Which is not an example of an ideal solution ?

Options

A. `C_6H_(14)+C_7H_(16)`
B. `H_2O+C_4H_9OH`
C. `C_2H_5Br+C_2H_5I`
D. `"CCl"_4+SiCl_4`

Answer

To determine which option is not an example of an ideal solution, we need to analyze the interactions between the components of each option. An ideal solution is characterized by the absence of significant interactions between the solute and solvent molecules, meaning that the enthalpy of mixing is zero and the properties of the solution are similar to those of the pure components.

### Step-by-Step Solution:

1. **Identify the Options**:
- Option A: C6H14 and C7H16
- Option B: H2O and C4H9OH
- Option C: CCl4 and SiCl4
- Option D: C2H5Br and C2H5I

2. **Analyze Option A (C6H14 and C7H16)**:
- Both C6H14 (hexane) and C7H16 (heptane) are non-polar hydrocarbons.
- Non-polar substances tend to mix well without significant interactions.
- **Conclusion**: This is an ideal solution.

3. **Analyze Option B (H2O and C4H9OH)**:
- H2O (water) is a polar solvent, and C4H9OH (butanol) is an alcohol that can form hydrogen bonds.
- The presence of hydrogen bonding indicates strong interactions between the molecules.
- **Conclusion**: This is not an ideal solution.

4. **Analyze Option C (CCl4 and SiCl4)**:
- Both CCl4 (carbon tetrachloride) and SiCl4 (silicon tetrachloride) are non-polar molecules.
- They are expected to mix well without significant interactions.
- **Conclusion**: This is an ideal solution.

5. **Analyze Option D (C2H5Br and C2H5I)**:
- Both C2H5Br (ethyl bromide) and C2H5I (ethyl iodide) are similar in structure and polarity.
- They are expected to mix well without significant interactions.
- **Conclusion**: This is an ideal solution.

6. **Final Conclusion**:
- The only option that does not represent an ideal solution is **Option B: H2O and C4H9OH** due to the presence of hydrogen bonding.

### Answer:
**Option B: H2O and C4H9OH is not an example of an ideal solution.**