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Ex. 500 mm of pH 2.2 rain falls on 200m x 400 m of soil.
Calculate how many kilograms of CaCO3 is needed to neutralize the H+ ions (molecular weight of CaCO3 = 100g/mol)
2x = 252,000 moles x 100g/mol 2x = 25,200,000 g x = 12,600,000 g = 12,600 kg
Q1. Why are 2 valence electrons accounted for in the equation in step 4 above?
Q2. If sodium hydroxide, NaOH, (where Na^+ + OH^- -> NaOH) was used to neutralize the acid rain instead of CaCO^3, how many hydrogen ions would each molecule of NaOh neutralize?
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