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 of the given options is not an example of an ideal solution, we first need to understand the characteristics of ideal solutions and how they behave according to Raoult's law.

### Step 1: Understand Ideal Solutions
An ideal solution is one that follows Raoult's law, which states that the partial vapor pressure of each component in the solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution. Ideal solutions are characterized by similar intermolecular forces between the components.

### Step 2: Identify the Given Options
The question provides several pairs of substances. We need to analyze each pair to see if they form an ideal solution or not. The pairs mentioned in the video are:
1. C6H14 (Hexane) and C7H14 (Heptane)
2. Water and Alcohol
3. C2H5 (Ethyl group) and C2H5I (Iodoethane)
4. CCl4 (Carbon Tetrachloride) and SCl4 (Sulfur Tetrafluoride)

### Step 3: Analyze Each Pair
1. **C6H14 and C7H14**: Both are non-polar hydrocarbons with similar intermolecular forces (London dispersion forces). This pair behaves ideally.

2. **Water and Alcohol**: Water (polar) and alcohol (also polar but with different hydrogen bonding capabilities) do not mix ideally. The hydrogen bonding interactions are disrupted, leading to a deviation from Raoult's law. This pair does not behave ideally.

3. **C2H5 and C2H5I**: This pair consists of an ethyl group and iodoethane. The presence of the iodine atom introduces a different interaction, but they are similar enough to exhibit ideal behavior.

4. **CCl4 and SCl4**: Both are non-polar and have similar intermolecular forces. Therefore, this pair behaves ideally.

### Step 4: Conclusion
From the analysis, the pair that does not represent an ideal solution is **Water and Alcohol**.

### Final Answer
**Water and Alcohol is not an example of an ideal solution.**

---