Question:
The conjugate base of $\text{H}_{2}\text{PO}_{4}^{-}$ is
The conjugate base of $\text{H}_{2}\text{PO}_{4}^{-}$ is
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Acid minus $\text{H}^{+}$ $\rightarrow$ Conjugate Base. Conversely, adding an $\text{H}^{+}$ proton to a base gives you its conjugate acid.
Updated On: Jun 3, 2026
- $\text{HPO}_{4}^{2-}$
- $\text{PO}_{4}^{3-}$
- $\text{H}_{3}\text{PO}_{4}$
- $\text{H}_{2}\text{PO}_{4}^{2-}$
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The Correct Option is A
Solution and Explanation
Step 1: Concept
According to the Brønsted-Lowry acid-base theory, an acid turns into its conjugate base after donating a proton ($\text{H}^{+}$).
Step 2: Meaning
To determine the conjugate base of any chemical species, remove exactly one hydrogen ion ($\text{H}^{+}$) from its formula and decrease its net electrical charge by one unit.
Step 3: Analysis
Starting with the dihydrogen phosphate ion, $\text{H}_{2}\text{PO}_{4}^{-}$: 1. Remove one $\text{H}^{+}$ ion, leaving behind $\text{HPO}_{4}$. 2. Decreasing the charge from $-1$ by one more unit results in a charge of $-2$. This yields the monohydrogen phosphate ion, $\text{HPO}_{4}^{2-}$.
Step 4: Conclusion
Thus, the conjugate base of $\text{H}_{2}\text{PO}_{4}^{-}$ is $\text{HPO}_{4}^{2-}$.
Final Answer: (A)
According to the Brønsted-Lowry acid-base theory, an acid turns into its conjugate base after donating a proton ($\text{H}^{+}$).
Step 2: Meaning
To determine the conjugate base of any chemical species, remove exactly one hydrogen ion ($\text{H}^{+}$) from its formula and decrease its net electrical charge by one unit.
Step 3: Analysis
Starting with the dihydrogen phosphate ion, $\text{H}_{2}\text{PO}_{4}^{-}$: 1. Remove one $\text{H}^{+}$ ion, leaving behind $\text{HPO}_{4}$. 2. Decreasing the charge from $-1$ by one more unit results in a charge of $-2$. This yields the monohydrogen phosphate ion, $\text{HPO}_{4}^{2-}$.
Step 4: Conclusion
Thus, the conjugate base of $\text{H}_{2}\text{PO}_{4}^{-}$ is $\text{HPO}_{4}^{2-}$.
Final Answer: (A)
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