In the following reaction `HC_(2)O_(4)^(-)(aq)+PO_(4)^(3-)(aq)hArrHPO_(4)^(-2)(aq)+C_(2)O_(4)^(2-)(aq)`, which are the two Bronsted bases?

Options

A. `HC_(2)O_(4)^(-)` and `PO_(4)^(3-)`
B. `HPO_(4)^(2-)+C_(2)O_(4)^(2-)`
C. `HC_(2)O_(4)^(-)` and `HPO_(4)^(2-)`
D. `PO_(4)^(3-)` and `C_(2)O_(4)^(2-)`

Explanation

To determine the two Bronsted bases in the given reaction:

**Reaction:**
\[ HC_2O_4^{-} (aq) + PO_4^{3-} (aq) \rightleftharpoons HPO_4^{2-} (aq) + C_2O_4^{2-} (aq) \]

**Step 1: Identify the acids and bases.**
- According to the Bronsted-Lowry theory, acids are proton (H⁺) donors, and bases are proton acceptors.
- In the reaction, \( HC_2O_4^{-} \) donates a proton to \( PO_4^{3-} \), forming \( HPO_4^{2-} \) and \( C_2O_4^{2-} \).
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