{"id":29059,"date":"2023-03-12T14:34:17","date_gmt":"2023-03-12T09:04:17","guid":{"rendered":"https:\/\/icsesolutions.com\/?p=29059"},"modified":"2023-03-13T10:12:52","modified_gmt":"2023-03-13T04:42:52","slug":"new-simplified-chemistry-class-10-icse-solutions-a-study-of-compounds-ammonia","status":"publish","type":"post","link":"https:\/\/icsesolutions.com\/new-simplified-chemistry-class-10-icse-solutions-a-study-of-compounds-ammonia\/","title":{"rendered":"New Simplified Chemistry Class 10 ICSE Solutions – Study Of Compounds : Ammonia"},"content":{"rendered":"

New Simplified Chemistry Class 10 ICSE Solutions – Study Of Compounds: Ammonia<\/span><\/h2>\n

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
\n<\/strong><\/span>2001<\/strong><\/span><\/p>\n

Question 1.<\/strong><\/span>
\nState what do you observe when :
\nNeutral litmus solution is added to an alkaline solution.
\nAnswer:<\/strong><\/span>
\nThe litmus solution turns to blue.<\/p>\n

Question 2.<\/strong><\/span>
\nName (formula is not acceptable) the gas produced in the following reaction :
\nWarming ammonium sulphate with sodium hydroxide solution.
\nAnswer:<\/strong><\/span>
\nAmmonia gas.<\/p>\n

Question 3.<\/strong><\/span>
\nWrite the equation for the preparation of NH3 from ammonium chloride and calcium hydroxide.
\nAnswer:<\/strong><\/span>
\n2NH4<\/sub>Cl + Ca(OH)2<\/sub> \u2192 CaCl2<\/sub> + 2NH3<\/sub> + 2H2<\/sub>O<\/p>\n

Question 4.<\/strong><\/span>
\nWhat are the products formed when ammonia is oxidized with copper oxide.
\nAnswer:
\n\"New
\n<\/strong><\/span><\/p>\n

2002<\/strong><\/span><\/p>\n

Question 1.<\/strong><\/span>
\nFrom the following gases – ammonia, chlorine, hydrogen chloride, sulphur dioxide, select the gas that turns moist red litmus paper blue.
\nWrite the equation for the reaction – when the gas is passed over heated CuO.
\nAnswer:<\/strong><\/span>
\nAmmonia gas.
\n3CuO + 2NH3<\/sub> \u2192 3Cu + N2<\/sub> + 3H2<\/sub>O<\/p>\n

2003<\/strong><\/span><\/p>\n

Question 1.<\/strong><\/span>
\nName a gas whose solution in water is alkaline.
\nAnswer:<\/strong><\/span>
\nAmmonia<\/p>\n

Question 2.<\/strong><\/span>
\nHow would you distinguish between Zn2+<\/sup> and Pb2+<\/sup> using ammonium hydroxide solution.
\nAnswer:<\/strong><\/span>
\nZinc salt gives white gelatinous ppt. and Pb2+<\/sup> gives chalky white ppt. with ammonium hydroxide.<\/p>\n

Question 3.<\/strong><\/span>
\nWrite the equation for the formation of ammonia by the action of water on mangesium nitride.
\nAnswer:<\/strong><\/span>
\nMg3<\/sub>N2<\/sub> + 6H2<\/sub>O \u2192 2NH3<\/sub> + 3Mg (OH)2<\/sub><\/p>\n

Question 4.<\/strong><\/span>
\nHow is ammonia collected. Why is ammonia not collected over water.
\nAnswer:<\/strong><\/span>
\nAmmonia gas is lighter than air and hence collected by the downward displacement of air.
\nAmmonia is not collected over water because it is highly soluble in water.<\/p>\n

Question 5.<\/strong><\/span>
\nWhich compound is normally used as a drying agent for ammonia.
\nAnswer:<\/strong><\/span>
\nQuicklime(Calcium oxide CaO).<\/p>\n

2004<\/strong><\/span><\/p>\n

Question 1.<\/strong><\/span>
\nFrom the gases ammonia, hydrogen chloride, hydrogen sulphide, sulphur dioxide – Select the following :<\/p>\n

    \n
  1. When this gas is bubbled through copper sulphate soln., a deep blue coloured solution is formed.<\/li>\n
  2. This gas burns in oxygen with a green flame.<\/li>\n<\/ol>\n

    Answer:<\/strong><\/span><\/p>\n

      \n
    1. ammonia<\/li>\n
    2. ammonia<\/li>\n<\/ol>\n

      Question 2.<\/strong><\/span>
      \nWrite the equation for the reaction in the Haber\u2019s process that forms ammonia.
      \nAnswer:
      \n\"New
      \n<\/strong><\/span><\/p>\n

      Question 3.<\/strong><\/span>
      \nState the purpose of liquefying the ammonia produced in the process.
      \nAnswer:<\/strong><\/span>
      \nBy liquefying ammonia, it can be easily seperated from unreacted N2<\/sub> and H2<\/sub> gases.<\/p>\n

      Question 4.<\/strong><\/span>
      \nWrite an equation for the reaction of chlorine with excess of ammonia.
      \nAnswer:
      \n\"New<\/strong><\/span><\/p>\n

      2005<\/strong><\/span><\/p>\n

      Question 1.<\/strong><\/span>
      \nName the ion other than ammonium ion formed when ammonia dissolves in water.
      \nAnswer:<\/strong><\/span>
      \nHydroxyl ion (NH3<\/sub> + H2<\/sub>O \u2192 NH+<\/sup>4\u00a0<\/sub>+ OH–<\/sup> )<\/p>\n

      Question 2.<\/strong><\/span>
      \nWrite the equations for the following reactions which result in the formation of ammonia.<\/p>\n

        \n
      1. A mixture of ammonium chloride and slaked lime is heated.<\/li>\n
      2. Aluminium nitride and water.<\/li>\n<\/ol>\n

        Answer:
        \n\"New
        \n<\/strong><\/span><\/p>\n

        2006<\/strong><\/span><\/p>\n

        Question 1.<\/strong><\/span>
        \nSelect the correct compound from the list given \u2014 Ammonia, Copper oxide, Copper sulphate, Hydrogen chloride, Hydrogen sulphide, Lead bromide \u2014 which matches the description given below :
        \nThe compound is not a metal hydroxide, its aqueous solution is alkaline in nature.
        \nAnswer:<\/strong><\/span>
        \nAmmonia.<\/p>\n

        Question 2.<\/strong><\/span>
        \nFrom the list of substances given \u2014 Ammonium sulphate, Lead carbonate, Chlorine, Copper nitrate, Ferrous sulphate \u2014 State :
        \nA compound which on heating with sodium hydroxide produces a gas which forms dense white fumes with hydrogen chloride.
        \nAnswer:<\/strong><\/span>
        \nAmmonium sulphate.<\/p>\n

        Question 3.<\/strong><\/span>
        \nState what is observed when excess of ammonia is passed through an aq. solution of lead nitrate.
        \nAnswer:<\/strong><\/span>
        \nChalky white insoluble ppt. is formed.<\/p>\n

        Question 4.<\/strong><\/span>
        \nName the substance used for drying ammonia,
        \nAnswer:<\/strong><\/span>
        \nQuick lime (CaO).<\/p>\n

        Question 5.<\/strong><\/span>
        \nWrite a balanced chemical equation to illustrate the reducing nature of ammonia.
        \nAnswer:<\/strong><\/span>
        \nReducing nature of ammonia.
        \n2NH3<\/sub> + 3CuO \u2192 3Cu + 3H2<\/sub> + N2<\/sub> (g)<\/p>\n

        Question 6.<\/strong><\/span>
        \nWith reference to Haber\u2019s process for the preparation of ammonia, write the equation and the conditions required.
        \nAnswer:
        \n<\/strong><\/span>\"New
        \nConditions for maximum yield of ammonia<\/strong><\/p>\n

          \n
        1. High Pressure (700-900 atm)<\/li>\n
        2. Optimum temperature (450-500\u00b0C)<\/li>\n
        3. Use of a catalyst : Iron (Fe) and use of a promotor : Molybdenum (Mo)<\/li>\n<\/ol>\n

          2007<\/strong><\/span><\/p>\n

          Question 1.<\/strong><\/span>
          \nWrite a balanced equation for the following reaction :
          \nAmmonium sulphate from ammonia and dilute sulphuric acid.
          \nAnswer:
          \n\"New
          \n<\/strong><\/span><\/p>\n

          Question 2.<\/strong><\/span>
          \nGive equation for – reaction in which NH3<\/sub> is oxidized by :<\/p>\n

            \n
          1. a metal oxide ;<\/li>\n
          2. a gas which is not oxygen.<\/li>\n<\/ol>\n

            Answer:
            \n\"New
            \n<\/strong><\/span><\/p>\n

            Question 3.<\/strong><\/span>
            \nYou enter a laboratory after a class has completed the Fountain Experiment. How will you be able to tell whether the gas used in the experiment was hydrogen chloride or ammonia.
            \nAnswer:<\/strong><\/span>
            \nIf the colour of the litmus solution in the round bottomed flask is blue the gas used was ammonia and if the colour of the litmus solution in the round bottomed flask is red, the gas used was hydrogen chloride. This is because hydrogen chloride(aq) is acidic in nature and turns purple litmus solution red and ammonia (aq) is basic in nature and turns purple neutral litmus solution blue.<\/p>\n

            2008<\/strong><\/span><\/p>\n

            Question 1.<\/strong><\/span>
            \nAmmonia can be obtained by adding water to : [Select the correct word]
            \nA Ammonium chloride
            \nB Ammonium nitrite
            \nC Magnesium nitride
            \nD Magnesium nitrate
            \nAnswer:<\/strong><\/span>
            \nC Magnesium nitride<\/p>\n

            Question 2.<\/strong><\/span>
            \nName : An alkaline gas A which gives dense white fumes with hydrogen chloride.
            \nAnswer:<\/strong><\/span>
            \nNH3<\/sub> (Ammonia)<\/p>\n

            Question 3.<\/strong><\/span>
            \nWrite the equation for the following reaction : Aluminium nitride and water.
            \nAnswer:
            \n\"New
            \n<\/strong><\/span><\/p>\n

            Question 4.<\/strong><\/span>
            \nComplete the table relating to an important industrial processes. [Output refers to the product of the process].
            \n\"New
            \nAnswer:
            \n\"New
            \n<\/strong><\/span><\/p>\n

            2009<\/strong><\/span><\/p>\n

            Question 1.<\/strong><\/span>
            \nName the gas – that burns in oxygen with a green flame.
            \nAnswer:<\/strong><\/span>
            \nAmmonia (NH3<\/sub>)<\/p>\n

            Question 2.<\/strong><\/span>
            \nWrite a fully balanced equation for the following : Magnesium nitride is treated with warm water.
            \nAnswer:
            \n\"New
            \n<\/strong><\/span><\/p>\n

            Question 3.<\/strong><\/span>
            \nIdentity the substances \u2018Q\u2019 based on the information given :
            \nThe white crystalline solid Q is soluble in water, it liberates a pungent smelling gas when heated with sodium hydroxide solution.
            \nAnswer:<\/strong><\/span>
            \nQ is Ammonium chloride and pungent smelling gas is ammonia.<\/p>\n

            2010<\/strong><\/span><\/p>\n

            Question 1.<\/strong><\/span>
            \nComplete the blanks (a) to (e) in the passage given, using the following words.
            \n(Ammonium, reddish brown, hydroxyl, nitrogen dioxide, ammonia, dirty green, alkaline, acidic) in the presence of a catalyst, nitrogen and hydrogen combine
            \nto give (a) _____ gas. When the same gas is passed through water, it forms a solution which will be _____ (b) in nature, and will contain the ions (c) _____ and (d) _____ (e) _____ coloured precipitate of iron [II] hydroxide is formed when the above solution is added to iron [II] sulphate solution, sssssss
            \nAnswer:<\/strong><\/span><\/p>\n

            (a)<\/strong> Ammonia
            \n(b)<\/strong> Alkaline
            \n(c)<\/strong> Ammonium
            \n(d)<\/strong> Hydroxyl
            \n(e)<\/strong> Dirty green<\/p>\n

            Question 2.<\/strong><\/span>
            \nState your observation when – in the absence of a catalyst ammonia gas is burnt in an atmosphere of oxygen.
            \nAnswer:<\/strong><\/span>
            \nGreenish yellow flame is observed.<\/p>\n

            Question 3.<\/strong><\/span>
            \nGive the equation for the reaction : ammonium chloride is heated with sodium hydroxide.
            \nAnswer:<\/strong><\/span>
            \nNH4<\/sub>Cl + NaOH \u2192 NaCl + NH3<\/sub> + H2<\/sub>O<\/p>\n

            Question 4.<\/strong><\/span>
            \nIn the manufacture of ammonia.<\/p>\n

              \n
            1. Name the process.<\/li>\n
            2. State the ratio must the reactants taken ?<\/li>\n
            3. State the catalyst used.<\/li>\n
            4. Give the equation for the manufacture of the gas ammonia.<\/li>\n<\/ol>\n

              Answer:
              \n\"New
              \n<\/strong><\/span><\/p>\n

              Question 5.<\/strong><\/span>
              \nWrite a relevant equation, to show that ammonia can act as a reducing agent
              \nAnswer:<\/strong><\/span>
              \n2NH3<\/sub>\u00a0+ 3Cl2<\/sub> \u2192 N2<\/sub> + 6HCl<\/p>\n

              Question 6.<\/strong><\/span>
              \nName two gases you have which can be used to study the fountain experiment.
              \nState the common property demonstrated by the fountain experiment ?
              \nAnswer:<\/strong><\/span>
              \nTwo gases which are used to study the fountain experiment are Hydrogen chloride gas (HCl) and Ammonia (NH3)
              \nThe common property of these two gases demonstrated by the fountain experiment is the solubility of gases<\/p>\n

              2011<\/strong><\/span><\/p>\n

              Question 1.<\/strong><\/span>
              \nState what is observed when – Ammonium hydroxide is first added in a small quantity and then in excess to a solution of copper sulphate.
              \nAnswer:<\/strong><\/span>
              \nOn adding ammonium hydroxide in small amount, pale blue precipitates will appear. On adding ammonium hydroxide in excess, blue precipitates will dissolve forming deep blue solution.
              \n\"New<\/p>\n

              Question 2.<\/strong><\/span>
              \nThe diagram shows set up for the laboratory preparation of a pungent alkaline gas.
              \n\"New<\/p>\n

                \n
              1. Name the gas collected in the jar.<\/li>\n
              2. Write the balanced equation for the above preparation<\/li>\n
              3. State how the gas is collected?<\/li>\n
              4. Name the drying agent used.<\/li>\n
              5. State how you will find out that the jar is full of pungent gas?<\/li>\n<\/ol>\n

                Answer:<\/strong><\/span><\/p>\n

                  \n
                1. Ammonia (NH3<\/sub>)<\/li>\n
                2. NH4<\/sub> Cl + Ca (OH)2<\/sub> \u2192 CaCl2<\/sub> + 2H2<\/sub>O + 2NH3<\/sub> \u2191<\/li>\n
                3. Downward displacement of air<\/li>\n
                4. Quicklime (CaO)<\/li>\n
                5. Bring a rod dipped in HCl near it. Dense white fumes of ammonium chloride will be formed.<\/li>\n<\/ol>\n

                  Question 3.<\/strong><\/span>
                  \nWrite a balanced chemical equation – Chlorine reacts with excess of ammonia.
                  \nAnswer:
                  \n\"New
                  \n<\/strong><\/span><\/p>\n

                  Question 4.<\/strong><\/span>
                  \nState your observation when – Water is added to the product formed, when aluminium is burnt in a jar of nitrogen gas.
                  \nAnswer:<\/strong><\/span>
                  \nPungent smelling and alkaline gas (NH3<\/sub>) is evolved.
                  \n\"New<\/p>\n

                  2012<\/strong><\/span><\/p>\n

                  Question 1.<\/strong><\/span>
                  \nName the gas produced when excess ammonia reacts with chlorine.
                  \nAnswer:<\/strong><\/span>
                  \nNitrogen.<\/p>\n

                  Question 2.<\/strong><\/span>
                  \nRewrite the correct statement with the missing word\/s Magnesium nitride reacts with water to liberate ammonia.
                  \nAnswer:<\/strong><\/span>
                  \nMagnesium nitride reacts with warm water to liberate ammonia along with magnesium hydroxide.<\/p>\n

                  Question 3.<\/strong><\/span>
                  \nGive balanced equation for the reaction : Ammonia and Oxygen in the presence of a catalyst.
                  \nAnswer:
                  \n\"New
                  \n<\/strong><\/span><\/p>\n

                  Question 4.<\/strong><\/span>
                  \nThe following questions are based on the preparation of ammonia gas in the laboratory:<\/p>\n

                    \n
                  1. Explain why ammonium nitrate is not used in the preparation of ammonia.<\/li>\n
                  2. Name the compound normally used as a drying agent during the process.<\/li>\n
                  3. How is ammonia gas collected ? Explain why it is not collected over water.<\/li>\n<\/ol>\n

                    Answer:<\/strong><\/span><\/p>\n

                      \n
                    1. Ammonium nitrate does not undergo a reversible sublimation reaction, it melts and then decompses into nitrogen oxide gas and water vapour. Thus it is not used in the preparation of ammonia.
                      \nNH4<\/sub>NO3<\/sub> \u2192 N2<\/sub>O + 2H2<\/sub>O<\/li>\n
                    2. Calcium oxide<\/li>\n
                    3. Ammonia is collected in an inverted dry gas jar by downward displacement of air.
                      \nIt is highly soluble in water and hence cannot be collected by downward displacement of water.<\/li>\n<\/ol>\n

                      2013<\/strong><\/span><\/p>\n

                      Question 1.<\/strong><\/span>
                      \nState one appropriate observation for :
                      \nExcess of chlorine gas is reacted with ammonia gas.
                      \nAnswer:<\/strong><\/span>
                      \nA yellow explosive liquid (Nitrogen trichloride) is formed.<\/p>\n

                      Question 2.<\/strong><\/span>
                      \nNitrogen gas can be obtained by heating :<\/p>\n

                      (a)<\/strong> Ammonium nitrate
                      \n(b)<\/strong> Ammonium nitrite
                      \n(c)<\/strong> Magnesium nitric
                      \n(d)<\/strong> Ammonium chloride<\/p>\n

                      Answer:<\/strong><\/span><\/p>\n

                      (b)<\/strong> Ammonium nitrite<\/p>\n

                      Question 3.<\/strong><\/span>
                      \nState two relevant observations for :
                      \nAmmonium hydroxide solution is added to zinc nitrate solution in minimum quantities and then in excess.
                      \nAnswer:<\/strong><\/span>
                      \nA white gelatin like precipitate of zinc hydroxide is formed which dissolves in excess of ammonium hydroxide.<\/p>\n

                      Question 4.<\/strong><\/span>
                      \nGive balanced equations for :<\/strong>
                      \nReduction of hot Copper (II) oxide to copper using ammonia gas.
                      \nAnswer:
                      \n\"New
                      \n<\/strong><\/span><\/p>\n

                      Question 5.<\/strong><\/span>
                      \nCopy and complete the following table relating to im\u00acportant industrial process :
                      \n\"New
                      \nAnswer:
                      \n\"New
                      \n<\/strong><\/span><\/p>\n

                      Question 6.<\/strong><\/span>
                      \nIdentify : An alkaline gas which produces dense white fumes when reacted with HCl gas.
                      \nAnswer:<\/strong><\/span>
                      \nAmmonia gas.<\/p>\n

                      2014<\/strong><\/span><\/p>\n

                      Question 1.<\/strong><\/span>
                      \nFill in the blank from the choices given in bracket : Ammonia gas is collected by _____ (upward displacement of air, a downward displacement of water, a downward displacement of air)
                      \nAnswer:<\/strong><\/span>
                      \nAmmonia gas is collected by a downward displacement of air.<\/p>\n

                      Question 2.<\/strong><\/span>
                      \nWrite balanced equation for : Action of warm water on magnesium nitride.
                      \nAnswer:<\/strong><\/span>
                      \nAction of warm water on magnesium nitride.
                      \n\"New<\/p>\n

                      Question 3.<\/strong><\/span>
                      \nDistinguish between the following pairs of compounds using the test given within bracket :<\/p>\n

                        \n
                      1. Iron(II)sulphate and iron (III) sulphate (using ammonium hydroxide)<\/li>\n
                      2. A lead salt and a zinc salt (using excess ammonium hydroxide)<\/li>\n<\/ol>\n

                        Answer:
                        \n\"New
                        \n\"New
                        \n<\/strong><\/span><\/p>\n

                        Question 4.<\/strong><\/span>
                        \nState your observation :<\/strong> Calcium hydroxide is heated with ammonium chloride crystals.
                        \nAnswer:
                        \n<\/strong><\/span>\"New
                        \nammonia gas is evolved which fumes strongly in moist air.<\/p>\n

                        Question 5.<\/strong><\/span>
                        \nName the other ion formed when ammonia dissolves in water. Give one test that can be used to detect the presence of the ion produced.
                        \nAnswer:
                        \n\"New
                        \n<\/strong><\/span><\/p>\n

                        Question 6.<\/strong><\/span>
                        \nState the conditions required for : Catalytic oxidation of ammonia to nitric oxide.
                        \nAnswer:<\/strong><\/span>
                        \nCatalytic oxidation of ammonia to nitric oxide.
                        \n\"New
                        \nConditions for catalytic oxidation of ammonia to nitric oxide : Platinum catalyst and 800\u00b0C temperature.<\/p>\n

                        2015<\/strong><\/span><\/p>\n

                        Question 1.<\/strong><\/span>
                        \nFrom the list the gases \u2014 Ammonia, ethane, hydrogen chloride, hydrogen sulphide, ethyne
                        \nSelect the gas which is used as a reducing agent in reducing copper oxide to copper.
                        \nAnswer:<\/strong><\/span>
                        \nHydrogen<\/p>\n

                        Question 2.<\/strong><\/span>
                        \nState one relevant observation \u2014 Ammonia gas is burnt in an atmosphere of excess oxygen.
                        \nAnswer:<\/strong><\/span>
                        \nAmmonia gas bums to form nitrogen gas and steamy fumes of water.<\/p>\n

                        Question 3.<\/strong><\/span>
                        \nA metal \u2018X\u2019 has valency 2 and a non-metal \u2018Y\u2019 has a valency 3.
                        \nIf \u2018Y \u2019 is a diatomic gas, write an equation for the direct combination of X and Y to from a compound.
                        \nAnswer:<\/strong><\/span>
                        \nThe equation for the direct combination of X and Y to form a compound is
                        \n\"New<\/p>\n

                        Question 4.<\/strong><\/span>
                        \nGive balanced chemical equations \u2014<\/strong><\/p>\n

                          \n
                        1. Lab. preparation of ammonia using an ammonium salt.<\/li>\n
                        2. Reaction of ammonia with excess chlorine.<\/li>\n
                        3. Reaction of ammonia with sulphuric acid.<\/li>\n<\/ol>\n

                          Answer:<\/strong><\/span><\/p>\n

                            \n
                          1. Ammonia is prepared in the laboratory by using ammonium chloride.
                            \n\"New<\/li>\n
                          2. When ammonia reacts with excess of chlorine, it forms nitrogen trichloride and HCl
                            \n\"New<\/li>\n
                          3. Ammonia reacts with sulphuric acid to form ammonium sulphate.
                            \n\"New<\/li>\n<\/ol>\n

                            2016<\/strong><\/span><\/p>\n

                            Question 1.<\/strong><\/span>
                            \nWrite balanced equations for :<\/strong><\/p>\n

                              \n
                            1. Action of warm water on AIN.<\/li>\n
                            2. Excess of ammonia is treated with chlorine.<\/li>\n
                            3. An equation to illustrate the reducing nature of ammonia.<\/li>\n<\/ol>\n

                              Answer:
                              \n\"New
                              \n<\/strong><\/span><\/p>\n

                              Question 2.<\/strong><\/span>
                              \nName the gas evolved when the following mixtures are heated :<\/p>\n

                                \n
                              1. Calcium hydroxide and Ammonium chloride.<\/li>\n
                              2. Sodium nitrite and Ammonium chloride.<\/li>\n<\/ol>\n

                                Answer:<\/strong><\/span><\/p>\n

                                  \n
                                1. Ammonia gas<\/li>\n
                                2. Nitrogen gas<\/li>\n<\/ol>\n

                                  2017<\/strong><\/span><\/p>\n

                                  Question 1.<\/strong><\/span>
                                  \nWrite the balanced chemical equation for each of the following –<\/p>\n

                                    \n
                                  1. Reaction of ammonia with heated copper oxide.<\/li>\n
                                  2. Laboratory preparation of ammonia from ammonium chloride.<\/li>\n<\/ol>\n

                                    Answer:
                                    \n\"New
                                    \n<\/strong><\/span><\/p>\n

                                    Question 2.<\/strong><\/span>
                                    \nState one relevant observation for the following reaction – Burning of ammonia in air.
                                    \nAnswer:<\/strong><\/span>
                                    \nAmmonia bums with a yellowish green flame.<\/p>\n

                                    Question 3.<\/strong><\/span>
                                    \nCertain blanks spaces are left in the following tables as C, D & E. Identify each of them.
                                    \n\"New
                                    \nAnswer:<\/strong><\/span><\/p>\n

                                    C :<\/strong> Reactants are Magnesium nitride(Mg3<\/sub>N2<\/sub>) and water(H2<\/sub>O).
                                    \nD :<\/strong> Drying agent is anhydrous calcium oxide (Quick lime).
                                    \nE :<\/strong> NH3<\/sub> gas is collected by the downward displacement of air.<\/p>\n

                                    Question 4.<\/strong><\/span>
                                    \nGive a balanced chemical equation for each of the following –<\/p>\n

                                      \n
                                    1. Catalytic oxidation of ammonia.<\/li>\n
                                    2. Reaction of ammonia with nitric acid.<\/li>\n<\/ol>\n

                                      Answer:
                                      \n\"New
                                      \n<\/strong><\/span><\/p>\n

                                      Additional Questions<\/strong><\/span><\/p>\n

                                      Question 1.<\/strong><\/span>
                                      \nState why nitrogenous matter produces ammonia. State a liquid source of ammonia.
                                      \nAnswer:<\/strong><\/span>
                                      \nWhen nitrogenous matter (such as animal and vegetable protiens) decays in the absence of air, the putrefying bacteria on the organic matter in the soil or ammonifying bacteria in organic matter produces ammonia.
                                      \nThe liquid souce of ammonia is decaying urine of animals.<\/p>\n

                                      Question 2.<\/strong><\/span>
                                      \nGive the word equation and balanced molecular equation for the laboratory preparation of ammonia from NH4Cl and calcium hydroxide.
                                      \nAnswer:<\/strong><\/span>
                                      \nAmmonium Chloride + Calcium Hydroxide\u00a0\u2192 Calcium Chloride + Water + Ammonia
                                      \n\"New<\/p>\n

                                      Question 3.<\/strong><\/span>
                                      \nConvert ammonium sulphate to ammonia using two different alkalis.
                                      \nAnswer:
                                      \n\"New
                                      \n<\/strong><\/span><\/p>\n

                                      Question 4.<\/strong><\/span>
                                      \nState why ammonia is not obtained in the laboratory from NH4<\/sub>NO3<\/sub> and NaOH.
                                      \nAnswer:<\/strong><\/span>
                                      \nAmmonium nitrate on heating decomposes explosively with the formation of nitrous oxide and water.
                                      \n\"New<\/p>\n

                                      Question 5.<\/strong><\/span>
                                      \nState the method used with reasons for drying and collecting ammonia gas.
                                      \nAnswer:<\/strong><\/span>
                                      \nCalcium oxide (quick lime) is used for drying ammonia. It is because, calcium oxide being basic in nature does not react chemically with ammonia.
                                      \nCaO + H2<\/sub>O \u2192 Ca(OH)2<\/sub>
                                      \nChemicals such as CaCl2<\/sub> (anhydrous), P2<\/sub>O5<\/sub> and cone H2<\/sub>SO4<\/sub> are not used for drying ammonia, because they react chemically with it as shown in the equation below :
                                      \n\"New
                                      \nAmmonia is collected by downward displacement of air. Ammonia gas is highly soluble in water, as such it cannot be collected over water. Further, ammonia is lighter than air. As such ammonia is collected by downward displacement of air.<\/p>\n

                                      Question 6.<\/strong><\/span>
                                      \nState how you would convert (i)<\/strong> Mg (ii)<\/strong> Ca (iii)<\/strong> Al – to ammonia.
                                      \nAnswer:
                                      \n\"New
                                      \n\"New
                                      \n<\/strong><\/span><\/p>\n

                                      Question 7.<\/strong><\/span>
                                      \nGive a balanced equation with all conditions to obtain NH3<\/sub>\u00a0from N2<\/sub> and H2<\/sub>.
                                      \nAnswer:
                                      \n<\/strong><\/span>\"New
                                      \nConditions for maximum yield of ammonia :<\/strong><\/p>\n

                                        \n
                                      • Pressure :<\/strong> 200-900\u00b0C (High pressure)<\/li>\n
                                      • Temperature :<\/strong> 450-500\u00b0C (Optimum temperature)<\/li>\n
                                      • Catalyst :<\/strong> Finely divided iron, Fe<\/li>\n
                                      • Promotor :<\/strong> Molybdenum, Mo<\/li>\n<\/ul>\n

                                        Question 8.<\/strong><\/span>
                                        \nState two physical properties of NH3<\/sub> which enable separation of NH3<\/sub> from a mixture of NH3<\/sub>, N2<\/sub> and H2<\/sub>.
                                        \nAnswer:<\/strong><\/span><\/p>\n

                                          \n
                                        1. Ammonia liquifies at a pressure 8 atmosphere at -33\u00b0C, but not hydrogen and nitrogen.<\/li>\n
                                        2. Ammonia is extremely soluble in water, but not hydrogen and nitrogen.<\/li>\n<\/ol>\n

                                          Question 9.<\/strong><\/span>
                                          \nCompare the density of ammonia with that of air. Name two gases lighter than ammonia.
                                          \nAnswer:<\/strong><\/span>
                                          \nThe vapour density of ammonia is 8.5 and that of air is 14.4. The two gases lighter than ammonia are<\/p>\n

                                            \n
                                          1. hydrogen<\/li>\n
                                          2. helium.<\/li>\n<\/ol>\n

                                            Question 10.<\/strong><\/span>
                                            \n\u2018Ammonia is highly soluble in water\u2019. Name two other gases showing similar solubility.
                                            \nAnswer:<\/strong><\/span>
                                            \nThe other highly soluble gases in water are :<\/strong><\/p>\n

                                              \n
                                            1. Hydrogen chloride<\/li>\n
                                            2. Sulphur trioxide.<\/li>\n<\/ol>\n

                                              Question 11.<\/strong><\/span>
                                              \nName the experiment and state its procedure to demonstrate the high solubility of ammonia.
                                              \nAnswer:<\/strong><\/span>
                                              \nHighly solubility of ammonia can be shown by Fountain Experiment.
                                              \nTo demonstrate the high solubility of ammonia gas in water.
                                              \n\"New
                                              \nApparatus :<\/strong><\/p>\n

                                                \n
                                              1. Round bottomed flask filled with ammonia gas.<\/li>\n
                                              2. Mouth of the flask with a rubber stopper with two holes, one for jet tube and other for dropper containing water.<\/li>\n
                                              3. Trough below contains red litmus solution.<\/li>\n<\/ol>\n

                                                Procedure :<\/strong><\/p>\n

                                                  \n
                                                1. The dropper containing water is squeezed and few drops of water enters the flask.<\/li>\n
                                                2. Ammonia gas present in the flask gets dissolved in water due to its high solubility, which creates a partial vacuum in the flask.<\/li>\n
                                                3. Since outside pressure is higher, so red litmus solution rush up the jet tube and emerge as a fountain. (Ammonia gas being basic changed red litmus blue.)
                                                  \nAmmonia gas is lighter than air, hence it is collected by downward displacement of air.<\/li>\n
                                                4. Easily liquified at low temperatures.<\/li>\n
                                                5. Liquid ammonia boils at – 33.5\u00b0C<\/li>\n
                                                6. Solid ammonia melts at – 77.5\u00b0C<\/li>\n<\/ol>\n

                                                  Question 12.<\/strong><\/span>
                                                  \nGive an equation for the burning of ammonia in oxygen. State the observation seen.
                                                  \nAnswer:<\/strong><\/span>
                                                  \nAmmonia bums in the atmosphere of oxygen with a pale blue flame, forming nitrogen gas and water vapour.
                                                  \n\"New<\/p>\n

                                                  Question 13.<\/strong><\/span>
                                                  \nConvert ammonia to nitric oxide by catalytic oxidation of ammonia. State all conditions.
                                                  \nAnswer:<\/strong><\/span>
                                                  \nWhen a mixture of 2 (vols.) of oxygen and l(vols.) of ammonia is passed over platinum gauze maintained at 800\u00b0C, it reacts to form nitric oxide and water vapour.
                                                  \n\"New<\/p>\n

                                                    \n
                                                  • Conditions for the reaction :<\/strong> Ostwald\u2019s process<\/li>\n
                                                  • Temperature :<\/strong> 800\u00b0C<\/li>\n
                                                  • Catalyst :<\/strong> Platinum (Pt)<\/li>\n<\/ul>\n

                                                    Question 14.<\/strong><\/span>
                                                    \nDraw a simple diagram for the catalytic oxidation of ammonia in the laboratory.
                                                    \nAnswer:
                                                    \n\"New
                                                    \n<\/strong><\/span><\/p>\n

                                                    Question 15.<\/strong><\/span>
                                                    \nGive reasons for the observation seen during catalytic oxidation of ammonia.
                                                    \nAnswer:<\/strong><\/span>
                                                    \nThe colourless nitric oxide formed undergoes further oxidation to give reddish brown vapours of nitrogen oxide.
                                                    \nThe platinum(catalyst) continues to emit a reddish glow even after the heating is discontinued since the catalytic oxidation of ammonia is an exothermic reaction.<\/p>\n

                                                    Question 16.<\/strong><\/span>
                                                    \nName an industrial process which involves ammonia, oxygen and a catalyst as its starting reactants.
                                                    \nAnswer:<\/strong><\/span>
                                                    \nThe industrial process is called Ostwald\u2019s process for preparing nitric acid.<\/p>\n

                                                    Question 17.<\/strong><\/span>
                                                    \nState what an aqueous solution of NH3<\/sub> is called. State how it is prepared giving reasons.
                                                    \nAnswer:<\/strong><\/span>
                                                    \nThe aqueous solution of ammonia is chemically ammonium hydroxide(NH4<\/sub>OH) (Liquor Ammonia).
                                                    \nIt is prepared by connecting the delivery tube of the apparatus generating ammonia with an inverted funnel whose rim is just dipping in water contained in beaker.
                                                    \nThis arrangement provides<\/p>\n

                                                      \n
                                                    1. large surface area for the absorption of ammonia and<\/li>\n
                                                    2. prevents back suction
                                                      \nNH3<\/sub> + H2<\/sub>O \u2192 NH4<\/sub> OH<\/li>\n<\/ol>\n

                                                      Question 18.<\/strong><\/span>
                                                      \nState why an aq. soln. of NH3<\/sub><\/p>\n

                                                        \n
                                                      1. turns red litmus blue<\/li>\n
                                                      2. is a weak base and a weak electrolyte.<\/li>\n<\/ol>\n

                                                        Answer:<\/strong><\/span><\/p>\n

                                                          \n
                                                        1. Ammonia on dissolving in water furnishes ammonium (NH4<\/sub>+<\/sup>) ions and hydroxyl (OH–<\/sup>) ions.
                                                          \n\"New
                                                          \nThe presence of OH–<\/sup> turns the red litmus blue.<\/li>\n
                                                        2. When ammonia dissolves in water, it forms ammonium hydroxide. The ammonium hydroxide dissociates to NH4<\/sub>+<\/sup>\u00a0ions and OH–<\/sup> ions.
                                                          \nHowever, the degree of dissociation of ammonium hydroxide molecules is very low. Thus, due to the presence of few OH- ions it is a weak base, as well as weak electrolyte.<\/li>\n<\/ol>\n

                                                          Question 19.<\/strong><\/span>
                                                          \nState two different methods of preparing NH4<\/sub>Cl using hydrochloric acid.
                                                          \nAnswer:<\/strong><\/span><\/p>\n

                                                            \n
                                                          1. When ammonium hydroxide is treated with hydrochloric acid, neutrilisation reaction takes place with formation of Ammonium chloride
                                                            \nNH4<\/sub>OH + HCl (dil.) \u2192 NH4<\/sub>Cl + H2<\/sub>O<\/li>\n
                                                          2. When ammounium carbonate is treated with hydrochloric acid, it forms ammonium chloride, carbon dioxide and water.
                                                            \n(NH4<\/sub>)2<\/sub>\u00a0CO3<\/sub> + 2HCl (dil.) \u2192 2NH4<\/sub>Cl + CO2<\/sub> + H2<\/sub>O<\/li>\n<\/ol>\n

                                                            Question 20.<\/strong><\/span>
                                                            \nConvert (i)<\/strong> ammonia (ii)<\/strong> ammonium hydroxide to an ammonium salt using (a)<\/strong> HNO3<\/sub> (b)<\/strong> H2<\/sub>SO4<\/sub>.
                                                            \nAnswer:
                                                            \n\"New
                                                            \n<\/strong><\/span><\/p>\n

                                                            Question 21.<\/strong><\/span>
                                                            \nState a reason why reaction of liquor ammonia with nitric acid is a neutralization reaction.
                                                            \nAnswer:<\/strong><\/span>
                                                            \nLiquor ammonia is a saturated solution of ammonia in water. Ammonia, NH3<\/sub> dissolves in water to give ammonium hydroxide which dissociates partially to give NH4<\/sub>+<\/sup> and OH–<\/sup> ions. Due to presence of OH–<\/sup> ions, ammonium hydroxide acts as an alkali.
                                                            \n\"New
                                                            \nThe reaction between an acid (nitric acid) and an alkali or base is a neutralisation reaction.
                                                            \n\"New
                                                            \nHence, the reaction between liquor ammonia and nitric acid is a neutralisation reaction.<\/p>\n

                                                            Question 22.<\/strong><\/span>
                                                            \nState why an aqueous solution of ammonia (NH4<\/sub>OH) is used for identifying cations.
                                                            \nAnswer:<\/strong><\/span>
                                                            \nBecause of its colour and solubility in excess NH4<\/sub>OH.<\/p>\n

                                                            Question 23.<\/strong><\/span>
                                                            \nState how NH4<\/sub>OH is used for identify :<\/p>\n

                                                              \n
                                                            1. Fe2+<\/sup><\/li>\n
                                                            2. Fe3+<\/sup><\/li>\n
                                                            3. pb2+<\/sup><\/li>\n
                                                            4. Zn2+<\/sup><\/li>\n
                                                            5. Cu2+<\/sup> cations.<\/li>\n<\/ol>\n

                                                              Give also a balanced equation in each case for a known example.
                                                              \nAnswer:
                                                              \n\"New
                                                              \n\"New
                                                              \n\"New
                                                              \n<\/strong><\/span><\/p>\n

                                                              Question 24.<\/strong><\/span>
                                                              \nState why the blue ppt. formed on addition of NH4<\/sub>OH to CuSO4<\/sub> soln. dissolves to give a deep blue solution with excess of NH4<\/sub>OH. Give an equation for the reaction. State why Zn(OH)2<\/sub> is soluble in excess of NH4<\/sub>OH.
                                                              \nAnswer:<\/strong><\/span>
                                                              \nCuSO4<\/sub> when reacts with excess of ammonia it produces needle shape crystals of tetraammine copper(II) sulphate complex which possess a beautiful deep blue colour.
                                                              \n\"New<\/p>\n

                                                              Question 25.<\/strong><\/span>
                                                              \nGive balanced equations for the reducing reactions of ammonia with
                                                              \n(i)<\/strong> copper (II) oxide,\u00a0(ii)<\/strong> lead (II) oxide,\u00a0(iii)<\/strong> chlorine using,\u00a0(a)<\/strong> excess NH3<\/sub>,\u00a0(b)<\/strong> excess Cl2<\/sub>.
                                                              \nAnswer:
                                                              \n\"New
                                                              \n\"New
                                                              \n\"New
                                                              \n<\/strong><\/span><\/p>\n

                                                              Question 26.<\/strong><\/span>
                                                              \nState five tests for ammonia where a colour change is involved.
                                                              \nAnswer:<\/strong><\/span>
                                                              \nTests for ammonia :<\/strong><\/p>\n

                                                                \n
                                                              1. Ammonia turns red (or purple) litmus solution to blue.<\/li>\n
                                                              2. Ammonia turns methyl orange solution to yellow.<\/li>\n
                                                              3. Ammonia turns phenolphthalein (colourless) solution to pink.<\/li>\n
                                                              4. Ammonia turns Nesseler\u2019 reagent (colourless) solution to pale brown.<\/li>\n
                                                              5. Ammonia (when in excess) gives a deep blue coloured solution with CuSO4<\/sub> (aq.)<\/li>\n<\/ol>\n

                                                                Question 27.<\/strong><\/span>
                                                                \nState (i)<\/strong> a light neutral gas (ii)<\/strong> an acid (iii)<\/strong> an explosive (iv)<\/strong> a fertilizer \u2014 obtained from ammonia.
                                                                \nAnswer:<\/strong><\/span><\/p>\n

                                                                  \n
                                                                1. Hydrogen<\/li>\n
                                                                2. Nitric acid<\/li>\n
                                                                3. NH4<\/sub>NO3<\/sub><\/li>\n
                                                                4. Ammonium sulphate.<\/li>\n<\/ol>\n

                                                                  Question 28.<\/strong><\/span>
                                                                  \nName an ammonium salt which is a constituent of (a)<\/strong> smelling salts (b)<\/strong> dry cells.
                                                                  \nGive reasons for the use of the named ammonium salt for the same.
                                                                  \nAnswer:<\/strong><\/span><\/p>\n

                                                                  (a) Smelling salts :<\/strong> Ammonium carbonate, (NH4<\/sub>)2<\/sub>CO3<\/sub> is used as smelling salt. It is an unstable white solid decomposes to give pungent smellingNH3<\/sub> gas.
                                                                  \n(NH4<\/sub>)2<\/sub>CO3<\/sub> \u2192 2NH3<\/sub> + CO2<\/sub> + H2<\/sub>O
                                                                  \nThe pungent smelling NH3<\/sub> gas revives a fainted person. (NH4<\/sub>)2<\/sub>CO3<\/sub> is always kept in a tightly closed container to prevent it from decomposition.
                                                                  \n(b) Dry cells :<\/strong> Ammonium chloride(NH4<\/sub>Cl) is used in dry cells. It oxidises Zn to Zn2+<\/sup> ions. The electrons so produced constitute the electric current.<\/p>\n

                                                                  Question 29.<\/strong><\/span>
                                                                  \nGive one use with reason of<\/p>\n

                                                                    \n
                                                                  1. an aqueous solution of NH3<\/sub><\/li>\n
                                                                  2. liquefied NH3<\/sub>.<\/li>\n<\/ol>\n

                                                                    Answer:<\/strong><\/span>
                                                                    \n(i) Use of an Aqueous solution of Ammonia (NH3<\/sub>) :<\/strong> An aqueous solution of NH3<\/sub> is called liquor ammonia. Being a base, it can easily emulsify oils and fats. Therefore, it is used for removing oil and fat stains from clothes carpets, upholstery etc. It is also used for cleaning window panes, porcelain articles etc.
                                                                    \n(ii) Use of Liqueified Ammonia (NH3<\/sub>) :<\/strong> Liquid ammonia is used as refrigerant i.e. for producing low temperature. This is due to the following reasons:<\/p>\n

                                                                    (a)<\/strong> It is highly volatile.
                                                                    \n(b)<\/strong> It can be easily liquefied under high pressure and low temperature.
                                                                    \n(c)<\/strong> It\u2019s latent heat of evaporation is very high.<\/p>\n

                                                                    Question 30.<\/strong><\/span>
                                                                    \nState what are chlorofluorocarbons and give their use. Give a reason why they are ozone depleting. State a suitable alternative to chlorofluorocarbons which are non-ozone depleting.
                                                                    \nAnswer:<\/strong><\/span>
                                                                    \nChlorofluorocarbons (CFC\u2019s) are compounds of carbon with chlorine or fluorine.
                                                                    \nCFC are chemicals which like liquefied ammonia gas are used in refrigeration gas. They are also used as coolants in refrigeration and A\/c Plants and aerosol sprays and cleansing agents.
                                                                    \nThese CFC\u2019s deplete ozone layer and also contribute to global warming. Thus these CFC\u2019s are harmful to life. The CFC\u2019s are decomposed by ultraviolet rays coming from sun to produce highly reactive chlorine atoms i.e. free Cl radicals.
                                                                    \nSuitable alternatives to chloroflurocarbons which are not depleting ozone are :<\/strong>
                                                                    \nHCFC – Hydrochloroflurocarbons; and HFC – 125 Hydrochloroflurocarbons ; which act as a substitute for CFCs, which are non-ozone depleting.<\/p>\n

                                                                    Unit Test Paper 7b \u2014Ammonia<\/strong><\/span><\/p>\n

                                                                    Q.1. Choose the letter corresponding to the correct answer from \u2014 A : NO2<\/sub>, B : NO, C : N2<\/sub>, D : N2<\/sub>O.<\/strong>
                                                                    \nThe gas obtained when –
                                                                    \n1. Dry ammonia and dry oxygen gas are ignited together.
                                                                    \n2. Ammonia is passed over heated litharge.
                                                                    \n3. A greenish yellow gas reacts with excess ammonia.
                                                                    \n4. (a) Dry NH3<\/sub> and O2<\/sub> are passed over heated Pt.
                                                                    \n(b) The gaseous product obtained is further oxidised.
                                                                    \n5. Ammonium nitrite undergoes thermal decomposition.
                                                                    \nAnswer:<\/strong><\/span><\/p>\n

                                                                      \n
                                                                    1. C(N2<\/sub>)<\/li>\n
                                                                    2. C(N2<\/sub>)<\/li>\n
                                                                    3. C(N2<\/sub>)<\/li>\n
                                                                    4. (a) B(NO),(b) A(NO2<\/sub>)<\/li>\n
                                                                    5. D(N2<\/sub>O)<\/li>\n<\/ol>\n

                                                                      Q.2. State the colour of :<\/strong><\/p>\n

                                                                      Question 1.<\/strong><\/span>
                                                                      \nPhenolphthalein solution after passage of ammonia through it.
                                                                      \nAnswer:<\/strong><\/span>
                                                                      \nColourless phenolphthalein changes to pink colour.<\/p>\n

                                                                      Question 2.<\/strong><\/span>
                                                                      \nCopper (II) hydroxide solution after-addition of ammonium hydroxide in excess to it.
                                                                      \nAnswer:<\/strong><\/span>
                                                                      \nThe pale blue precipitate turns into a deep blue coloured solution.<\/p>\n

                                                                      Question 3.<\/strong><\/span>
                                                                      \nThe flame obtained on burning dry ammonia in oxygen.
                                                                      \nAnswer:<\/strong><\/span>
                                                                      \nGreenish yellow flame.<\/p>\n

                                                                      Question 4.<\/strong><\/span>
                                                                      \nThe solution obtained on addition of excess ammonium hydroxide to zinc sulphate solution.
                                                                      \nAnswer:<\/strong><\/span>
                                                                      \nWhite gelantinous precipitate dissolves.<\/p>\n

                                                                      Question 5.<\/strong><\/span>
                                                                      \nThe vapours obtained when ammonia-oxygen gas mixture is passed over heated Pt.
                                                                      \nAnswer:<\/strong><\/span>
                                                                      \nThe colourless NO gas first produced is further oxidises to brown coloured NO2<\/sub>.<\/p>\n

                                                                      Q.3. Give balanced equations for the following conversions \u2014 A, B, C, D and E.
                                                                      \n<\/strong>\"New
                                                                      \nAnswer:
                                                                      \n\"New
                                                                      \n<\/strong><\/span><\/p>\n

                                                                      Q.4. Give reasons for the following.<\/strong><\/p>\n

                                                                        \n
                                                                      1. An aqueous solution of ammonia acts as a weak base.<\/li>\n
                                                                      2. A mixture of ammonium nitrate and slaked lime are not used in the lab. preparation of ammonia gas.<\/li>\n
                                                                      3. Finely divided iron catalyst does not affect the percentage yield of ammonia in Haber\u2019s process.<\/li>\n
                                                                      4. Ammonium salts are formed when ammonia reacts with dilute acids in the gaseous or aq. medium.<\/li>\n
                                                                      5. Aqueous solution of lead and zinc nitrate can be distinguished using an aqueous solution of ammonia.<\/li>\n<\/ol>\n

                                                                        Answer:<\/strong><\/span><\/p>\n

                                                                          \n
                                                                        1. Ammonia molecule contains a lone pair of electrons on N- atom, which accepts a proton from water, and forms ammonium ion and hydroxide ion, this makes ammonia solution alkaline and thus, it acts as a base.
                                                                          \nNH3<\/sub>+ H2<\/sub>O \u2192 NH4<\/sub>+<\/sup>\u00a0+ OH–<\/sup>
                                                                          \nHowever, as the concentration of the hydroxyl ions that are furnished is less, therefore aqueous solution of ammonia acts as a weak base.<\/li>\n
                                                                        2. Because ammonium nitrate is explosive and decomposes itself.<\/li>\n
                                                                        3. Formation of NH3<\/sub> from N2<\/sub> and H2<\/sub> in haber\u2019s process is a reversible reaction. In a reversible reaction, a catalyst does not increase the yield of the product. It only helps in attaining the equilibrium in a shorter time.
                                                                          \n\"New<\/li>\n
                                                                        4. Ammonia in gaseous form neutralises acids to form salts.<\/li>\n
                                                                        5. Zinc nitrate forms white gelatinous ppt. while lead nitrate forms chalky white ppt.<\/li>\n<\/ol>\n

                                                                          Q.5. Complete the statements by selecting the correct word from the words in brackets.<\/strong><\/p>\n

                                                                            \n
                                                                          1. The salt solution which does not give an insoluble precipitate on addition of ammonium hydroxide in small amount is _____ (Mg(NO3<\/sub>)2<\/sub> \/ NaNO3<\/sub>\/Cu(NO3<\/sub>)2<\/sub>]<\/li>\n
                                                                          2. The alkaline behaviour of liquor ammonia is due to the presence of _____ ions, (ammonium \/ hydronium \/ hydroxyl)<\/li>\n
                                                                          3. Ammonia in the liquefied form is _____ (acidic \/ basic \/ neutral)<\/li>\n
                                                                          4. Ammonia reduces chlorine to _____ (nitrogen \/ hydrogen chloride \/ ammonium chloride)<\/li>\n
                                                                          5. The chemical not responsible for ozone depletion is _____ [methyl chloride \/ ammonia \/ chloroflourocarbons]<\/li>\n<\/ol>\n

                                                                            Answer:<\/strong><\/span><\/p>\n

                                                                              \n
                                                                            1. NaNO3<\/sub><\/li>\n
                                                                            2. Hydroxyl<\/li>\n
                                                                            3. basic<\/li>\n
                                                                            4. Ammonium chloride .<\/li>\n
                                                                            5. Ammonia<\/li>\n<\/ol>\n

                                                                              Q.6. Select the most probable substance from A, B, C, D and E which need to be added to distinguish :
                                                                              \n<\/strong>\"New
                                                                              \n\"New
                                                                              \nAnswer:
                                                                              \n\"New
                                                                              \n<\/strong><\/span><\/p>\n

                                                                              For More Resources<\/strong><\/p>\n

                                                                              \n