{"id":29056,"date":"2023-03-12T15:54:29","date_gmt":"2023-03-12T10:24:29","guid":{"rendered":"https:\/\/icsesolutions.com\/?p=29056"},"modified":"2023-03-13T10:13:02","modified_gmt":"2023-03-13T04:43:02","slug":"new-simplified-chemistry-class-10-icse-solutions-nitric-acids","status":"publish","type":"post","link":"https:\/\/icsesolutions.com\/new-simplified-chemistry-class-10-icse-solutions-nitric-acids\/","title":{"rendered":"New Simplified Chemistry Class 10 ICSE Solutions – Nitric Acids"},"content":{"rendered":"
ICSE Solutions<\/a>Selina ICSE Solutions<\/a>ML Aggarwal Solutions<\/a><\/p>\n Viraf J Dalal Chemistry Class 10 Solutions and Answers<\/strong><\/p>\n Simplified Chemistry<\/a>English<\/a>Maths<\/a>Physics<\/a>Chemistry<\/a>Biology<\/a><\/p>\n QUESTIONS<\/span> Question 1.<\/span><\/strong> 2001<\/span><\/strong><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> Question 4.<\/span><\/strong> 2002<\/strong><\/span><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> The NO2<\/sub> so produced dissolves in cone. HNO3<\/sub>. The yellow colour of cone, nitric acid is due to NO2<\/sub> dissolved in it.<\/p>\n Question 4.<\/span><\/strong> Question 5.<\/span><\/strong> 2003<\/strong><\/span><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> Question 5.<\/span><\/strong> 2004<\/span><\/strong><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0\u00a0 2005<\/strong><\/span><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> Question 4.<\/span><\/strong> 2006<\/strong><\/span><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> 2007<\/strong><\/span><\/p>\n Question 1.<\/span><\/strong> Question 2.<\/span><\/strong> Question 3.<\/span><\/strong> 2008<\/strong><\/span><\/p>\n
\n<\/strong>2000<\/strong><\/span><\/p>\n
\nWhat do you see when concentrated nitric acid is added to copper.
\nAnswer:<\/strong><\/span>
\nA pungent smelling reddish brown coloured gas (NO2<\/sub>) is produced and the solution turns greenish blue.
\nCu + 4HNO3<\/sub> (cone.) \u2192 Cu (NO3<\/sub>)2<\/sub> + 2H2<\/sub>O + 2NO2<\/sub><\/p>\n
\nName the gas produced in the reaction:<\/strong>
\nAction of concentrated nitric acid on copper.
\nAnswer:<\/strong><\/span>
\nNitrogen dioxide.<\/p>\n
\nChoose the correct word from the brackets to complete the sentence. Sodium nitrate reacts with \u2014 (concentrated \/ dilute) sulphuric acid to produce nitric acid. Write equation for the same.
\nAnswer:<\/strong><\/span>
\nSodium nitrate reacts with concentrated sulphuric acid to produce nitric acid.
\n<\/p>\n
\nWrite the equations for the following reaction : Between copper and concentrated nitric acid.
\nAnswer:<\/strong><\/span>
\nCu + 4HNO3<\/sub> (cone.) \u2192 Cu (NO3<\/sub>)2<\/sub> + 2H2<\/sub>O+ 2NO2<\/sub><\/p>\n
\nFrom the formulae listed below, choose, one, corresponding to the salt having the given description:
\nAgCl, CuCO3<\/sub>, CuSO4<\/sub>. 5H2<\/sub>O, KNO3<\/sub>, NaCl, NaHSO,, Pb(NO3<\/sub>)2<\/sub>, ZnCO3<\/sub>, ZnSO4<\/sub>.7H2<\/sub>O.
\nThis salt gives nitrogen dioxide on heating.
\nAnswer:<\/strong><\/span>
\nPb(NO3<\/sub>)2
\n
\n<\/sub><\/p>\n
\nGive equations for the action of heat on –
\n<\/strong>(1) NH4<\/sub>Cl
\n(2) NH4<\/sub>NO3<\/sub>.
\nState whether each reaction is an example of thermal decomposition\u00a0\u00a0 or thermal dissociation.
\n(1) Dissociation
\n(2) decomposition
\nAnswer:<\/strong><\/span>
\n<\/p>\n
\nWhat compounds are required for the laboratory preparation of nitric acid.
\nAnswer:<\/strong><\/span>
\nPotassium nitrate and cone, sulphuric acid.<\/p>\n
\nState why pure nitric acid takes on a yellowish brown colour when exposed to light.
\nAnswer:<\/strong><\/span>
\nIn the presence of sunlight nitric acid decomposes even at room temperature to give nitrogen dioxide, water and oxygen.
\n<\/p>\n
\nWrite an equation for the following reaction:
\n<\/strong>Copper and concentrated nitric acid.
\nAnswer:<\/strong><\/span>
\nCu + 4HNO3<\/sub> (cone.) \u2192 Cu (NO3<\/sub>)2<\/sub> + 2H2<\/sub>O + 2NO2<\/sub>.<\/p>\n
\nThe first step in the manufacture of HNO3<\/sub> is the catalytic oxidation of NH3<\/sub>. Name the catalyst used.
\nAnswer:<\/strong><\/span>
\nPlatinum.<\/p>\n
\nName a solution which gives nitrogen dioxide with copper.
\nAnswer:<\/strong><\/span>
\nConcentrated nitric acid (HNO3<\/sub>).<\/p>\n
\nWhen nitric acid is prepared by the action of concentrated sulphuric acid on potassium nitrate, what is the special feature of the apparatus used.
\nAnswer:<\/strong><\/span>
\nAll glass apparatus is used in the laboratory preparation of nitric acid.<\/p>\n
\nWrite the equation for the lab. preparation of H2<\/sub>NO3<\/sub> from potassium nitrate and cone. H2<\/sub>SO4<\/sub>.
\nAnswer:<\/strong><\/span>
\n
\nQuestion 4.<\/span><\/strong>
\nPotassium nitrate prepared from KOH and nitric acid. State the type of reaction involved.
\nAnswer:<\/strong><\/span>
\nNeutralization reaction.<\/p>\n
\nState the cone, acid which will oxidise sulphur directly to H2<\/sub>SO4<\/sub>. Write the equation for the same.
\nAnswer:<\/strong><\/span>
\nHot and cone, nitric acid will oxidises sulphur directly to sulphuric acid.
\nS + 6HNO3<\/sub> \u2192 H2<\/sub>SO4<\/sub> + 2H2<\/sub>O + 6NO2<\/sub><\/p>\n
\nX, Y and Z are three crystalline solids which are soluble in water and have a common anion. To help you
\nto identify X, Y and Z, you are provided with the following experimental observations. Copy and complete the corresponding inferences in.
\nA reddish-brown gas is obtained when X, Y and Z are separately warmed with concentrated sulphuric acid and copper turnings added to the mixture. The common anion is the ion.
\nAnswer:<\/strong><\/span>
\n[NO–<\/sup>] Nitrate<\/p>\n
\nWrite a balanced equation for the reaction of cone. HNO3 <\/sub>when added to copper turnings kept in a beaker.
\nAnswer:<\/strong><\/span>
\nCu + 4HNO3<\/sub> \u2192 Cu(NO3<\/sub>)2<\/sub> + 2NO2<\/sub> + 2H2<\/sub>O<\/p>\n
\nWrite a balanced equation for the reaction of cone. HN03 <\/sub>when added to copper turnings kept in a beaker.
\nAnswer:<\/strong><\/span>
\nCu + 4HNO3<\/sub> \u2192 Cu(NO3<\/sub>)2<\/sub> + 2NO2<\/sub> + 2H2<\/sub>O<\/p>\n
\nWrite a balanced equation for the reaction of – sulphur and hot concentrated nitric acid.
\nAnswer:<\/strong><\/span>
\n<\/p>\n
\nDilute 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\u00a0metals.
\nAnswer:<\/strong><\/span>
\nMetals, lying above hydrogen in the electro chemical series, give hydrogen from the acid. In case of nitric acid which is a strong\u00a0oxidising agent, hydrogen produced in the nascent state reduces\u00a0excess nitric acid and produces water and a reduction productof nitric acid. The reduction product depends on the dilution of\u00a0the acid.<\/p>\n
\nWrite the equation for the reaction of dilute nitric acid with copper.
\nAnswer:<\/strong><\/span>
\n3Cu + 8HNO3<\/sub> \u2192 3Cu(NO3<\/sub>)2<\/sub> + 4H2<\/sub>O + 2NO<\/p>\n
\nState why a yellow colour that appears in concentrated\u00a0\u00a0nitric acid when it is left standing in an ordinary glass bottle.
\nAns.
\nIt turns yellow because cone. HNO3<\/sub> decomposes by the action of sunlight to give brown coloured NO2
\n<\/sub>
\nThe brown coloured NO2<\/sub> dissolves in cone. HNO3<\/sub>, to give it a yellow colour.<\/p>\n
\nFrom the substances – Ammonium sulphate, Lead carbonate, Chlorine, Copper nitrate, Ferrous sulphate \u2014 State:<\/strong>
\nA compound which releases a reddish brown gas on reaction with concentrated sulphuric acid and copper turnings.
\nAnswer:<\/strong><\/span>
\nCopper Nitrate.<\/p>\n
\nState what is observed when nitric acid is kept in a reagent bottle for a long time.
\nAnswer:<\/strong><\/span>
\nBrown vapours are seen in the reagent bottle and nitric acid turns yellowish in colour.<\/p>\n
\nExplain why only all-glass apparatus should be used for the preparation of nitric acid by heating concentrated sulphuric acid and potassium nitrate.
\nAnswer:<\/strong><\/span>
\nNitric acid is highly corrossive and a strong oxidising agent. It attacks rubber and wooden corks. Therefore, all glass apparatus should be used for the preparation of nitric acid in the laboratory.<\/p>\n
\nIn the laboratory preparation of nitric acid:\u00a0<\/strong>Name the reactants A (a liquid) and B (a solid) used.
\nAnswer:<\/strong><\/span>
\n(A)<\/strong> Cone, sulphuric acid (B)<\/strong> Potassium nitrate (Nitre)<\/p>\n
\nWrite an equation to show how nitric acid undergoes decomposition.
\nAnswer:<\/strong><\/span>
\n<\/p>\n
\nWrite the equation for the reaction in which copper is oxidized by concentrated nitric acid.
\nAnswer:<\/strong><\/span>
\nCu + 4HNO3<\/sub> \u2192 Cu(NO3<\/sub>)2<\/sub> + 2H2<\/sub>O + 2NO2<\/sub><\/p>\n