Question:
What is the conjugate acid of \(H_{3}P_{2}O_{6}^{-}\)?
What is the conjugate acid of \(H_{3}P_{2}O_{6}^{-}\)?
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For conjugate acid–base problems: just add one \(H^+\) (increase H by 1 and increase charge by +1).
Updated On: Jun 8, 2026
- Orthophosphorus acid
- Hypophosphorus acid
- Pyrophosphoric acid
- Hypophosphoric acid
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The Correct Option is D
Solution and Explanation
Concept:
A conjugate acid is formed when a species accepts one proton (\(H^+\)). Hence, we simply add one \(H^+\) to the given anion.
Step 1: Identify the base species.
The given species is: \[ H_3P_2O_6^- \] Since it carries a negative charge, it can accept a proton and act as a Brønsted base.
Step 2: Add one proton to form conjugate acid.
\[ H_3P_2O_6^- + H^+ \rightarrow H_4P_2O_6 \] So the conjugate acid has formula: \[ H_4P_2O_6 \]
Step 3: Identify the compound.
The species \(H_4P_2O_6\) corresponds to hypophosphoric acid.
Step 4: Final answer.
\[ \boxed{\text{Hypophosphoric acid}} \]
Step 1: Identify the base species.
The given species is: \[ H_3P_2O_6^- \] Since it carries a negative charge, it can accept a proton and act as a Brønsted base.
Step 2: Add one proton to form conjugate acid.
\[ H_3P_2O_6^- + H^+ \rightarrow H_4P_2O_6 \] So the conjugate acid has formula: \[ H_4P_2O_6 \]
Step 3: Identify the compound.
The species \(H_4P_2O_6\) corresponds to hypophosphoric acid.
Step 4: Final answer.
\[ \boxed{\text{Hypophosphoric acid}} \]
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