Amongst the following the most basic compound is :

Options

A. Benzylamine
B. Aniline
C. Acetanilide
D. p-Nitroaniline

Explanation

To determine which of the given compounds is the most basic, we need to analyze the structures and the availability of the lone pair of electrons on the nitrogen atom in each compound. The basicity of a compound is related to how readily it can donate its lone pair of electrons to accept a proton (H⁺).

### Step-by-Step Solution:

1. **Identify the Compounds**:
- Benzylamine
- Aniline
- Acetanilide
- Paranitroaniline

2. **Draw the Structures**:
- **Benzylamine**: C₆H₅-CH₂-NH₂
- **Aniline**: C₆H₅-NH₂
- **Acetanilide**: C₆H₅-NH-CO-CH₃
- **Paranitroaniline**: C₆H₄(NH₂)(NO₂)

3. **Analyze Basicity**:
- **Benzylamine**: The nitrogen has a lone pair that is not involved in resonance with the benzene ring, making it readily available to accept a proton. Thus, it is basic.
- **Aniline**: The lone pair on nitrogen is partially delocalized into the benzene ring, which reduces its availability to accept a proton. Therefore, it is less basic than benzylamine.
- **Acetanilide**: The lone pair on nitrogen is involved in resonance with the carbonyl group (C=O), further reducing its availability. Hence, it is even less basic.
- **Paranitroaniline**: The presence of the nitro group (NO₂) at the para position withdraws electron density from the nitrogen, making it less basic compared to aniline.

4. **Conclusion**:
- Among the four compounds, **Benzylamine** has the most available lone pair on nitrogen and is therefore the most basic compound.

### Final Answer:
**Benzylamine is the most basic compound among the given options.**