`Na_(3)PO_(4)+Fe_(2)(SO_(4))_(3) to FePO_(4) darr+Na_(2)SO_(4)`

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Answer

To analyze the reaction of sodium phosphate (Na₃PO₄) with iron(III) sulfate (Fe₂(SO₄)₃) and determine the nature of the product formed, we can follow these steps:

### Step 1: Write the Balanced Chemical Equation
We start with the unbalanced reaction:
\[ \text{Na}_3\text{PO}_4 + \text{Fe}_2(\text{SO}_4)_3 \rightarrow \text{FePO}_4 + \text{Na}_2\text{SO}_4 \]

To balance this equation, we need to ensure that the number of atoms of each element is the same on both sides.

1. Sodium (Na): There are 3 Na in Na₃PO₄ and 2 Na in Na₂SO₄. Thus, we need to balance sodium by adjusting the coefficients.
2. Phosphate (PO₄): There is 1 phosphate group from Na₃PO₄ and 1 from FePO₄, which is balanced.
3. Iron (Fe): There are 2 Fe in Fe₂(SO₄)₃ and 1 in FePO₄, so we need to adjust the coefficient of FePO₄.
4. Sulfate (SO₄): There are 3 sulfate ions in Fe₂(SO₄)₃ and 2 in Na₂SO₄.

The balanced equation becomes:
\[ 2 \text{Na}_3\text{PO}_4 + 3 \text{Fe}_2(\text{SO}_4)_3 \rightarrow 6 \text{FePO}_4 + 3 \text{Na}_2\text{SO}_4 \]

### Step 2: Identify the Products
From the balanced equation, we see that the products are:
- Iron(III) phosphate (FePO₄)
- Sodium sulfate (Na₂SO₄)

### Step 3: Determine the Nature of the Precipitate
Next, we need to determine the physical state and color of the precipitate formed:
- FePO₄ is known to be a precipitate that is typically yellow-brown in color.

### Step 4: Conclusion
Since FePO₄ is a colored precipitate, we conclude that the reaction produces a yellow-brown precipitate.

### Final Answer
The answer to the question is that the reaction forms a colored precipitate (specifically, a yellow-brown precipitate).

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