Class 10 SELINA Solutions Chemistry Chapter 10 - Study of Compounds C. Nitric Acid
Study of Compounds C. Nitric Acid Exercise Intext 1
Solution 1
(a) Aqua fortis: Nitric acid is called aqua fortis. Aqua fortis means strong water. It is so called because it reacts with nearly all metals.
(b) Aqua Regia: Conc. Nitric acid (1part by volume) when mixed with conc. Hydrochloric acid (3 parts by volume) gives a mixture called aqua regia. It means Royal water.
HNO3 +3HCl 
NOCl +2H2O +2[Cl]
(c) Fixation of Nitrogen: The conversion of free atmospheric nitrogen into useful nitrogenous compounds in the soil is known as fixation of atmospheric nitrogen.
Solution 2
During lightning discharge, the nitrogen present in the atmosphere reacts with oxygen to form nitric oxide.
N2+ O2 
2NO
Nitric oxide is further oxidized to nitrogen dioxide.
2NO +O22NO2
The nitrogen dioxide dissolves in atmospheric moisture in the presence of oxygen of the air and forms nitric acid which is washed down by the rain and combines with the salt present on the surface of the earth.
4NO2+2H2O +O2 
4HNO3
Solution 3
(a) A mixture of air and dry ammonia in the ratio of 10:1 by volume
(b) Platinum gauze
(c) Oxygen
(d) ammonia : dry air :: 1 : 10
(e) Quartz is acid resistant. When packed in layers, it helps in dissolving nitrogen dioxide uniformly in water.
Solution 4
(a)Chemical equation is:
KNO3 +H2SO4 
KHSO4 +HNO3
(b) Concentrated hydrochloric acid cannot replace Conc. Sulphuric acid for the preparation of nitric acid because hydrochloric acid is volatile acid and hence nitric acid vapours will carry HCl vapours.
(c) Conc. Nitric acid prepared in the laboratory is yellow in colour due to the dissolution of reddish brown coloured nitrogen dioxide gas in acid. This gas is produced due to the thermal dissociation of a portion of nitric acid.
4HNO3 
2H2O + 4NO2 + O2
The yellow colour of the acid is removed:
If dry air or CO2 is bubbled through the yellow acid, the acid turns colourless because it drives out NO2 from warm acid which is further oxidized to nitric acid.
By addition of excess of water, nitrogen dioxide gas dissolves in water and thus the yellow colour of the acid is removed.
(d)The temperature of the mixture of concentrated sulphuric acid and sodium nitrate should not exceed 200oC because sodium sulphate formed at higher temperature forms a hard crust which sticks to the walls of the retort and is difficult to remove. At higher temperature nitric acid may also decompose.
NaNO3 + NaHSO4 
Na2SO4 + HNO3
Solution 5(a)
Nitric acid forms a constant boiling mixture with water containing 68% acid. This mixture boils constantly at constant boiling point without any change in its composition. At this temperature, the gas and the water vapour escape together. Hence the composition of the solution remains unchanged. So nitric acid cannot be concentrated beyond 68% by distillation of dilute solution of HNO3.
Solution 5(b)
Iron becomes inert when reacted with nitric acid due to the formation of extremely thin layer of insoluble metallic oxide which stops the reaction.
Passivity can be removed by rubbing the surface layer with the sand paper or by treating with strong reducing agent.
Solution 6
(a) When carbon and conc. Nitric acid is heated the products formed are Carbon dioxide, Nitrogen dioxide and water.
C + 4HNO3 
CO2 + 2H2O +4NO2
(b) Copper when reacts with dilute HNO3 forms Copper nitrate, Nitric oxide and water.
3Cu + 8 HNO3 3Cu(NO3) 2 +4H2O + 2NO
Solution 7
(a) Reaction of nitric acid with non-metals:
C + 4HNO3 
CO2 + 2H2O + 4 NO2
S + 6 HNO3 H2SO4 + 2H2O + 6 NO2
(b) Nitric acid showing acidic character:
K2O + 2HNO3 2KNO3 + H2O
ZnO + 2HNO3 Zn(NO3)2 + H2O
(c) Nitric acid acting as oxidizing agent
P4 +20HNO3 4H3PO4 + 4H2O + 20NO2
3Zn +8HNO3 3Zn(NO3)2 +4H2O +2NO
Solution 8
(a) When Sodium hydrogen carbonate is added to nitric acid sodium nitrate, carbon dioxide and water is formed.
NaHCO3 + HNO3 
NaNO3 +H2O +CO2
(b) When Cupric oxide reacts with dilute nitric acid, it forms Copper nitrate.
CuO +2HNO3 Cu(NO3)2 +H2O
(c) Zinc reacts with nitric acid to form Zinc nitrate, nitric oxide and water.
3 Zn +8HNO3 3Zn(NO3)2 +4H2O +2NO
(d) 4HNO32H2O + 4NO2 + O2
Solution 9
(a) Sodium nitrate:
NaOH + HNO3 
NaNO3 +H2O
Sodium hydroxide reacts with nitric acid to form sodium nitrate.
(b) Copper nitrate:
CuO + 2HNO3 Cu(NO3)2 + H2O
Copper oxide reacts with nitric acid to form copper nitrate.
(c) Lead nitrate:
Pb +4HNO3 Pb(NO3)2 +2H2O +2NO2
Lead reacts with conc. nitric acid to form lead nitrate.
(d) Magnesium nitrate:
Mg +2HNO3 Mg(NO3)2 +H2
Magnesium with dil. nitric acid to form magnesium nitrate.
(e) Ferric nitrate:
Fe + 6HNO3 Fe(NO3)3 +3H2O + 3NO2
Iron reacts with conc. nitric acid to form ferric nitrate.
(f) Aqua regia:
HNO3 + 3HCl NOCl +2H2O +2[Cl]
Nitric acid reacts with hydrochloric acid to form a mixture called aqua regia.
Solution 10
A: Copper can be converted into copper nitrate.
3Cu + 8HNO3 
3Cu(NO3)2 + 4H2O+ 2NO
B:2Cu(NO3)2 
2CuO + 4NO2 + O2
C:2Cu+ O2 2CuO
D:By reduction
2CuO + C 2Cu + CO2
Solution 11
(a) HNO3 is strong oxidizing agent.
(b) NaNO3 gives NaNO2 and oxygen on heating.
(c) Constant boiling nitric acid contains 68% nitric acid by weight.
(d) Nitric acid turns yellow solution when exposed to light.
Study of Compounds C. Nitric Acid Exercise Ex. 10
Solution 1
(a)KNO3
(b) FeSO4
(c) NO2
Solution 2
(a) Sodium nitrate
2NaNO3 
2NaNO2 +O2
(b) A nitrate which on heating leaves no residue behind- Ammonium nitrate.
(c) A metal nitrate which on heating is changed into metal oxide- Calcium nitrate
(d) A metal nitrate which on heating is changed into metal- Silver nitrate
(e) A solution which absorbs nitric oxide- Freshly prepared ferrous sulphate
(f) The oxide of nitrogen which turns brown on exposure to air. - nitric oxide
By catalytic oxidation of ammonia.
4 NH3 + 5 O2 
4 NO + 6 H2O + Heat
Solution 3
(a) Three important uses of Nitric acid and the property of nitric acid involved is:
|
S.NO. |
Use |
Property |
|
1. |
To etch designs on copper and brassware. |
Nitric acid act as solvent for large number of metals. |
|
2. |
To purify gold. |
Impurities like Cu, Ag, Zn, etc. dissolve in nitric acid. |
|
3. |
Preparation of aqua regia. |
Dissolves noble metals. |
(b) Brown ring test
Procedure:
(i) Add freshly prepared saturated solution of iron (II)sulphate to the aq. solution of nitric acid.
(ii) Now add conc. Sulphuric acid carefully from the sides of the test tube, so that it should not fall drop wise in the test tube.
(iii) Cool the test tube in water.
(iv) A brown ring appears at the junction of the two liquids.
(c) A freshly prepared ferrous sulphate solution is used because on exposure to the atmosphere, it is oxidized to ferric sulphate which will not give the brown ring.
Solution 4
(a) Potassium nitrate
(b) Ammonium nitrate
(c) Lead nitrate
(d) Lead nitrate
Solution 5
a. X is copper nitrate.
Y is nitrogen dioxide.
Z is hydrogen sulphate.
b. 
c. 
Solution 6
(a) Nitrate.
(b) Sodium or potassium
(c) Lead
(d) Ammonia
(e) (1)KNO3 + H2SO4 
KHSO4 + HNO3
(2) 2Pb(NO3)2 
2PbO + 4NO2 +O2
(3) Cu +4HNO3 
Cu(NO3)2 +H2O +2NO2
Solution 7
a. Dilute nitric acid is generally considered a typical acid except for its reaction with metals because it does not liberate hydrogen. It is a powerful oxidising agent, and nascent oxygen formed oxidises hydrogen in water.
b.
i. Reaction of dilute nitric acid with copper:
3Cu + 8HNO3→ 3Cu(NO3) + 4H2O + 2NO
ii. Reaction of conc. nitric acid with copper:
Cu + 4HNO3→ Cu(NO3) + 2H2O + 2NO2
Solution 8
a. The glass apparatus is purposely used because nitric acid vapours are highly corrosive in nature and corrode cork, rubber etc. if used as a stopper.
b. Pure nitric acid is unstable to heat or sunlight. In the presence of sunlight, it decomposes even at room temperature.
Nitric acid stored in a bottle turns yellow. This colour is due to dissolved NO2 in HNO3. To avoid decomposition, nitric acid is normally stored in coloured bottles.
Solution 9
a. A (a liquid): Conc. sulphuric acid
B (a solid): Sodium nitrate
C (a liquid): Nitric acid
b.
c.
i. Reaction of dilute nitric acid with copper:
3Cu + 8HNO3→ 3Cu(NO3) + 4H2O + 2NO
ii. Reaction of conc. nitric acid with copper:
Cu + 4HNO3→ Cu(NO3) + 2H2O + 2NO2
Solution 10
a. The dilute acid is nitric acid.
Reaction of dilute nitric acid with copper:
3Cu + 8HNO3 →3Cu(NO3) + 4H2O + 2NO
b.
|
Name of Process |
Inputs |
Equations |
Output |
|
Ostwald process |
Ammonia + Air |
|
Nitric acid |
c. Its oxidising property allows it to react with copper.
d.
(i) Reddish brown gas of NO2 is observed.
(ii) Yellow solid is formed which fuses with glass.
Solution 2012
a. Nitrogen dioxide gas is produced when copper reacts with conc. HNO3.
b. When zinc nitrate crystals are strongly heated, they decompose into yellow-coloured zinc oxides and nitrogen dioxides, and oxygen gas is liberated.
c. Very dilute (about 1%) acid reacts with magnesium at room temperature to give magnesium nitrate and hydrogen gas.
d. Iron is rendered passive with fuming HNO3. This is due to the formation of insoluble metallic oxide which stops the reaction.
e. 
Solution 2013
a.
i. When sulphur is treated with conc. nitric acid, it produces nitrogen dioxide gas.
ii. When a few crystals of KNO3 are heated in a hard glass test tube, it decomposes to form KNO2, and O2 gas is librated.
b. First, it decomposes with slight decrepitation, and second, it is reddish brown in colour when hot. After cooling, it turns yellow and fuses in glass.
c. 
Solution 2014
a. Nitric oxide
b.
i. 
ii. Reaction of dilute nitric acid with copper:
3Cu + 8HNO3→ 3Cu(NO3) + 4H2O + 2NO Reaction of conc. nitric acid with copper:
Cu + 4HNO3→ Cu(NO3) + 2H2O + 2NO2
Solution 2015 (a)
(i) Sulphuric acid
(ii) Nitric acid
Solution 2015 (b)
Reddish brown nitrogen dioxide gas is released, and the residue left behind is black copper oxide.
Solution 2015 (c)
(i) Dilute nitric acid is generally considered a typical acid but not in its reaction with metals, because the action of nitric acid on metals depends on the temperature and concentration of nitric acid. These conditions are not required in case of hydrochloric acid or sulphuric acid.
(ii) Although pure concentrated nitric acid is colourless, it appears yellow when left standing in a glass bottle due to the dissolution of reddish brown nitrogen dioxide gas in the acid. Nitrogen dioxide is produced because of the thermal decomposition of a portion of nitric acid.
4HNO3 → 2H2O + 4NO2 + O2
(iii) An all-glass apparatus is used in the laboratory preparation of nitric acid, because nitric acid vapour corrodes rubber and cork.
