Please help!...
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. Write ionic and net ionic equations to show how limestone reacts with HNO3 and H2SO4 to neutralize them. How would you be able to tell if the neutralization process was working?
2HNO3 + CaCO3 ==> CO2 + H2O + Ca(NO3)2
H2SO4 + CaCO3 ==> CO2 + H2O + CaSO4
You can turn them into ionic and net ionic equations.
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 1.7×10^−5M in H2SO4 and 8.8×10−6M in HNO3?
Well, if I were a limestone, I would say to HNO3 and H2SO4, "Hey acids, let's neutralize this situation!" Here's how it would go down in ionic and net ionic equation form:
For the reaction with HNO3:
Ionic equation: CaCO3 (s) + 2H+ (aq) + 2NO3- (aq) -> Ca2+ (aq) + 2NO3- (aq) + H2O (l) + CO2 (g)
Net ionic equation: CaCO3 (s) + 2H+ (aq) -> Ca2+ (aq) + H2O (l) + CO2 (g)
And now for the H2SO4 party:
Ionic equation: CaCO3 (s) + H+ (aq) + SO42- (aq) -> Ca2+ (aq) + SO42- (aq) + H2O (l) + CO2 (g)
Net ionic equation: CaCO3 (s) + H+ (aq) -> Ca2+ (aq) + H2O (l) + CO2 (g)
To see if the neutralization process is working, you can use a couple of indicators. One option is to test the pH of the water and see if it moves closer to a neutral pH of 7. Additionally, you can do a visual observation of the water. If it becomes less cloudy or clears up, then it's a good sign that the acid be gone!
To write the ionic and net ionic equations for the neutralization of HNO3 and H2SO4 by limestone, we need to consider the dissociation of these acids and the reaction with calcium carbonate (limestone).
1. HNO3 + CaCO3 → Ca(NO3)2 + H2O + CO2
The ionic equation of the reaction is:
H+ + NO3- + CaCO3 → Ca2+ + 2NO3- + H2O + CO2
The net ionic equation is:
H+ + CaCO3 → Ca2+ + CO2 + H2O
2. H2SO4 + CaCO3 → CaSO4 + H2O + CO2
The ionic equation of the reaction is:
2H+ + SO4- + CaCO3 → Ca2+ + SO4- + H2O + CO2
The net ionic equation is:
2H+ + CaCO3 → Ca2+ + CO2 + H2O
To determine if the neutralization process is working, you can observe the following phenomena:
1. pH: The addition of limestone should increase the pH of the acidified water toward a neutral pH of 7.
2. Effervescence: The formation of carbon dioxide gas (CO2) during the reaction would cause bubbling or effervescence in the water.
3. Calcium precipitation: Calcium carbonate (CaCO3) is likely to precipitate as a white solid upon neutralization. The presence of a white precipitate indicates that the neutralization process is occurring.
Overall, monitoring changes in pH, observation of effervescence, and the formation of a white precipitate can indicate if the neutralization process is working.
To write the ionic and net ionic equations for the reaction between limestone (CaCO3) and acids such as HNO3 and H2SO4, we first need to know the chemical formulas and charges of the ions involved.
Ionic equation for the reaction between CaCO3 and HNO3:
CaCO3 + 2HNO3 → Ca(NO3)2 + CO2 + H2O
In this reaction, the calcium carbonate (CaCO3) reacts with two molecules of nitric acid (HNO3) to form calcium nitrate (Ca(NO3)2), carbon dioxide (CO2), and water (H2O).
Net ionic equation for the reaction between CaCO3 and HNO3:
CaCO3 + 2H+ → Ca2+ + CO2 + H2O
By canceling out spectator ions (ions that do not participate in the chemical reaction), we can simplify the ionic equation to obtain the net ionic equation. In this case, the spectator ions are the nitrate ions (NO3-).
Ionic equation for the reaction between CaCO3 and H2SO4:
CaCO3 + H2SO4 → CaSO4 + CO2 + H2O
In this reaction, the calcium carbonate (CaCO3) reacts with sulfuric acid (H2SO4) to form calcium sulfate (CaSO4), carbon dioxide (CO2), and water (H2O).
Net ionic equation for the reaction between CaCO3 and H2SO4:
CaCO3 + H+ → Ca2+ + CO2 + H2O
Again, by canceling out spectator ions (in this case, the sulfate ions (SO4-2)), we obtain the simplified net ionic equation.
To determine if the neutralization process is working, you can perform a few tests:
1. pH test: Monitor the pH of the acidified water before and after the addition of limestone. If the pH increases significantly after adding limestone, it indicates that the acidity has decreased, suggesting a successful neutralization process.
2. Carbon dioxide test: Collect a gas sample from the acidified water before and after the addition of limestone. Bubble the collected gas through limewater (Ca(OH)2 solution) or use an indicator solution that changes color in the presence of carbon dioxide. If the gas sample from the neutralized water produces a positive result, it confirms the production of carbon dioxide gas during the neutralization reaction.
3. Observation of precipitation: If the neutralization process is successful, the formation of a precipitate (solid) should occur. In the case of the reaction between limestone and H2SO4, the formation of calcium sulfate (CaSO4) as a precipitate indicates neutralization.
By employing these tests, you can assess if the neutralization process using limestone is effective in neutralizing acidified water.