{"id":16374,"date":"2017-07-20T05:46:29","date_gmt":"2017-07-20T00:16:29","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=16374"},"modified":"2019-08-27T16:51:30","modified_gmt":"2019-08-27T11:21:30","slug":"selina-icse-solutions-class-10-chemistry-study-compounds-nitric-acid","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/selina-icse-solutions-class-10-chemistry-study-compounds-nitric-acid\/","title":{"rendered":"Selina Concise Chemistry Class 10 ICSE Solutions Study of Compounds – Nitric Acid"},"content":{"rendered":"
APlusTopper.com provides step by step solutions for Selina Concise ICSE Solutions for Class 10 Chemistry Chapter 10 Nitric Acid. You can download the Selina Concise Chemistry ICSE Solutions for Class 10 with Free PDF download option. Selina Publishers Concise Chemistry for Class 10 ICSE Solutions all questions are solved and explained by expert teachers as per ICSE board guidelines.<\/p>\n
Download Formulae Handbook For ICSE Class 9 and 10<\/a><\/p>\n ICSE Solutions<\/a>Selina ICSE Solutions<\/a><\/p>\n Selina ICSE Solutions for Class 10 Chemistry Chapter 10\u00a0Study of Compounds – Nitric Acid<\/strong><\/p>\n Exercise 1<\/strong><\/span><\/p>\n Solution 1.<\/strong><\/span><\/p>\n (a) Aqua fortis: Nitric acid<\/a> is called aqua fortis. Aqua fortis means strong water. It is so called because it reacts with nearly all metals.<\/p>\n (b) Aqua Regia:\u00a0Conc. 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. (c) Fixation of Nitrogen: The conversion of free atmospheric nitrogen into useful nitrogenous compounds in the soil is known as fixation of atmospheric nitrogen.<\/p>\n Solution 2.<\/strong><\/span><\/p>\n During lightning discharge, the nitrogen present in the atmosphere reacts with oxygen to form nitric oxide. Solution 3.<\/strong><\/span><\/p>\n (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. (d)The temperature of the mixture of concentrated sulphuric acid and sodium nitrate should not exceed 200o<\/sup>C 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. Solution 4.<\/strong><\/span><\/p>\n 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<\/sub>.<\/p>\n Solution 5.<\/strong><\/span><\/p>\n Iron becomes inert when reacted with nitric acid due to the formation of extremely thin layer of insoluble metallic oxide which stops the reaction. Solution 6.<\/strong><\/span><\/p>\n (a) When carbon and conc. Nitric acid is heated the products formed are Carbon dioxide, Nitrogen dioxide and water. (b) Copper when reacts with dilute HNO3<\/sub>\u00a0forms Copper nitrate, Nitric oxide and water. Solution 7.<\/strong><\/span><\/p>\n (a) Reaction of nitric acid with non-metals: (b) Nitric acid showing acidic character: (c) Nitric acid acting as oxidizing agent Solution 8.<\/strong><\/span><\/p>\n (a) When Sodium hydrogen carbonate is added to nitric acid sodium nitrate, carbon dioxide and water is formed. (b) When Cupric oxide reacts with dilute nitric acid, it forms Copper nitrate. (c) Zinc reacts with nitric acid to form Zinc nitrate, nitric oxide and water. (d) 4HNO3<\/sub>\u00a0\u2192 2H2<\/sub>O + 4NO2<\/sub>\u00a0+ O2<\/sub><\/p>\n Solution 9.<\/strong><\/span><\/p>\n <\/p>\n Solution 10.<\/strong><\/span><\/p>\n (a) Sodium nitrate: (b) Copper nitrate: (c) Lead nitrate: (d) Magnesium nitrate: (e) Ferric nitrate: (f) Aqua regia: Solution 11.<\/strong><\/span><\/p>\n (a) HNO3<\/sub>\u00a0is strong oxidizing agent. Solution 12.<\/strong><\/span><\/p>\n <\/p>\n Solution 13.<\/strong><\/span><\/p>\n The chemical name of the brown ring is Nitroso ferrous sulphate. Solution 14.<\/strong><\/span><\/p>\n Three important uses of Nitric acid and the property of nitric acid involved is:<\/p>\n
\nHNO3<\/sub>\u00a0+3HCl\u00a0\u2192 NOCl +2H2<\/sub>O +2[Cl]<\/p>\n
\n
\nThe 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.
\n4NO2\u00a0<\/sub>+ 2H2<\/sub>O + O2<\/sub>\u00a0\u2192 4HNO3<\/sub><\/p>\n
\n(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.<\/p>\n
\n4HNO3<\/sub>\u00a0\u2192 2H2<\/sub>O + 4NO2<\/sub>\u00a0+ O2
\n<\/sub>The yellow colour of the acid is removed:
\nIf dry air or CO2<\/sub>\u00a0is bubbled through the yellow acid, the acid turns colourless because it drives out NO2<\/sub>\u00a0from warm acid which is further oxidized to nitric acid.
\nBy addition of excess of water, nitrogen dioxide gas dissolves in water and thus the yellow colour of the acid is removed.<\/p>\n
\n<\/p>\n
\nPassivity can be removed by rubbing the surface layer with the sand paper or by treating with strong reducing agent.<\/p>\n
\nC + 4HNO3<\/sub>\u00a0\u2192 CO2<\/sub>\u00a0+ 2H2<\/sub>O + 4NO2<\/sub><\/p>\n
\n3Cu + 8 HNO3<\/sub>\u00a0\u2192 3Cu(NO3<\/sub>)\u00a02<\/sub>\u00a0+ 4H2<\/sub>O + 2NO<\/p>\n
\nC + 4HNO3<\/sub>\u00a0\u2192 CO2<\/sub>\u00a0+ 2H2<\/sub>O + 4 NO2
\n<\/sub>S + 6 HNO3<\/sub>\u00a0\u2192 H2<\/sub>SO4<\/sub>\u00a0+ 2H2<\/sub>O + 6 NO2<\/sub><\/p>\n
\nK2<\/sub>O + 2HNO3<\/sub>\u00a0\u2192 2KNO3<\/sub>\u00a0+ H2<\/sub>O
\nZnO + 2HNO3<\/sub>\u00a0\u2192 Zn(NO3<\/sub>)2<\/sub>\u00a0+ H2<\/sub>O<\/p>\n
\nP4<\/sub>\u00a0+20HNO3<\/sub>\u00a0\u2192 4H3<\/sub>PO4<\/sub>\u00a0+ 4H2<\/sub>O + 20NO2
\n<\/sub>3Zn +8HNO3<\/sub>\u00a0\u2192 3Zn(NO3<\/sub>)2<\/sub>\u00a0+4H2<\/sub>O +2NO<\/p>\n
\nNaHCO3<\/sub>\u00a0+ HNO3<\/sub>\u00a0NaNO3\u00a0<\/sub>+ H2<\/sub>O + CO2<\/sub><\/p>\n
\nCuO + 2HNO3<\/sub>\u00a0\u2192 Cu(NO3<\/sub>)2<\/sub>\u00a0+ H2<\/sub>O<\/p>\n
\n3 Zn + 8HNO3<\/sub>\u00a0\u2192 3Zn(NO3<\/sub>)2<\/sub>\u00a0+ 4H2<\/sub>O + 2NO<\/p>\n
\nNaOH + HNO3<\/sub>\u00a0\u2192 NaNO3<\/sub>\u00a0+H2<\/sub>O
\nSodium hydroxide reacts with nitric acid to form sodium nitrate.<\/p>\n
\nCuO + 2HNO3<\/sub>\u00a0\u2192 Cu(NO3<\/sub>)2<\/sub>\u00a0+ H2<\/sub>O
\nCopper oxide reacts with nitric acid to form copper nitrate.<\/p>\n
\nPb + 4HNO3<\/sub>\u00a0\u2192 Pb(NO3<\/sub>)2<\/sub>\u00a0+ 2H2<\/sub>O + 2NO2
\n<\/sub>Lead reacts with conc. nitric acid to form lead nitrate.<\/p>\n
\nMg +2HNO3<\/sub>\u00a0\u2192 Mg(NO3<\/sub>)2<\/sub>\u00a0+ H2
\n<\/sub>Magnesium with dil. nitric acid to form magnesium nitrate.<\/p>\n
\nFe + 6HNO3<\/sub>\u00a0\u2192 Fe(NO3<\/sub>)3<\/sub>\u00a0+ 3H2<\/sub>O + 3NO2
\n<\/sub>Iron reacts with conc. nitric acid to form ferric nitrate.<\/p>\n
\nHNO3<\/sub>\u00a0+ 3HCl\u00a0NOCl +2H2<\/sub>O + 2[Cl]
\nNitric acid reacts with hydrochloric acid to form a mixture called aqua regia.<\/p>\n
\n(b) NaNO3<\/sub>\u00a0gives NaNO2<\/sub>\u00a0and oxygen on heating.
\n(c) Constant boiling nitric acid contains 68% nitric acid by weight.
\n(d) Nitric acid turns yellow solution when exposed to light.<\/p>\n
\nFormula: FeSO4<\/sub>. NO<\/p>\n