ICSE CHEMISTRY MCQs on Practical Chemistry

ICSE Multiple choice Questions on Practical Chemistry

 

Choose the correct answer from A, B, C and D for each of the following statements.

Question 1

The gas with greenish yellow colour

A) Hydrogen gas

B) Oxygen gas

C) Chlorine gas

D) Ammonia gas

 

Question 2

The observation when Sodium chloride is heated with Conc. Sulphuric acid:

A) A colourless pungent odour gas which turns Nessler’s reagent to brown

B) A colourless gas which gives dense white fumes with Ammonia gas

C) A gas with rotten egg smell which turns Lead acetate paper to silvery black

D) Reddish brown vapours evolved

 

Question 3

When dilute Hydrochloric acid is added to Silver nitrate solution

A) A white precipitate is formed which dissolves in excess Ammonium hydroxide

B) A white precipitate is formed which is insoluble in excess Ammonium hydroxide

C) A white precipitate which dissolves on heating

D) No precipitate is formed

 

Question 4

A salt ‘X’ gives brisk effervescence of a colourless gas which turns lime water milky but has no effect on acidified KMnO₄ solution. The anion present in the salt ‘X’ is

A) Sulphide ion

B) Nitrate ion

C) Carbonate ion

D) Sulphite ion

 

 

Question 5

The cation present in the salt which gives lilac flame in flame test:

A) Potassium ion

B) Calcium ion

C) Copper ion

D) Sodium ion

 

Question 6

The gas which turns lime water milky and acidified Potassium dichromate to clear green solution:

A) Sulphur dioxide gas

B) Carbon dioxide gas

C) Hydrogen chloride gas

D) Carbon dioxide gas

 

Question 7

Which of the following salts would give a bluish white precipitate with barium chloride solution and the precipitate is insoluble in dilute Nitric acid?

A) Zinc sulphate

B) Copper (II) sulphate

C) Silver nitrate
D) Copper chloride

 

Question 8

Which of the following gases turns moist red litmus to blue?

A) Hydrogen chloride gas

B) Chlorine gas

C) Ammonia gas

D) Oxygen gas

 

Question 9

Which of the following reagents gives a white precipitate with dilute Hydrochloric acid but not with dilute Nitric acid?

A)    Lead chloride

B)    Lead nitrate solution

C)    Sodium chloride solution

D)    Nessler’s reagent

 

Question 10

Which of the following cations would give a white precipitate with Sodium hydroxide but not with Ammonium hydroxide?

A) Calcium ion

B) Zinc ion
C) Ferrous ion

D) Lead ion

 

Question 11

Which of the following precipitates dissolves in excess Ammonium hydroxide and gives a deep blue solution?

A) Zinc hydroxide

B) Lead hydroxide

C) Ferrous hydroxide

D) Copper hydroxide

 

Question 12

The ion present in the salt solution which gives a Gelatinous white precipitate with small amount of Ammonium hydroxide

 

A) Cu²⁺

B) Zn²⁺

C) Fe²⁺

D) Pb²⁺

 

Question 13

Sodium hydroxide solution is added to Lead nitrate solution in small amounts first  and then in excess amount:

A) White precipitate is formed then dissolved

B) White precipitate is formed and remains precipitate

C) Blue precipitate is formed which dissolves in excess NaOH

D) Blue precipitate insoluble in excess NaOH

 

Question 14

Ferrous hydroxide:

A) dissolves in excess NaOH but not in Excess Ammonium hydroxide

B) dissolves in excess Ammonium hydroxide but not in Excess Sodium hydroxide

C) Soluble in both NaOH and NH₄OH in excess

D) insoluble in both of NaOH and NH₄OH

 

Question 15

Which of the following compounds is soluble in excess Sodium hydroxide but not in Ammonium hydroxide?

A) Cu(OH)₂

B) Pb(OH)₂

C) Zn(OH)₂

D) Fe(OH)₂

ELECTROLYSIS - ICSE - QUICK REVISION TEST 1

ELECTROLYSIS - CLASS 10 ICSE - QUICK REVISION TEST

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1. A solid substance is composed of only ions. It acts as a ___________ (strong/ weak/ non) eelctrolyte.

2. The flow of current in an electrolyte ____________ (increases/ decreases) with the increase in the concentration of free ions in it.

3. An electrolyte which conducts electricity in large amounts in its aqueous solution undergoes _______ (complete/partial/no) dissociation.

4. An example of a polar covalent compound which acts as an electrovalent compound in its aqueous solutions and is a strong electrolyte.

5. Pure water does not conduct electricity hence this acid is added to water before its electrolysis.

6. The separation of ions of an electrovalent compound when it is dissolved in water is called ___________ (dissociation/ ionization).

7. Oxygen is released at _________ (anode/cathode) in the electrolysis of acidified water.

8. Metal is deposited at ________ (anode/cathode) during an electrolysis of a salt solution.

9. ____________ electrode accepts electrons from _______ hence it is called oxidation electrode.

10. ________ migrate towards anode and ______ migrate towards cathode in electrolysis process.

11. The ease of reduction of a metal ion ____________ as we move down the electrochemical series.

12. This ion is called spectator ion in the electrolysis process. 

13. The following diagram shows the electrorefining of impure copper metal.

i) State one appropriate observation in this.

ii) Why a pure thin sheet of Copper is taken as cathode.

iii) Where are the impurities collected in this process. 

Sureshot questions from Study of compounds - Chemistry ICSE class 10

Sureshot questions from Study of compounds ICSE CHEMISTRY

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Give one suitable reason for each of the followings

1.      Hydrogen chloride gas dissolved using Funnel arrangement.

Reduces back-suction and provides a large surface area for the absorption of HCl gas in water.

2.      Quick lime is not used as drying agent in the purification of Hydrogen chloride gas.

Hydrogen chloride gas reacts with Calcium oxide and forms Calcium chloride and Water.

3.      Low temperature is maintained in the laboratory preparation of Hydrogen chloride gas.

Maintaining high temperature causes fuel wastage and Sodium sulphate formed here forms a hard crust inside the round bottom flask.

4.      Calcium hydroxide is taken in excess amount in the preparation of Ammonia gas in laboratory method.

Excess Calcium hydroxide prevents the sublimation of Ammonium chloride.

5.      All glass apparatus is used in the laboratory preparation of Nitric acid.

Nitric acid vapours being highly corrosive destroys rubber or cork but does not affect Glass.

6.      Nitric acid prepared in laboratory method appears in yellow colour.

The yellow tinge in Nitric acid is due to the dissolved Nitrogen dioxide in it.

7.      Dilute Sulphuric acid can form two types of salts.

Sulphuric acid is a dibasic acid.

State one appropriate observation for each of the followings.

1.      Silver nitrate solution is added to dilute hydrochloric acid then heated.

A white precipitate is formed which dissolve on heating.

2.      Lead nitrate solution is added to dilute Hydrochloric acid followed by excess ammonium hydroxide.

A white precipitate is formed which dissolves in Ammonium hydroxide.

3.      Barium chloride solution is added to dilute Sulphuric acid.

A white precipitate is formed

4.      Excess Ammonia gas is passed into Copper sulphate solution.

A pale blue precipitate turns into a deep blue solution.

5.      Conc. Nitric acid is added to Copper turnings.

A blue filtrate/ Reddish brown vapours evolved

 

6.      Dilute Nitric acid is added to Copper turnings.

A blue filtrate is formed

7.      Conc. Sulphuric acid is added to Copper sulphate crystals.

Blue crystals turns into white amorphous solid

8.      Conc. sulphuric acid is added to sugar crystals.

A black spongy mass is left.

9.      Dilute Sulphuric acid is added to Copper oxide.

A blue solution is formed.

10.  A dilute acid is added to sodium carbonate.

Brisk effervescence of a colourless gas evolved which turns lime water milky but has no effect on acidified Potassium permanganate.

11.  A dilute  acid is added to sodium sulphite.

A suffocating colourless gas evolved which turns lime water milky decolourizes acidified Potassium permanganate.

12.  A dilute acid is added to Sodium sulphide.

A colourless gas with rotten egg smell evolved which turns Lead acetate paper to silvery black.

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Metallurgy Test

Electrolysis Test

Chemical Bonding - test

The Periodic Table

Practical Chemistry Test - anions

Practical Chemistry Test - Cations

Practical Chemistry Test - Observation Based

Sureshot questions in ICSE CHEMISTRY

Sureshot questions in ICSE CHEMISTRY Board exam with solutions - Study of Compounds

Sureshot questions in Class 10 CHEMISTRY Board exam with solutions - ICSE

Sureshot questions in ICSE CHEMISTRY Board exam with solutions. Topics Hydrogen chloride, Ammonia, Nitric acid, Sulphuric acid

 Name the following.

1.      A basic gas which turns Nesslers reagent to brown precipitate and gives dense white fumes with a glass rod dipped Conc. Hydrochloric acid.

Ammonia gas

2.      The industrial process in which Ammonia gas is prepared.

Haber’s Process

3.      The white precipitate obtained when a dilute acid is added to silver nitrate solution and dissolves on heating.

Lead nitrate

4.      The dilute acid which does not give Hydrogen gas with any active metal but gives Hydrogen gas with Magnesium and Manganese.

Nitric acid

5.      The acid used as a drying agent in the purification of hydrogen chloride gas.

Conc. Sulphuric acid

6.      The liquid reactant used in the laboratory preparation of Nitric acid.

Conc. Sulphuric acid

7.      The reactant which is taken in excess amount in the laboratory preparation of Ammonia gas.

Calcium hydroxide

8.      The process in which Nitric acid is prepared in large scale.

Ostwald’s process

9.      The gas other than oxygen which is released when dilute nitric acid reacts with Copper metal.

Nitric oxide

10.  The arrangement used to dissolve Hydrogen chloride gas in water.

Funnel arrangement

11.  The solid reactant used in the laboratory preparation of hydrogen chloride gas.

Sodium chloride

12.  A dibasic acid which acts a strong oxidizing agent as well.

Conc. Sulphuric acid

13.  A mono basic acid which is a strong oxidizing agent.

Conc. Nitric acid

14.  The property of Conc. sulphuric acid which allows it to remove water molecules from blue Copper sulphate.

Dehydrating agent

15.  The property shown by Conc. Sulphuric acid in the preparation of Hydrogen chloride gas.

Non-volatile acid

16.  The gas produced when a dilute acid is added to Sodium carbonate.

Carbon dioxide

17.  The gas released when a dilute acid is added to Sodium sulphite.

Sulphur dioxide

18.  The acid which on thermal decomposition gives a reddish brown gas.

Conc. Nitric acid

19.  The catalyst used in the Haber’s process.

Iron

20.  The drying agent used in purification of Ammonia gas.

Quick lime (Calcium oxide)

21.  The gas other than Hydrogen chloride whose high solubility in water is proved using Fountain experiment.

Ammonia gas

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Observation based questions - Practical chemistry 2

Questions on Analytical chemistry 

Identification of cations using Ammonium hydroxide and Sodium hydroxide

Identify the cation present in each of the following cases based on the colour of the precipitate formed.

1. A salt solution gives a gelatinous white precipitate with small amount of Ammonium hydroxide, and the precipitate is soluble in excess Ammonium hydroxide.

Ans: Zinc ion

2. A salt solution forms a reddish brown precipitate with Ammonium hydroxide which remains insoluble.

Ans:  Ferric ion

3. This salt solution gives a pale blue precipitate with Ammonium hydroxide, this precipitate turns deep (inky) blue solution in excess Ammonium hydroxide.

Ans: Cupric ion

4. When Ammonium hydroxide is added to this salt solution a dirty green precipitate is formed whih is isoluble in excess Ammonium hydroxide.

Ans: Ferrous ion

5. When this salt solution is treated with Ammonium hydroxide solution a white precipitate is formed and insoluble in excess Ammonium hydroxide.

Ans: Lead ion

6. A salt solution is treated with Sodium hydroxide then it gives a gelatinous white precipitate and that white precipitate disappears when excess Sodium hydroxide is added.

Ans: Zinc ion

7. When Sodium hydroxide solution is added to a salt solution, a pale blue precipitate is formed which remains insoluble in excess Sodium hydroxide.

Ans: Zinc ion

8. Two salt solutions A and B are treated with Sodium hydroxide and A reddish brown precipitate and a dirty green precipitate are formed respectively.

Ans: Solution 'A' contains Ferric ion

Solution 'B' contains Ferrous ion

Observation based questions - Practical chemistry - ICSE

Observation based questions - Practical chemistry - ICSE - IMPORTANT for VIVA

IDENTIFICATION OF GASES

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1. Name a gas which is neutral in nature and burns with blue flame.

Ans: Hydrogen gas

2. Name the gas which turns lime water milky but has no effect of acidified Potassium permanganate and acidified Potassium dichromate.

Ans: Carbon dioxide gas

3. The gas, which is greenish yellow in colour, turns moist blue litnus paper to red and then bleaches it.

Ans: Chlorine gas.

4. A which is released by the oxidation of Conc. HCl using an oxidizing agent.

Ans: Chlorine gas

5. A basic gas which is used in the manufacturing of a fertilizer called Urea.

Ans: Ammonia gas

6. These vapours turn anhydrous Copper sulphate to blue.

Ans: Water vapour

7. A suffocating gas which turns lime water milky and highly soluble in water.

Ans: Sulphur dioxide gas.

8. This gas is released when  Sodium chloride (mineral) is heated with a non-volatile acid.

Ans: Hydrogen chloride gas

9. A coloured gas which gives Iodine vapours with Potassium iodide crystals.

Ans: Nitrogen dioxide

10. A gas which is released when a dilute acid reacts with a metal sulphide.

Ans: Hydrogen sulphide

Comparison between Polar and Non-polar compounds for class 10 ICSE

Comparison between Polar and Non-polar compounds

Polar covalent and non polar molecules

Polar molecules	Non-polar molecules
1.      Due to the electronegativity difference between the atoms the electrons are distributed unequally which leads to charge separation.	1.  There is no charge separation since the electron pair is equally distributed between the atoms.
2.      Example: HCl, H2O , NH3 etc.	2. Example: H2, Cl2, O2, N2, CCl4, CH4 etc

 

Ø  Charge separation in Hydrogen chloride molecule:

In HCl molecule Chlorine is more electronegative than Hydrogen so the electron pair is more strongly attracted by Chlorine atom due this a slight negative charge is developed on Chlorine and a slight positive charge on Hydrogen atom. Hence it becomes a polar compound

Class 10 Practical Chemistry ICSE pdf

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Identification of Cations anions and Gases

Class 10 Nitric acid ICSE notes pdf free download

Class 10 Nitric acid ICSE notes

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 Class 10 Ammonia ICSE notes pdf

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Ammonia notes class 10, ICSE class 10 Ammonia notes, Preparation of Ammonia gas, Haber's process, Properties of Ammonia gas, analytical use of Ammonium hydroxide....

CLASS 10 Chemical Bonding ICSE notes

 CLASS 10 Chemical Bonding ICSE notes

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Covalent bond:

The bond formed by the mutual sharing of electron pairs between the given pairs of atoms (of same or different kind) of non metals.

Covalent compound (molecule) : The compounds (molecules) formed as a result of mutual sharing of electrons between the atoms are called covalent compounds.

Covalency: The number of electron pairs that an atom shares with other atom/s to get stable electronic configuration.

Formation covalent molecules - Electron dot representation

·         The element which has 7 valence electrons (i.e. short of one electron for octet configuration) contributes one electron and shares one pair of electron with other atom.

     

            Cl - 2,8,7         Cl - 2,8,7                     Chlorine molecule     single covalent bond

·         The element having 6 valence electrons (short of 2 electrons) contributes 2 electrons hence shares two pairs of electrons.

Oxygen       Oxygen                       Oxygen molecule       Double bond

                 2,6               2,6

 

·         Similarly the element with 5 valence electrons contributes 3 electrons and shares three pairs of electrons.

Nitrogen        Nitrogen        Nitrogen molecule

2,5                  2,5                                                            Triple bond

 

·            Formation of Hydrogen molecule

 

 

·            Formation of Methane molecule (CH₄)

 

·         Formation of Carbon tetra chloride molecule (CCl₄)

Formation of Hydrogen chloride molecules (HCl)

 

·         Formation of Water molecule:

 

·         Formation of Ammonia molecule

Ø Lone pair: The pair of electrons which is not involved in any bond formation.

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