Idea of the experiment:

(1) Qualitative investigation of [Al+++] in a systemic

cycle.

(2) Preparation of different [Al+++] compounds.

(3) Inter-conversion of [Al+++] compounds.

Systemic Investigation of [AI++

+]

SI - 8

Systemic Investigation of [AI++

+]

SI - 8

Whit ppt. Aluminum phosphate

White gelationus ppt. Aluminum hydroxide

Coloreless

Exp. 1

Exp. 2

Exp. 3

HCl

Al+++

Chloride Salt

(SI-8)Reagents Used:

(1) Acid:

HCl: (1:1 solution).

(2) Alkali:NaOH

(3) Salts:Sodium phosphate.

Add (1 ml) of sodium hydroxide solution to ca. (2 ml) of aluminum chloride solution.What do you observe?

Exp. 1

Observation:

White gelatinous ppt. of Al (OH)3.

Equation:

Aluminum chloride, (5 gm) of the solid dissolved in (100 ml) of distilled water.

NaCl3(OH)AlNaOH3AlCl 33

Dissolve the precipitate obtained from experiment (1) in (2 ml) NaOH solution.What do you observe?

Exp. 2

Observation:

The precipitate dissolves in NaOH.

Equation:

OHOAlNaNaOH(OH)Al 223

1- Add one ml of HCl to the solution produced from exp. 2.

What do you observe?

Exp. 3

White ppt. of Al(OH)3.Observation:

Equation:

FinallyDissolving the Al PO4 precipitate in HCl, gives the starting solution of AlCl3.

FinallyDissolving the Al PO4 precipitate in HCl, gives the starting solution of AlCl3.

332 AlClNaCl3OH2AlHCl6OAl3Na

1- Dissolve the precipitate obtained in 0.5 ml of HCl and then add few drops of sodium phosphate.

What do you observe?

White ppt. of aluminum Phosphate. Observation:

Equation:NaCl34POlA4PO3NaAlCl3

Idea of the experiment:

(1) Qualitative investigation of [Fe+++] in a systemic

cycle.

(2) Preparation of different [Fe+++] compounds.

(3) Inter-conversion of [Fe+++] compounds.

Systemic Investigation of [Fe++

+]

SI - 9

Systemic Investigation of [Fe++

+]

SI - 9

Exp.1

Fe+++

(Violet color)Iron salycilate complex

Exp.2

HCl

(SI - 9)

(Reddish brown ppt.)Iron (III) hydroxide

Chloride salt

Reagents Used:

(1) Acid:HCl: (1:1 solution).Salicylic acid

(2) Alkali:Sodium hydroxide

(3) Salts:Ferric chloride, (5 gm) of the solid dissolved in (100 ml) of distilled water.

Add (1 ml) of sodium hydroxide solution to ca. (2 ml) of Iron (III) solution.What do you observe?

Exp. 1

Observation:

Reddish brown ppt. of iron (III) hydroxide. Equation:

NaCl3OHFeNaOH3FeCl 33

Dissolve the precipitate from experiment (1) in (1 ml) dil HCl and then add few drops of salicylic acid.What do you observe?

Exp. 2

Observation:

Violet colour of iron salicylate complex.

Finally

Dissolving iron salicylate complex in HCl,

gives the starting solution of FeCl3.

Finally

Dissolving iron salicylate complex in HCl,

gives the starting solution of FeCl3.

IF EXP. (II) GIVES NO PRECIPITATE THEN CARRY

OUT EXP. IV

IF EXP. (II) GIVES NO PRECIPITATE THEN CARRY

OUT EXP. IV

EXPERIMENT. IVEXPERIMENT. IV

To (1 ml) of the unknown solution, add (2ml) of ammonium chloride and (1 ml) of ammonium hydroxide and (1 ml) of sodium sulphide solution.What do you observe?

If black ppt. If buff ppt. If white gelatinous

ppt.

This means that (Ni2+)or (Co2+) may be presentInvestigate the cation byusing (SI - 10) or (SI- 11)

This means that(Mn2+) is present .

Carry out (SI- 12) toconfirm this result.

This means that(Zn2+) is present .

Carry out (SI- 13) toconfirm this result.

Observation:

Systemic Investigation of [Ni2+]

(SI - 10)Systemic Investigation of [Ni2+]

(SI - 10)

Idea of experiment:

(1) Qualitative investigation of [Ni2+] in a systemic

cycle.

(2) Preparation of different [Ni2+] compounds.

(3) Inter-conversion of [Ni2+] compounds.

Reagents Used: - Nickel chloride- Dimethylglyoxime.- Sodium hydroxide.- Ammonium Hydroxide.- Hydrochloric acid.

Exp.1

Exp.2

HCl

Exp.4

Chloride Salt

Exp.3

Ni2+

Green ppt.Ni (OH)2

Green ppt.Ni (OH)2

Blue solution.[Ni (NH3)4]2+

Red ppt.Ni (DMG)2

(SI - 10)

Exp. 1Add (1/2 ml) of NH4OH very dilute solution to ca. (2ml) of nickel chloride solution. What do you observe?

Observation:Green ppt. of nickel hydroxide.

Equation:

Cl2NHNi(OH)OHNH2NiCl 4242

Exp. 2

Dissolve the precipitate obtained from exp.1 in excess NH4OH ca. (2ml).What do you observe?

Observation:Blue solution of [Ni(NH3)4]2+ complex.

Exp. 3Add (1 ml) of NaOH to the solution produced from exp. 2.What do you observe? Observation:

Green ppt. of Ni(OH)2.

Exp.4Add (1 ml) of NH4Cl to the precipitate obtained from exp. 3. to dissolve the ppt. Then, add ca. (1/2 ml) of dimethylglyoxime. What do you observe? Observation:

Red ppt. of nickel dimethylglyoxime complex.

FinallyAddition of (1-2 ml) of HCl to the complex obtained from exp. 4 gives the starting NiCl2 solution.

FinallyAddition of (1-2 ml) of HCl to the complex obtained from exp. 4 gives the starting NiCl2 solution.

Idea of the experiment:

(1) Qualitative investigation of [CO2+] in a systemic

cycle.

(2) Preparation of different [CO2+] compounds.

(3) Inter-conversion of [CO2+] compounds.

Systemic Investigation of [CO2+]

(SI - 11)

Systemic Investigation of [CO2+]

(SI - 11)

Reagents Used:

Exp.1

Exp.2

HCl Chloride Salt

Exp.3

CoCl2

Blue ppt.Basic cobalt salt

Blue ppt. Co (OH)2

Pink solution Cobalt amine complex

(SI - 11)

- HCl (1:1 Solution).- HNO3 (1:1 Solution).- Cobalt (II) Chloride.- Sodium Hydroxide.- Ammonium Hydroxide.

Exp. 1Add ca. (1/2 ml) of NH4OH solution to ca. (2 ml) of CoCl2 solution.What do you observe?

Observation:Blue ppt of Co(OH)2.

Equation:

Cl2NH Co(OH) OH2NH CoCl 4242

Exp. 2Dissolve the precipitate from experiment (1) in (2 ml) NH4OH, and then add (1 ml) of NaOH.What do you observe?

Observation: Blue ppt of basic cobalt salt.

Heat the precipitate obtained from exp. 2.What do you observe?

Exp. 3

Observation:

Pink solution of cobalt - amine complex.

Cl4NH (OH))Co(NH4 OO6H8NH ClOH4Co 433223

FinallyAddition of HCl to the solution obtained from exp. 3, gives the starting CoCl2 solution.

FinallyAddition of HCl to the solution obtained from exp. 3, gives the starting CoCl2 solution.

Idea of the experiment:

(1) Qualitative investigation of [Mn2+] in a

systemic cycle.

(2) Preparation of different [Mn2+] compounds.

(3) Inter-conversion of [Mn2+] compounds.

Systemic Investigation of [Mn2+]

(SI - 12)

Systemic Investigation of [Mn2+]

(SI - 12)

Exp.1

Mn2+

Buff ppt.MnS

Exp.2

HCl

(SI - 12)

Buff ppt.Mn (OH)2

Chloride salt

Reagents Used:

- Manganese chloride.- HCl, (1:1 Solution).- Ammonium Chloride.- Ammonium Hydroxide.- Sodium sulphide.

Add (1 ml) of ammonium hydroxide to ca. (2 ml) of manganese chloride solution.What do you observe?

Exp. 1

Observation:

Buff ppt. of Mn(OH)2

Equation:

ClNH 2 Mn(OH) OH2NH MnCl 4242

Add ca. (2 ml) of ammonium chloride to the precipitate obtained from exp. 1 and then add (1 ml) of sodium sulphide.What do you observe?

Exp. 2

Observation:

Buff ppt of MnS.

Finallydissolving the precipitate obtained from exp. 2 in conc. HCl, gives the starting solution of MnCl2

Finallydissolving the precipitate obtained from exp. 2 in conc. HCl, gives the starting solution of MnCl2

Equation:

NaCl 2 MnS SNa MnCl 22