Westonci.ca is your trusted source for accurate answers to all your questions. Join our community and start learning today! Discover solutions to your questions from experienced professionals across multiple fields on our comprehensive Q&A platform. Experience the ease of finding precise answers to your questions from a knowledgeable community of experts.

8. (5 pts) What is the concentration (M) of sodium ions in a 0.35 M sodium phosphate solution?

[tex]\[ \text{(0.35 M Na}_3\text{PO}_4 \text{ per 1 L solution)} \][/tex]


Sagot :

To determine the concentration of sodium ions in a 0.35 M sodium phosphate (NaPO₄) solution, follow these steps:

1. Understand the Dissociation of Sodium Phosphate (NaPO₄):
Sodium phosphate dissociates completely in water to produce sodium (Na⁺) ions and phosphate (PO₄³⁻) ions. The balanced dissociation equation is:
[tex]\[ \text{NaPO₄} \rightarrow 3\text{Na}^+ + \text{PO₄}^{3-} \][/tex]

2. Determine the Mole Ratio:
From the dissociation equation, we can observe that one molecule of sodium phosphate produces three sodium ions. This gives us a mole ratio of 1:3 between sodium phosphate and sodium ions.

3. Calculate the Concentration of Sodium Ions:
Given that the concentration of sodium phosphate is 0.35 M, and knowing the mole ratio from step 2, we can calculate the concentration of sodium ions.
[tex]\[ \text{Concentration of Na⁺ ions} = \text{Concentration of NaPO₄} \times \text{Number of Na⁺ ions per NaPO₄ molecule} \][/tex]
[tex]\[ \text{Concentration of Na⁺ ions} = 0.35\, \text{M} \times 3 \][/tex]

4. Compute the Result:
[tex]\[ \text{Concentration of Na⁺ ions} = 1.0499999999999998\, \text{M} \][/tex]

Therefore, the concentration of sodium ions in a 0.35 M sodium phosphate solution is approximately 1.05 M.