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Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a
Chapter 7, Problem 104P(choose chapter or problem)
Lakes that have been acidified by acid rain (\(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\)) can be neutralized by a process called liming, in which limestone (\(\mathrm{CaCO}_{3}\)) is added to the acidified water. Write ionic and net ionic equations to show how limestone reacts with \(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) to neutralize them. How would you be able to tell if the neutralization process was working?
Questions & Answers
QUESTION:
Lakes that have been acidified by acid rain (\(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\)) can be neutralized by a process called liming, in which limestone (\(\mathrm{CaCO}_{3}\)) is added to the acidified water. Write ionic and net ionic equations to show how limestone reacts with \(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) to neutralize them. How would you be able to tell if the neutralization process was working?
ANSWER:Step 1 of 2
Let's consider Nitric acid \(\left(\mathrm{HNO}_{3}\right)\) and limestone (Calcium carbonate \(\left.\left(\mathrm{CaCO}_{3}\right)\right)\) :
The balanced molecular equation is:
\(2 \mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{~s})+\mathrm{CO}_{2}(\mathrm{gas})+\mathrm{H}_{2} \mathrm{O}(\mathbf{l})\)
The complete ionic equation :
\(\mathbf{H}^{+}(\mathbf{a q})+\mathrm{NO}_{3}^{-(a q)}+\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{Ca}^{2+}(\text { aq })+\mathrm{NO}_{3}^{-(a q)}+\mathrm{CO}_{2}(\text { gas })+\mathrm{H}_{2} \mathrm{O}(\mathbf{l})\)
The net ionic equation:
To write net ionic equation, we cancel out the ions that is on both the sides, which are spectator ions.
\(\mathrm{H}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{Ca}^{2+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{gas})+\mathrm{H}_{2} \mathrm{O}(1)\)
And the net ionic equation is as follows:
\(\mathbf{H}^{+}(\mathbf{a q})+\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{Ca}^{2+}(\mathbf{a q})+\mathrm{CO}_{2}(\text { gas })+\mathrm{H}_{2} \mathrm{O}(\mathbf{l})\)
In the above reactions, we can say that by adding limestone, the nitric acid neutralized to form calcium nitrate and precipitated and water was formed and \(\mathrm{CO}_{2}\) was liberated.