In the laboratory preparation of hydrogen peroxide, why is hydrated barium peroxide () specifically — Hydrogen Chemistry Question
Question
In the laboratory preparation of hydrogen peroxide, why is hydrated barium peroxide ($BaO_2 \cdot 8H_2O$) specifically preferred over anhydrous barium peroxide ($BaO_2$) when reacting with dilute sulphuric acid?
Answer: C
💡 Solution & Explanation
During the reaction $BaO_2 + H_2SO_4 \rightarrow BaSO_4 \downarrow + H_2O_2$, insoluble $BaSO_4$ is formed. If anhydrous $BaO_2$ is used, this insoluble precipitate forms a thin, protective layer around the unreacted $BaO_2$, choking off the acid supply and stopping the reaction. Hydrated barium peroxide avoids this surface coating issue.
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