To determine the proton donor and acceptor in the reaction:
[tex]\[ CO_3^{2-}(aq) + H_2O(l) \rightarrow HCO_3^-(aq) + OH^-(aq) \][/tex]
we need to understand the basic concept of acid-base reactions involving proton transfers.
1. Identify the proton donor:
A proton donor is a species that loses or donates a proton (H⁺) during the reaction. In this context, we need to examine what happens to each species in the reaction.
- Water (H₂O) can donate a proton to become OH⁻.
- Assuming water donates a proton, it will transform to OH⁻, which is exactly shown in the product side of the reaction.
2. Identify the proton acceptor:
A proton acceptor is a species that gains or accepts a proton during the reaction.
- Carbonate ion (CO₃²⁻) when it accepts a proton, will convert into bicarbonate ion (HCO₃⁻).
- Since we see that HCO₃⁻ is a product, it indicates that CO₃²⁻ has gained a proton, thus acting as the proton acceptor.
From this analysis:
- Proton donor: H₂O (which donates a proton and turns into OH⁻)
- Proton acceptor: CO₃²⁻ (which accepts the proton and turns into HCO₃⁻)
Therefore, the correct identification is:
- Donor: [tex]\( H_2O \)[/tex]
- Acceptor: [tex]\( CO_3^{2-} \)[/tex]
Thus, the correct answer is:
- Donor: [tex]\( H_2O \)[/tex]; acceptor: [tex]\( CO_3^{2-} \)[/tex]
