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. Systemic Investigation of [Pb ++ ] SI - 1 Systemic Investigation of [Pb ++ ] SI - 1

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

3. Reagents Used: (1) Acids: HCl, 1:1 solution. HNO 3. (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. Add (1 ml) of sodium oxalate solution to (2 ml) of lead solution. What do you observe? Exp. 1 Observation: White ppt of lead osxlate. Equation: Dissolve the precipitate from the exp. (1) in (1ml) of dil HNO 3. What do you observe? Exp. 2

5. The precipitate dissolves in HNO 3. Observation: Add (1 ml) of NH 4 OH to the solution produced from the exp.2. What do you observe? Exp. 3 White ppt of lead hydroxide. Observation: Equation:

6. Dissolve the precipitate obtained from the exp.3 in (0.5 ml) of HNO 3 and then add few drop of Na 2 CO 3. What do you observe? Exp. 4 Observation: White ppt of lead carbonate. Equation: Dissolve the precipitate obtained from exp.4 in (0.5 ml) of HNO 3 and then add one or two drops from KI. What do you observe? Exp. 5

7. Yellow ppt of lead iodide. Observation: Equation: Finally Dissolve the precipitate obtained from exp.5 in a few drops of HNO 3 and then heat. The product is the starting solution of Pb(NO 3 ) 2. Finally Dissolve the precipitate obtained from exp.5 in a few drops of HNO 3 and then heat. The product is the starting solution of Pb(NO 3 ) 2.

8. Systemic Investigation of [Ag + ] SI - 2 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. White ppt. Silver phosphate White ppt. Silver sulphite. White ppt. Silver carbonate Exp. 1 Exp. 2 Exp. 3 HNO 3 Ag + Silver nitrate. (SI-2) Reagents Used: (1) Acids: HNO 3.: 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. Add (1 ml) of sodium sulphite solution to ca. (2 ml) of silver nitrate solution. What do you observe? Exp. 1 Observation: White ppt. of silver sulphite. Equation: Dissolve the precipitate from experiment (1) in (1ml) dil. HNO 3, then add (3ml) of sodium carbonate solution. What do you observe? Exp. 2

11. Observation: White ppt. of silver carbonate. Equation: Dissolve the precipitate obtained from exp.2 in (0.5 ml) of HNO 3 and then add few drops of (Na 3 PO 4 ). What do you observe? Exp. 3 Observation: Yellow ppt. of silver Phosphate.

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

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 Na 2 S solution. What do you observe?

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

15. Exp.1 Cadmium chloride Cd 2+ (yellow canary ppt.) Cadmium sulphide (white ppt.) Cadmium carbonate (white ppt.) Cadmium hydroxide Exp.2 Exp.4 Exp.3 Nitrate salt HNO 3 (SI - 3) Reagents Used: (1) Acids: HCl.: 1:1 solution. HNO 3 (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. Observation: White ppt. of cadmium hydroxide. Exp. 3 Add (3 ml) of sodium hydroxide solution. What do you observe? Equation:

18. Dissolve the percipitate obtained from exp.3 in (1 ml) of HCl and then add few drops of (Na 2 S) solution. What do you observe? Exp. 4 Observation: Canary yellow ppt. of cadmium sulphide. Equation: Finally Dissolve the precipitate formed from exp.3 in a few drops of conc HNO 3. The product is the starting solution of cadmium nitrate. Finally Dissolve the precipitate formed from exp.3 in a few drops of conc HNO 3. The product is the starting solution of cadmium nitrate.