Selina Class 10 ICSE Solutions Chemistry : Chapter 8- Study of Compounds - Hydrogen Chloride

Class 10: Chemistry Chapter 8 solutions. Complete Class 10 Chemistry Chapter 8 Notes.

Selina Class 10 ICSE Solutions Chemistry : Chapter 8- Study of Compounds - Hydrogen Chloride

Selina 10th Chemistry Chapter 8, Class 10 Chemistry Chapter 8 solutions

Exercise 1

Solution 1.

Solution 2.

(a) Hydrogen chloride is dried by passing through conc. Sulphuric acid.
(b) Phosphorous pentoxide and CaO cannot be used to dry HCl because they react with HCl.
2P₂O₅+ 3HCl → POCl₃ + 3HPO₃
CaO + 2HCl → CaCl₂ + H₂O

Solution 3.

(a) Anhydrous HCl is poor conductor due to the absence of ions in it whereas aqueous HCl is excellent conductor since it contains ions.

(b) When the stopper is opened HCl gas comes in contact with water vapors of air and gives white fumes due to the formation of hydrochloric acid.

(c) A solution of HCl in water gives hydronium ions and conducts electricity, but HCl is also soluble in dry toluene, but in that case it neither (i) turns blue litmus red (ii) nor does conducts electricity. This indicates the absence of H⁺ ions in toluene showing thereby that hydrogen chloride is a covalent compound.

(d) When ammonium hydroxide is brought near the mouth of HCl, dense white fumes are formed due to the formation of ammonium chloride.
HCl + NH₄OH → NH₄Cl + H₂O

(e) Dry hydrogen chloride is not acidic whereas moist Hydrogen chloride is acidic. In presence of a drop of water HCl gas dissolves in water and forms hydrochloric acid which turns blue litmus paper red.

(f) Hydrogen chloride is not collected over water as it is highly soluble in water.

Solution 4.

Difference between Hydrogen chloride gas and Hydrochloric acid is:

Hydrogen chloride gas	Hydrochloric acid
1. Dry hydrogen chloride gas does not turn blue litmus red due to non-acidic character.2. Hydrogen chloride gas does not conduct electricity.	1. Being acidic it turns blue litmus red.2. Hydrochloric acid is a good conductor of electricity.

Solution 5.

(a) Hydrochloric acid is prepared by this method.
(b) The reactants are sodium chloride and Sulphuric acid.
(c) The empty flask acts as Anti-Suction device. In case the back suction occurs the water will collect in it and will not reach the generating flask.
(d) The drying agent is Conc. Sulphuric acid. Sulphuric acid is chosen as drying agent because it does not react with HCl.
(e) The Inverted funnel :
Prevents or minimizes back suction of water.
Provides a large surface area for absorption of HCl gas.

Solution 6.

(a) Chlorine.
The compound formed which is strongly acidic in water, is HCl.
H₂ + Cl₂ →  2HCl

(b) A dilute aqueous solution of hydrochloric acid gets gradually concentrated on distillation, till the concentration of the acid reaches 22.2% HCl by weight which boils at 110⁰C.When this concentration is reached, no further increase in concentration of the acid becomes possible by boiling. This is because vapours evolved before 110⁰C are vapours of water but at temperature above 110⁰C vapours consist mostly of molecules of HCl.

Solution 7.

We can prove that hydrochloric acid contains both hydrogen and chlorine by the following experiment.
Take a voltameter used for electrolysis of water, fitted with platinum cathode and graphite anode.
Into the voltameter pour 4 molar HCl and pass direct current.
It is seen that a colourless gas is evolved at cathode and a greenish gas is evolved at anode.
When a burning splinter is brought near a colourless gas, it bursts into flame thereby proving that it is hydrogen gas.
When moist starch iodide paper is held in the greenish yellow gas, it turns blue black, thereby proving that the gas is chlorine.
2HCl → H₂ + Cl₂
This experiment proves that hydrochloric acid contains both hydrogen and chlorine.

Solution 8.

(a) Manganese dioxide
(b) Hydrogen chloride and ammonia
(c) Hydrogen and oxygen
(d) AgCl(Silver chloride)
(e) Aqua regia
(f) Fountain experiment
(g) Hydrogen chloride gas

Solution 9.

(a) An aqueous solution of chlorine is acidic as it dissolves in water to form hydrochloric and hypochlorous acids.
(b) Silver nitrate reacts with hydrochloric acid to form thick curdy white ppt. of silver chloride whereas silver nitrate does not react with nitric acid.
AgNO₃ + HCl → AgCl + HNO₃
(White ppt.)

Solution 10.

A is Silver nitrate
B is Hydrochloric acid
C is Silver chloride

Solution 11.

a. Sodium carbonate on treating withdil.HCl results in the formation of sodium chloride with the liberation of carbon dioxide gas.
Na₂CO₃ + 2HCl → 2NaCl + H₂O + CO₂ ↑
Sodium sulphite on treating with dil.HCl results in the formation of sodium chloride with the liberation of sulphur dioxide gas.
Na₂SO₃ + 2HCl → 2NaCl + H₂O + SO₂ ↑

b. Sodiumthiosulphate reacts with dil. HCl to produce sulphur dioxide gas and precipitates yellow sulphur.
Na₂S₂O₃ + 2HCl → 2NaCl + H₂O + SO₂ + S↓
Sulphur is not precipitated when sulphites are treated with dil.HCl.

Solution 12.

Three tests are:

1. HCl gas gives thick white fumes of ammonium chloride when glass rod dipped in ammonia solution is held near the vapours of the acid.
   NH₃ + HCl NH₄Cl
2. With silver nitrate HCl gives white precipitate of silver chloride. The precipitate is insoluble in nitric acid but soluble in ammonium hydroxide.
   AgNO₃ + HCl AgCl + HNO₃
3. A greenish yellow gas is liberated when concentrated hydrochloric acid is heated with oxidizing agent like manganese dioxide.
   MnO₂ + 4HCl MnCl₂ +2H₂O + Cl₂

Solution 13.

MnO₂, PbO₂ and red lead react with conc. HCl acid to liberate Cl₂. This shows that hydrochloric acid is oxidized to chlorine by oxidizing agents.

Solution 14.

HCl dissolves both in water and toluene, when HCl dissolves in water it ionizes and forms hydronium and chloride ions. Whereas this ionization is not observed in toluene hence a solution of HCl in water can be used as an electrolyte.

Solution 15.

Solution 16.

A mixture having three parts of conc. Hydrochloric acid and one part of conc. Nitric acid is called aqua-regia.
Nitric acid acts as oxidizing agent.

Solution 17.

Solution 18.

Solution 1 (2004).

Solution 1 (2005).

(a) (i) CuO +2HCl CuCl₂ + H₂O
(ii) MnO₂+ 4HCl MnCl₂ +2H₂O +Cl₂

(b) (i) The experiment is called Fountain Experiment.
(ii) This experiment shows that hydrogen chloride is highly soluble in water.
(iii) Red

Solution 1 (2008).

When hydrogen chloride is collected by downward delivery or upward displacement, it shows that it is heavier than air.

Solution 2 (2008).

Hydrogen chloride is not collected over water as it is soluble in water.

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Selina Class 10 ICSE Solutions Chemistry : Chapter 2- Chemical Bonding

Download PDF: Selina Class 10 ICSE Solutions Chemistry : Chapter 2- Chemical Bonding PDF

Chapterwise Selina Publishers ICSE Solutions for Class 10 Chemistry :

• Chapter 1- Periodic Table, Periodic Properties and Variations of Properties
• Chapter 2- Chemical Bonding
• Chapter 3- Acids, Bases and Salts
• Chapter 4- Analytical Chemistry: Uses of Ammonium Hydroxide And Sodium Hydroxide
• Chapter 5- Mole Concept and Stoichiometry
• Chapter 6- Electrolysis
• Chapter 7- Metallurgy
• Chapter 8- Study of Compounds - Hydrogen Chloride
• Chapter 9- Study of Compounds - Study of Compounds - Ammonia
• Chapter 10- Study of Compounds - Nitric Acid
• Chapter 11- Sulphuric Acid
• Chapter 12- Organic Chemistry
• Chapter 13- Practical Work

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