APPARATUS REQUIRED:
1) Beaker
2) Whatman no 42 filter paper
3) Funnel
4) Crucible
5) Burner
CHEMICALS REQUIRED:
1) 1 ml of HCL
2) Barium chloride solution
THEORY:
when a solution of known weight of barium chloride is treated with an excess of dil. H₂SO4 barium is precipitated as BaSO4. From the weight of BaSO4 the amount of barium is calculated.
BaCL2 +H2S04 —>BaSO4 + 2HCL
233.36g of BaSO4 = 137.36g of Ba
1g of BaSO4 = 137.36/233.36 =0.588g
xg of BaSO4 = 0.588*x g of Ba
PROCEDURE:
9 ml of Barium chloride solution & 2 ml of conc. HCI was taken in a beaker & it was heated to boiling. Then about 1 ml of bench H₂SO4 was added slowly by stirring. Then the precipitate was allowed to settle down then the precipitate was transferred to filter paper & washed with hot water. Then it was kept into the crucible & was weighed & then it was ignited in the crucible until it was converted into ashes.
CALCULATION:
Wt of crucible ( a) = 25.2gm
Wt. of Crucible wt. of substance (b)=25.6gm
Wt. of substance = b-a = 25.6-25.2= 0.4gm
We know,
Wt. of substance = Wt. of BaSO4
233.36 gm of BaSO4 = 137.36g of Ba
0.4 gm of BaSO4 = 137.36/233.36 *0.4g of Ba
=0.235 g of Ba
RESULT:
Hence the amount of barium in Barium chloride was found to be 0.235g.
CONCLUSION:
Hence, the amount of Barium in the given solution of Barium chloride was estimated &
was found to be 0.235 g of Barium.
PRECAUTION:
1) Glassware should be handled carefully.
2) Weight should be noted carefully.