Procedure:

• The given barium chloride solution is made up to 100mL in a standard flask.
• 20mL of solution is pipetted into a 250 mL beaker.
• About 5mL 2N HCl is added and diluted to 150mL with distilled water.
• The solution is heated to boiling and a hot solution of 4N H₂SO₄ (10 - 15mL) is added drop by drop with constant stirring, till the precipitation is complete.
• The solution containing the precipitate is heated in a water bath for 5 minutes.
• The precipitate is allowed to stand for an hour.
• The clear solution is decanted through an ashless filter paper (whatman No. 40).
• The precipitate is washed with hot distilled water to free sulphate ions.
• The particles adhering to the sides of the beaker and glass rod are removed by a policeman.
• Finally the precipitate is washed once again.
• The dried filter paper is folded and placed in a crucible which has been previously weighed.
• The filter paper with the precipitate is first incinerated on a Bunsen burner by a low flame and then transferred to an electric burner.
• The crucible is transferred to desiccator and cooled.
• When cold, the crucible is weighed.
• Heating, cooling and weighing are repeated till concordant values are obtained.

Calculation:

Mass of crucible + lid = a g

Mass of crucible + lid + Bariumsulphate = b g

Mass of Bariumsulphate = (b-a) g.

233.36 of barium sulphate contain 137.36 g of barium.

Mass of barium in (b-a) g of Bariumsulphate =

Therefore, Mass of Barium in the whole of the given solution =

Result:

Mass of Barium in the whole of the given solution = ------------ g.