{"id":13208,"date":"2020-11-30T05:50:46","date_gmt":"2020-11-30T00:20:46","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=13208"},"modified":"2020-11-30T17:05:27","modified_gmt":"2020-11-30T11:35:27","slug":"action-heat-salts","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/action-heat-salts\/","title":{"rendered":"Action of Heat on Salts"},"content":{"rendered":"

Action of Heat on Salts<\/strong><\/h2>\n
    \n
  1. Heating a salt may cause it to decompose. The decomposition may result in
    \n(a) a colour change<\/strong>
    \n(b) evolution of a gas<\/strong>
    \n(c) liberation of water vapour<\/strong><\/li>\n
  2. Gases such as carbon dioxide, sulphur dioxide, nitrogen dioxide, ammonia<\/strong> or oxygen<\/strong> can be evolved. By identifying the gas or gases liberated, it is possible to pinpoint the anion<\/strong> present in the salt.<\/li>\n
  3. Examination of the residue<\/strong> can provide information to identify the cation in the salt.
    \n\"Action<\/li>\n<\/ol>\n

    Action of Heat on Carbonate Salts<\/strong><\/h2>\n
      \n
    1. Most metal carbonates<\/strong> decompose on heating to produce metal oxides and carbon dioxide gas.
      \nMetal carbonate \u2192\u00a0metal oxide + carbon dioxide
      \n\"Action<\/li>\n
    2. When the carbon dioxide gas is bubbled through limewater, it will turn the limewater milky.<\/li>\n<\/ol>\n

      Table shows the action of heat on carbonate salts.<\/strong><\/p>\n\n\n\n\n\n\n\n
      Carbonate salt<\/strong><\/td>\nAction of heat<\/strong><\/td>\n<\/tr>\n
      Potassium carbonate
      \nSodium carbonate<\/td>\n      		Do not decompose<\/td>\n<\/tr>\n
      Calcium carbonate
      \nMagnesium carbonate
      \nAluminium carbonate
      \nZinc carbonate
      \nIron(III) carbonate
      \nLead(II) carbonate
      \nCopper(II) carbonate<\/td>\n      		Decompose to produce metal oxide and carbon dioxide
      \nMetal carbonate\u00a0\u2192 metal oxide + carbon dioxide
      \nFor example,
      \nCaCO3<\/sub>(s) \u2192\u00a0CaO(s) + CO2<\/sub>(g)<\/td>\n<\/tr>\n
      Silver carbonate<\/td>\n\n

      Decomposes to produce metal, oxygen and carbon dioxide
      \n2Ag2<\/sub>CO3<\/sub>(s)\u00a0\u2192 4Ag(s) + O2<\/sub>(g) + 2CO2<\/sub>(g)<\/p>\n<\/td>\n<\/tr>\n

      Ammonium carbonate<\/td>\n\n

      Decomposes to produce ammonia, water and carbon dioxide
      \n(NH4<\/sub>)2<\/sub>CO3<\/sub>(s) \u2192\u00a02NH3<\/sub>(g) + H2<\/sub>O(l) + CO2<\/sub>(g)<\/p>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

      People also ask<\/strong><\/p>\n