Write the balanced net ionic equation for the following reaction and determine the conjugate acid-base pairs.
HNO3(aq)+Li2CO3(aq)<--->LiNo3(aq)+LiHCO3(aq)
Which component in the net ionic equation is the acid, the base, the conjugate base, and the conjugate acid
Thank you
This is the equation given. I came up with H+(aq)+CO32-(aq)<-->HCO3-(aq)
and the net ionic acid is HNO3(aq), the base NO3-(aq), conjugate acid HCO3-(aq)and the conjugant acid as CO32-(aq)
Net ionic equation: H3O+(aq) + CO3^2-(aq) <--> HCO3-(aq) + H2O(l)
Acid: H3O+
Base: CO3^2-
Conjugate Acid: HCO3-
Conjugate Base: H2O
The hydrogen ion (H+) doesn't exist on its own in aqueous solutions because it's attracted to the unshared oxygen electrons in water. This forms hydronium (H3O+) ions, which are more stable.
Water is amphiprotic/amphoteric which means it can act as either acid or base. In this case, we need it to act as the missing base and to balance the net equation.
Please do not ask me why this is the answer, I have no clue, and what's above is just how I made it make sense for me.
I apologize for any confusion, but let's take a closer look at the balanced net ionic equation and the conjugate acid-base pairs.
The balanced net ionic equation for the reaction is:
H+(aq) + CO32-(aq) ↔ HCO3-(aq)
In this equation, the H+(aq) is the acid, as it donates a proton (H+) to the base, CO32-(aq). The CO32-(aq) is the base, as it accepts a proton (H+).
The HCO3-(aq) is the conjugate base, as it is formed when the acid loses a proton (H+). The CO32-(aq) is the conjugate acid, as it is formed when the base gains a proton (H+).
To clarify:
Acid: H+(aq)
Base: CO32-(aq)
Conjugate Base: HCO3-(aq)
Conjugate Acid: CO32-(aq)
I hope this clears things up!
To write the balanced net ionic equation, we need to start with the balanced molecular equation:
HNO3(aq) + Li2CO3(aq) ↔ LiNO3(aq) + LiHCO3(aq)
First, we identify the strong electrolytes, which are the compounds that dissociate into ions when they are in aqueous solution. In this case, HNO3, LiNO3, and LiHCO3 are all strong electrolytes. However, Li2CO3 is a weak electrolyte because it does not completely dissociate into ions.
Next, we need to write the balanced ionic equation by separating the soluble strong electrolytes into their respective ions:
H+(aq) + NO3-(aq) + Li+(aq) + CO3^2-(aq) ↔ Li+(aq) + NO3-(aq) + Li+(aq) + HCO3-(aq)
Now, we can see that the NO3- ions and the Li+ ions exist on both sides of the equation. These ions are considered "spectator ions" and can be eliminated from the equation.
H+(aq) + CO3^2-(aq) ↔ HCO3-(aq)
This is the balanced net ionic equation.
Now, let's determine the conjugate acid-base pairs:
Acid: HNO3(aq) is the acid in the balanced molecular equation.
Base: Li2CO3(aq) is the base in the balanced molecular equation.
Conjugate acid: HCO3-(aq) is the conjugate acid formed from the base CO3^2-.
Conjugate base: CO3^2-(aq) is the conjugate base formed from the acid HCO3-.
So, in summary:
Acid: HNO3(aq)
Base: Li2CO3(aq)
Conjugate acid: HCO3-(aq)
Conjugate base: CO3^2-(aq)
Your net ionic equation is correct. Good work. However, I think the problem is a little misleading since the net ionic equation doesn't have a conjugate base for the acid. If you write
H^+ + CO3^2- ==> HCO3^- as the net ionic equation, which I believe is correct, then the CO3^2- is the base and HCO3^- is the conjugate acid. Then H^+ is the acid but no conjugate base is shown because the NO3^- cancels when the net ionic equation is written. If you write HNO3 + CO3^2- ==> HCO3^- + NO3^- then HNO3 is the acid with NO3^- as its conjugate base while CO3^2- is the base with HCO3^- as the conjugate acid. I hope this makes sense. The main reason I think the problem is misleading is because it asks for the net ionic pairs yet the ionic part of the conjugate base (nitrate) cancels when one writes the net ionic equation. Technically I don't think that part has an answer.