ICSE Worksheet for chapter-4 Analytical Chemistry class 10

Worksheet For class 10

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  • Introduction- color of salts
  • Action of sodium and ammonium hydroxide on solutions of salts
  • Action of alkalis on certain metals and their oxides.

Section - 1 

Q1. State the colour of the following salts:

  1. Copper chloride
  2. Ferric chloride
  3. Copper nitrate
  4. Lead nitrate
  5. Calcium carbonate
  6. Zinc hydroxide

Q2. State the colour of the aqueous solution of the following salts:

  1. Calcium sulphate crystals
  2. Ferrous chloride crystals
  3. Ferric chloride crystals
  4. Ferrous sulphate crystals
  5. Ferric sulphate crystals
  6. Copper sulphate crystals

Q3. A metal, whose alloy is used in the construction of aircrafts, in the powered form was added to sodium hydroxide solution, a colourless gas was evolved and after the reaction was over the solution was colorless.

  1. Name the powdered metal added to sodium hydroxide solution.
  2. Name the gas evolved.
  3. Name the salt present in the colorless solution.

Q4. Name:

  1. An amphoteric oxide.
  2. A salt of zinc which is efflorescent.
  3. An alkali
  4. One metal which forms more than one type of positive ions.
  5. The ion responsible for the blue colour of an aqueous solution of a salt.

Section - 2

Q5. What are amphoteric metals? Describe their reactions with hot caustic alkali. What are amphoteric oxides? Why these oxides react with NaOH?

Q6. State the effect of adding a small amount of

  • Sodium hydroxide
  • Ammonium hydroxide

Followed by an excess in each case to sample of each of the salt solutions.

  • Calcium nitrate
  • Zinc nitrate
  • Lead nitrate

Q7. Using sodium hydroxide solution, how would you distinguish (ICSE 2009)

  • Ammonium sulphate from sodium sulphate
  • Zinc nitrate solution from calcium nitrate solution
  • Iron (II) chloride from iron (III) chloride
  • Calcium nitrate solution from calcium chloride solution

Q8. Name the anion present in each of the following compounds :

  • Compound A when warmed with concentrated sulphuric acid gives a gas which fumes in moist air and which gives dense white fumes with ammonia.
  • When barium chloride solution is added to a solution of compound B , a white precipitate insoluble in dilute hydrochloric acid is formed.
  • The action of heat on the insoluble compound C produces a gas which turns lime water turbid.
  • Compound D when warmed with dilute sulphuric acid gives a gas which turns acidified dichromate solution green.

Q9. Answer the Following

  • Choose the correct pair of substances from copper, copper oxide and dilute sulphuric acid in order to prepare a solution of copper sulphate in the laboratory.
  • Write the balanced equation for the reaction occurring in 4(a)(i)
  • What is seen when ammonium hydroxide is added to copper sulphate solution till it is in excess?
  • Copper sulphate solution is electrolysed with copper electrodes.
  • At which electrode (anode or cathode) are copper ions discharged?
  • When copper ions are being discharged at one electrode, what is happening at the other electrode?
  • One electrode gaind in mass. The gain in mass is (less than, the same as, more than) the loss in mass of the other electrode.(Choose the correct phrase from those in brackets).
  • Does the colour of the copper sulphate solution change or remain unchanged during the lectrolysis?
  • What is the practical value of this particular electrolysis?

Q10. Two elements A and B are stored under water and kerosene oil respectively. When a small piece of element is left in the open air, both starts warming up. The product in each case is dissolved in water. The solution from the residue of A was found to be acidic which that of residue was basic.

  • Identify elements for the reaction of elements A and B on exposure to air.
  • Write chemical equations for the reaction of elements A and B exposure to air.
  • Write chemical equations for the reaction of the products formed in ‘(ii) with water.
  • What is meant by “Activity series of Metals”?

Q11. State what you see when

  • A piece of moist blue litmus paper is placed in a jar of chlorine.
  • A piece of red litmus paper is placed in a jar of ammonia.
  • A burning splint is plunged in a jar containing carbon dioxide .
  • Hydrogen and chlorine react in direct sunlight.
  • Nitric oxide reacts with oxygen.

Q12. Calculate the relative molecular mass ammonium chloroplatinate.


[N=14,H=1, Pt=195, Cl=35.5]

  • Thin strips of three different metals A, B and C are known to be magnesium, copper amd iron respectively.
  • Write down what you would observe in each case when the metals are treated as follows:
  • When each metal is heated in air.
  • When each metal is treated with dilute hydrochloric warmed, if necessary.
  • Arrange the metal A, B and C in the descending order of activity.
  • At which electrode are the metals liberated during the electrolysis of metal slats?

Q13. Name and state the gas law which his explained by Avogadro’s law.

  • Describe the changes you would observe when concentrated sulphuric acid is added to formic acid, HCOOH and warmed. Give equations.
  • Name two crystalline substances which don’t contain water of crystallization
  • Give the name and formula of acid salt which gives sodium ions and sulphate ions in solution.

Q14.  A strip of copper is placed in four different colourless salt solution. They are KNO3, AgNO3, Zn(NO3)2. Which one of the solutions will finally turn blue? Give a reason.

  • How can you obtain (i) chlorine from hydrochloric acid and (ii) hydrochloric acid from chlorine? Give necessary equation.
  • How is hydrogen chloride gas collected and dried?

Q15. Why in the laboratory preparation of nitric acid, the apparatus is made of all glass?

  • On heating magnesium powder in dry nitrogen, a light yellow solid is produced . This solid produces a pungent smelling basic gas when warmed with water. Write equation for the reaction mentioned above.
  • Complete the following table:

Q16. For each of the conversions P to T in the scheme below, write one equation:

Q17. The number of atoms in 1 mole of hydrogen is twice the number of atoms in 1 mole of helium at the same temperature and pressure, why?

  • What is the function of manganese dioxide in the preparation of chlorine from concentrated hydrochloric acid?
  • Give one chemical test to distinguish between dilute hydrochloric acid and dilute sulphuric acid.

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