Barium Oxide Reacts with Sulfuric Acid As Follows Calculate

This guide explains how to calculate the reaction between barium oxide (BaO) and sulfuric acid (H₂SO₄), including the balanced chemical equation, stoichiometric calculations, and practical applications. The reaction is highly exothermic and produces barium sulfate (BaSO₄) and water (H₂O).

Balanced Chemical Equation

The reaction between barium oxide and sulfuric acid can be represented by the following balanced chemical equation:

BaO + H₂SO₄ → BaSO₄ + H₂O

This equation shows that one mole of barium oxide reacts with one mole of sulfuric acid to produce one mole of barium sulfate and one mole of water. The reaction is a neutralization reaction where a basic oxide reacts with an acidic oxide to form a salt and water.

Stoichiometry of the Reaction

Stoichiometry allows us to calculate the quantities of reactants and products involved in the reaction. The balanced equation provides the mole ratios:

1 mole of BaO reacts with 1 mole of H₂SO₄
1 mole of BaO produces 1 mole of BaSO₄
1 mole of H₂SO₄ produces 1 mole of H₂O

For example, if you have 50 grams of barium oxide (molar mass of BaO is 153.33 g/mol), you can calculate the moles of BaO:

moles of BaO = mass / molar mass moles of BaO = 50 g / 153.33 g/mol ≈ 0.326 mol

According to the stoichiometry, 0.326 moles of BaO will react with 0.326 moles of H₂SO₄ to produce 0.326 moles of BaSO₄ and 0.326 moles of H₂O.

Practical Applications

The reaction between barium oxide and sulfuric acid has several practical applications:

Production of barium sulfate: Barium sulfate is used in medical imaging (X-rays) and as a filler in paints and plastics.
Water treatment: The reaction can be used to remove barium ions from water, which is important in industrial processes.
Laboratory synthesis: The reaction is commonly used in chemistry laboratories to prepare barium sulfate for various experiments.

Note: The reaction is highly exothermic, so proper safety measures must be taken to prevent thermal runaway and ensure safe handling of the reactants and products.

Safety Considerations

When performing this reaction, it is essential to follow safety guidelines:

Personal protective equipment: Wear gloves, safety goggles, and a lab coat to protect against splashes and fumes.
Ventilation: Conduct the reaction in a well-ventilated area or under a fume hood to disperse any hydrogen sulfide gas that may form as a byproduct.
Thermal management: The reaction is exothermic, so add reactants slowly and use a cooling bath if necessary to prevent overheating.
Disposal: Properly dispose of the solid barium sulfate and any aqueous solutions according to local regulations.

Frequently Asked Questions

What is the balanced equation for the reaction between barium oxide and sulfuric acid?

The balanced equation is: BaO + H₂SO₄ → BaSO₄ + H₂O. This shows that one mole of barium oxide reacts with one mole of sulfuric acid to produce one mole of barium sulfate and one mole of water.

How do I calculate the amount of barium sulfate produced from a given amount of barium oxide?

Use the stoichiometric ratio from the balanced equation. For example, if you have 50 grams of barium oxide, calculate the moles of BaO (moles = mass / molar mass), then use the 1:1 ratio to find the moles of BaSO₄ produced.

What safety precautions should I take when performing this reaction?

Wear personal protective equipment, conduct the reaction in a well-ventilated area, manage the exothermic nature of the reaction, and properly dispose of the products according to local regulations.