Question

As a chemical engineer, it is your job to fully neutralize the H2SO4waste being generated by a manufacturing plant. Your goal is to do this usingthe least amount of NaOHrequired in orderto save costs. Ifthe plant generates 1.0 ton (1.0 × 103kg) of sulfuric acid per day, how much NaOH willyou need to purchase to fully neutralize the H2SO4for next week (7 days)?

Answer 1

The balanced equation is : H₂SO₄ + 2 NaOH Na₂SO₄ + 2 H₂O

mass H₂SO₄ per day = 1.0 x 10³ kg/day

total mass of H₂SO₄ = (mass H₂SO₄ per day) * (7 days)

total mass of H₂SO₄ = (1.0 x 10³ kg/day) * (7 days)

total mass of H₂SO₄ = 7.0 x 10³ kg

moles of H₂SO₄ = (total mass of H₂SO₄ ) / (molar mass H₂SO₄)

moles of H₂SO₄ = (7.0 x 10³ kg) / (98.08 kg/kmol)

moles of H₂SO₄ = 71.37 kmol

moles NaOH required = 2 * (moles of H₂SO₄)

moles NaOH required = 2 * (71.37 kmol)

moles NaOH required = 142.74 kmol

mass NaOH required = (moles NaOH required) * (molar mass NaOH)

mass NaOH required = (142.74 kmol) * (40.0 kg/kmol)

mass NaOH required = 5709.7 kg

mass NaOH required = 5.7 x 10³ kg