ICSE Worksheet for chapter-3 Acid Bases And Salts class 10

Worksheet For class 10

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  • Definitions of acids, bases, alkalis.
  • Classification of acids and bases on the basis of salt
  1. Source
  2. Molecular composition
  3. Strength
  4. Concentration
  5. Basicity
  6. Preparation, properties and uses of acids and bases.
  7. Neutralization, Indicators.
  8. Salts- Definition, Classification, Solubility and Preparation.

Preparat​ion of specific salts-

  1. CuSO4.5H2O
  2. Na2SO4.10H2O
  3. FeSO4 or ZnSO4
  4. FeCl3
  5. PbCl2, CaCO3
  6. General properties of salts and hydrolysis of salts.

Section - 1

Q1. Which of the following salts give acidic solutions, alkaline solutions and neutral solutions in water:

  1. Potassium nitrate, KNO3
  2. Ammonium sulphate, (NH4)2SO4
  3. Potassium carbonate, K2CO3
  4. Sodium chloride, NaCl
  5. Sodium acetate, CH3COONa
  6. Copper sulphate, CuSO4.
  7. Acidic solutions: _______________________________________
  8. Alkaline solutions:______________________________________
  9. Neutral solutions: ______________________________________

Q2. Fill in the blanks in the following statements with the help of suitable words:

Deliquescence takes place because of the difference in

  1. _______ of atmospheric
  2. _______ and that of the deliquescent substance. The vapour pressure of atmospheric humidity is
  3. ______ than that of the deliquescent substance. The substances which take up water on exposure to atmosphere, without forming a solution are known as
  4. ________substances.

Q3. Answer the following questions, relating your answers only to salts in the list given below:

Anhydrous Calcium chloride, Copper sulphate.5H2O, Sodium carbonate.10H2O.

  1. Which compound is efflorescent?
  2. Which compound is blue in color?
  3. Which compound is deliquescent?
  4. What would be seen on mixing a solution of calcium chloride with a solution of sodium carbonate?
  5. Write the balanced equation for the reaction occurring when a solution of calcium chloride is mixed with a solution of sodium carbonate.

Q4. Match the following : (ICSE 2007 )

A. Acid salt (a) sodium potassium carbonate
B. Mixed salt (b) Alum
C. Complex salt (c) Sodium carbonate
D. Double salt (d) Sodium zincate
E. Normal salt (e) Sodium hydrogen carbonate

Q5. Find the odd one out and explain your choice .

  1. Al(OH)3 , Pb(OH)2 , Mg(OH)2 , Zn(OH)2
  2. Formic acid , nitric acid , acetic acid, propanoic acid

Section - 2

Q6. Write the equations for the laboratory preparation of the following salts using sulphuric acid.

  1. Iron (II) sulphate from iron.
  2. Copper sulphate from copper
  3. Lead sulphate from lead nitrate
  4. Sodium sulphate from sodium carbonate

Q7. Give reasons why:

  1. We pour acid into water not water into acid.
  2. Fused calcium chloride is used in the preparation of FeCl3.
  3. It is necessary to find out the ratio of reactants required in the preparation of sodium sulphate.
  4. Nitric acid is not used in the preparation of hydrogen by active metals.

Q8. What is observed when neutral litmus solution is added to sodium hydrogen carbonate solution ?

Q9. Solution A is a sodium hydroxide solution. Solution B is a weak acid. (ICSE 2010)

Solution C is dilute sulphuric acid. Which solution will :

  1. Liberate sulphur dioxide from sodium sulphite.
  2. Give a white precipitate with zinc sulphate solution.
  3. Contain solute molecules and ions ?

Q10. Give one important use of the following bases :

  1. Sodium hydroxide
  2. Aluminium hydroxide
  3. Potassium hydroxide
  4. Ammonium hydroxide

Q11. (a) solution X has a pH of 13, solution Y has a pH of 6 and solution Z has a pH of 2.

  1. Which solution will liberate ammonia from ammonium chloride on heating?
  2. Which solution is a strong acid?
  3. Which solution contains solute molecules as well as ions?

(b) From the list of substances given below, choose the pair required to prepare the slats (i) to (iii) in the laboratory and write down the relevant equations, naming the method of preparation involved. The substances are-

  1. Anhydrous iron (III) chloride
  2. Copper (II) sulphate
  3. Sodium sulphate

(c) All ammonium salts are decomposed on heating. What other property do ammonium salts have in common?

Q12. In terms of Ionic Theory, define the following:

  1. An acid
  2. An alkali
  3. Neutralisation

Name an acid salt that is present in:

  • Health salts
  • Baking powder
  • Laxative

Give two examples of each of the following methods to prepare salts in the laboratory:

  1. By the direct union of elements
  2. By the reaction between solution of two different salts to form a precipitate
  3. By the action of a solution of an acid on the solution of a base.

Q13. How can the effects of sulphur acid burns be counteracted?

  1. Give an example of hydrated salt which is
  2. Soluble in water
  3. Efflorescent
  4. Give ionic definition of a salt

Q14. Three solutions X, Y, Z have pH 13, 6, 3 respectively .

  1. Which solution is a strong acid?
  2. Which solution will react with zinc and aluminium?
  3. Which solution contains molecules as well as ions?
  4. Table salt gets moist in wet weather explain.
  5. Aqueous solution of ammonia precipitated hydroxide of metal from the solution of their salts for identifying positive radicals or cations. State the colour of precipitate for the slat solution of
  • Fe++
  • Fe+++
  • Pb++
  • Zn++
  • Cu++

Q15. Write down the names of the acids and bases (hydroxides) from which the following salts may be prepared:

  1. Aluminium chloride
  2. Iron
  3. Sulphate
  4. Copper
  5. nitrate
  6. Zinc nitrate

Q16. What is meant by ‘basicity of an acid’? Give three examples.

  1. What is meant by “acidity of a base”? Give three examples.
  2. Suggest methods for preparing (i) an acid from an element, and (ii) an alkali from an element. Give chemical equations involved.

Q17. (a) Give one equation for the preparation of base by the following methods:

  1. By action of water on soluble metallic oxide
  2. By thermal decomposition
  3. By direct synthesis

(b) Give one equation for the preparation of acid by the following methods:

  1. By action of water on acidic oxides
  2. By displacement from acid with other acid
  3. By direct synthesis

(c) What a meant by

  1. A strong base
  2. A weak base

Q18. (a) Ammonia is oxidized according to the equation:

4NH3+SO2→4NO+6H2 O

(b) How many litres of nitric oxide are formed when 90 litres of oxygen react with ammonia at STP?

  1. Calculate the mass of chromium atoms in 0.5 kg of cr2S3 [Cr=52, S=32]
  2. What is the net ionic reaction of neutralization reactions?

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