Question

For the reaction 2NaOH + H₂SO₄, how many grams of sulfuric acid are required?

Answer 1

To determine the number of grams of sulfuric acid required in the reaction 2NaOH + H₂SO₄, you need to know the molar mass of sulfuric acid and the stoichiometry of the reaction. The molar mass of sulfuric acid (H₂SO₄) is 98 g/mol. From the balanced chemical equation, you can see that for every 1 mole of sulfuric acid, you need 2 moles of sodium hydroxide (NaOH). By following the steps outlined above, you can calculate the number of grams of sulfuric acid required.

Step-by-step explanation:

To determine the number of grams of sulfuric acid required in the reaction 2NaOH + H₂SO₄, you need to know the molar mass of sulfuric acid and the stoichiometry of the reaction. The molar mass of sulfuric acid (H₂SO₄) is 98 g/mol. From the balanced chemical equation, you can see that for every 1 mole of sulfuric acid, you need 2 moles of sodium hydroxide (NaOH).

Here's the step-by-step calculation:

1. Convert the volume of sodium hydroxide used to moles. Use the given molarity (0.250 M) and volume (32.20 mL) to calculate the number of moles of sodium hydroxide used.
2. Use the mole ratio from the balanced chemical equation (2 moles NaOH: 1 mole H₂SO₄) to determine the number of moles of sulfuric acid required.
3. Convert the moles of sulfuric acid to grams using the molar mass of sulfuric acid (98 g/mol).

By following these steps, you can calculate the number of grams of sulfuric acid required.