An aqueous solution ofsodiumphosphatecontains0.34*M*sodiumions. If the solution contains no substances other thansodiumphosphateand water, what is the concentration ofphosphateions in the solution?

Given that the solution contains sodium phosphate (\(Na_3PO_4\)), let's determine the concentration of phosphate ions (\(PO_4^{3-}\)) in the solution.

### Step 1: Understanding the Dissociation of Sodium Phosphate
When sodium phosphate dissolves in water, it dissociates into sodium ions (\(Na^+\)) and phosphate ions (\(PO_4^{3-}\)) according to the equation:

\[
Na_3PO_4 \rightarrow 3Na^+ + PO_4^{3-}
\]

### Step 2: Relationship Between Sodium and Phosphate Ions
From the dissociation equation, you can see that for every 1 mole of sodium phosphate (\(Na_3PO_4\)), you get 3 moles of sodium ions (\(Na^+\)) and 1 mole of phosphate ions (\(PO_4^{3-}\)).

### Step 3: Concentration of Phosphate Ions
You are given that the concentration of sodium ions is \(0.34 \, M\). Since the ratio of sodium ions to phosphate ions is 3:1, the concentration of phosphate ions can be calculated as follows:

\[
\text{Concentration of } PO_4^{3-} = \frac{\text{Concentration of } Na^+}{3} = \frac{0.34 \, M}{3} = 0.1133 \, M
\]

### Final Answer:
The concentration of phosphate ions (\(PO_4^{3-}\)) in the solution is \(0.1133 \, M\).

Would you like to go over any details or have any questions?

Here are five related questions for further exploration:
1. How would the concentration of phosphate ions change if the concentration of sodium ions were doubled?
2. What is the molar mass of sodium phosphate, and how would you calculate it?
3. How would you prepare a 1-liter solution with a specific molarity of sodium phosphate?
4. What would be the concentration of hydroxide ions in the solution if it were basic?
5. How does the solubility of sodium phosphate compare to other phosphates in water?

**Tip:** Always make sure to double-check the dissociation equation of the compound when solving concentration problems to ensure accurate stoichiometric ratios.

Learn how to calculate the concentration of phosphate ions in an aqueous solution of sodium phosphate with a detailed step-by-step solution. Understand stoichiometry principles and solution chemistry. Suitable for advanced high school students and chemistry enthusiasts.

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