The reaction of white phosphorous with aqueous `NaOH` gives phosphine along with another phosphorous containing compound. The reaction type , the oxidation state of phosphorous in phosphine and in the other products are, respectively,

Options

A. redox reaction , `- 3 and - 5`
B. redox reaction , `+3 and + 5`
C. disproportionation reaction , ` - 3 and + 5`
D. Disproportionation reaction , ` - 3 and + 3`.

Explanation

To solve the problem, we need to analyze the reaction of white phosphorus with aqueous sodium hydroxide (NaOH) and identify the products formed, the type of reaction, and the oxidation states of phosphorus in the relevant compounds. Here’s a step-by-step breakdown:

### Step 1: Identify the Reaction
White phosphorus (P₄) reacts with aqueous NaOH. The reaction can be represented as:
\[ P_4 + NaOH \rightarrow PH_3 + Na_3PO_3 \]
Where Na₃PO₃ is sodium phosphite.

### Step 2: Identify the Products
In this reaction, phosphine (PH₃) is produced along with sodium phosphite (Na₃PO₃).

### Step 3: Determine the Oxidation State of Phosphorus in Phosphine (PH₃)
In phosphine (PH₃), phosphorus is bonded to three hydrogen atoms. The oxidation state can be calculated as follows:
- Let the oxidation state of phosphorus be \( x \).
- The oxidation state of hydrogen is +1.
- The equation becomes:
\[ x + 3(+1) = 0 \]
Solving this gives:
\[ x + 3 = 0 \implies x = -3 \]
Thus, the oxidation state of phosphorus in phosphine (PH₃) is **-3**.

### Step 4: Determine the Oxidation State of Phosphorus in Sodium Phosphite (Na₃PO₃)
For sodium phosphite (Na₃PO₃):
- Sodium (Na) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- Let the oxidation state of phosphorus be \( y \).
- The equation for sodium phosphite becomes:
\[ 3(+1) + y + 3(-2) = 0 \]
Solving this gives:
\[ 3 + y - 6 = 0 \implies y - 3 = 0 \implies y = +3 \]
Thus, the oxidation state of phosphorus in sodium phosphite (Na₃PO₃) is **+3**.

### Step 5: Determine the Reaction Type
Since the same element (phosphorus) is both oxidized and reduced in this reaction, it is classified as a **disproportionation reaction**.

### Step 6: Summary of Findings
- The reaction type is **disproportionation**.
- The oxidation state of phosphorus in phosphine (PH₃) is **-3**.
- The oxidation state of phosphorus in sodium phosphite (Na₃PO₃) is **+3**.

### Final Answer
- Reaction Type: **Disproportionation**
- Oxidation State of Phosphorus in PH₃: **-3**
- Oxidation State of Phosphorus in Na₃PO₃: **+3**