Consider of following reactions
`CHF_(3) overset(K_(a))(to)CF_(3)^(-)+H^(+)`
`CHCl_(3)^(-) overset(K_(a)^(+))(to)C Cl_(3)^(-)+H^(+)`
Then regarding given reactions which of the following statement(s) is /are correct:

Options

A. `K_(a)gtK'_(a)`
B. `CHF_(3)` act as a stronger bronsted acid than `CHCl_(3)`
C. `C Cl_(3)^(-)` is more stable than `CF_(3)^(-)`
D. `C Cl_(3)^(-)` is weaker lewis base than `CF_(3)^(-)`

Explanation

To analyze the given reactions and determine the correctness of the statements, we will follow these steps:

### Step 1: Write the Reactions
The reactions provided are:
1. \( CHF_3 \overset{K_a}{\rightleftharpoons} CF_3^- + H^+ \)
2. \( CHCl_3 \overset{K_a'}{\rightleftharpoons} CCl_3^- + H^+ \)

### Step 2: Understand the Equilibrium Constants
The equilibrium constant \( K \) for a reaction is defined as:
\[ K = \frac{[\text{products}]}{[\text{reactants}]} \]
In these reactions, \( K_a \) and \( K_a' \) represent the equilibrium constants for the dissociation of CHF3 and CHCl3, respectively.

### Step 3: Compare the Stability of the Anions
- **For \( CF_3^- \)**:
- The negative charge is localized on carbon, which is bonded to three fluorine atoms. Fluorine is highly electronegative, which leads to increased electron density and repulsion around the carbon atom.

- **For \( CCl_3^- \)**:
- The negative charge is also localized on carbon, but chlorine has vacant 3d orbitals that allow for delocalization of the negative charge. This delocalization reduces electron repulsion and stabilizes the anion.

### Step 4: Determine the Relative Strength of the Acids
- A stronger acid will produce a more stable anion upon dissociation. Since \( CCl_3^- \) is more stable than \( CF_3^- \), it follows that:
\[ K_a' > K_a \]
This indicates that \( CHCl_3 \) is a stronger acid than \( CHF_3 \).

### Step 5: Analyze the Statements
1. **Statement 1**: \( K_a' > K_a \) (CCl3- is more stable than CF3-)
- This statement is **correct**.

2. **Statement 2**: CHF3 acts as a stronger Brønsted acid than CHCl3.
- This statement is **incorrect** because \( CHCl_3 \) is the stronger acid.

3. **Statement 3**: CCl3- is more stable than CF3-.
- This statement is **correct** based on the stability analysis.

4. **Statement 4**: CCl3- is a weaker Lewis base than CF3-.
- This statement is **correct** because the negative charge on CF3- is more available for donation compared to CCl3-.

### Conclusion
The correct statements are:
- CCl3- is more stable than CF3-.
- CCl3- is a weaker Lewis base than CF3-.