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Idea of the experiment:

Systemic Investigation of [Pb ++ ] SI - 1. Idea of the experiment: . (1) Qualitative investigation of [Pb ++ ] in a systemic cycle. (2) Preparation of different [Pb ++ ] compounds. (3) Inter-conversion of [Pb ++ ] compounds. . Pb ++. HNO 3. Exp.1. Nitrate Salt . White ppt.

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Idea of the experiment:

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  1. Systemic Investigation of [Pb++] SI - 1 Idea of the experiment: • (1)Qualitative investigation of [Pb++] in a systemic cycle. • (2) Preparation of different [Pb++] compounds. • (3)Inter-conversion of [Pb++] compounds.

  2. Pb++ HNO3 Exp.1 Nitrate Salt White ppt. Lead Oxalate Yellow ppt Lead iodide Exp.2 Exp.5 Lead Nitrate White ppt Lead carbonate Exp.3 Exp.4 White ppt Lead hydroxide (SI -1)

  3. Reagents Used: • (1) Acids: • HCl, 1:1 solution. • HNO3. • (2) Salts: • Sodium Oxalate • Sodium Carbonate • Potassium iodide • Lead nitrate, (5gm) of the solid salt in (100 ml) of • distilled water. • (3) Ammonium hydroxide.

  4. Exp. 1 Add (1 ml) of sodium oxalate solution to (2 ml) of lead solution. What do you observe? • Observation: White ppt of lead osxlate. • Equation: • Exp. 2 Dissolve the precipitate from the exp. (1) in (1ml) of dil HNO3. What do you observe?

  5. Observation: The precipitate dissolves in HNO3. • Exp. 3 Add (1 ml) of NH4OH to the solution produced from the exp.2. What do you observe? • Observation: White ppt of lead hydroxide. • Equation:

  6. Exp. 4 Dissolve the precipitate obtained from the exp.3 in (0.5 ml) of HNO3 and then add few drop of Na2CO3. What do you observe? • Observation: White ppt of lead carbonate. • Equation: • Exp. 5 Dissolve the precipitate obtained from exp.4 in (0.5 ml) of HNO3 and then add one or two drops from KI. What do you observe?

  7. Observation: Yellow ppt of lead iodide. • Equation: Finally Dissolve the precipitate obtained from exp.5 in a few drops of HNO3 and then heat. The product is the starting solution of Pb(NO3)2.

  8. Systemic Investigation of [Ag+] SI - 2 Idea of the experiment: • (1)Qualitative investigation of [Ag+] in a systemic cycle. • (2) Preparation of different [Ag+] compounds. • (3)Inter-conversion of [Ag+] compounds.

  9. Exp. 1 Ag+ Silver nitrate. White ppt. Silver sulphite. Exp. 2 HNO3 Exp. 3 White ppt. Silver phosphate White ppt. Silver carbonate (SI-2) Reagents Used: • (1) Acids: • HNO3.: 1:1 solution. • (2) Salts: • Sodium Sulphite • Sodium Carbonate • Potassium phosphate • Silver nitrate, (1.35) of the solid salt in (100 ml) of • distilled water.

  10. Exp. 1 Add (1 ml) of sodium sulphite solution to ca. (2 ml) of silver nitrate solution. What do you observe? • Observation: • White ppt. of silver sulphite. • Equation: • Exp. 2 Dissolve the precipitate from experiment (1) in (1ml) dil. HNO3, then add (3ml) of sodium carbonate solution. What do you observe?

  11. Observation: • White ppt. of silver carbonate. • Equation: • Exp. 3 Dissolve the precipitate obtained from exp.2 in (0.5 ml) of HNO3 and then add few drops of (Na3PO4). What do you observe? • Observation: • Yellow ppt. of silver Phosphate.

  12. Equation: • Finally • Dissolve the precipitate formed from exp.3 in a few drops of HNO3. The product is the starting solution of silver nitrate.

  13. IF EXP. (I) GIVES NO PRECIPITATE THEN CARRY OUT EXP. II EXPERIMENT. II To (1 ml) of the unknown solution add (1 ml) of dil. HCl and (1 ml) solution of Na2S solution. What do you observe?

  14. Systemic Investigation of [Cd2+] SI - 3 Idea of experiment: • (1)Qualitative investigation of [Cd2+] in a systemic cycle. • (2) Preparation of different [Cd2+] compounds. • (3)Inter-conversion of [Cd2+] compounds.

  15. Cd2+ HNO3 Exp.1 Nitrate salt (white ppt.) Cadmium carbonate (yellow canary ppt.) Cadmium sulphide Exp.2 Exp.4 (white ppt.) Cadmium hydroxide Exp.3 Cadmium chloride (SI - 3) Reagents Used: • (1) Acids: • HCl.: 1:1 solution. • HNO3 (Conc.). • (2) Alkali: • NaOH (0.1 M solution).

  16. (3) Salts: • Sodium Carbonate. • Sodium Sulphide. Exp. 1 Add (1 ml) of sodium carbonate solution to ca. (2 ml) of the original cadmium solution. What do you observe? Observation: White ppt. of cadmium carbonate. Equation:

  17. Exp. 2 Dissolve the precipitate from experiment (1) in (1 ml) dil. HCl. Exp. 3 Add (3 ml) of sodium hydroxide solution. What do you observe? Observation: White ppt. of cadmium hydroxide. Equation:

  18. Exp. 4 Dissolve the percipitate obtained from exp.3 in (1 ml) of HCl and then add few drops of (Na2S) solution. What do you observe? • Observation: Canary yellow ppt. of cadmium sulphide. • Equation: Finally Dissolve the precipitate formed from exp.3 in a few drops of conc HNO3. The product is the starting solution of cadmium nitrate.

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