Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to the reaction bao2(s)+h2so4(aq)⟶baso4(s)+h2o2(aq) how many milliliters of 3.75 m h2so4(aq) are needed to react completely with 53.5 g bao2(s)?

84.43 milliliters of 3.75 M Sulfuric acid are needed.

Explanation:

Moles of barium oxide =

According to reaction, 1 mole of barium oxide reacts with 1 mole of sulfuric acid.

Then 0.3166 moles of barium oxide will react with:

of sulfuric acid.

Where: V = Volume of the solution in Liters

Moles of sulfuric acid = 0.3166 mol

Volume of the sulfuric acid solution = V = ?

Molarity of sulfuric acid = 3.75 M

0.08443 L = 84.43 mL (1 L = 1000 mL)

84.43 milliliters of 3.75 M Sulfuric acid are needed.