Question

What volume requires a basic solution of 0.15 M sodium hydroxide to produce 135.0 g of sodium sulfate to completely react with sulfuric acid? How many grams of sulfuric acid react?

Answer 1

Volume can be calculated by :-

Concentration = 0.15 M = Number of moles of solute / Volume of solution in litres

Number of moles of solute = Actual mass (grams) / Molar Mass

The masses of reactants and products can be worked out from the equation:

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

98 + (2x40) = 142 + (2x18)

98 + 80 = 142 + 36

Now, 142g of Na₂SO₄ is made from 98g of H₂SO₄

         135g of Na₂SO₄ is made from 135 x (98 ÷ 142) = 93.169g of H₂SO₄

So, 93.169 grams of sulfuric acid react.