Study of Compounds-Nitric Acid Solutions for Class 10 Chemistry

Intex Questions

1. What is:

a)  Aqua Fortis: 

Ans: Nitric acid is called aqua Fortis. Aqua means water and Fortis means strong, it is so-called because nitric acid is a colorless liquid that is highly corrosive. It reacts with nearly all metals (except gold) and converts them to corresponding soluble nitrates. It can even dissolve silver which is not dissolved in any other acid. It has a molecular formula as HNO3. 

b)  Aqua Regia: 

Ans: Aqua regia (Latin for royal water) is a freshly prepared mixture of concentrated hydrochloric acid and concentrated nitric acid mixed in the ratio of 3 : 1 by volume. It can dissolve gold and platinum. The acids combine to evolve nascent chlorine (Cl). Nascent chlorine is very reactive and reacts with both gold and platinum. Hence, gold and platinum are soluble in it

3HCl + HNO3      \[\to \]  NOCl+2 H2O +2[Cl] 

Nitrosyl      Chloride        Nascent  

               Au +  3 [Cl]       \[\to \]  AuCl3

               Pt +  4 [Cl]        \[\to \] PtCl4

Aqua regia helps to remove the dull layer from the surface of gold giving it a shining look.

c) Fixation of Nitrogen: 

Ans: The process of converting atmospheric nitrogen (N2) into useful nitrogenous compounds such as ammonia etc. is known as fixation of nitrogen.  The triple bond of nitrogen breaks and nitrogen combines with hydrogen and oxygen to form the nitrogenous compounds.

2. During thunderstorms, rain water contains nitric acid. Explain with reactions.

Ans:  During thunderstorms, the nitrogen present in the atmosphere reacts with oxygen to form nitric oxide when lightning discharges. 

            N2+O2  \[\to \]  2 NO

                                Nitric oxide

 Nitric oxide is further oxidized to nitrogen dioxide.

         2 NO   +    O2    \[\to \]    2 NO2 

                                    Nitrogen Dioxide 

The nitrogen dioxide reacts with the atmospheric moisture or rain water in the presence of oxygen in air and forms nitric acid which is washed down during rain and combines with the salt present on the surface of the earth.

        4 NO2 +    2 H2O    +     O2    +    4 HNO3 

                                                          Nitric Acid 

3. Ammonia is used in the Ostwald process

a. Give the source of reactants used in this process.

Ans:  Dry ammonia (free from moisture) produced in Haber’s process and dry air free from carbon dioxide are the sources of reactants used in the Ostwald process.

b. Name the catalyst used in the process.

Ans:  Platinum is used as a catalyst in the process. Platinum catalyses the ammonia in the presence of oxygen to nitric oxide, which is further oxidised to nitrogen dioxide.

4 NH3  +   5O2 \[\to \]   4 NO  +  6 H2O    +     Heat  

c)   Name the oxidising agent used in this process.  

Ans: Oxygen is the oxidising agent used in this process, which oxidises the nitric oxide to nitrogen dioxide.

               2 NO        +         O2   \[\to \]     2 NO2 

          Nitric Oxide                                Nitrogen Dioxide

Nitrogen dioxide further undergoes hydrogenation in the presence of oxygen to form nitric acid.

d) What is the ratio of ammonia and air taken in this process?

Ans: The ratio of ammonia and air is taken in the process is 1:10. This means that 1 volume of ammonia will react with 10 volumes of air. 

e) Why is quartz used in this process?

Ans:  Quartz used in this process is acid-resistant and helps in the absorption of nitrogen dioxide in water in a uniform manner to form nitric oxide when packed in layers.

4. (a) Write a balanced chemical equation for the laboratory preparation of nitric acid.

Ans: The balanced chemical equation for the laboratory preparation of nitric acid is:

  KNO3              +          H2SO4    \[\to \]       KHSO4          +            HNO3

Potassium Nitrate        Conc.                                                   Nitric Acid

In the laboratory, nitric acid is prepared by distilling conc. sulphuric acid with potassium nitrate, KNO3 (nitre) or sodium nitrate, NaNO3 (Chile saltpetre).

b) In the preparation of nitric acid from KNO3. Concentrated hydrochloric acid is not used in place of concentrated sulphuric acid. Explain why.

Ans:  Concentrated hydrochloric acid cannot be used in place of conc. sulphuric acid in the preparation of nitric acid from KNO3 because hydrochloric acid is a volatile acid and hence nitric acid vapours will carry HCI vapours with it in the preparation of HNO3 and it will be difficult to get the nitric acid from the mixture. 

c) Conc. nitric acid prepared in the laboratory is yellow in colour. Why? How is this colour removed?

Ans:  Concentrated nitric acid prepared in the laboratory is yellow in color due to dissolution of reddish brown nitrogen dioxide gas in the acid.  Nitric acid is unstable to heat and sunlight and thermally decompose to form nitrogen dioxide gas as shown below:

              4 HNO3   \[\to \]    2 H2O     +      4 NO2          +    O2

The yellow color of the acid can be removed by bubbling the dry air or carbon dioxide, CO2 gas through the acid as it drives out the NO2 gas from the acid, which is further oxidised to form the colorless nitric acid. Also by adding excess water, nitrogen dioxide gas will dissolve in water and the yellow color of acid is removed and hence the colorless nitric acid is obtained.

d)  Give reasons for the following:

In the laboratory preparation of nitric acid, the mixture of concentrated sulphuric acid and sodium nitrate should not be heated very strongly above 200°C.

Ans:  In the laboratory preparation of nitric acid, the mixture of concentrated sulphuric acid and sodium nitrate should not be heated very strongly above 200°C because:

• Sodium sulphate formed at high temperature forms a hard crust that sticks to the wall of the retort and is quite difficult to remove. 

• Glass apparatus may be damaged at higher temperatures.

• At higher temperatures, the nitric acid also decomposes to give nitrogen dioxide.

5. (a) Nitric acid cannot be concentrated beyond 68% by the distillation of a dilute solution of HNO3. State the reason. 

Ans: The mixture of nitric acid with water forms a constant boiling mixture which is 68% concentrated nitric acid. This mixture boils with uniform composition at a constant boiling point. At this temperature, the volatile nitric acid and the water vapour escape having uniform composition. So nitric acid cannot be concentrated beyond 68% by distillation of a dilute solution of HNO3. 

(b) What is passive iron? How is passivity removed? 

Ans:  The iron becomes chemically inert or passive when dipped in concentrated nitric acid due to the formation of the thin layer of oxide Fe3O4 on its surface. This inert iron is known as passive iron.  Passivity can be removed by heating the passive iron with a strong reducing agent or by rubbing the surface of the passive iron with the sandpaper.

6. Name the product formed when:

a. Carbon and conc. nitric acid is heated 

Ans:   The products formed when carbon and conc. nitric acid is heated are carbon dioxide, nitrogen dioxide and water.

       C     +       4 HNO 3       \[\to \]        CO2   +     2 H2O       +  4 NO2

b. Dilute HNO3 is added to copper.

Ans:   The products formed when dilute HNO3 is added to copper are copper nitrate, nitric oxide and water.

     3 Cu     +       8 HNO 3      \[\to \]          3 Cu(NO3)2   +     4 H2O       +    4 NO

7.  Give two chemical equations for each of the following:

a) Reactions of nitric acid with non-metals.

Ans: Carbon and sulphur are the non-metals their reactions with nitric acid are as follows.

   C    +      4 HNO3       \[\to \]         CO2              +           2 H2O        +            4 NO2

   S    +      6 HNO3       \[\to \]       H2SO4           +          2 H2O         +            6 NO2

b) Nitric acid showing as acidic character.

Ans:  Metal oxides behave as alkalis, react with nitric oxide and undergo a neutralisation reaction to form the corresponding soluble metal nitrates and water.

   K2O        +      2 HNO3         \[\to \]         2KNO3       +           H2O

   ZnO       +       2 HNO3        \[\to \]           Zn(NO3)2    +            H2O

c) Nitric acid acting as oxidizing agent.

Ans: Nitric acid acts as a strong oxidizing agent and readily oxidises non-metals, metals, inorganic and organic compounds.

  P4     +   20 HNO3     \[\to \]        4 H3PO4            +        4 H2O       +            20 NO2

3 Zn    +    8 HNO3      \[\to \]       3 Zn(NO3)2   +        4 H2O       +             2 NO

8. Write balanced equations and name the products formed when:

(a) Sodium hydrogen carbonate is added to nitric acid.

Ans: Nitric acid reacts with carbonates and bicarbonates to give salt, water and carbon dioxide. Hence, when sodium hydrogen carbonate is added to nitric acid sodium nitrate, carbon dioxide and water are formed. 

     NaHCO3    +     HNO3     \[\to \]        NaNO3      +     H2O      +      CO2

b)  Cupric oxide reacts with dilute nitric acid

Ans: Cupric oxide is a metal oxide which behaves as alkali and undergo netralisation reaction when react with nitric acid. Hence, when cupric oxide reacts with dilute nitric acid, it forms copper nitrate salts, and water. 

       CuO       +     2 HNO3       \[\to \]       Cu(NO3)2    +         H2O 

c)  Zinc reacts with dilute nitric acid

Ans: Zinc reacts with nitric acid to form zinc nitrate, nitric oxide and water.

3 Zn    +    8 HNO3          \[\to \]        3 Zn(NO3)2         +      4 H2O       +     2 NO

Nitric acid reacts with all metals except platinum and gold.  The action of nitric acid and metals depends upon the concentration of nitric acid and temperature. Dilute nitric acid oxidises metals to their corresponding nitrates and evolves nitric oxide.

4. Concentrated nitric acid is heated

Ans: When concentrated nitric acid is heated it undergoes a decomposition reaction to form nitrogen dioxide gas, water and oxygen gas.

4 HNO3    \[\to \]     2 H2O      +      4 NO2         +     O2

9.  How will you prepare the following from nitric acid? 

(a) Sodium nitrate 

Ans:  Sodium hydroxide reacts with nitric acid to form sodium nitrate.

           NaOH       +         HNO3        \[\to \]         NaNO3      +       H2O

                                                                Sodium Nitrate 

(b) Copper nitrate

Ans: Copper oxide is a metallic oxide which behaves as basic oxide reacts with nitric acid and undergoes a neutralisation reaction  to form copper nitrate and water.

            CuO      +    2 HNO3       \[\to \]       Cu(NO3)2       +       H2O 

(c) Lead nitrate

Ans: Lead reacts with conc. nitric acid to form lead nitrate. Nitric acid reacts with metals to form metal nitrates and nitrogen dioxide.

     Pb      +     4 HNO3     \[\to \]      Pb(NO3)2       +     2 H2O     +       2 NO2

d) Magnesium nitrate

Ans: Dilute solution of nitric acid reacts with magnesium and manganese to give their nitrates and hydrogen gas. Hence, magnesium with dil. nitric acid forms magnesium nitrate and hydrogen  gas is evolved.

       Mg     +     2 HNO3       \[\to \]    Mg(NO3)2        +       H2

(e) Ferric nitrate 

Ans:  Iron does not react with dilute nitric acid as it forms a layer of oxide over its surface, but it reacts with concentrated nitric acid to form ferric nitrate and liberates nitrogen dioxide gas.

        Fe       +       6 HNO3       \[\to \]       Fe(NO3)3       +     3 H2O     +   3 NO2 

(f) Aqua regia 

Ans: Aqua regia (Latin for royal water) is a freshly prepared mixture of concentrated hydrochloric acid and concentrated nitric acid mixed in the ratio of 3:1 by volume. It can dissolve gold and platinum. The acids combine to evolve nascent chlorine (Cl). 

3 HCl    +    HNO3              \[\to \]             NOCl          +            2 H2O      +     2 [Cl] 

                                                                              Nitrosyl Chloride                            Nascent  

10.  Write the equation for the following conversions A, B. C and D.

Ans: 

Explanation: 

3 Cu       +   8 HNO3      \[\to \]     3 Cu(NO3)2    +    4 H2O    +  2 NO

2 Cu(NO3)2    \[\to \]   2 Cu    +    4 NO2     +    O2  (Decomposition)

2 Cu      +   O2    \[\to \]   2 CuO      (Oxidation)

CuO      +   H2    \[\to \]    Cu        +       H2O     (Reduction)

11:  Correct the following, if required:

a. HNO3 is a strong reducing agent

Ans: HNO3 is a strong reducing agent - Correct.

2. NaNO3  gives NO2  and O2 on heating.

Ans:  NaNO3 gives NO2  and O2 on heating- Incorrect

          NaNO3  gives NaNO2  and O2 on heating- Correct

c. Constant boiling nitric acid contains 80% nitric acid by weight.

Ans:  Constant boiling nitric acid contains 80% nitric acid by weight- Incorrect

          Constant boiling nitric acid contains 68% nitric acid by weight- Correct

4. Nitric acid remains colorless even when exposed to light.

Ans:  Nitric acid remains colorless even when exposed to light.- Incorrect

          Nitric acid turns yellow when exposed to light.- Correct

Exercise Questions 

1. Choose the correct answer

a. The nitrate salt which does not give a mixture of NO2 and O2 on heating is:

I. AgNO3  

II. KNO3

III. Cu(NO3)2

IV. Zn(NO3)2 

Solution: II. KNO3 is the nitrate salt which does not give a mixture of NO2 and O2 on heating.

The alkali metal nitrates such as sodium or potassium nitrates when heated melts into colourless liquids which decompose on heating to give oxygen gas.  The colorless liquid burns into flame due to the formation of oxygen gas when the glowing splinter is brought near.

   2 KNO3   \[\to \]       2  KNO2    +   O2 

                                       Colourless Crystalline 

(b) The chemical used in the brown ring test is:

I. CuSO4

II. FeSO4

III. Fe2(SO4)3

IV. ZnSO4 

Ans: II. The chemical used in the brown ring test is FeSO4.

Explanation:  The brown ring is formed at the junction of ferrous sulphate and sulphuric acid as the conc. sulphuric acid being heavier settles down and the ferrous sulphate layer remains above it resulting in the formation of a brown ring at the junction as the reaction given below:

      6 FeSO4  +  3 H2SO4  + 2 HNO3     \[\to \]     3 Fe2(SO4)3   + 4 H2SO4   +  NO   

                            FeSO4       +      NO    \[\to \]      FeSO4  . NO

                                                          (Nitroso Ferrous sulfate, a brown complex)

(c) Lead nitrate decomposes on heating to give:

I. NO

II. N2O

III. NO2

IV. N2O5

Ans: II. Lead nitrate decomposes on heating to give NO2.

 Lead nitrate decomposes on heating to give lead oxide, nitrogen dioxide and oxygen.

            2 Pb(NO3)2        \[\to \]        2 PbO    +   4 NO2    +    O2  

                                               Yellow solid

2.  Name 

a)  a nitrate of metal which on heating does not give nitrogen dioxide.

Ans:   A nitrate of metal that on heating does not give nitrogen dioxide is sodium nitrate.

b)  a nitrate which on heating leaves no residue behind.

Ans:  A nitrate that on heating leaves no residue behind is ammonium nitrate.

c) a metal nitrate which on heating is changed into metal oxide.

Ans: A metal nitrate that on heating is changed into metal oxide is calcium nitrate. 

d) a metal nitrate which on heating is changed into metal.

Ans: A metal nitrate that on heating is changed into metal oxide is mercury nitrate. 

e) a solution that absorbs nitric oxide.

Ans: A solution that absorbs nitric oxide is a ferrous sulfate solution.

f) the oxide of nitrogen which turns brown on exposure to air. How is it prepared? 

Ans: Nitric oxide is the oxide of nitrogen that turns brown on exposure to air.

               2 NO     +    O2        \[\to \]         NO2

            Nitric Oxide       Nitrogen Dioxide (brown gas)

Nitric oxide can be prepared during catalytic oxidation by platinum at 800C of ammonia as shown below:

                 4 NH3   +   5 O2  \[\to \]  4 NO  +  6 H2O    +     Heat    

Explanation:

Alkali metals such as sodium and potassium nitrate melts into colourless liquid on heating and decomposes to give oxygen.

2 NaNO3          \[\to \]         2 NaNO2       +    O2 

2 KNO3           \[\to \]          2 KNO2         +    O2 

When a glowing splinter is brought near the molten liquid, it burst into flames as oxygen gas is evolved.

All other nitrates except those of silver and mercury decompose to give their oxides, nitrogen dioxide and oxygen.

2 Ca(NO3)2   \[\to \]    2 CaO    +    4 NO2   +   O2 

                                                            Brown gas

2 Zn(NO3)2  \[\to \]      2 ZnO     +    4 NO2    +   O2 

2 Pb(NO3)2   \[\to \]     2 PbO     +    4 NO2    +   O2                                                        

2 Cu(NO3)2   \[\to \]     2 CuO    +    4 NO2    +   O2   

• Silver and mercury nitrates decompose to give their respective metals nitrogen dioxide and oxygen.

                2 AgNO3  \[\to \]    2 Ag    +    2 NO2    +   O2 

                2 Hg(NO3)2  \[\to \]     Hg      +    2 NO2    +   O2 

• Ammonium nitrate decomposes explosively to give no residue as N2O gas is evolved and water as steam evaporated leaving behind no residue.

                2 NH4NO3    \[\to \]     N2O(g)     +    2 H2O   

                                  Nitrous Oxide (Laughing gas)

• Ferrous sulphate solution absorbs nitric oxide to form nitroso ferrous sulphate, a brown complex. 

                2 FeSO4     +     H2O     +      NO     \[\to \]      [Fe (H2O)NO]SO4

                                                 Nitric Oxide            Brown Complex

• Nitric oxide turns brown on exposure to air due to formation of nitrogen dioxide (brown gas). Nitric oxide can be prepared by catalytic oxidation by platinum at 800C of ammonia.

3. Mention three important uses of nitric acid. Give the property of nitric acid involved in the use.

Ans:  

4. (a) Explain with the help of a balanced equation, the brown ring test for nitric acid. 

Ans:  In the brown ring test for nitric acid, the brown ring is formed at the junction of ferrous sulphate and sulphuric acid as the conc. sulphuric acid being heavier settles down and the ferrous sulphate layer remains above it resulting in the formation of a brown ring at the junction due to the formation of brown complex compound as the reaction given below:

6 FeSO4  +  3 H2SO4  + 2 HNO3    \[\to \]      3Fe2(SO4)3   + 4 H2SO4  +  NO   

                      FeSO4       +      NO   \[\to \]     FeSO4. NO

                                                 (Nitroso Ferrous sulphate, a brown compound)

b. Why is a freshly prepared ferrous sulphate solution used for testing the nitrate radical in the brown ring test?

Ans: A freshly prepared ferrous sulphate solution is used for testing the nitrate radical in the brown ring test because on exposure to the atmosphere, it is oxidised to ferric sulphate due to which it will not give the brown ring test.

5. From the following list of substances, choose one substance in each case that matches the description given below: 

Ammonium nitrate, calcium hydrogen carbonate, copper carbonate, lead nitrate, potassium nitrate, sodium carbonate, sodium hydrogen carbonate, zinc carbonate. 

A substance that gives off only oxygen when heated. 

Ans: Potassium nitrate gives off only oxygen when heated.

Alkali metals such as sodium and potassium nitrate melts into colourless liquid on heating and decompose to give oxygen.

2 NaNO3         \[\to \]           2 NaNO2     +    O2 

2 KNO3   \[\to \]        2 KNO2          +    O2 

When a glowing splinter is brought near the molten liquid, it burst into flames as oxygen gas is evolved.

b. A substance that on heating decomposes into dinitrogen oxide (nitrous oxide) and steam.

Ans: Ammonium nitrate on heating decomposes into dinitrogen oxide (nitrous oxide) and steam.

Ammonium nitrate decomposes explosively to give no residue as

2 NH4NO3       \[\to \]             N2O(g)     +    2 H2O   

                             Nitrous Oxide (Laughing gas)

c. A substance that gives off oxygen and nitrogen dioxide when heated. 

Ans: Lead nitrate off oxygen and nitrogen dioxide when heated.

Explanation:

All other nitrates except those of silver and mercury decompose to give their oxides, nitrogen dioxide and oxygen.

2 Ca(NO3)2    \[\to \]      2 CaO     +    4 NO2    +   O2 

                                                                     Brown gas

2 Zn(NO3)2    \[\to \]      2 ZnO     +    4 NO2    +   O2 

2 Pb(NO3)2     \[\to \]      2 PbO      +    4 NO2    +   O2                                                         

2 Cu(NO3)2    \[\to \]       2 CuO       +    4 NO2    +   O2   

d. A substance which on heating leaves yellow residue

Ans: Zinc carbonate on heating leaves yellow residue.

Explanation: 

Zinc carbonate on heating form zinc oxide and carbon dioxide gas is evolved leaving behind the yellow ZnO.

ZnCO3      \[\to \]         ZnO       +     CO2    +   O2 

                                        Yellow solid when hot,

                                            white when cold

6. The action of heat on the blue crystalline solid X, gives a reddish-brown gas Y, a gas that re-lights a glowing splint and leaves a black residue. When gas Z, which has a rotten egg smell, is passed through a solution of X. a black ppt. is formed.  

a. Identify X, Y, and Z. 

Ans: X is copper nitrate [Cu(NO3)2], Y is nitrogen dioxide [NO2] and Z is hydrogen sulfide [H2S].

b. Write an equation for the action of heat on X.

Ans: When copper nitrate [Cu(NO3)2] is heated, a brown color gas of nitrogen dioxide NO2 with oxygen gas is evolved leaving behind a black residue of copper oxide, CuO.  As oxygen gas is evolved, glowing splints will re-lights.

     2 Cu(NO3)2     \[\to \]        2 CuO     +    4 NO2    +   O2   

                                                          Reddish-brown

c. Write equation between the solution of X and gas Z.

Ans:      Cu(NO3)2      +     H2S      \[\to \]        CuS      +    2 HNO3  

Explanation: 

Salt of copper and their solution are blue in colour. Copper nitrate [Cu(NO3)2] is a blue crystalline solid X, when heated, gives  reddish-brown NO2 gas, oxygen gas which re-lights a glowing splint and leaves a black residue of CuO. 

         2 Cu(NO3)2     \[\to \]         2 CuO     +    4 NO2    +   O2   

                                                             Reddish-brown

When a H2S gas, which has a rotten egg smell, is passed through a solution of Cu(NO3)2, a black ppt. of CuS is formed.

2 Cu(NO3)2      +     H2S       \[\to \]           2 CuS      +    2 HNO3  

                                                              Black ppt.

7. X. Y and Z are three crystalline solids that are soluble in water and have a common anion. To help you to identify X. Y and Z, you are provided with the following experimental observations. Copy and complete the corresponding inferences in (a) to (e). 

a. A reddish-brown gas is obtained when X, Y and Z are separately warmed with concentrated sulphuric acid and copper turning added to the mixture. 

INFERENCE I: The common anion is the _____________ ion. 

Ans:  The common anion is the nitrate ion.

As the reddish-brown gas is obtained when X, Y, and Z are separately warmed with concentrated sulphuric acid when these have anion as nitrate which evolve into brown NO2 gas that intensifies when copper turning added to this acidified mixture.

      Metallic nitrates      \[\to \]         Metallic Oxides     +    NO2     +    O2  

b. When X is heated, it melts and gives off only one gas which re-lights a glowing splint. 

Inference 2: The cation in X is either __________ or ___________.

Ans: The cation in X is either sodium or potassium.

Sodium and potassium nitrates or alkali nitrates melts into colorless liquid on heating and decomposes to give oxygen.

2 NaNO3    \[\to \]         2 NaNO2      +    O2 

                        Slightly delinquent

KNO3    \[\to \]       KNO2   +   O2 

                Colorless Crystalline 

When the glowing splinter is brought near, the colorless liquid, it re-lights due to the evolution of oxygen gas.

c. The action of heat on Y produces a reddish-brown gas and a yellow residue which fuses with the glass of the test tube. 

Inference 3: The metal ion present in Y is the ___________ ion.

Ans: The metal ion present in Y is the lead ion.

Lead nitrate is Y which is a colorless crystalline solid when heated from a yellow solid of lead oxide which fuses with glass and reddish-brown nitrogen dioxide gas is evolved along with oxygen.

      2 Pb(NO3)2         \[\to \]           2 PbO    +   4 NO2    +    O2  

          Colorless                                     Yellow solid 

          Crystals                                   fuses with glass

d. When Z is heated, it leaves no residue. Warming Z with sodium hydroxide solution liberates a gas which turns moist red litmus paper blue. 

Inference 4: Z contains the __________ ion. 

Ans: Z contains the ammonium cation. 

Ammonium nitrate decomposes explosively to give no residue as N2O gas is evolved and water as steam evaporated leaving behind no residue.

2 NH4NO3    \[\to \]       N2O(g)     +    2 H2O   

                      Nitrous Oxide (Laughing gas)

When ammonium nitrate gives ammonia gas which is basic in nature and moist red litmus paper blue.

       2 NH4NO3       +       NaOH        \[\to \]          NaNO3     +     NH3      +      H2O  

e. Write the equations for the following reactions. 

(i) X and concentrated sulphuric acid (below 210° C). (One equation only for either of the cations given in INFERENCE 2). 

Ans: X can be sodium and potassium nitrates and their reactions with concentrated sulphuric acid (below 210°C) form. When sodium and potassium nitrates react with concentrated sulphuric acid form nitric acid.

      2 NaNO3       +       H2SO4        \[\to \]         Na2SO4     +        2 HNO3  

           KNO3       +       H2SO4       \[\to \]           KHSO4      +          HNO3  

(ii) Action of heat on Y. 

Ans: Y, which is lead nitrate decomposes on heat and form a yellow solid of lead oxide which fuses with glass and reddish-brown nitrogen dioxide gas is evolved along with oxygen.

      2 Pb(NO3)2    \[\to \]       2 PbO    +   4 NO2    +    O2  

          Colorless                             Yellow solid 

          Crystals                             fuses with glass

(iii) Concentrated nitric acid is added to copper turnings kept in a beaker. 

Ans: When concentrated nitric acid is added to copper turnings kept in a beaker, dense reddish-brown fumes of nitrogen dioxide gas are evolve.

Cu       +       4 HNO3      \[\to \]         Cu(NO3)2   +   2 H2O     +    2 NO2 

                                                                                            Reddish brown

8.(a) Dilute nitric acid is generally considered a typical acid except for its reaction with metals. In what way is dilute nitric acid different from other acids when it reacts with metals?

Ans: Generally, acids react with metals to form salts and hydrogen gas but not the same case with nitric acid. Dilute nitric acid is considered a typical acid except for its reaction with metals since it does not liberate hydrogen. It is a powerful oxidising agent and the nascent oxygen formed oxidises the hydrogen to water.

All metals (except Mn and Mg) react with dil. nitric acid to evolve nitrate salt of corresponding metal, water and nitric oxide.

3 Cu       +     8 HNO3        \[\to \]           3 Cu(NO3)2   +   4 H2O       +    2 NO

3 Zn       +     8 HNO3        \[\to \]            3 Zn(NO3)2   +   4 H2O       +    2 NO 

3 Fe       +     8 HNO3         \[\to \]           3 Fe(NO3)2   +   4 H2O       +    2 NO 

b. Write the equation for the reaction of dilute nitric acid and conc. nitric acid with copper. 

Ans: The equation for the reaction of dilute nitric acid and conc. nitric acid with copper is:

Reaction with dil. HNO3:

3 Cu       +     8 HNO3        \[\to \]          3 Cu(NO3)2   +   4 H2O       +    2 NO

Reaction with conc.HNO3:

 Cu       +     4 HNO3         \[\to \]          3 Cu(NO3)2     +    2 H2O      +    2 NO2

9.  Explain why

a. Only all-glass apparatus should be used for the preparation of nitric acid by heating concentrated sulphuric acid and potassium nitrate. 

Ans: Only all-glass apparatus should be used for the preparation of nitric acid by heating concentrated sulphuric acid and potassium nitrate because fumes of nitric acid formed during the reaction are acidic and highly corrosive and react with cocks, rubber etc. if used as stopper.

b. Nitric acid is kept in a reagent bottle for a long time.

Ans: Nitric acid is kept in a reagent bottle for a long time because pure nitric acid is unstable to sunlight and heat and to avoid its decomposition it is kept in reagent bottle.

4 HNO3      \[\to \]         O2    +    2 H2O      +    2 NO2  

Due to the formation of brown NO2 gas, nitric acid turns yellowish in color because of the dissolution of NO2 gas in HNO3. 

10. The figure given below illustrates the apparatus used in the laboratory preparation of nitric acid.

a. Name A (a liquid), B (a solid) and C (a liquid). (Do not give the formulae). 

Ans: A(a liquid) is concentrated sulphuric acid, B (a solid) is sodium nitrate or potassium nitrate and C (a liquid) is nitric acid.

b. Write an equation to show how nitric acid undergoes decomposition. 

Ans: Nitric acid decomposes to liberate nitrogen dioxide along with oxygen and form water.

         4 HNO3      \[\to \]         O2    +    2 H2O      +    2 NO2  

c. Write the equation for the reaction in which copper is oxidized by concentrated nitric acid. 

Ans: Copper metal is oxidized by concentrated nitric acid to copper nitrate.

            Cu    +      4 HNO3     \[\to \]      Cu(NO3)2     +      2 H2O    +      2 NO2

11. 

a. A dilute acid B does not normally give hydrogen when reacted with metals but does give a gas when reacts with copper. Identify B. Write equation with copper. 

Ans: Acid B is nitric acid as it oxidises the hydrogen formed when reacted with metals to form water and hence does not normally give hydrogen gas. Nitric acid reacts with copper to evolve nitrogen dioxide gas.

       Cu       +     4 HNO3     \[\to \]        3 Cu(NO3)2     +    2 H2O      +    2 NO2

b. Complete the table: 

Ans:

c. What is the property of nitric acid which allows it to react with copper? 

Ans: Oxidising property of nitric acid allows it to react with copper.

d. State one observation:

i) Concentrated nitric acid is reacted with sulphur.

Ans: When concentrated nitric acid is reacted with sulphur, dense brown fumes of nitrogen dioxide are observed. 

               S       +     6 HNO3    \[\to \]          H2SO4      +    H2O      +   6 NO2

ii) Lead nitrate is heated strongly in a test tube.

Ans: Lead nitrate decomposes on heating strongly in a test and brown gas of nitrogen dioxide is observed.

           2 Pb(NO3)2      \[\to \]      2 PbO    +   4 NO2    +    O2  

                                                             Yellow solid

2012: 

a. Name - the gas produced when copper reacts with conc. nitric acid.

Ans: Nitrogen gas is evolved when copper reacts with conc. nitric acid.

       Cu    +    4 HNO3     \[\to \]      Cu(NO3)2   +   2 H2O       +    2 NO2 

                                                                                               Reddish brown

b. State observation - zinc nitrate crystals are strongly heated.

Ans:  When zinc nitrate crystals are strongly heated, brown fumes of nitrogen dioxide gas is observed leaving behind the yellow residue of zinc oxide which turns white when cooled.

         2 Zn(NO3)2    \[\to \]        2 ZnO       +    4 NO2    +   O2 

                                                          Yellow(when hot), 

                                                          white(when cold)

c. Correct the statement: 

Magnesium reacts with nitric acid to liberate hydrogen gas.

Ans:  Magnesium reacts with nitric acid to liberate hydrogen gas.- Incorrect

Magnesium reacts with dilute nitric acid to liberate hydrogen gas. - Correct.

Very dilute (about 1%) acid reacts with magnesium (and manganese) at room temperature to give its nitrates and hydrogen gas. The oxidizing action of the acid is much reduced due to the dilution of the acid.

           Mg     +      2 HNO3     \[\to \]      Mg(NO3)2    +      H2

                                       (Very Dilute)

d. Iron is rendered passive with fuming HNO3.

Ans:  Iron forms a thin layer of insoluble iron oxide with fuming HNO3 which makes it passive (or inert). 

e. Give the balanced equation for dilute nitric acid and copper carbonate.

Ans:       CuCO3   +  2 HNO3    \[\to \]     Cu(NO3)2     +     H2O     +    CO2

2013:

a. Identify the gas evolved when.

i) Sulphur is treated with conc. nitric acid.  

Ans:  Nitrogen dioxide gas is evolved when sulphur is treated with conc. nitric acid.

         S    +      6 HNO3     \[\to \]      H2SO4         +       2H2O      +        6 NO2

ii) A few crystals of KNO3 are heated in a hard glass test tube.

Ans:  Oxygen gas is evolved when a few crystals of KNO3 are heated in a hard glass test tube.

          2 KNO3  ⟶    2 KNO2    +   O2  

b. State two relevant observations for lead nitrate crystals heated in a hard glass test tube. 

Ans: The two relevant observations for lead nitrate crystals heated in a hard glass test tube are:

i) Brown fumes of nitrogen dioxide gas evolved.

ii) Yellow solid PbO which fuses with glass is formed as a residue.

    2 Pb(NO3)2      \[\to \]        2 PbO    +   4 NO2    +    O2  

                                                 Yellow solid

c. Give a balanced equation for oxidation of carbon with conc. HNO3. 

Ans: The balanced equation for oxidation of carbon with conc. HNO3 is:

            C     +       4 HNO3     \[\to \]     CO2   +     2 H2O   +  4 NO2

                              conc.

2014:

a. Fill In the blank 

Cold dil. nitric acid reacts with copper to form _________ (hydrogen, nitrogen dioxide. nitric oxide).

Ans: Cold dil. nitric acid reacts with copper to form nitric oxide.

      3 Cu     +       8 HNO3     \[\to \]         3 Cu(NO3)2   +     4 H2O     +    4 NO

                                                                                                           Nitric oxide

b. Give balanced equations for the following:

I.  Laboratory preparation of nitric acid. 

Ans:   KNO3      +    H2SO4       \[\to \]          2 KHSO4       +     HNO3

                                       Conc.

NaNO3      +    H2SO4       \[\to \]       2 NaHSO4       +    HNO3

                          Conc.

Nitrate acid is prepared in the laboratory by heating the sodium or potassium nitrate salt above 200C with concentrated sulphuric acid.

II. The action of heat on a mixture of copper and nitric acid.

Ans:  Cu       +       4 HNO3      \[\to \]        Cu(NO3)2   +   2 H2O       +    2 NO2

                                                           Reddish brown 

2015

a. Identify the acid 

I. Which is used for the preparation of non-volatile acid.

Ans:  Nitric acid is used for the preparation of non-volatile acid

              S    +   6 HNO3     \[\to \]    H2SO4           +    2H2O      +      6 NO2

                                              Non-volatile Acid

II. The acid is prepared by catalytic oxidation of ammonia. 

Ans:  Nitric acid is the acid which is prepared by catalytic oxidation of ammonia.

                               4 NH3   +   5 O2 \[\to \]  4 NO  +  6 H2O    +     Heat  

                                           2 NO + O2  \[\to \]   2 NO2 

                         4 NO2 + 2 H2O  +   O2    \[\to \]   4 HNO3 

b. State one appropriate observation; when crystals of copper nitrate are heated in a test tube. 

Ans: When crystals of copper nitrate are heated in a test tube, the evolution of brown gas of nitrogen dioxide is observed.

             2 Cu(NO3)2      \[\to \]        2 CuO       +    4 NO2    +   O2  

                                                                     Reddish-brown 

c. Explain the following: 

I. Dil. HNO3 is generally considered a typical acid but not so in the reaction with metals. 

Ans: Generally acids react with the metal to evolve hydrogen gas but not so for the reaction of dil. HNO3 with metals because nitric acid acts as an oxidizing agent and oxidizes the evolved hydrogen gas to water. Hence, dil. HNO3 is not considered a typical acid.

II. When it is left standing in a glass bottle concentrated nitric acid appears yellow. 

Ans: Concentrated nitric acid is unstable to sunlight and heat and so decomposes when it is left standing in a glass bottle. 

         4 HNO3    \[\to \]     O2    +    2 H2O      +    2 NO2 

                                                                 Reddish brown 

The formed brown nitrogen dioxide gas dissolves in the nitric acid due to which it appears yellow in color.

III. In the laboratory preparation of nitric acid, an all-glass apparatus is used. 

Ans: Nitric acid is a highly corrosive acid, the fumes of nitric acid can corrode the cork, and rubber is used as a stopper in the laboratory preparation of nitric acid so as to avoid corrosion of the apparatus an all-glass apparatus is used.

Introduction to Nitric Acid

Many industrial and commercial products are manufactured using nitric acid, which is one of the most important compounds. Thus, it is very important for science students to become familiar with nitric acid early on and obtain a thorough understanding. This chapter basically encapsulates the essence of this topic because students learn about the laboratory procedure of preparing nitric acid from potassium nitrate or sodium nitrate in this chapter. In addition, Chemistry Class 10 Solutions for Chapter 10 directs students to examine the experiments from the viewpoint of reactants, equations, settings, products, conditions, diagrams, precautions, and collections.

The synthesis of nitric acid was first recorded around 1500. Nitric acid is also known as aqua fortis and spirits of nitre. Alchemical work in the year 800 AD by Jabir ibn Hayyan a.k.a. Gerber.

• HNO₃ is the formula for the reaction

• with a molecular mass of 63.01 grams per mole

• densities of 1.51 grams/cubic centimetre

• with boiling points of 83°C

• and melting points of -42°C

The acid has a pungent odour and a suffocating smell. It is highly toxic to inhale and highly corrosive to metals and tissues.

As part of acid rain, nitric acid is emitted. Water vapour in the air and nitrogen oxides emitted from automobile engines combine to form nitric acid. When this acid rain falls to earth, it causes harm to plants and animals.

It is prepared by oxidizing nitrogen dioxide (NO₂) in the presence of a platinum catalyst at high temperatures (Ostwald process) to form nitric oxide. Commercially, nitric acid is produced by oxidizing anhydrous ammonia to nitric oxide.

Students preparing for the board exams can find maximum information in Solutions for Class 10 Study of Compounds Nitric Acid. The answers to the questions are step-by-step and simple to understand. Using them, students can very quickly understand the concepts behind the solutions. Students will not only benefit by being more prepared to answer all sorts of questions in examinations, but they will also have a better chance of retaining the information. During the chapter on Nitric Acid Solutions Class 10, students are encouraged to answer questions in a correct manner so that they can achieve maximum marks.

Preparation Tips for Class 10 Chemistry Exam

Learn the topics covered in your Chemistry textbooks like acids, bases, salts, and carbon and its compounds, and analyze how these topics apply to real-life scenarios, as science can be found in everything.

Solve Sample Papers

Exam simulation helps you test your skills in a real exam room. By solving sample papers, you get the chance to create the atmosphere of an exam room. You will be able to think fast in stressful situations when you are using this strategy. This is great if you want to practice in preparation for exams.

Use Mnemonics

In your Chemistry syllabus, there are many topics that require more memorization rather than solving, which is a difficult challenge for all students. Mnemonics are useful when dealing with such topics as they are creative tools that aid in the retention of information. 

A Study from the Prescribed Textbooks

ICSE Board question papers are based strictly on the syllabus that the board sets, so it is an absolute must that you examine your prescribed textbooks rather than relying on too many other sources. 

Always Balance the Equations

Regardless of what the question requires, you should write chemically balanced equations. Make a list of balanced equations and use mnemonics to remember them all if you are having difficulty memorizing them.