1 mole of `[OH^(-)]` is present in how many moles of`H_(2)O ` ?

Options

A. 0.1 mole
B. `1 dm^(3)`
C. 1 mole
D. 0.5 mole

Explanation

To solve the question of how many moles of \( H_2O \) are needed to produce 1 mole of \( OH^- \), we can follow these steps:

### Step 1: Understand the dissociation of water
Water (\( H_2O \)) can dissociate into hydrogen ions (\( H^+ \)) and hydroxide ions (\( OH^- \)) according to the following reaction:
\[ H_2O \rightleftharpoons H^+ + OH^- \]

### Step 2: Analyze the stoichiometry of the reaction
From the dissociation reaction, we can see that:
- 1 mole of \( H_2O \) produces 1 mole of \( H^+ \) and 1 mole of \( OH^- \).

### Step 3: Relate moles of \( OH^- \) to moles of \( H_2O \)
Since the dissociation of water shows a 1:1 ratio between \( H_2O \) and \( OH^- \), this means:
- If we have 1 mole of \( OH^- \), it must have come from 1 mole of \( H_2O \).

### Conclusion
Thus, 1 mole of \( OH^- \) is present in 1 mole of \( H_2O \).

### Final Answer
1 mole of \( OH^- \) is present in 1 mole of \( H_2O \).

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