Salt + Hydrogen sulphide

The skin has and needs natural oils. Why is it advisable to wear gloves while working with strong allkalis?

Why are alkalis soapy to touch? What do you understand by PH value?

Complete the table:

Indicator Indicator Acidic Acidic

Litmus

Phenolphthalein

Purple

 

Colourless

   

Two solutions X and Y have Ph values of 4 and 10 respectively. Which one of these two will give a pink colour with phenolphthalein indicator?

You are supplied with five solutions: A, B, C, D and E with Ph values as follows: A= 1.8, B = 7, C= 8.5, D = 13, and E=5
Classify these solutions as neutral, slightly or strongly acidic and slightly or strongly alkaline.

Which solution would be most likely to liberate hydrogen with:
(a) magnesium powder,
(b) powdered zinc metal. Give a word equation for each reaction.

what are the acidic range and the alkaline range in the Ph scale?

State one advantage of using ‘Ph paper’ for measuring the Ph value of an unknown solution.

Distinguish between a common acid base indicator and a universal indicator.

Distinguish between acidity of bases and basicity of acids.

Distinguish between acid and alkali (other than indicators).

How does tooth enamel get damaged? What should be done to prevent it?

Chapter 3: Acids, Bases and Salts solutions [Page 0]

Define an acidic salt.

Define a normal salt.

Define a mixed salt.

Give two examples of a normal salt.

Give two examples of an acid salt.

Give two examples of a mixed salt.

What is a ‘salt’?

What kind of salt prepared by direct combination. Write an equation for the reaction that takes place in preparing the salt you have named.

Name a salt prepared by direct combination. Write an equation for the equation for the reaction that takes place in preparing the salt you have named.

Name the procedure used to prepare a sodium salt such as sodium sulphate.

How is the following salt prepared:
Calcium sulphate from calcium carbonate,

How is the following salt prepared:
Lead (II) oxide from lead.

How is the following salt prepared:
Lead carbonate from lead nitrate.

How is the following salt prepared:
Sodium nitrate from sodium hydroxide.

How is the following salt prepared:
Magnesium carbonate from magnesium chloride.

How is the following salt prepared:
Copper (II) sulphate from copper (II) oxide?

How is lead sulphate prepared in the aboratory?

Why lead sulphate cannot be prepared by the action of dilute H2SO4 on lead oxide?

Describe giving all practical details, how would you prepare:

Copper sulphate crystals from a mixture of charcoal and black copper oxide.

Describe giving all practical details, how would you prepare:

zinc sulphate crystals from zinc dust (powdered zinc and zinc oxide).

Describe giving all practical details, how would you prepare:

lead sulphate from metallic lead.

Describe giving all practical details, how would you prepare:

sodium hydrogen carbonate crystals.

The following is a list of methods for the preparation of salts.
A – direct combination of two elements
B – reaction of a dilute acid with a metal.
C – reaction of a dilute acid with an insoluble base.
D – titration of a dilute acid with a solution of soluble base.
E – reaction of two solutions of salts to form a precipitate.
Choose from the above list A to E, the best method of preparing the following salts by giving a suitable equation in each case:
1. Anhydrous ferric chloride,
2. Lead chloride,
3. Sodium sulphate.
4. Copper sulphate.

Name a chloride which is insoluble in cold water but dissolves in hot water.

Name a chloride which is insoluble.

Name two sulphates which are insoluble.

Name a basic salt.

Name an acidic salt.

Name a mixed salt.

Name a complex salt.

Name a double salt.

Name two salts whose solubility increases with temperature.

Name a salt whose solubility decreases with temperature.

Explain ‘salt hydrolysis’

name two salts which are acidic.

name two salts which are basic.

name two salts which are neutral, when dissolved in water.

What would you observe when blue litmus is introduced into a solution of ferric chloride?

What would you observe when red litmus paper is introduced into a solution of sodium sulphate?

What would you observe when red litmus paper is introduced in sodium carbonate solution?

Write the balanced equation for the preparation of the following salt in the laboratory:

A soluble sulphate by the action of an acid on an insoluble base.

Write the balanced equation for the preparation of the following salts in the laboratory:

An insoluble salt by the action of an acid on another salt.

 

Write the balanced equation for the preparation of the following salts in the laboratory:

An insoluble base by the action of a solube base on a soluble salt.

 

Write the balanced equation for the preparation of the following salts in the laboratory:

A soluble sulphate by the action of an acid on a metal.

 

Give the preparation of the salt shown in the left column by matching with the methods given in the right column. Write a balanced equation for each preparation.

Salt                                               Method of preparation
Zinc sulphate                              Precipitation
Ferrous sulphide                         Oxidation
Barium sulphate                          Displacement
Ferric sulphate                            Neutralisation
Sodium sulphate                        synthesis

You are provided with the following chemicals: NaOH, Na2CO3, H2O, Zn(OH)2, CO2, HCI, Fe, H2SO4, CI2, Zn. Using the suitable chemicals from the given list only, state briefly how you would prepare:
(a) iron (III) chloride,
(b) sodium sulphate,
(c) sodium zincate
(d) iron (II) sulphate,
(e) sodium chloride?

Define the term neutralization, Give a reaction, mentioning clearly acid and base used in the reaction.

Define the term neutralization, if one mole of a strong acid reacts with one mole of a strong base, the heat produced is always the same. Why?

Explain why It is necessary to find out the ration of reactants required in the preparation of sodium sulphate.

Explain why, fused calcium chloride is used in the preparation of FeCI3?

Give the Ph value of pure water. Does it change if common salt it added to it?

Classify the following solutions as acids, bases or salts ammonium hydroxide, barium chloride, sodium chloride, sodium hydroxide, H2SO4 and HNO3

Chapter 3: Acids, Bases and Salts solutions [Page 0]

What do you understand by water of crystallization?

Give four substances which contain water of crystallization and write their common names.

Define efflorescence. Give examples.

define deliquescence. Give examples.

Distinguish between drying and dehydrating agent.

Explain clearly how conc, H2SO4 is used as dehydrating as well as drying agent.

M is an element in the form of a powder. M burns in oxygen and the product obtained is soluble in water. The solution is tested with litmus. Write down only the word which will correctly complete each of the following sentences.

(i) If M is a metal, then the litmus will turn _____________.
(ii) If M is a non-metal, then the litmus will turn ______________.
(iii) If M is a reactive metal, then _________________ will be evolved when M reacts with dilute sulphuric acid.
(iv) If M is a metal, it will form ______________ oxide, which will form ____________ solution with water.
(v) If M is a non-metal, it will not conduct electricity in the form of __________.

Give reason for the following:

Sodium hydrogen sulphate is not an acid but it dissolves in water to give hydrogen ions, according to the equation
NaHSO4 ⇆ H+ + Na+ + SO42-

Give reason for the following:

Anhydrous calcium chloride is used in a desiccator.

State whether a sample of the following would increase or decrease in a mass if exposed to air.
Solid NaOH.

State whether a sample of the following would increase or decrease in a mass if exposed to air.

Solid CaCI2

State whether a sample of the following would increase or decrease in a mass if exposed to air.

Solid Na2CO3 10H2O

State whether a sample of the following would increase or decrease in a mass if exposed to air.

Conc, sulphuric acid

State whether a sample of the following would increase or decrease in a mass if exposed to air.

Iron (III) Chloride

why does common salt get wet during the rainy season?

How can impurities be removed common salt?

Name a substance which changes the blue colour of copper sulphate crystals to white.

Name two crystalline substances which do not contain water of crystallization.

Chapter 3: Acids, Bases and Salts

Selina Selina ICSE Concise Chemistry Class 10

Selina ICSE Concise Chemistry for Class 10 - Shaalaa.com

Selina solutions for Class 10 Chemistry chapter 3 - Acids, Bases and Salts

Selina solutions for Class 10 Chemistry chapter 3 (Acids, Bases and Salts) include all questions with solution and detail explanation. This will clear students doubts about any question and improve application skills while preparing for board exams. The detailed, step-by-step solutions will help you understand the concepts better and clear your confusions, if any. Shaalaa.com has the CISCE Selina ICSE Concise Chemistry for Class 10 solutions in a manner that help students grasp basic concepts better and faster.

Further, we at Shaalaa.com are providing such solutions so that students can prepare for written exams. Selina textbook solutions can be a core help for self-study and acts as a perfect self-help guidance for students.

Concepts covered in Class 10 Chemistry chapter 3 Acids, Bases and Salts are Concept of Acids and Bases, Concept of Molecule, Preparation - Laboratory Preparation of Salts (Normal and Acid Salts) – Relevant Laboratory, General Properties of Salts:, Types of Salts, Use of Litmus and pH Paper to Test for Acidity and Alkalinity, Ions Present in Mineral Acids, Alkalis and Salts and Their Solutions.

Using Selina Class 10 solutions Acids, Bases and Salts exercise by students are an easy way to prepare for the exams, as they involve solutions arranged chapter-wise also page wise. The questions involved in Selina Solutions are important questions that can be asked in the final exam. Maximum students of CISCE Class 10 prefer Selina Textbook Solutions to score more in exam.

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