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Class 10 SELINA Solutions Chemistry Chapter 11 - Study of Compounds D. Sulphuric Acid

Study of Compounds D. Sulphuric Acid Exercise Intext 1

Solution 1

(a) Sulphuric acid is called King of Chemicals because there is no other manufactured compound which is used by such a large number of key industries.

(b) Sulphuric acid is referred to as Oil of vitriol as it was obtained as an oily viscous liquid by heating crystals of green vitriol.

Solution 2

(a) Two balanced equations to obtain SO2 is:

(i) 4FeS2 + 11O2 2Fe2O3 +8SO2

(ii) S +O2 SO2

(b) The conditions for the oxidation of SO2 are:

(i) The temperature should be as low as possible. The yield has been found to be maximum at about 4100C-450oC

(ii) High pressure (2 atm) is favoured because the product formed has less volume than reactant.

(iii) Excess of oxygen increases the production of sulphur trioxide.

(iv) Vanadium pentoxide or platinised asbestos is used as catalyst.

(c) Vanadium pentoxide (V2O5)

(d) Sulphuric acid is not obtained directly by reacting SO3 with water because the reaction is highly exothermic which produce the fine misty droplets of sulphuric acid that is not directly absorbed by water.

(e)The chemical used to dissolve SO3 is concentrated sulphuric acid. The product formed is oleum.

Reaction involved in this process:

SO3 + H2SO4 → H2S2O7

Solution 3

Impurity of ARSENIC poisons the catalyst [i.e. deactivates the catalyst]. So, it must be removed before passing the mixture of SO2 air through the catalytic chamber.

Solution 4

(a) The catalyst which helps in the conversion of sulphur dioxide to sulphur trioxide in step C is Vanadium pentoxide.

(b) The two steps for the conversion of sulphur trioxide to sulphuric acid is:

(i) SO3 + H2SO4H2S2O7

(ii) H2S2O7 + H2O 2H2SO4

(c)The substance that will liberate sulphur dioxide in step E is dilute H2SO4.

(d) The equation for the reaction by which sulphur dioxide is converted to sodium sulphite in step F is:




Study of Compounds D. Sulphuric Acid Exercise Ex. 11

Solution B 1

(a) Active metal + Acid ⟶ Metal sulphate + Hydrogen

(b) Base + Acid ⟶ Salt + Water

(c) Carbonate/hydrogen carbonate + Acid ⟶ Salt + Water + Carbon dioxide

(d) Sulphide/hydrogen sulphite + Acid ⟶ Salt + Water + Sulphur dioxide

(e) Sulphide + Acid ⟶ Salt + Hydrogen sulphide

Solution B 2(a)

The acid formed when sulphur dioxide dissolves in water is sulphurous acid.

Solution B 2(b)

Carbondioxide gas is released when sodium carbonate is added to solution of sulphur dioxide.

Solution B 2(e)

Dilute sulphuric acid. 

Solution B 3

The name of the salt of

(a) Hydrogen sulphites and Sulphites.

(b) Sulphate and bisulphate.

Solution B 6

(i) B

(ii) C

(iii) A

(iv) A

Solution B 9


Column 1

Substance reacted with acid

Column 2

Dilute or concentrated acid

Column 3


Zinc Dilute sulphuric acid


 Calcium carbonate  Concentrated sulphuric acid

Carbon dioxide

 Bleaching power CaOCl2  Dilute sulphuric acid

Only chlorine

Solution C 1

(a) Two types of salts are formed when sulphuric acid reacts with NaOH because sulphuric acid is dibasic.

NaOH + H2SO4 NaHSO4 + H2O

2NaOH + H2SO4Na2SO4 + 2H2O

(b) A piece of wood becomes black when concentrated sulphuric acid is poured on it because it gives a mass of carbon.

(c) When sulphuric acid is added to sodium carbonate it liberates carbon dioxide which produces brisk effervescence.

Na2CO3+H2SO4Na2SO4 +H2O+CO2

Solution C 2

Water is not added to concentrated acid since it is an exothermic reaction. If water is added to the acid, there is a sudden increase in temperature and the acid being in bulk tends to spurt out with serious consequences.

Solution C 3

(a) Concentrated sulphuric acid is hygroscopic substance that absorbs moisture when exposed to air. Hence, it is stored in air tight bottles.

(b) Sulphuric acid is not a drying agent for H2S because it reacts with H2S to form sulphur.

H2SO4+H2S 2H2O+SO2+S

(c) Concentrated sulphuric acid has high boiling point (356oC). So, it is considered to be non-volatile. Hence, it is used for preparing volatile acids like Hydrochloric acid and Nitric acids from their salts by double decomposition.



Solution C 5



 S + H2SO4  3SO2 +2H2O.

(d) C12H22O11  + Conc. H2SO4  6C + 6H2O

(e) C12H22O11 + Conc. H2SO4→ 6C + 6H2O

(f) C + H2SO4 → CO2 + 2H2O + 2SO2.

Solution C 6

(a) BaCl2 + H2SO4  →   BaSO4↓ +  2HCl


(b) Na2S + H2SO4   →  Na2SO4  +  H2S↑


(c) ZnS + H2SO4 ZnSO4 + H2S↑


Solution C 9(c)

Sulphuric acid precipitates the insoluble sulphate of barium from the solution of barium chloride.

BaCl2 + H2SO4 BaSO4 + 2HCl

Dilute HCl does not react with barium chloride solution, and thus, no precipitate is produced in the reaction.

Solution C 11

(a) Zn + dil. H2SO4 ZnSO4 + H2 

(b) Na2CO3 + dil. H2SO4 Na2SO4 + H2O + CO2

(c) Pb(NO3) + dil. H2SO4 PbSO4  + 2HNO3

(d) Zn + dil. H2SO4 ZnSO4 + H2

ZnSO4 + Na2CO3 ZnCO3 + Na2SO4

Solution C 13

In the contact process for the manufacture of sulphuric acid, the equations for the conversion of sulphur trioxide to sulphuric acid are

 SO3 + H2SO4 H2S2O7

 (oleum or pyrosulphuric acid)

 H2S2O7 + H2O 2H2SO4

Solution D 1

(a) Due to its reducing property. i.e, it is a non-volatile acid.

NaCl+ H2SO4NaHSO4 + HCl


(b) It is a dehydrating agent.


(c) Acidic property: Magnesium is present above hydrogen in the reactivity series so sulphuric acid is able to liberate hydrogen gas by reacting with magnesium strip.

Mg + H2SO4 MgSO4+H2

(d) Due to its oxidizing character

Cu +H2SO4 CuSO4 +2H2O +SO2

(e) Due to its dehydrating property Hydrogen chloride gas is passed through concentrated sulphuric acid, it dries hydrogen chloride gas.

H2SO4 + H2O → H3O+ + HSO4


(i) Reaction with Ethanol -  dehydrating agent

(ii) Reaction with Carbon - oxidising agent


Solution D 2(a)

Sulphuric acid is powerful dehydrating agent on account of its strong affinity towards water.

Solution D 2(b)

Concentrated sulphuric acid as

 i. Oxidising agent:

 The oxidising property of conc. sulphuric acid its due to the fact that on thermal decomposition, it yeilds nacent oxygen [O].

 H2SO4 H2O + SO2 + [O] 

 ii. Non-volatile acid:

 conc. sulphuric acid has high boiling point (338°C) that why it is said to be a non volitile compound, therefore it is used for preparing volatile acids like hydrochloric acids, nitric acids from there salts by double decomposition

  H2SO4 + NaCl NaHSO4 + HCl

Solution 2

Balanced reactions are:

(a) Acidic nature:

(i) Dilute H2SO4 reacts with basic oxides to form sulphate and water.

2 NaOH+H2SO4 Na2SO4+2H2O

(ii) CuO+H2SO4 CuSO4+H2O

(iii) It reacts with carbonate to produce CO2.


(b) Oxidising agent:

H2SO4 H2O +SO2 +[O]

Nascent oxygen oxidizes non-metals, metals and inorganic compounds.

For example,

Carbon to carbon dioxide

C+H2SO4 CO2 +H2O +2SO2

Sulphur to sulphur dioxide

S +H2SO4 3SO2 +2H2O

(d) Non-volatile nature:

It has a high boiling point (356oC) so it is considered to be non-volatile. Therefore, it is used for preparing volatile acids like hydrochloric acid, nitric acid from their salts by double decomposition reaction.

NaCl + H2SO4NaHSO4 +HCl

KCl + H2SO4 KHSO4 +HCl

Solution 3

(a) When dilute hydrochloric acid is treated with lead nitrate, lead chloride formed is soluble in hot water and when dilute sulphuric acid is treated with lead nitrate lead sulphate formed does not dissolve in hot water.



1. Dilute sulphuric acid treated with zinc gives Hydrogen gas which bums with pop sound.

Concentrated H2SO4 gives SO2 gas with zinc and the gas turns Acidified potassium dichromate paper green.

2.Barium chloride solution gives white ppt. with dilute H2SO4, This white ppt. is insoluble in all acids.

Concentrated H2SO4 and NaCl mixture when heated gives dense white fumes if glass rod dipped in Ammonia solution is brought near it.

Solution 4

(a) When sulphuric acid reacts with sulphur the product formed is Sulphur dioxide is formed.

S +2H2SO4 3SO2 + 2H2O

(b) When sulphuric acid reacts with sodium hydroxide it neutralizes base to form sodium sulphate.

2NaOH + H2SO4 Na2SO4 + 2H2O

(c) When sulphuric acid reacts with sugar it forms carbon

C12 H22O1112C + 11H2O

(d) When sulphuric acid reacts with carbon it forms carbon dioxide and sulphur dioxide gas.

C +2H2SO4 CO2 + 2H2O + 2SO2

(e) When sulphuric acid reacts with copper it forms copper sulphate and sulphur dioxide.

Cu + H2SO4 CuSO4 + 2H2O + SO2

Solution A 1

(a) Hydrogen sulphide

Solution A 2

(b) Oxidising agent 

Solution A 3

(c) Lead nitrate

Solution B 2(c)

Liquid E is Ethanol.

Solution B 2(d)

Hydrogen Chloride.

Solution B 2(f)

Hydrogen Sulphide (H2S).

Solution B 2(g)

Sulphuric acid (H2SO4)

Solution B 2(h)

Concentrated sulphuric acid

Solution B 2(i)

Concentrated sulphuric acid.

Solution B 4

(a) The property of concentrated sulphuric acid which allows it to be used in is used in the action when sugar turns black in its presence is its dehydrating property. 

(b) The property of concentrated sulphuric acid which allows it to be used in the preparation of hydrogen chloride and nitric acid is its non-volatility.

H2SO+ BaCl2   BaSO+ 2HCl

Solution B 5

(a) Non-volatile nature

(b) as an oxidising agent

(c) dehydrating

Solution B 7

(a) (B) Dehydrating agent

(b) (D) Oxidising agent

(c) (C) Non-volatile acid

(d) (A) Dilute acid

(e) (D) Oxidising agent

Solution B 8


Name of process



Equation for catalyzed reaction output



Contact process

Sulphur dioxide + oxygen

Platinum or V2O5

2SO2 + O2  2SO3

Sulphuric acid

Solution C 4(a)

Charring of sugar takes place. Sulphuric acid dehydrates sugar leaving behind carbon which is black in colour.

Solution C 4(b)

When Conc. H2SO4 is added to a crystal of hydrated copper sulphate,it removes water of crystalisation from salt.

Solution C 10

Two conditions for the conversion of sulphur dioxide to sulphur trioxide is as follows: 

Temperature: 450-500° C Catalyst: V2O5


Solution C 12

(a) Action of sulphuric acid on potassium hydrogen carbonate

 2KHCO3+ H2SO4 K2SO4+ 2H2O + 2CO2 

(b) Action of sulphuric acid on sulphur

 S + 2H2SO4 3SO+ 2H2O

Solution C 14

ZnO + H2SO ZnSO4 + H2O. 

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