prettygirlgwen24
21.02.2020 •
Chemistry
The amount of sulfuric acid produced can be determined by titration with sodium hydroxide of known concentration. A 631.0 g sample of air that is known to contain sulfur dioxide was reacted with excess hydrogen peroxide. Given that 18.50 mL of 0.00250 M NaOH ( aq ) was required to neutralize the H 2 SO 4 ( aq ) produced, calculate the mass percentage of SO 2 ( g ) in the air sample.
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Ответ:
0.000234 %
Explanation:
Equation of reaction of SO₂ and H₂O₂
SO₂ + H₂O₂ → H₂SO₄
Equation of neutralization of NaOH and H₂SO₄
H₂SO₄ + 2 NaOH → Na₂SO₄ + 2 H₂O
Molar mass of NaOH = 29.997 g/mol
molar mass of H₂SO₄ = 98.079 g/mol
molar mass of SO₂ =64.066 g/mol
number of moles of NaOH = molarity × volume in L = 0.00250 M × (18.50 / 1000) = 0.00004625 mol
comparing the equation
2 moles of NaOH requires 1 mole of H₂SO₄
0.00004625 mol will require 0.000023125 mole of H₂SO₄
1 mole of SO₂ produced 1 mole of H₂SO₄
0.000023125 mole of SO₂ will produce 0.000023125 mole of H₂SO₄
Mass of SO₂ = 0.000023125 mole × 64.066 g/mol ( mole x molar mass) = 0.00148 g
mass percentage of SO₂ = 0.00148 g / 631 g × 100 = 0.000234 %
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