Problem: Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3 ) is added to the acidified water.What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 1.8×10−5 M in H2SO4 and 8.8×10−6 M in HNO3 ?

🤓 Based on our data, we think this question is relevant for Professor Lockhart's class at Adelphi University.

FREE Expert Solution
  • First thing is to write the balanced acid-base reaction of CaCO3 with HNOand H2SO4. Then use stoichiometry to calculate the mass of CaCO3 from the given molarity and volume of acids. We need the Molar mass of CaCO3 in this case.
  • Acid-base reactions produce water and salt in the process
  • The following molecules dissociates as CaCO(Ca2+ and CO32-), HNO3 (Hand NO3-) and H2SO4 (H+ and SO42-)
  • Acid-base reaction is also a double displacement reaction so we just exchange the counter ions
  • CaCO3 (s) and HNO(aq) will produce Ca(NO3)2 + *H2CO3 or H2O (l) + CO(g) (*H2CO3 will spontaneously transform to COand H2O in natural conditions)
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Problem Details

Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3 ) is added to the acidified water.

What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 1.8×10−5 M in H2SO4 and 8.8×10−6 M in HNO3 ?

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Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

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Based on our data, we think this problem is relevant for Professor Lockhart's class at Adelphi University.