In which of the following pairs the first one is the stronger base than second.

Options

A. `CH_3COO^(Theta),HCOO^(Theta)`
B. `HO^(Theta),NH_2^(Theta)`
C. `CH_2=Coverset(Theta)H: , H-C=Coverset(Theta)`
D. `CH_3NH_2, CH_3OH`

Explanation

To determine which of the given pairs has the first compound as a stronger base than the second, we need to analyze the stability of the negative charge or lone pairs in each compound. A stronger base is typically one that has a less stable negative charge or is more willing to donate its lone pair.

### Step-by-Step Solution:

1. **Identify the Compounds**: Let's denote the compounds in the pairs as A and B. For example, if we have the pair (Cs3COO⁻, HCOO⁻), we will analyze Cs3COO⁻ (A) and HCOO⁻ (B).

2. **Analyze the Negative Charge**:
- For Cs3COO⁻ (acetate ion), the negative charge is on the oxygen atom. The presence of three methyl groups (Cs3) provides a +I (inductive) effect, which stabilizes the negative charge on the oxygen.
- For HCOO⁻ (formate ion), the negative charge is also on the oxygen atom, but it is less stabilized by inductive effects since it has a hydrogen atom instead of alkyl groups.

3. **Determine Stability of Negative Charges**:
- In Cs3COO⁻, the negative charge is less stable due to the +I effect from the three methyl groups, making it a stronger base.
- In HCOO⁻, the negative charge is more stable because there are no electron-donating groups to destabilize it.

4. **Conclusion**: Since Cs3COO⁻ has a less stable negative charge compared to HCOO⁻, it is a stronger base. Therefore, in the pair (Cs3COO⁻, HCOO⁻), Cs3COO⁻ is the stronger base.

5. **Repeat for Other Pairs**: You would repeat this process for any other pairs provided in the question, analyzing the stability of the negative charge or lone pairs in each compound.

### Final Answer:
In the pair (Cs3COO⁻, HCOO⁻), Cs3COO⁻ is the stronger base.