BaCl2 + H2SO4 | Barium Chloride and Sulfuric Acid Reaction
Barium chloride (BaCl2) is a strong electrolyte salt and
sulfuric acid (H2SO4) is a strong acid.
Because both barium ions and sulfate ions are met and mixed in same aqueous solution, barium sulfate (BaSO4) which is a white
precipitate is formed. However, to form barium sulfate precipitate, there should be enough barium ion and sulfate ion concentrations.
Written by: Eng. Heshan Nipuna, Chemical Engineer, Chemistry School
BaCl2 + H2SO4 → BaSO4 + HCl
Because barium chloride is a strong electrolyte, it dissociates completely in water and releases barium ions and chloride ions.
TO occur this reaction, you can use either solid barium chloride or aqueous barium chloride. Sulfuric acid is commonly met as aqueous solution in
laboratory.
When barium chloride and sulfuric acid solutions are mixed, barium ions and sulfate ions exits in a same solution for a moment. Immediately,
with the mixing you will see a white precipitate is formed.
That white precipitate isbarium sulfate. As the other product, hydrochloric
acid (HCl) is given.
Balaced equation of BaCl2 + H2SO4
If aqueous barium chloide is used, balanced chemical reaction can be given like below. Except barium sulfate, all other compounds exist as aqueous solutions.
BaCl2(aq) + H2SO4(aq) → BaSO4(s) + 2HCl(aq)
If solid barium chloide is used, balanced chemical reaction can be given like below. Hoever, when solid barium chloride is added to aqueous sulfuric
acid solution, barium chloride immediately dissociates to ions and react with sulfuric acid.
BaCl2(s) + H2SO4(aq) → BaSO4(s) + 2HCl(aq)
If same concentration (0.1 mol dm-3) and same volumes of barium chloride and sulfuric acid are mixed, what will be the final pH of solution?
Initial H+ ion concentration of sulfuric acid solution is 0.2 mol dm. Because H+ ion concentration is reduced by half due to volume increment in two times, H+ concentration is 0.1 mol dm-3. That means pH is 1.
