Question

Strong reducing behaviour of \( \text{H}_3 \text{PO}_4 \) is due to

• A. presence of one \( -OH \) group and two P-H bonds
• B. high electron gain enthalpy of phosphorus
• C. high oxidation state of phosphorus
• D. presence of two \( -OH \) groups and one P-H bond

Hint:

Reducing agents typically have bonds that are easy to break, such as \( -OH \) and P-H in the case of \( \text{H}_3 \text{PO}_4 \).

Answer 1

The Correct Option is A

Step 1: Understand the reducing nature.
The reducing behavior of \( \text{H}_3 \text{PO}_4 \) is largely due to the presence of the \( -OH \) group and P-H bonds. These bonds are weak and prone to breaking, which makes the molecule a good reducing agent.
Step 2: Conclusion.
The strong reducing behavior of \( \text{H}_3 \text{PO}_4 \) is due to the presence of one \( -OH \) group and two P-H bonds. Final Answer: \[ \boxed{\text{Presence of one } -OH \text{ group and two P-H bonds}} \]