The conjugate acid of `overset(Theta)NH_(2)` is

Options

A. `NH_(4) OH`
B. `NH_(4)^(+)`
C. `NH^(-2)`
D. `NH_(3)`

Answer

To find the conjugate acid of the amide ion (NH₂⁻), we need to follow these steps:

### Step 1: Understand the concept of conjugate acids and bases
A conjugate acid is formed when a base gains a proton (H⁺). In this case, the base we are considering is the amide ion (NH₂⁻).

**Hint:** Remember that the conjugate acid is formed by adding a proton to the base.

### Step 2: Identify the base
The base given in the question is the amide ion, which is represented as NH₂⁻.

**Hint:** Recognize that NH₂⁻ is a negatively charged ion, indicating it can accept a proton.

### Step 3: Add a proton to the base
When we add a proton (H⁺) to the amide ion (NH₂⁻), we perform the following reaction:
\[ \text{NH}_2^- + \text{H}^+ \rightarrow \text{NH}_3 \]

**Hint:** The addition of a proton changes the charge and the structure of the ion.

### Step 4: Determine the product
The product of this reaction is ammonia (NH₃). Thus, the conjugate acid of the amide ion (NH₂⁻) is ammonia (NH₃).

**Hint:** Check if the resulting compound is neutral; ammonia has no charge.

### Conclusion
The conjugate acid of NH₂⁻ is NH₃ (ammonia).

**Final Answer:** NH₃