Question

The conjugate base of HPO4^(-2) is
1. PO4^(-3)
2. PO4^(-2)
3. H2PO4^(-1)
4. H3PO4 ​

Answer 1

PO4^3-

To find the conjugate acid, Add a H+ to get

H2PO4−

Note the charge is only -1 now. This ion can lose the proton to go back to it’s conjugate base form or it can also gain a second proton to become the conjugate acid. This is an amphiprotic ion. It goes both ways.

H3PO4

This final ion is phosphoric acid.

The first species mentioned in the question is also amphiprotic and could have lost its one proton to become the phosphate ion.

PO4^3-
The conjugate base of H2 PO4 - is HPO4 -2. 

Answer 2

The conjugate base of $HPO_4^{2-}$ is $PO_4^{3-}$

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

• An acid is defined as a substance which looses or donates protons and thus forming conjugate base.
• A base is defined as a substance which accepts protons and thus forming conjugate acid.

To form a conjugate base of $HPO_4^{2-}$, this compound will loose one proton to form $PO_4^{3-}$

The chemical equation for the formation of conjugate base follows:

$HPO_4^{2-}\rightarrow PO_4^{3-}+H^+$

The conjugate base formed is phosphate ion

Learn more about Bronsted-Lowry conjugate acid-base theory:

https://brainly.com/question/14203816

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