# Acid rain titration problem

1. Homework Statement
Estimate the volume of acid rain in L that can be neutralized by 1.00 g of limestone. Assume the pH of rainwater collected in your rain gauge is a representative value for acid rain. Assume that acid rain contains sulfuric acid as the source of hydrogen ions. The molecular weight of calcium carbonate is 100.09 g/mol.
This is a question from my meteorology lab and I haven't had chemistry in 4 years, so I'm a bit rusty. Any help would be gladly appreciated!

2. Homework Equations
The net reaction between the two is
H2SO4 + CaCO3 --> CaSO4H20 +CO2

3. The Attempt at a Solution

I know that we had 1.00 g CaCO3 and the molecular weight is 100.09. So I think I divide and plug this into the moles of CaCO3. Then our pH for the rainwater which would be 7.04, but I'm not really sure what to do with it since its not in mols?
I'm pretty lost.

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TMM
Do you remember the definition of pH?

It's -log(molar concentration of H+ ions). You can use this to find the mols/L of H+ ions in the rain water.

Ok so if I did this right, we have 9.12e-8 mol/L of H+ ions. Then we had 100.09 mols of CaCO3. I also know that the pH of the solution after neutralization is 4.36, but I don't really understand how to plug these into the equation since all of the units are different.

GCT