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Chapter 3: Study Of Acids, Bases and Salts

Exercise

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 70]

Exercise | Q 1 | Page 70

Define an acid.

Exercise | Q 2.1 | Page 70

Give the name and formula of two : Strong monobasic acids

Exercise | Q 2.2 | Page 70

Give the name and formula of two : Weak dibasic acids

Exercise | Q 2.3 | Page 70

Give the name and formula of two : Non-volatile acids

Exercise | Q 2.4 | Page 70

Give the name and formula of two : Volatile acids

Exercise | Q 3.1 | Page 70

Define a base.

Exercise | Q 3.2 | Page 70

Explain, all alkalis are bases but all bases are not alkalis.

Exercise | Q 4.1 | Page 70

Define pH.

Exercise | Q 4.2 | Page 70

State three applications of pH scale.

Exercise | Q 5.1 | Page 70

Define an indicator.

Exercise | Q 5.2 | Page 70

Explain, why a universal indicator is preferred to acid-base indicators.

Exercise | Q 6.1 | Page 70

What is the difference between : An alkali and a base?

Exercise | Q 6.2 | Page 70

What is the difference between : An alkali and a metal hydroxide?

Exercise | Q 7.1 | Page 70

Name the ions furnished by : Bases in solution

Exercise | Q 7.2 | Page 70

Name the ions furnished by : a weak alkali

Exercise | Q 7.3 | Page 70

Name the ions furnished by : an acid

Exercise | Q 8 | Page 70

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

Exercise | Q 9.1 | Page 70

Give one example : Basic oxide which is soluble in water.

Exercise | Q 9.2 | Page 70

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

Exercise | Q 9.3 | Page 70

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

Exercise | Q 9.4 | Page 70

Give one example : A hydroxide which is insoluble in water.

Exercise | Q 9.5 | Page 70

Give one example : A weak mineral acid.

Exercise | Q 9.6 | Page 70

Give one example : A base which is not an alkali.

Exercise | Q 9.7 | Page 70

Give one example : An oxide which is a base.

Exercise | Q 9.8 | Page 70

Give one example : A hydrogen containing compound which is not an acid.

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 71]

Exercise | Q 1 | Page 71

An hydrous hydrogen chloride is not an acid but its aqueous solution is a strong acid. Explain.

Exercise | Q 2 | Page 71

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

Exercise | Q 3 | Page 71

What do you understand by the strength of an acid? On what factors does the strength of an acid depend?

Exercise | Q 4 | Page 71

How is an acid prepared from a non metal and a base from a metal? Give equation.

Exercise | Q 5 | Page 71

Two solutions A and B have pH values of 2 and 9 respectively which one of these two will give a pink colour with phenolphthalein indicator?

Exercise | Q 6 | Page 71

Name two indicators which can identify the presence of an acid?

Exercise | Q 7.1 | Page 71

State how would you prepare copper (II) oxide from
Copper nitrate

Exercise | Q 7.2 | Page 71

State how would you prepare copper (II) oxide from
Copper Carbonate

Exercise | Q 7.3 | Page 71

State how would you prepare copper (II) oxide from
copper sulphate

Exercise | Q 8 | Page 71

Give four examples of preparation of acids by synthesis.

Exercise | Q 9.1 | Page 71

Define an acid salt and a normal salt.

Exercise | Q 9.2 | Page 71

How many salts can be obtained from ortho phosphoric acid? Is there any difference in the salts formed by the acid?

Exercise | Q 10.1 | Page 71

Give equation to prepare the following as directed
MgCO3 from MgCl2

Exercise | Q 10.2 | Page 71

Give equation to prepare the following as directed
PbCO3 from Pb(NO3)

Exercise | Q 10.3 | Page 71

Give equation to prepare the following as directed
NaHCO3 from Na2CO3

Exercise | Q 11.1 | Page 71

Define the following term : Efflorescence.

Exercise | Q 11.2 | Page 71

Define the following term : Hygroscopy.

Exercise | Q 11.3 | Page 71

Define the following term : Water of crystallization

Exercise | Q 12 | Page 71

What is deliquescence? What name is given to the compounds exhibiting such property?

Exercise | Q 13 | Page 71

Explain salt hydrolysis. Name two salts which are (a) acidic (b) basic (c) neutral, when dissolved in water.

Exercise | Q 14 | Page 71

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

Salt Method of Preparation
Zinc sulphate Precipitation
Ferrous sulphide Displacement
Barium sulphate Neutralization 
Sodium sulphate Synthesis
Exercise | Q 15.1 | Page 71

Why common salt gets wet during rainy season?

Exercise | Q 15.2 | Page 71

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

Exercise | Q 16 | Page 71

Write the reactions of SO2 and oxides of nitrogen which leads to acid rain formation.

Exercise | Q 17.1 | Page 71

Fill in the blank
The word acid comes from latin word acidus meaning _________

Exercise | Q 17.2 | Page 71

Fill in the blank
Vinegar is the source of ________ acid.

Exercise | Q 17.3 | Page 71

Fill in the blank
Magnesia is used in making __________.

Exercise | Q 17.4 | Page 71

Fill in the blank
pH scale was introduced by _________ in 1909.

Exercise | Q 17.5 | Page 71

Fill in the blank
___________ is the phenomenon by which hydrated salts on exposure to dry air, lose their water of crystallization and crumble to powder.

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 72]

Exercise | Q 1.1 | Page 72

Choose the correct answer from the options given below
Which of them occurs in solid state?

  • Citric acid

  • Formic acid

  • Acetic acid

  • Hydrochloric acid

Exercise | Q 1.2 | Page 72

Choose the correct answer from the options given below:
Benzoic acid is used for/in/as

  • Baking powder

  • Food preservative

  • Fertilizers

  • Explosives

Exercise | Q 1.3 | Page 72

Choose the correct answer from the options given below:
Which colour with the universal indicator indicates highly alkaline solution?

  • Dark red

  • Yellow

  • Green

  • Violet

Exercise | Q 1.4 | Page 72

Choose the correct answer from the options given below:
Which one is the acidic salt?

  • KNO3

  • Sodium acetate

  • Calcium chloride

  • Ammonium acetate

Exercise | Q 2.1 | Page 72

A solution has a pH of 7. Explain, how you would:
Increase its pH, If a solution changes the color of litmus from red to blue, what can you say about its pH?

Exercise | Q 2.2 | Page 72

A solution has a pH of 7. Explain, how you would:
Decrease its pH, If a solution changes the color of litmus from red to blue, what can you say about its pH?

Exercise | Q 3 | Page 72

What can you say about the pH of a solution that liberates carbon dioxide from sodium carbonate?

Exercise | Q 4 | Page 72

From the list of the substances given, name the substances which you would use to prepare each of the following salts:
List of substances: Copper, lead, sodium, zinc, copper oxide, lead carbonate, sodium carbonate solution, dilute hydrochloric acid, dilute nitric acid and dilute sulphuric acid.
Salts: (a) zinc sulphate (b) copper sulphate (c) sodium sulphate (d) lead sulphate.

Exercise | Q 5 | Page 72

Define the meaning of the term 'acid salt'.

Exercise | Q 6.1 | Page 72

What is the purpose of the pH scale?

Exercise | Q 6.2 | Page 72

What is the pH of pure water?

Exercise | Q 6.3 | Page 72

A is a soluble acidic oxide; B is a soluble base. Compared to the pH of pure water, what is the pH of (a) a solution of A (b) a solution of B.

Exercise | Q 7.1 | Page 72

Taking sodium carbonate as an example, give the meaning of the following terms: Water of crystallization.

Exercise | Q 7.2 | Page 72

Taking sodium carbonate as an example, give the meaning of the following terms: Anhydrous.

Exercise | Q 8 | Page 72

Outline the steps required to convert hydrogen chloride to anhydrous iron (III) chloride. Write the equations for the reactions.

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 73]

Exercise | Q 1 | Page 73

Answer the following questions below, relating your answers only to salts in the following list:
Sodium chloride, anhydrous calcium chloride, copper sulphate-5-water.
(i) What is the name given to the water in the compound copper sulphate-5-water?
(ii) If copper sulphate-5-water is heated, the water is driven off leaving anhydrous copper sulphate. What is the colour of anhydrous copper sulphate?
(iii) By what means, other than heating, you can dehydrate copper sulphate-5-water and obtain anhydrous copper sulphate?
(iv) Which one of the salts in the given list is deliquescent?

Exercise | Q 2 | Page 73

What is meant by the term weak acid?

Exercise | Q 3.1 | Page 73

Solution P has a pH of 13, solution Q has a pH of 6, and a solution R has a pH of 2.
Which solution: Will liberate ammonia from ammonium sulphate on heating?

Exercise | Q 3.2 | Page 73

Solution P has a pH of 13, solution Q has a pH of 6, and a solution R has a pH of 2.
Which solution: Is a strong acid.

Exercise | Q 3.3 | Page 73

Solution P has a pH of 13, solution Q has a pH of 6, and a solution R has a pH of 2.
Which solution : Contains molecules as well as ions?

Exercise | Q 4 | Page 73

Give the name and formula of the acid salt which gives sodium ions and sulphate ions in solution.

Exercise | Q 5.1 | Page 73

Define the following term: Acid.

Exercise | Q 5.1 | Page 73

Define the following term : Neutralisation

Exercise | Q 5.1 | Page 73

Define the following term :  pH scale

Exercise | Q 5.2 | Page 73

A solution of iron (III) chloride has a pH less than 7. Is the solution acidic or alkaline?

Exercise | Q 5.2 | Page 73

If iron reacts with dilute sulphuric acid, what will be the products?

Exercise | Q 5.2 | Page 73

Outline the steps that would be necessary to convert insoluble lead (II) oxide into insoluble chloride.

Exercise | Q 5.2 | Page 73

Write the balanced equations for the reaction required to convert insoluble lead (II) oxide into insoluble lead chloride.

Exercise | Q 6 | Page 73

Some methods used for the laboratory preparation of salts are:
(a) Metal + acid
(b) Carbonate + acid
(c) Precipitation
(d) Direct combination
(e) Titration
Copy and complete the following table : 

Salt Method of Preparation
Ammonium Sulphate  
Calcium carbonate  
Iron (III) chloride  
Lead nitrate  
Zinc sulphate  

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 74]

Exercise | Q 1.1 | Page 74

Choosing only substances from the list given in the box below, write equations for the reactions which you would use in the laboratory to obtain:
(i) Sodium sulphate
(ii) Copper sulphate
(iii) Iron (II) sulphate
(iv) Zinc carbonate

Dilute sulphuric acid

Copper, Iron,
Sodium, Zinc

Copper carbonate,
Sodium carbonate
Exercise | Q 1.2 | Page 74

From the formulae listed below, choose one in each case corresponding to the salt having the given description :
AgCI, CuCO3, CuSO4.5H2O, KNO3, NaCI, NaHSO4, Pb(NO3), ZnCO3, ZnSO4.7H2O
(a) An acid salt
(b) An insoluble chloride 
(c) On treating with concentrated sulphuric acid, this salt changes from blue to white.
(d) On heating this salt changes from green to black.
(e) This salt gives nitrogen dioxide on heating

Exercise | Q 2.1 | Page 74

Write the balanced equation for the preparation of the following compounds, starting from iron and other substance:
Iron (II) sulphide

Exercise | Q 2.1 | Page 74

Write the balanced equation for the preparation of the following compounds, starting from iron and other substance:
Iron (II) sulphate

Exercise | Q 2.1 | Page 74

Write the balanced equation for the preparation of the following compounds, starting from iron and using other substance: Iron (II) chloride

Exercise | Q 2.1 | Page 74

Write the balanced equation for the preparation of the following compounds, starting from iron and other substance:
Iron (III) chloride

Exercise | Q 2.2 | Page 74

Write the equation for the laboratory preparation of sodium sulphate using dilute sulphuric acid.

Exercise | Q 2.2 | Page 74

Write the balanced equation for the preparation of the following compounds, starting from iron and other substance:
lead sulphate using dilute sulphuric acid.

Exercise | Q 3.1 | Page 74

Choosing the correct words given in brackets, complete the sentence given below:
An acid is a compound which, when dissolved in water gives ______ ( hydronium / hydroxide) ions as the only ______ (positive/negative) ions.

Exercise | Q 3.2 | Page 74

Choosing the correct words given in brackets, complete the sentence given below:
A(n) ______ (acid/basic) salt is one in which the hydrogen of an acid has been partially replaced by a ______ (metal/non-metal).

Exercise | Q 4.1 | Page 74

Write equation for the laboratory preparation of the following salt, using sulphuric acid: Iron (II) sulphate from the iron.

Exercise | Q 4.2 | Page 74

Choosing the correct words given in brackets, complete the sentence given below: Copper sulphate from copper.

Exercise | Q 4.3 | Page 74

Choosing the correct words given in brackets, complete the sentence given below: Lead sulphate from lead nitrate.

Exercise | Q 4.4 | Page 74

Choosing the correct words given in brackets, complete the sentence given below: Sodium sulphate from sodium carbonate.

Exercise | Q 5 | Page 74

Which of the following methods, (a), (b), (c), (d) or (e) is generally used for preparing the chlorides listed below from (i) to (v). Answer by writing down the chloride and the letter pertaining to the corresponding method. Each letter is to be used only once.
(a) Action of an acid on a metal.
(b) Action of an acid on an oxide or carbonate.
(c) Direct combination.
(d) Neutralization of an alkali by an acid.
(e) Precipitation (double decomposition).
(i) copper(II) chloride.
(ii) iron(III) chloride.
(iii) iron(II) chloride.
(iv) lead (II) chloride.
(v) sodium chloride.

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 75]

Exercise | Q 1.1 | Page 75

The preparation of lead sulphate from lead carbonate is a two step process (lead sulphate cannot be prepared by adding dilute sulphuric acid to lead carbonate)
What is the first step that is required to prepare lead sulphate from lead carbonate?

Exercise | Q 1.2 | Page 75

The preparation of lead sulphate from lead carbonate is a two step process (lead sulphate cannot be prepared by adding dilute sulphuric acid to lead carbonate)
Write the equation for the reaction that will take place when this first step is carried out.

Exercise | Q 1.3 | Page 75

The preparation of lead sulphate from lead carbonate is a two step process (lead sulphate cannot be prepared by adding dilute sulphuric acid to lead carbonate)
Why is the direct addition of dilute sulphuric acid to lead carbonate an impractical method of preparing lead sulphate?

Exercise | Q 2.1 | Page 75

Fill in the blank.
An acid is a compound which when dissolved in water forms hydronium ions as the only ______ ions.

Exercise | Q 2.2 | Page 75

Fill in the blanks.
A base is a compound which if soluble in water contains ______ ions. A base reacts with an acid to form ______ and water only. This type of reaction is known as ______.

Exercise | Q 3 | Page 75

What is observed when neutral litmus solution is added to sodium hydrogen carbonate solution?

Exercise | Q 4.1 | Page 75

Mention the colour changes observed when the following indicator is added to acid: Alkaline phenolphthalein solution.

Exercise | Q 4.2 | Page 75

Mention the colour changes observed when the following indicator is added to acid: Methyl orange solution.

Exercise | Q 4.3 | Page 75

Mention the colour changes observed when the following indicator is added to acid: Neutral litmus solution.

Exercise | Q 5 | Page 75

From the list given below. Select the word(s) required to correctly complete the blanks (i) to (v) in the following passage:
Ammonia, Ammonium, Carbonate, Carbon dioxide, Hydrogen, Hydronium,
A solution 'X' turns blue litmus red so it must contain (i) ______ ions; another solution 'Y' turns red litmus blue and therefore must contain(ii) ______ ions. When solutions X and Y are mixed together, the products will be a (iii) ______ and ______ (iv) ______. If a piece of magnesium was put into solution X, (v) ______ gas would be evolved.

Exercise | Q 6 | Page 75

Macth the following.

Column A Column B
1. Acid salt a. Sodium potassium carbonate
2. Mixed salt b. Alum
3. Complex salt c. Sodium Carbonate
4. Double salt d. Sodium zincate

5. Normal salt

e. Sodium hydrogen carbonate

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Pages 76 - 77]

Exercise | Q 1.1 | Page 76

What is the term defined in below? 
A salt containing a metal ion surrounded by other ions or molecules.

Exercise | Q 1.2 | Page 76

What is the term defined below?
A base which is soluble in water.

Exercise | Q 2 | Page 77

Write the equation for the following reaction:
Magnesium sulphate solution is mixed with barium chloride solution.

Exercise | Q 2 | Page 76

Choose the correct answer.
Carbon dioxide and sulphur dioxide gas can be distinguished by using

  • Moist blue litmus paper.

  • Lime water

  • Acidified potassium dichromate paper

  • None of the above.

Exercise | Q 3 | Page 76

Solution A is a strong acid.
Solution B is a weak acid.
Solution C is a strong alkali.
(i) Which solution contains solute molecules in addition to water molecules?
(ii) Which solution will give a gelatinous white precipitate with zinc sulphate solution? The precipitate disappears when an excess of the solution is added.
(iii) Which solution could be a solution of glacial acetic acid?
(iv) Give an example of a solution which is a weak alkali.

Exercise | Q 3.1 | Page 77

Give the equation for the preparation of the following salt from the starting material given.
Copper sulphate from copper (II) oxide

Exercise | Q 3.2 | Page 77

Give the equation for the preparation of the following salt from the starting material given.
Iron (III) Chloride from Iron

Exercise | Q 3.3 | Page 77

Give the equation for the preparation of the following salt from the starting material given.
Potassium sulphate from potassium hydroxide solution

Exercise | Q 3.4 | Page 77

Give the equation for the preparation of the following salt from the starting material given.
Lead chloride from lead carbonate (two equations)

Exercise | Q 4 | Page 77

Solution A is a sodium hydroxide solution. Solution B is a weak acid. Solution C is dilute sulphuric acid. Which solution will.
(i) Liberate sulphur dioxide from sodium sulphite
(ii) Give a white precipitate with zinc sulphate solution,(iii) Contain solute molecules and ions?

 

Exercise | Q 4.1 | Page 77

The diagram given below is to prepare iron (III) chloride in the laboratory.

(i) What is substance B?
(ii) What is the purpose of B?
(iii)Why is iron (III) chloride to be stored in a closed container?
(iv) Write the equation for the reaction between iron and chloride ?

Exercise | Q 4.2 | Page 77

Write the equations for the reaction to prepare lead sulphate from lead carbonate. 

Exercise | Q 5 | Page 77

What happen to the crystals of washing soda when exposed to air? Name the phenomenon exhibited.

Exercise | Q 6 | Page 77

Name the method used for preparation of the following salts from the list given below:
(i) Sodium nitrate
(ii) Iron (III) chloride
(iii) Lead chloride
(iv) Zinc sulphate
(v) Sodium hydrogen sulphate

List :
(a) Simple displacement
(b) Neutralization
(c) Decomposition by acid
(d) Double decomposition
(e) Direct synthesis

Exercise | Q 7 | Page 77

From the list given below, select the word(s) required to correctly complete blanks (i) to (v) in the following passage. The words from the list are to be used only once. Write the answers as (a) (i), (ii) (iii) and so on. Do not copy the passage.
Ammonia, ammonium, carbonate, carbon dioxide, hydrogen, hydronium,hydroxide,precipitate,salt,water

(a) A solution M turns blue litmus red, so it must contain (i) _______ ions; another, solution O turns red litmus blue and hence, must contain (ii)__________ ions.

(b) When Solutions M and O are mixed together, the products will be (iii) ________ and (iv) ________.

(c) If a piece of magnesium was put into a solution M.(v) _________________Gas would be evolved.

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 77]

Exercise | Q 1.1 | Page 77

Select the correct answer from the choices a,b,c and d which are given.Write only the letter corresponding to the correct answer.
A particular solution contains molecules and ions of the solute so it is a

  •  Weak acid

  • Strong acid

  • Strong base

  •  Salt solution

Exercise | Q 1.2 | Page 77

Select the correct answer from the choices a,b,c and d which are given.Write only the letter corresponding to the correct answer.
 An organic weak acid is

  • Formic acid

  • Sulphuric acid

  • Sulphuric base

  • Hydrochloric acid

Exercise | Q 1.3 | Page 77

Select the correct answer from the choices a,b,c and d which are given.Write only the letter corresponding to the correct answer.
An example of a complex salt is

  • Zinc sulphate

  • Solution hydrogen sulphate

  • Iron(II) ammonium sulphate

  • Tetramine copper (II) sulphate

Chapter 3: Study Of Acids, Bases and Salts Exercise Exercise solutions [Page 78]

Exercise | Q 1.1 | Page 78

State what would you observe when :
Washing soda crystals are exposed to the atmosphere.

Exercise | Q 1.2 | Page 78

State what would you observe when :
The salt ferric chloride is exposed to the atmosphere.

Exercise | Q 2 | Page 78

Match the salts given in Column I with their method of preparation given in Column II:

Column I

Column II

(i) P(NO3)2 from PbO

(ii) MgCl2 from Mg

(iii) FeClfrom Fe

(iv) NaNO3 from NaOH

(v) ZnCO3 from ZnSO4

(A) Simple displacement

(B) Titration

(C) Neutralisation

(D) Precipitation

(E) Combination

Exercise | Q 3 | Page 78

Fill in the blank from the choices given in bracket.
When a metallic oxide is dissolved in water, the solution formed has a high concentration of ___________ ions. (H+,H3O+,OH-)

Exercise | Q 4 | Page 78

To increase the pH value of neutral solution, we should add

  • An acid

  • An acid salt

  • An alkali

  • A salt

Chapter 3: Study Of Acids, Bases and Salts

Exercise

Frank Frank Class 10 Chemistry Part 2

Frank Class 10 Chemistry Part 2 - Shaalaa.com

Frank solutions for Class 10 Chemistry chapter 3 - Study Of Acids, Bases and Salts

Frank solutions for Class 10 Chemistry chapter 3 (Study Of 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 Frank Class 10 Chemistry Part 2 solutions in a manner that help students grasp basic concepts better and faster.

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Concepts covered in Class 10 Chemistry chapter 3 Study Of 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.

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