5) A solution is made by combining 75.0 mL of 0.0040 M Na2SO4 and 25.0 mL of 0.080 M AgNO3. Calculate the final concentrations of all four ions in solution. The Ksp of Ag2SO4 is 1.5 x 10-5. 75,0ML Na₂ soy 2 50ml. 1002
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![### Problem Statement:
A solution is made by combining 75.0 mL of 0.0040 M Na₂SO₄ and 25.0 mL of 0.080 M AgNO₃. Calculate the final concentrations of all four ions in solution. The \( K_{sp} \) of Ag₂SO₄ is \( 1.5 \times 10^{-5} \).
### Solution Steps:
1. **Volume and Mol Calculations:**
We have:
- 75.0 mL of 0.0040 M Na₂SO₄
- 25.0 mL of 0.080 M AgNO₃
- Final total volume = 100 mL
2. **Concentration Adjustments for Dilution:**
For Na₂SO₄:
\[ C_1 = 0.0040 \, \text{M} \]
\[ V_1 = 75 \, \text{mL} \]
\[ V_f = 100 \, \text{mL} \]
\[ C_f (Na₂SO₄) = C_1 \times \frac{V_1}{V_f} = 0.0040 \times \frac{75}{100} = 0.0030 \, \text{M} \]
Splitting into ions:
\[ Na₂SO₄ \rightarrow 2Na^+ + SO₄^{2-} \]
\[ SO₄^{2-} = 0.0030 \, \text{M} \]
\[ Na^+ = 2 \times 0.0030 \, \text{M} = 0.0060 \, \text{M} \]
For AgNO₃:
\[ C_3 = 0.080 \, \text{M} \]
\[ V_3 = 25 \, \text{mL} \]
\[ V_f = 100 \, \text{mL} \]
\[ C_f (AgNO₃) = C_3 \times \frac{V_3}{V_f} = 0.080 \times \frac{25}{100} = 0.020 \, \text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F148e7587-3577-41ee-af46-bb8597b6d4e9%2F1b7290fa-698a-483d-8f3c-66e8ba0bfa4e%2F0d6hr2_processed.jpeg&w=3840&q=75)
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