Type the correct answer in the box. Express your answer to three significant figures. This balanced equation shows the reaction of sodium hydroxide and sulfuric acid: 2NaOH + H2SO4 → Na2SO4 + 2H2O. In a laboratory experiment, a student mixes 355 grams of sulfuric acid with an excess of sodium hydroxide. What is the theoretical mass of sodium sulfate produced? Refer to the periodic table and the polyatomic ion resource. The theoretical mass of sodium sulfate is grams.

514.5 g.

Explanation:

The balanced equation of the reaction is: 2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O. It is clear that every 2.0 moles of NaOH react with 1.0 mole of H₂SO₄ to produce 1.0 mole of Na₂SO₄ and 2.0 moles of 2H₂O. Since NaOH is in excess, so H₂SO₄ is the limiting reactant. We need to calculate the no. of moles of 355.0 g of H₂SO₄:

n of H₂SO₄ = mass/molar mass = (355.0 g) / (98.0 g/mol) = 3.622 mol.

Using cross multiplication:

∵ 1.0 mol H₂SO₄ produces → 1.0 mol of Na₂SO₄.

∴ 3.622 mol H₂SO₄ produces → 3.662 mol of Na₂SO₄.

Now, we can get the theoretical mass of Na₂SO₄:

∴ mass of Na₂SO₄ = no. of moles x molar mass = (3.662 mol) (142.04 g/mol) = 514.5 g.