Which amongst the following is the strongest acid?

Options

A. `CHl_(3)`
B. `CHBr_(3)`
C. `CHCl_(3)`
D. `CH(CN)_(3)`

Explanation

To determine which among the given options is the strongest acid, we need to analyze the stability of their conjugate bases. The stronger the acid, the more stable its conjugate base will be. Here’s a step-by-step solution:

### Step 1: Identify the Acids
We have the following acids to consider:
- A: CH₃I (Iodomethane)
- B: CH₃Br (Bromomethane)
- C: CH₃Cl (Chloromethane)
- D: CH₃CN (Acetonitrile)

### Step 2: Write the Dissociation Reaction
Each acid dissociates to form H⁺ and its respective conjugate base:
- CH₃I → H⁺ + CH₃I⁻
- CH₃Br → H⁺ + CH₃Br⁻
- CH₃Cl → H⁺ + CH₃Cl⁻
- CH₃CN → H⁺ + CH₃CN⁻

### Step 3: Analyze the Conjugate Bases
The conjugate bases formed are:
- I⁻ (from CH₃I)
- Br⁻ (from CH₃Br)
- Cl⁻ (from CH₃Cl)
- CN⁻ (from CH₃CN)

### Step 4: Stability of Conjugate Bases
The stability of the conjugate bases can be analyzed based on their ability to stabilize the negative charge:
- I⁻, Br⁻, and Cl⁻ are halides and are relatively stable due to their size and ability to disperse the negative charge.
- CN⁻ (the conjugate base of acetonitrile) is stabilized by resonance due to the presence of the triple bond with carbon, which can delocalize the negative charge.

### Step 5: Order of Stability
The order of stability of the conjugate bases is:
CN⁻ > I⁻ > Br⁻ > Cl⁻

### Step 6: Conclusion
Since CN⁻ is the most stable conjugate base among the options, CH₃CN (acetonitrile) is the strongest acid.

### Final Answer
The strongest acid among the given options is **D: CH₃CN**.

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