1) Compute the molar concentration of SO3, according to Smith's analysis. Note that one British grain = 0.0648 grams, and one British gallon = 4.546 liters.
2) Estimate the pH of Glasgow rain, assuming that each mole of SO3 becomes one mole of H2SO4.
3) Elsewhere in his book, Smith noted that much of the acid found in the rainwater of towns was actually sulphurous acid (H2SO3) rather than sulphuric acid (H2SO4). What would the pH be if the [SO3] concentration computed above was equivalent to H2SO3? The acid dissociation constant for
H2SO3 < ---- > H+ + HSO3-is Ka = 1.54x10-2 . (Hint: considering only the first dissociation constant is sufficient for this problem; however, assuming that equilibrium [H2SO3] is the same as initial [H2SO3] is not permissible.)
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