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The quantity of atmospheric SO2(g) can be determined by reaction with H2O2(aq) The amount of sulfuric...

The quantity of atmospheric SO2(g) can be determined by reaction with H2O2(aq)

The amount of sulfuric acid produced can be determined by titration with sodium hydroxide of known concentration. An 571.0 gram sample of an air that is known to contain sulfur dioxide was reacted with excess hydrogen peroxide. Given that 18.50 mL of a 0.00250 M NaOH(aq) were required to neutralize the H2SO4(aq) produced, calculate the mass percentage of SO2(g) in the air sample.

Expert Solution

Balanced reaction between SO₂ and H₂O₂

SO₂ + H₂O₂ H₂SO₄

this H₂SO₄ requied 18.50 ml 0.00250 M NaOH to neutrilize

no. of mole = molarity X volume of solution in liter

18.50 ml = 0.0185 liter

no. of mole of NaOH = 0.00250 X 0.0185 = 4.625 X 10^-5 mole of NaOH

Balanced neutrilization reaction between NaOH and H₂SO₄ is

H₂SO₄ + 2 NaOH Na₂SO₄ + 2H₂O

According to reaction 2 mole NaOH react wirh 1 mole H₂SO₄ therefore to react with 4.625 X 10^-5 mole of NaOH requied H₂SO₄ = 4.625 X 10^-5 / 2 = 2.3125 X 10^-5 mole

2.3125 X 10^-5 mole of H₂SO₄ produced from SO₂

1 mole SO₂ prodce 1 mole of H₂SO₄ therefore to produce 2.3125 X 10^-5 mole H₂SO₄ requied SO₂ =

2.3125 X 10^-5 mole

molar mass of SO₂ = 64.066 gm/mole then 2.3125 X 10^-5 mole of SO₂ = 2.3125 X 10^-5 X 64.066 = 0.001482 gm

0.001482 gm of SO₂ in 571 gm air sample

% by mass of solute = mass of solute X 100 / mass of solution

% by mass of SO₂ = 0.001482 X 100 / 571

= 0.0002595 %

mass % concentration of SO₂ = 0.0002595 %

queen_honey_blossom answered 2 years ago

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