A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour. Most of the coal burned in the United States contains 1 to 4 % by weight sulfur in the form of pyrite, which is oxidized as the coal burns: 4FeS2(s) 11 O2(g) 2 Fe2O3(s) 8 SO2(g) Once in the atmosphere, the SO2 is oxidized to SO3, which then reacts with water in the atmosphere to form sulfuric acid: SO3(g) H2O(l) H2SO4(aq) If 61.7 metric tons of coal that contains 1.20 % by weight S is burned and all of the sulfuric acid that is formed rains down into a pond of dimensions 397 m x 258 m x 5.64 m, what is the pH of the pond

the pH of the pond is 4.0963

Explanation:

 Given the data in the question;

4FeS₂(s) + 11O₂(g)  >  2Fe₂O₃(s) + 8SO₂(g)

and oxidation of sulfur dioxide to trioxide

SO₃(g) + H₂O(l)  > H₂SO₄(aq)

given that; coal = 61.7 metric tons = 61700 kg

1.20 % by weight S, therefore mass of sulfur in coal will be;

⇒ 61700 × 1.20% = 740.4 kg

moles of sulfur = (740.4 × 1000 g) / 32 g/mole = 23,137.5 moles

moles of so₂ produced

= same moles of so₃ and same moles of H₂SO₄ = 23,137.5 moles

volume of pond = 397 m x 258 m x 5.64 m = 577,682.64 m³ = 577682640 L

Molarity = moles / volume = 23,137.5 / 577682640 = 4.0052 × 10⁻⁵ M

now each mole of  H₂SO₄ will give 2 moles of H⁺

[H⁺] = 2 × 4.0052 × 10⁻⁵ =  8.0104 × 10⁻⁵ M

pH = -log[H⁺]  

pH = -log [ 8.0104 × 10⁻⁵ M ]

pH = 4.0963

Therefore, the pH of the pond is 4.0963

samuel de champlain. in 1608, king henry iv sponsored pierre dugua, sieur de mons and samuel de champlain as founders of the city of quebec with 28 men. this was the second permanent french settlement in the colony of canada.