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analytical chemistry

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Analytical Chemistry 1. When sodium hydroxide solution is added first drop by drop and then in excess to the salt solutions of magnesium, iron (II), iron (III), copper (II), zinc and lead, following observations are made as shown in table below : Ion Colour of salt solution Mg2+ Magnesium chloride (Colourless) Iron (II) Sulphate (light green) Iron (III) chloride (reddish brown) Copper (II) Sulphate (blue) Zinc Sulphate (colourless) Fe2+ Fe3+ Cu2+ Zn2+ Pb2+ Lead nitrate(colourless) Colour of ppt. when NaOH is Colour of ppt/sol with excess added drop by drop of NaOH sol. Dull white ppt. insoluble in Mg(OH)2 dull white ppt. excess. Dirty green ppt. insoluble in Fe(OH)3 Dirty green ppt. excess. Fe(OH)3 Reddish brown ppt Reddish brown ppt. insoluble in excess. Pale blue ppt. insoluble in Cu(OH)2 Pale blue ppt. excess. Zn(OH)2 White gelatin like Colourless sol. due to the formation ppt. of sodium zincate Colourless sol. due to the Pb(OH)2 Chalky white ppt. formation of sodium plumbite 2. Action of sodium hydroxide on soluble salts of Mg2+, Fe2+, Fe3+, Cu2+, Zn2+ and Pb2+. Given salt + NaOH Sodium Salt + Precipitate 2NaCl + Mg(OH)2 1. MgCl2 + 2NaOH Mg(OH)2 is a dull white ppt. insoluble in excess of NaOH Na2SO4 + Fe(OH)2 2. FeSO4 + 2NaOH Fe(OH)2 is a dirty green ppt. insoluble in excess of NaOH 3NaCl + Fe(OH)3 3. FeCl3 + 3NaOH Fe(OH)3 is a reddish brown ppt. insoluble in excess of NaOH. Na2SO4 + Cu(OH)2 4. CuSO4 + 2NaOH Cu(OH)2 is pale blue ppt. insoluble in excess of NaOH. 1 Key Points

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