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Experiment No. N

Analysis of Lead(II) Iodide (Pb(I)₂)

Aim

To determine the presence of anion and cation in the given salt

Preliminary Test

  • Odor: Odorless
  • Texture: Crystalline
  • Color: White
  • Solubility: Soluble in water

Test of Anion

ExperimentObservationInference
Take 0.1 g of salt in a test tube and add conc. H₂SO₄Deep violet vapour with a pungent odour is evolvedI⁻ may be present
Confirmatory Tests
Layer Test
Take test solution or extract, add CHCl₃/CCl₄ and chlorine water dropwise, then shake vigorously		Violet colouration appears in the organic layerI⁻ is confirmed
Silver Nitrate Test
Acidify sodium carbonate extract with dilute HNO₃ and add AgNO₃		Yellow precipitate is obtained, insoluble in excess NH₄OHI⁻ is confirmed

Test of Cation

ExperimentObservationInference
Original solution + Dilute HClWhite precipitatePb²⁺ may be present
Confirmatory Tests
Potassium Iodide Test
Dissolve one part of the hot precipitate in hot water and add potassium iodide solution		Yellow precipitate is formedPresence of Pb²⁺ is confirmed
Potassium Chromate Test
To the acidified solution obtained above, add potassium chromate solution		Yellow precipitate is formedPresence of Pb²⁺ is confirmed
Lead Sulphate Test
Dissolve lead sulphide precipitate in dilute HNO₃, then add a few drops of dilute H₂SO₄ and alcohol		White precipitate of lead sulphate is formedPresence of Pb²⁺ is confirmed

Result

The given salt contains Pb²⁺ ions as cation and I⁻ ions as anion. The salt is Pb(I)₂.

Precautions

  1. Handle the chemicals with care.
  2. Don't use excess of chemicals.
  3. Keep the mouth of the test tube away from the face.