Equal volumes of 0.1 M NaCl and 0.06 M `CaCl_(2)` solutions are separated by a semi - permeable membrane in container. For this system, choose the correct answer

Options

A. Water flows from NaCl solution towards `CaCl_(2)` solution
B. There is no movement of any solution across the membrane
C. Osmotic pressure of 0.1 M NaCl is lower than the
osmotic pressure of `CaCl_(2)` (Assume complete dissociation)
D. Water flows from `CaCl_(2)` solution towards `NaCl` soltuion

Answer

To solve the problem, we need to calculate the osmotic pressure of both the NaCl and CaCl₂ solutions and then determine the direction of water flow based on these pressures.

### Step-by-Step Solution:

1. **Identify the Dissociation of Solutes:**
- NaCl dissociates into two ions: Na⁺ and Cl⁻.
- CaCl₂ dissociates into three ions: Ca²⁺ and 2Cl⁻.

2. **Calculate the Van 't Hoff Factor (i):**
- For NaCl: \( i = 2 \) (1 Na⁺ + 1 Cl⁻)
- For CaCl₂: \( i = 3 \) (1 Ca²⁺ + 2 Cl⁻)

3. **Calculate the Effective Concentration (C_eff):**
- For NaCl:
\[ C_{\text{eff, NaCl}} = i \times C = 2 \times 0.1 \, \text{M} = 0.2 \, \text{M} \]
- For CaCl₂:
\[ C_{\text{eff, CaCl₂}} = i \times C = 3 \times 0.06 \, \text{M} = 0.18 \, \text{M} \]

4. **Determine the Osmotic Pressure (π):**
- The formula for osmotic pressure is given by:
\[ \pi = C_{\text{eff}} \cdot R \cdot T \]
- Since R and T are constants, we can compare the effective concentrations directly:
- For NaCl: \( \pi_{\text{NaCl}} \propto 0.2 \)
- For CaCl₂: \( \pi_{\text{CaCl₂}} \propto 0.18 \)

5. **Compare the Osmotic Pressures:**
- Since \( 0.2 \, \text{M} > 0.18 \, \text{M} \), we conclude:
\[ \pi_{\text{NaCl}} > \pi_{\text{CaCl₂}} \]

6. **Determine the Direction of Water Flow:**
- Water flows from the solution with lower osmotic pressure to the solution with higher osmotic pressure.
- Therefore, water will flow from the CaCl₂ solution to the NaCl solution.

### Final Conclusion:
Water flows from the CaCl₂ solution towards the NaCl solution.