Conjugate base of `overset(Theta)OH` is

Options

A. `H_(2)O`
B. `H_(3)O^(o+)`
C. `H^(o+)`
D. `O^(2-)`

Explanation

To find the conjugate base of \( \text{OH}^- \), we can follow these steps:

### Step 1: Understand the Concept of Conjugate Bases
A conjugate base is formed when an acid donates a proton (H\(^+\)). In this case, \( \text{OH}^- \) acts as an acid.

**Hint:** Remember that the conjugate base is what remains after an acid loses a proton.

### Step 2: Identify the Species
The species we are dealing with is \( \text{OH}^- \), which is the hydroxide ion.

**Hint:** Identify the ion and its charge before proceeding to the next step.

### Step 3: Remove a Proton
When \( \text{OH}^- \) loses a proton (H\(^+\)), we need to determine what remains. The removal of H\(^+\) from \( \text{OH}^- \) can be represented as:
\[ \text{OH}^- \rightarrow \text{O}^{2-} + \text{H}^+ \]

**Hint:** Think about what happens to the charge of the ion when a proton is removed.

### Step 4: Determine the Resulting Ion
After the removal of the proton, the remaining species is \( \text{O}^{2-} \), which is the oxide ion.

**Hint:** Make sure to check the charge of the resulting ion after the proton is removed.

### Conclusion
Thus, the conjugate base of \( \text{OH}^- \) is \( \text{O}^{2-} \).

**Final Answer:** The conjugate base of \( \text{OH}^- \) is \( \text{O}^{2-} \).