Oxidising product of substance `Na_(3)AsO_(3)` would be

Options

A. `As_(2)O_(3)^(3-)`
B. `AsO_(3)^(-3)`
C. `AsO_(2)^(-4)`
D. `AsO_(4)^(-3)`

Answer

To determine the oxidizing product of the substance \( \text{Na}_3\text{AsO}_3 \), we need to follow these steps:

### Step 1: Determine the oxidation state of arsenic (As) in \( \text{Na}_3\text{AsO}_3 \).

The formula for calculating the oxidation state of arsenic in \( \text{Na}_3\text{AsO}_3 \) is as follows:

\[ \text{Oxidation state of Na} + \text{Oxidation state of As} + \text{Oxidation state of O} = 0 \]

Given that sodium (Na) has an oxidation state of +1 and oxygen (O) has an oxidation state of -2, we can set up the equation:

\[ 3(+1) + x + 3(-2) = 0 \]

Where \( x \) is the oxidation state of arsenic (As).

### Step 2: Solve the equation.

Substituting the values into the equation:

\[ 3 + x - 6 = 0 \]

This simplifies to:

\[ x - 3 = 0 \]

Thus,

\[ x = +3 \]

### Step 3: Identify the oxidizing product.

Since the oxidation state of arsenic in \( \text{Na}_3\text{AsO}_3 \) is +3, we need to find a product where the oxidation state of arsenic is greater than +3, indicating that oxidation has occurred (loss of electrons).

### Step 4: Evaluate the options.

We will evaluate the oxidation states of arsenic in the given options:

- **Option A: \( \text{As}_2\text{O}_3^{3-} \)**

\[ 2x - 6 = -3 \quad \Rightarrow \quad 2x = 3 \quad \Rightarrow \quad x = +1.5 \]

- **Option B: \( \text{AsO}_3^{3-} \)**

\[ x - 6 = -3 \quad \Rightarrow \quad x = +3 \]

- **Option C: \( \text{AsO}_4^{3-} \)**

\[ x - 8 = -3 \quad \Rightarrow \quad x = +5 \]

### Step 5: Conclusion.

Among the options, the only one where the oxidation state of arsenic is greater than +3 is:

- **Option C: \( \text{AsO}_4^{3-} \)** with an oxidation state of +5.

Thus, the oxidizing product of \( \text{Na}_3\text{AsO}_3 \) is \( \text{AsO}_4^{3-} \).

### Final Answer:
The oxidizing product of \( \text{Na}_3\text{AsO}_3 \) is \( \text{AsO}_4^{3-} \).

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