BaSO4 (Barium Sulfate) Titration
- Page ID
- 127576
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Required Training |
Required PPE |
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UC Lab Safety Fundamentals |
Lab coat, safety glasses/goggles, nitrile gloves |
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Equipment |
Chemicals |
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Demo set-up |
1.89g Barium Hydroxide |
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Beaker |
0.25M Sulfuric acid |
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Access to wall socket |
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Procedure:
** Please handle the ring stand, stir plate, burette and electrode carefully as one unit **
- Dissolve the barium hydroxide in 100ml DI water in the 300ml beaker. This may take a little time.
- Lower the electrode into the solution.
- Before adding the sulfuric acid to the beaker, make sure that the electronics are functioning properly and the light bulb is bright.
- Start adding the acid while stirring.
- At about 17-19ml the light will turn off.
- Additional acid added will bring the light back on.
Discussion:
The two prongs of the demonstration set-up are conductors; if the solution in between them is an electrolyte, then the light will turn on. In this case, the light is on except when there is a stoichiometric ratio of barium hydroxide and sulfuric acid. In the beginning, the dissolution of barium hydroxide provides the ions, while in the end, excess sulfuric acid provides the ions. The reaction is shown below:
Ba(OH)2 + H2SO4 → BaSO4 (s) + H2O
The fact that we can see the light bulb dim shows that this process is gradual as more acid is added and more barium precipitates out.
Hazards:
Sulfuric acid should be handled with care especially as the demo is transported. Acid spills should be neutralized according to MSDS with sodium bicarbonate or another suitable material. Barium hydroxide is incompatible with acids; make sure the dry hydroxide is not exposed to accidental release of sulfuric acid.
SOP: 
Corrosive – Barium Hydroxide, Sulfuric Acid
Disposal (by Storeroom)
Return the spent solution to the storeroom for proper disposal through EH&S. Barium is an environmental hazard and cannot be flushed down the drain.