Chemistry · Group 13 to Group 18 Elements
Complete the following reaction,
Complete the following reaction, \( P_{4}+ \) \( N a O H+H_{2} O \rightarrow ? \)
- A. \( P H_{3}+N a_{2} H P O_{2} \)
- B. \( P H_{3}+N a H_{2} P O_{2} \)
- C. \( H_{3} P O_{4}+N a O \)
- D. \( P H_{3}+N a_{2} P O_{4} \)
Step-by-step solution
White phosphorus (P4) reacts with aqueous NaOH in a disproportionation reaction. P4 is both oxidized and reduced: the oxidation state of phosphorus in PH3 is -3 (reduction) and in NaH2PO2 it is +1 (oxidation). The balanced equation is: P4 + 3NaOH + 3H2O → PH3 + 3NaH2PO2. Hence, the products are phosphine and sodium hypophosphite.
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