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# Frank solutions for Class 10 Chemistry chapter 4 - Analytical Chemistry

## Chapter 4: Analytical Chemistry

Exercise

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 85]

Exercise | Q 1.1 | Page 85

Write the colour of the following salts: Cuprous salts.

Exercise | Q 1.2 | Page 85

Write the colour of the following salt : Cupric salts.

Exercise | Q 1.3 | Page 85

Write the colour of the following salt : Aluminium salts.

Exercise | Q 1.4 | Page 85

Write the colour of the following salt : Ferrous salts.

Exercise | Q 1.5 | Page 85

Write the colour of the following salt : Ferric salts.

Exercise | Q 1.6 | Page 85

Write the colour of the following salt : Calcium salts.

Exercise | Q 2.1 | Page 85

Using ammonium hydroxide, how would you distinguish between the following pair of ions in solution?
Ferrous ion and Ferric ion.

Exercise | Q 2.2 | Page 85

Name the method used for preparation of the following salt from the list given below:

Exercise | Q 3 | Page 85

You are provided with PbCO3, ZnCO3 and CaCO3. How will you identify these cations?

Exercise | Q 4 | Page 85

Z is a compound. With dilute HCl it gives a gas turning dichromatic solution green. Z gives lilac flame. Name Z.

Exercise | Q 5.1 | Page 85

What do you observe when caustic soda solution is added to the following solution: first a little and then in excess : FeCl3

Exercise | Q 5.2 | Page 85

What do you observe when caustic soda solution is added to the following solution: first a little and then in excess : ZnSO4

Exercise | Q 5.3 | Page 85

What do you observe when caustic soda solution is added to the following solution: first a little and then in excess : Pb(NO3)2

Exercise | Q 5.4 | Page 85

What do you observe when caustic soda solution is added to the following solution: first a little and then in excess : CuSO4

Exercise | Q 6 | Page 85

What is the reaction of freshly precipitated aluminium hydroxide with caustic soda solution? Give equation.

Exercise | Q 7 | Page 85

What do you understand by amphoteric oxide? Give the balanced equations for the reaction with three different amphoteric oxides with a caustic alkali. Write your observation if any.

Exercise | Q 8.1 | Page 85

Name a solution that will separate the component of the following mixture: Zn(OH)2 from Pb(OH)2

Exercise | Q 8.2 | Page 85

Name a solution that will separate the component of the following mixture: CaO from PbO

Exercise | Q 8.3 | Page 85

Name a solution that will separate the component of the following mixture: CuO from ZnO

Exercise | Q 9 | Page 85

Give two examples of amphoteric hydroxides.

Exercise | Q 10 | Page 85

A metal whose alloy finds use in the construction of aircrafts in the powdered form is added to sodium hydroxide solution. A colourless gas was evolved and after reaction was over, the solution was colourless.
(a) Name the powdered metal added to sodium hydroxide solution.
(b) Name the gas evolved.
(c) Name the salt present in the colorless solution.

Exercise | Q 11.1 | Page 85

Name: A metallic hydroxide soluble in excess of NH4OH

Exercise | Q 11.2 | Page 85

Name: A metallic oxide soluble in excess of caustic soda solution.

Exercise | Q 11.3 | Page 85

Name: A strong alkali

Exercise | Q 11.4 | Page 85

Name: A weak alkali.

Exercise | Q 11.5 | Page 85

Name: Two coloured ions

Exercise | Q 11.6 | Page 85

Name: Two bases which are not alkalis but dissolve in strong alkalis.

Exercise | Q 11.7 | Page 85

Name: A coloured metallic oxide which dissolves in alkalis to yield colourless solutions.

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 86]

Exercise | Q 1.1 | Page 86

What happens when ammonia solution is added first dropwise and then in excess to the following solution:
CuSO4
Write balanced reactions for these equation.

Exercise | Q 1.2 | Page 86

What happens when ammonia solution is added first dropwise and then in excess to the following solution:
ZnSO4
Write balanced equations for these reactions.

Exercise | Q 1.3 | Page 86

What happens when ammonia solution is added first dropwise and then in excess to the following solution:
FeCl3
Write balanced equations for these reactions.

Exercise | Q 2 | Page 86

Name the chloride of a metal which is soluble in excess of ammonium hydroxide.

Exercise | Q 3 | Page 86

On adding dilute ammonia solution to a colourless solution of a salt, a white gelatinous precipitate appears. This precipitate however dissolves on addition of excess of ammonia solution. Identify (Choose from Na, l, Zn, Pb, Fe)
(a) Which metal salt solution was used?
(b) What is the formula of white gelatinous precipitate obtained?

Exercise | Q 4.1 | Page 86

Name : A yellow monoxide that dissolves in hot and concentrated caustic alkali.

Exercise | Q 4.2 | Page 86

Name : A white, insoluble oxide that dissolves when fused with caustic soda or potash.

Exercise | Q 4.3 | Page 86

Name : A compound containing zinc in the anion.

Exercise | Q 5.1 | Page 86

Fill in the blanks.
Salts of ______ [normal / transition] elements are generally coloured.  From the ions K1+, Cr3+, Fe2+, Ca2+, $\ce{SO^2-_3}$, $\ce{Mn^1-_4}$,$\ce{NO^1_3}$ the ions generally coloured are ______.

Exercise | Q 5.2 | Page 86

Fill in the blank.
The hydroxide which is soluble in excess of NaOH is _________ [Zn(OH)2 / Fe(OH)3 / Fe(OH)2].

Exercise | Q 5.3 | Page 86

Fill in the blank.
The salt which will not react with NH4OH solution ______[ZnCl2, CuCl2 / NH4Cl/ FeCl2]

Exercise | Q 5.4 | Page 86

Fill in the blank.
The substance/s which react with hot conc. NaOH solution and undergoes a neutralization reaction ______ [Al2O3 / Al / Al(OH)3]

Exercise | Q 5.5 | Page 86

Fill in the blank.
To distinguish soluble  salts of zinc and lead ______ [NaOH / NH4OH]can be used.

Exercise | Q 6.1 | Page 86

Choose the correct answer from the options given below :
Color of ferrous ion is

• Blue

• Green

• Pink

• Light green

Exercise | Q 6.2 | Page 86

Choose the correct answer from the options given below :
Which one is colourless anion?

• $\ce{HCO^-_3}$

• $\ce{Cr 20^2-_7}$

• $\ce{Cr O^2-_7}$

• $\ce{Mn O^-_4}$

Exercise | Q 6.3 | Page 86

Choose the correct answer from the options given below :
Sodium zincate (Na2ZnO2) is

• Pale blue ppt

• Reddish brown ppt

• Colourless

• Dirty green ppt

Exercise | Q 6.4 | Page 86

Choose the correct answer from the options given below :
Metal + alkali → salt + _________

•  N2

•  H2

• H2O

• OH

Exercise | Q 6.5 | Page 86

Choose the correct answer from the options given below :
Which salt solution is soluble in excess of NH4OH

• Iron (II) salts

• Iron (III) salts

• Copper (II) salts

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 87]

Exercise | Q 1.1 | Page 87

You are given a mixture of precipitated copper hydroxide and zinc hydroxide. Name a solvent which will dissolve:
Only copper hydroxide

Exercise | Q 1.2 | Page 87

You are given a mixture of precipitated copper hydroxide and zinc hydroxide. Name a solvent which will dissolve:
Only zinc hydroxide

Exercise | Q 1.3 | Page 87

You are given a mixture of precipitated copper hydroxide and zinc hydroxide. Name a solvent which will dissolve:
Both copper hydroxide and zinc hydroxide

Exercise | Q 2.1 | Page 87

Using sodium hydroxide solution, how will you distinguish: Zinc nitrate solution from calcium nitrate solution

Exercise | Q 2.2 | Page 87

Using sodium hydroxide solution, how will you distinguish:
Iron (II) chloride from iron (III) chloride

Exercise | Q 2.3 | Page 87

Using sodium hydroxide solution, how will you distinguish:

Exercise | Q 3.1 | Page 87

Sodium hydroxide solution is added to solution A. A white precipitate is formed which is soluble in excess sodium hydroxide. Name the metal ion present in A.

Exercise | Q 3.2 | Page 87

When ammonium hydroxide is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide to give an inky blue solution. Name the cation present in solution B. What is the probable colour of solution B?

Exercise | Q 4 | Page 87

What do you see when sodium hydroxide solution is added to zinc sulphate solution, till it is in excess?

Exercise | Q 5 | Page 87

You are given three white powders-calcium carbonate, lead carbonate and zinc carbonate. Describe the tests you would carry out in solution, to identify the metal ion in each of the above compounds. Indicate clearly how you would prepare the solutions for the tests.

Exercise | Q 6 | Page 87

Write equation for the reaction that will take place when copper sulphate solution is added to sodium hydroxide solution.

Exercise | Q 7.1 | Page 87

Three test tubes contain calcium nitrate solution, zinc nitrate solution and lead nitrate solution.Describe the effect of Adding sodium hydroxide solution to each portion in turn till it is in excess.

Exercise | Q 7.2 | Page 87

Three test tubes contain calcium nitrate solution, zinc nitrate solution and lead nitrate solution.Describe the effect of Adding ammonium hydroxide to each portion in turn till it is in excess.

Exercise | Q 8.2 | Page 87

What will you observe when barium chloride solution is added to iron(II) sulphate solution.

Exercise | Q 8.3 | Page 87

How will the action of dilute hydrochloric acid on sodium carbonate and sodium sulphite enables you to distinguish between these two compounds?

Exercise | Q 8.4 | Page 87

Sodium hydroxide solution can be used to distinguish between i. iron (II) sulphate solution and (ii) iron (III) sulphate solution; because these solutions give different coloured precipitates with sodium hydroxide solution. Give the colour of the precipitate formed with each of the solution.

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 88]

Exercise | Q 1.1 | Page 88

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.

Exercise | Q 1.2 | Page 88

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Sodium sulphate solution and sodium chloride solution.

Exercise | Q 1.3 | Page 88

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Calcium nitrate solution and zinc nitrate solution.

Exercise | Q 2.1 | Page 88

Write balanced equation for the following reaction:
Iron(II) chloride solution with sodium hydroxide solution.

Exercise | Q 2.2 | Page 88

Write balanced equation for the following reaction:
Chlorine and cold dilute sodium hydroxide solution.

Exercise | Q 2.3 | Page 88

Write balanced equation for the following reaction:
Zinc and sodium hydroxide solution

Exercise | Q 2.4 | Page 88

Write balanced equation for the following reaction:
Sulphur dioxide and sodium hydroxide solution
(Give the equation for the formation of the normal salt)

Exercise | Q 3.1 | Page 88

State what do you observe when:
Neutral litmus solution is added to alkaline solution

Exercise | Q 3.2 | Page 88

State what do you observe when:
Ammonium hydroxide is added to iron (III) sulphate solution.

Exercise | Q 3.3 | Page 88

State what do you observe when:
Lead nitrate and sodium chloride are mixed.

Exercise | Q 3.4 | Page 88

State what do you observe when:
Ethane is bubbled through a solution of bromine in tetrachloromethane (carbon tetra chloride).

Exercise | Q 3.5 | Page 88

State what do you observe when:
Sulphur burns.

Exercise | Q 4.1 | Page 88

How would you distinguish between Zn2+ and Pb2+ ions, using ammonium hydroxide solution?

Exercise | Q 4.2 | Page 88

Copy and complete the following table which refers to the action of heat on some carbonates :

 Carbonate Colour of residue on cooling Zinc carbonate Lead carbonate Copper carbonate
Exercise | Q 5.1 | Page 88

Write the observation, and balanced equation for the following reaction:
Sodium hydroxide is added dropwise to a solution of zinc sulphate, till it is in excess.

Exercise | Q 5.2 | Page 88

Write the observation, and balanced equation for the following reaction:
Ammonium hydroxide is added first in a small quantity, and then in excess, to a solution of copper sulphate.

Exercise | Q 5.3 | Page 88

Write the observation, and balanced equation for the following reaction:
Excess of ammonium hydroxide is added to a substance, obtained by adding hydrochloric acid to silver nitrate solution.

Exercise | Q 5.4 | Page 88

Write the observation, and balanced equation for the following reaction:
Moist starch iodide paper is placed at the mouth of a test tube containing chlorine gas.

Exercise | Q 5.5 | Page 88

Write the observation, and balanced equation for the following reaction:
A paper dipped in potassium permanganate solution is placed at the mouth of a test tube, containing sulphur dioxide gas.

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 89]

Exercise | Q 1 | Page 89

Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solutions of copper (II) sulphate, zinc nitrate, lead nitrate, calcium chloride and iron (III) sulphate. Copy the following table and write the colour of the precipitate in (i) to (v) and the nature of the precipiatate (soluble or insoluble) in (vi) to (x)

 Aqueous salt Solution Colour of Participitate when NaOH is added in a samll quantity Nature of precipitate(soluble or insoluble) when NaOH added in excess Copper (II) Solution Zinc nitrate Lead nitrate Calcium chloride Iron(III) sulphate
Exercise | Q 2 | Page 89

The questions (i) to (v) refer to the following salt solutions listed A to F :
A. Copper nitrate
B. Iron (II) sulphate

C. Iron (III) chloride
E. Magnesium sulphate
F. Zinc chloride
(i) Which two solutions will give a white precipitate when treated with dilute hydrochloric acid followed by barium chloride solution/
(ii) Which two solutions will give a white precipitate when treated with dilute nitric acid followed by silver nitrate solution?
(iii) Which solution will give a white precipitate when either dilute hydrochloric acid or dilute sulphuric acid is added to it?
(iv) Which solution becomes a deep/inky blue colour when excess of ammonium hydroxide is added to it?
(v) Which solution gives a white precipitate with excess ammonium hydroxide?

Exercise | Q 3 | Page 89

Match the following :

 Column A Column B 1. A substance that turns moist starch iodide paper blue. A. Ammonium sulphate 2. A compound which releases a reddish brown gas on reactionwith concentrated sulphuricacid and copper turnings. B. Lead carbonate 3 . A solu tion of this compound gives a dirty green preci pi ta tewith sodium hydroxide. C. Chlorine 4 . A compound which on heating with sodium hydroxide produces a gas which formsdense white fumes withhydrogen chloride. D. Copper nitrate 5 . A white solid which gives ayellow residue on heating. E. Ferrous sulphate

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 90]

Exercise | Q 1 | Page 90

The metal oxide which can react with acid as well as alkali is:

• Silver oxide.

• Copper (II) oxide.

• Aluminium oxide

• Calcium oxide

Exercise | Q 2.1 | Page 90

Identify the substance P based on the information given below:
The deliquescent salt P, turns yellow on dissolving in water, and gives a reddish brown precipitate with sodium hydroxide solution.

Exercise | Q 2.2 | Page 90

Identify the substance Q based on the information given below:
The white crystalline solid Q is soluble in water. It liberates a pungent smelling gas when heated with sodium hydroxide solution.

Exercise | Q 2.3 | Page 90

Identify the substance Q based on the information given below:
The pale green solid R turns reddish brown on heating. Its aqueous solution gives a white precipitate with barium chloride solution. The precipitate is insoluble in mineral acids.

Exercise | Q 3.1 | Page 90

Give one chemical test to distinguish between the following pair of compound:
Zinc sulphate solution and Zinc chloride solution.

Exercise | Q 3.2 | Page 90

Give one chemical test to distinguish between the following pair of compound:
Iron (II) chloride solution and iron (III) chloride solution.

Exercise | Q 4 | Page 90

From the list given below, select the word (s) required complete the blanks (i) to (v) in the following passage :
Note : words chosen from the list are to be used only once. Write only the answers. Do not copy the passage
[reddish brown, ammonium, nitrogen dioxide, hydroxyl, dirty green, ammonia, acidic, alkaline]
Nitrogen and hydrogen combine in the presence of a catalyst to give (i) ________ gas. When the above mentioned gas is passed through water it forms a solution which will be (ii) ______ in nature and the solution contains (iii) ______ ions and (iv) _______ions. The above solution when added to iron (II) sulphate solution gives a (v) _________coloured precipitate of iron (II) hydroxide.

Exercise | Q 5 | Page 90

Write the equation for the following reaction :
Zinc oxide is treated with sodium hydroxide solution.

Exercise | Q 6.1 | Page 90

Choose the correct answer from the options given below :
Hydroxide of this metal is soluble is sodium hydroxide solution

• Magnesium

• Silver

• Copper

Exercise | Q 6.2 | Page 90

Choose the correct answer from the options given below :
When dilute sulphuric acid reacts with iron sulphide, the gas evolved is _______

• Hydrogen sulphide

• Sulphur dioxide

• Sulphur trioxide

• Vapour of sulphuric acid

#### Chapter 4: Analytical Chemistry Exercise Exercise solutions [Page 91]

Exercise | Q 1.1 | Page 91

State two relevant observation of the following:
Ammonium hydroxide solution is added to copper (II) nitrate solution in small quantities and then in excess

Exercise | Q 1.2 | Page 91

State two relevant observation of the following:
Ammonium hydroxide solution is added to zinc nitrate solution in minimum quantities and then in excess

Exercise | Q 2.1 | Page 91

Distinguish between the following pair of compound using the test given within bracket.
Iron (II) Sulpate an and iron(III) using ammonium hydroxide)

Exercise | Q 2.2 | Page 91

Distinguish between the following pair of compound using the test given within bracket.
A lead salt and a zinc salt (using excess ammonium hydroxide

Exercise | Q 3 | Page 91

State your observations when ammonium hydroxide solution is added drop by drop and then in excess to each of the following solutions :
1) Copper sulphate solution

2) Zinc sulfate solution.

Exercise | Q 4 | Page 91

Fill in the blank.
Potassium sulphite on reacting with hydrochloric acid releases ________

Exercise | Q 5 | Page 91

Choose the correct answer from the options given below :
A chloride which forms a precipitate that is soluble in excess of ammonium hydroxide is :

• Calcium chloride

• Ferrous chloride

• Ferric chloride

• Copper chloride

Exercise

## Frank solutions for Class 10 Chemistry chapter 4 - Analytical Chemistry

Frank solutions for Class 10 Chemistry chapter 4 (Analytical Chemistry) 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 4 Analytical Chemistry are Action of Alkalis (Naoh, Koh) on Certain Metals, Their Oxides and Hydroxides, On Solution of Salts - Sodium Hydroxide on Ammonium Salts, On Solution of Salts - Special Action of Ammonium Hydroxide on Solutions of Copper Salt, Formation and Colour of Hydroxide Precipitated for Solutions of Salts of Ca, Fe, Cu, Zn and Pb, On Solution of Salts - Colour of Salt and Its Solution, Analytical Chemistry.

Using Frank Class 10 solutions Analytical Chemistry 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 Frank Solutions are important questions that can be asked in the final exam. Maximum students of CISCE Class 10 prefer Frank Textbook Solutions to score more in exam.

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