Hey..can you check this for me. It has to do with Predicting Acid-Base Reactions. So here it is:
I have to:
Predict the most likely acid base reaction(s) that occur.
For each reaction, state if the reaction is quantitative, or, if not, state whether products or reactants are favoured at equilibrium.
Here is the question:
1. 100 mL of 0.1 mol/L nitric acid reacts with 100 mL of 0.1 mol/L ammonium hydrogen carbonate
My answer:
Acid-base reaction: 2H3O+ + H2CO3- >>> H3CO3- + 2H2O
Quantitative: yes
Is this right and did I cover all points of the question? One more thing, what does quantitative mean in this situation?
Quantitative, to me, means that the reaction goes as predicted at essentially 100% yield; i.e., we get the amount of product which we predict we will get. As for your answer, ammonium hydrogen carbonate is NH4HCO3 but I don't see that anywhere in your equation. And I have no idea what H3CO3^- is. I, too, think the reaction is quantitative in that 100 mL of 0.1 M acid reacts with exactly 100 mL of 0.1 M base. You may want to try the equation again. May I suggest you write the molecular equation and not the ionic equation.
You're correct about the meaning of quantitative in this context. However, the answer you provided doesn't seem to correspond to the given reactants.
Remember that the reactants are nitric acid (HNO₃) and ammonium hydrogen carbonate (NH₄HCO₃).
Here's the correct molecular equation for the reaction between nitric acid and ammonium hydrogen carbonate:
HNO₃ + NH₄HCO₃ → NH₄NO₃ + CO₂ + H₂O
The reaction is quantitative, meaning that both reactants will react completely to form the products, assuming the concentrations are equal, as given in the question.
To predict acid-base reactions and determine if they are quantitative or not, you need to follow these steps:
1. Identify the acid and the base in the reaction. In this case, nitric acid (HNO3) is the acid and ammonium hydrogen carbonate (NH4HCO3) is the base.
2. Write down the balanced equation for the acid-base reaction. In this case, nitric acid (HNO3) donates a proton (H+) to ammonium hydrogen carbonate (NH4HCO3), forming nitrate ion (NO3-) and water (H2O):
HNO3 + NH4HCO3 → NH4NO3 + H2O
3. To determine if the reaction is quantitative, you need to consider whether it goes to completion (100% yield of products) or not. In this case, since the reaction involves a strong acid (HNO3) and a weak base (NH4HCO3), it is expected to go to completion. Therefore, the reaction is quantitative.
Now, let's address the issue with your answer. You wrote the equation as:
2H3O+ + H2CO3- → H3CO3- + 2H2O
However, this equation does not match the reactants in the question, and it includes species like H3CO3^- that are not relevant to this specific reaction.
In summary, the corrected equation for the reaction described in the question is:
HNO3 + NH4HCO3 → NH4NO3 + H2O
And you correctly determined that this reaction is quantitative, meaning it goes to completion with a 100% yield of products.