FRANK Solutions for Class 10 Chemistry Chapter 4 - Analytical Chemistry

Revise Chemistry concepts with our Frank Solutions for ICSE Class 10 Chemistry Chapter 4 Analytical Chemistry. Learn to identify the given cations with clear answers by TopperLearning’s Chemistry experts. Relearn the concept of amphoteric oxides. Find out how to write balanced equations to explain the reaction of amphoteric oxides with a caustic alkali.

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Chapter 4 - Analytical Chemistry Exercise 85

Question 1
Write the colour of the following salts:
(a) Cuprous salts.
(b) Cupric salts.
(c) Aluminium salts.
(d) Ferrous salts.
(e) Ferric salts.
(f) Calcium salts.
Solution 1
(a) Cuprous salts = Colourless
(b) Cupric salts = Blue
(c) Aluminium salts = Colourless
(d) Ferrous salts= Light green
(e) Ferric salts = Yellow
(f) Calcium salts = Colourless
Question 2
Using ammonium hydroxide, how would you distinguish between the following pairs of ions in solution?
(a) Ferrous ion and Ferric ion.
(b) Zinc ion and Lead ion.
Solution 2
Question 3
You are provided with PbCO3, ZnCO3 and CaCO3. How will you identify these cations?
Solution 3

Question 4
Z is a compound. With dilute HCl it gives a gas turning dichromatic solution green. Z gives lilac flame. Name Z.
Solution 4
K2SO4.
Question 5
What do you observe when caustic soda solution is added to the following solution: first a little and then in excess
(a) FeCl3
(b) ZnSO4
(c) Pb(NO3)2
(d) CuSO4
Solution 5
Question 6
What is the reaction of freshly precipitated aluminium hydroxide with caustic soda solution? Give equation.
Solution 6
Question 7
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.
Solution 7

Question 8
Name a solution that will separate the components of the following mixtures:
(a) Zn(OH)2 from Pb(OH)2
(b) CaO from PbO
(c) CuO from ZnO
Solution 8
Question 9
Give two examples of amphoteric hydroxides.
Solution 9
Examples of amphoteric hydroxides are: Zn(OH)2, Al(OH)3.
Question 10
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.
Solution 10
Question 11
Name:
(a) A metallic hydroxide soluble in excess of NH4OH
(a) A metallic oxide soluble in excess of caustic soda solution.
(b) A strong alkali
(c) A weak alkali.
(d) Two coloured ions
(e) Two bases which are not alkalis but dissolve in strong alkalis.
(f) A coloured metallic oxide which dissolves in alkalis to yield colourless solutions.
Solution 11

Chapter 4 - Analytical Chemistry Exercise 86

Question 12
What happens when ammonia solution is added
(a) Dropwise and then
(b) In excess to the following solutions:
(i) CuSO4
(ii) ZnSO4
(iii) FeCl3
(c) Write balanced reactions.
Solution 12

Question 13
Name the chloride of a metal which is soluble in excess of ammonium hydroxide.
Solution 13
The chloride of a metal which is soluble in excess of ammonium hydroxide is zinc chloride i.e. ZnCl2.
Question 14
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?
Solution 14
Question 15
Name
(a) A yellow monoxide that dissolves in hot and concentrated caustic alkali.
(b) A white, insoluble oxide that dissolves when fused with caustic soda or potash.
(c) A compound containing zinc in the anion.
Solution 15
(a) PbO
(b) Al2O3
(c) Na2ZnO2
Question 16

Fill in the blanks:
(a) Salts of ______ [normal / transition] elements are generally coloured. From the ions K1+, Cr3+, Fe2+, Ca2+, begin mathsize 10px style SO subscript 3 superscript 2 minus end superscript comma space MnO subscript 4 superscript 1 minus end superscript comma NO subscript 3 superscript 1 end style the ions generally coloured are ______.
(b) The hydroxide which is soluble in excess of NaOH is ______ [Zn(OH)2 / Fe(OH)3 / Fe(OH)2].
(c) The salt which will not react with NH4OH solution ______[ZnCl2, CuCl2 / NH4Cl/ FeCl2]
(d) The substance/s which react with hot conc. NaOH solution and undergoes a neutralization reaction ______ [Al2O3 / Al / Al(OH)3]
(e) To distinguish soluble  salts of zinc and lead ______ [NaOH / NH4OH]can be used.

Solution 16

(a) transition, Cr3+, Fe2+, MnO44-.
(b) Zn(OH)2
(c) NH4Cl
(d) Al2O3, Al
(e) NH4OH

Question 17

Choose the correct answer from the options given below :

(i) Color of ferrous ion is

(a) Blue

(b) Green

(c) Pink

(d) Light green

 

(ii) Which one is colourless anion?

  

 

(iii) Sodium zincate (Na2ZnO2) is

(a) Pale blue ppt

(b) Reddish brown ppt

(c) Colourless

(d) Dirty green ppt

 

(iv) Metal + alkali salt + _________

(a) N2

(b) H2

(c) H2O

(d) OH

 

(v) Which salt solution is soluble in excess of NH4OH

(a) Iron (II) salts

(b) Iron (III) salts

(c) Lead salts

(d) Copper (II) salts

Solution 17

(i) Green

(ii)   

(iii) Colourless

(iv) H2

(v) Copper(II) salts

Chapter 4 - Analytical Chemistry Exercise 87

Question 1992-1

You are given a mixture of precipitated copper hydroxide and zinc hydroxide. Name a solvent which will dissolve:
(a) Only copper hydroxide
(b) Only zinc hydroxide
(c) Both copper hydroxide and zinc hydroxide

Solution 1992-1

(a) Addition of KCN
(b) Addition of excess of NaOH.
(c) Addition of excess of NH4OH.

Question 1993-1
Using sodium hydroxide solution, how will you distinguish:
(a) Zinc nitrate solution from calcium nitrate solution
(b) Iron (II) chloride from iron (III) chloride
(c) Lead hydroxide from magnesium hydroxide.
Solution 1993-1
Question 1995-1
(a) 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.
(b) 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?
Solution 1995-1
(a) The metal ion present in solution A is Pb2+.
(b) The cation present in solution B is Cu2+. The probable colour of solution B is blue.
Question 1996-1
What do you see when sodium hydroxide solution is added to zinc sulphate solution, till it is in excess?
Solution 1996-1
Question 1996-2
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.
Solution 1996-2
The solutions for the tests will be prepared by dissolving the given powders separately in water.
(i) Solution of Calcium carbonate:
Calcium carbonate is CaCO3 and contains Ca2+ ions. Sodium hydroxide solution NaOH can be used to identify Ca2+ since its addition to calcium carbonate solution will give white precipitates of Ca(OH)2 which are sparingly soluble in excess of NaOH.
(ii) Solution of Lead carbonate:
Lead carbonate is PbCO3 and contains Pb2+ ions. Ammonium hydroxide solution NH4OH can be used to identify Pb2+ since its addition to lead carbonate solution will give white precipitates of Pb(OH)2 which are insoluble in excess of NH4OH.
(iii) Solution of Zinc carbonate:
Zinc carbonate is ZnCO3 and contains Zn2+ ions. Sodium hydroxide solution NaOH can be used to identify Zn2+ since its addition to zinc carbonate solution will give white gelatinous precipitates of Zn(OH)2 which are soluble in excess of NaOH.
Question 1996-3
Write equation for the reaction that will take place when copper sulphate solution is added to sodium hydroxide solution.
Solution 1996-3
Question 1997-1
Three test tubes contain calcium nitrate solution, zinc nitrate solution and lead nitrate solution. Each solution is divided into two portions (i) and (ii). Describe the effect of
(i) Adding sodium hydroxide solution to each portion in turn till it is in excess.
(ii) Adding ammonium hydroxide to each portion in turn till it is in excess.
Solution 1997-1
Question 1998-1
(a) 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.
(b) What will you observe when barium chloride solution is added to iron(II) sulphate solution.
(c) How will the action of dilute hydrochloric acid on sodium carbonate and sodium sulphite enables you to distinguish between these two compounds?
Solution 1998-1

Chapter 4 - Analytical Chemistry Exercise 88

Question 1999-1
Describe in each case, one chemical test that would enable you to distinguish between the following pairs of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
(i) Sodium chloride solution and sodium nitrate solution.
(ii) Sodium sulphate solution and sodium chloride solution.
(iii) Calcium nitrate solution and zinc nitrate solution.
Solution 1999-1
Question 2000-1

Write balanced equations for the following reactions:
(i) Iron(II) chloride solution with sodium hydroxide solution.
(ii) Chlorine and cold dilute sodium hydroxide solution.
(iii) Zinc and sodium hydroxide solution
(iv) Sulphur dioxide and sodium hydroxide solution

(Give the equation for the formation of the normal salt)

Solution 2000-1

Question 2001-1
State what do you observe when:
(i) Neutral litmus solution is added to alkaline solution
(ii) Ammonium hydroxide is added to iron (III) sulphate solution.
(iii) Lead nitrate and sodium chloride are mixed.
(iv) Ethane is bubbled through a solution of bromine in tetrachloromethane (carbon tetra chloride).
(v) Sulphur burns.
Solution 2001-1
Question 2003-1
Solution 2003-1
Question 2003-2
Write the observations, and balanced equations for the following reactions:
(i) Sodium hydroxide is added dropwise to a solution of zinc sulphate, till it is in excess.
(ii) Ammonium hydroxide is added first in a small quantity, and then in excess, to a solution of copper sulphate.
(iii) Excess of ammonium hydroxide is added to a substance, obtained by adding hydrochloric acid to silver nitrate solution.
(iv) Moist starch iodide paper is placed at the mouth of a test tube containing chlorine gas.
(v) A paper dipped in potassium permanganate solution is placed at the mouth of a test tube, containing sulphur dioxide gas.
Solution 2003-2

Chapter 4 - Analytical Chemistry Exercise 89

Question 2004-1
Solution 2004-1
Question 2005-1
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
D. Lead nitrate
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?
Solution 2005-1
(i) B and E (Iron (II) sulphate and Magnesium sulphate)
(ii) C and F (Iron (III) chloride and Zinc chloride)
(iii) D (Lead nitrate)
(iv) A (Copper nitrate)
(v) F (Zinc chloride)
Question 2006-1

Solution 2006-1

Chapter 4 - Analytical Chemistry Exercise 90

Question 2009-1
Choose the correct answer:
The metal oxide which can react with acid as well as alkali is:
(a) Silver oxide.
(b) Copper (II) oxide.
(c) Aluminium oxide
(d) Calcium oxide
Solution 2009-1
C ( Aluminium oxide)
Question 2009-2

Identify the substances P, Q and R in each case based on the information given below:
(i) The deliquescent salt P, turns yellow on dissolving in water, and gives a reddish brown precipitate with sodium hydroxide solution.
(ii) The white crystalline solid Q is soluble in water. It liberates a pungent smelling gas when heated with sodium hydroxide solution.
(iii) 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.

Solution 2009-2

(i) P is Ferric chloride
(ii) Q is an ammonium salt
(iii) R is ferrous sulphate

Question 2009-3
Give one chemical test to distinguish between the following pairs of compounds:
(i) Zinc sulphate solution and Zinc chloride solution.
(ii) Iron (II) chloride solution and iron (III) chloride solution.
Solution 2009-3
(i) When BaCl2 solution is added to the given solution ZnSO4 gives a white precipitate while no precipitate is obtained with ZnCl2 solution.
(ii) When NaOH solution is added to the given solution, iron (II) chloride gives dirty green precipitate while reddish brown precipitate is obtained with iron(III) chloride.
Question 2010-1

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

Solution 2010-1

(i) Ammonia

(ii) Alkaline

(iii) Ammonium

(iv) Hydroxyl

(v) Dirty green

Question 2010-2

Write the equation for the following reaction :

Zinc oxide is treated with sodium hydroxide solution.

Solution 2010-2

Question 2011-1

Choose the correct answer from the options given below :

(i) Hydroxide of this metal is soluble is sodium hydroxide solution

(a) Magnesium

(b) Lead

(c) Silver

(d) Copper

 

(ii) When dilute sulphuric acid reacts with iron sulphide, the gas evolved is _______

(a) Hydrogen sulphide

(b) Sulphur dioxide

(c) Sulphur trioxide

(d) Vapour of sulphuric acid

Solution 2011-1

(i) Lead

(ii) Hydrogen sulphide

Chapter 4 - Analytical Chemistry Exercise 91

Question 2013-1

State two relevant observations for each of the following:

(i) Ammonium hydroxide solution is added to copper (II) nitrate solution in small quantities and then in excess

(ii) Ammonium hydroxide solution is added to zinc nitrate solution in minimum quantities and then in excess

Solution 2013-1

(i) (a) When NH4OH is added to copper (II) nitrate solution in small quantities, a pale blue precipitate is observed.

 (b) When added in excess, NH4OH dissolves to give an inky blue solution forming a complex salt.

 

(ii) (a) When NH4OH is added to zinc nitrate solution in minimum quantity, it forms a gelatinous white precipitate.

 (b) When added in excess, it dissolves to form a complex salt.

Question 2014-1

Distinguish between the following pairs of compound using the test given within brackets.

(i) Iron (II) Sulpate an and iron(III) using ammonium hydroxide)

(ii) A lead salt and a zinc salt (using excess ammonium hydroxide

Solution 2014-1

(i) Iron (II):

  

 

Iron (III):

  

 

(ii) Pb(NO3)2+2 NH4OH Pb(OH)2+2NH4NO3

 

On adding excess of NH4OH, chalky white ppt. of

insoluble Pb(OH)2 is formed.

 

ZnSO4 + 2NH4OH Zn(OH)2 + (NH4)2SO4

 

With excess of NH4OH, white gelatinous ppt. of soluble Zn(OH)2 is formed.

Question 2016-1

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

(i) Copper sulphate solution

(ii) Zinc sulphate solution

Solution 2016-1

i) When NH4OH is added to copper sulphate solution drop-wise, a pale blue ppt. is obtained.

 CuSO4 + 2NH4OH  Cu(OH)2 + (NH4)2SO4 + 4H2O

  With excess of NH4OH, the ppt. dissolves to give a deep blue solution of tetra amine copper (II) sulphate.

 Cu(OH)2 + (NH4)2SO4 + NH4OH   [Cu(NH3)4]SO4 + H2O

 

ii) When NH4OH is added to zinc sulphate solution drop-wise, a white, gelatinous ppt. is obtained.

 ZnSO4 + 2NH4OH  Zn(OH)2 + (NH4)2SO4

 With an excess of NH4OH, the ppt. dissolves to give a colourless solution of tetra amine zinc (II) sulphate.

 Zn(OH)2 + (NH4)2SO4 + 2NH4OH [Zn(NH3)4]SO4 + 4H2O

Question 2017-1

Fill in the blank from the choices given in bracket.

Potassium sulphite on reacting with hydrochloric acid releases ________

Solution 2017-1

Potassium sulphite on reacting with hydrochloric acid releases sulphur dioxide.

Question 2017-2

Choose the correct answer from the options given below :

A chloride which forms a precipitate that is soluble in excess of ammonium hydroxide is :

(a) Calcium chloride

(b) Ferrous chloride

(c) Ferric chloride

(d) Copper chloride

Solution 2017-2

Copper chloride