The ion HPO4–2 has both a conjugate base as well as a conjugate acid. The conjugate base of this ion is (1) while the conjugate acid is (2).
a) (1) = H2PO4– (2) H3PO4
b) (1) = PO4– (2) H2PO4+
c) (1) = PO4–3 (2) H2PO4–
d) (1) = HPO5–3 (2) HPO3–
e) (1) = H2PO4– (2) PO4–3
help! don't know what to do
You're over thinking this. Write out the corresponding reactions.
First, it can donate a proton as in
HPO4^2- ==> H^+ + PO4^3-
And it can accept a proton.
HPO4^2- + H^+ ==> H2PO4^-
That's all there is to it. You add a proton or you take away a proton.
To determine the conjugate base and conjugate acid for the ion HPO4–2, we need to understand the concept of conjugate acids and bases.
A conjugate acid is formed when a base gains a proton (H+), and a conjugate base is formed when an acid loses a proton (H+). In this case, the ion HPO4–2 acts as a conjugate base because it can accept a proton (H+) to form its conjugate acid.
To find the conjugate acid, we need to identify the species that can donate a proton (H+) to the ion HPO4–2. The conjugate acid will have one more proton (H+) than the original ion.
Let's analyze the answer choices:
a) (1) = H2PO4– and (2) = H3PO4
b) (1) = PO4– and (2) = H2PO4+
c) (1) = PO4–3 and (2) = H2PO4–
d) (1) = HPO5–3 and (2) = HPO3–
e) (1) = H2PO4– and (2) = PO4–3
The correct pair for the conjugate base and conjugate acid is (1) = H2PO4– and (2) = H3PO4. This is because H3PO4 has one more proton (H+) than H2PO4–, making it the conjugate acid.
Therefore, the answer is option a) (1) = H2PO4– and (2) = H3PO4.