(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

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. Relevant 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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# Acid rain titration problem

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