The pH vaue of 0.1 M NaOH solution is (when there is a given reaction `[H^(+)][OH^(-)] = 10^(-14)`

Options

A. 13
B. 12
C. 11
D. 2

Explanation

To find the pH value of a 0.1 M NaOH solution, we can follow these steps:

### Step 1: Understand the Ionization of NaOH
NaOH is a strong base that completely dissociates in water. The dissociation can be represented as:
\[ \text{NaOH} \rightarrow \text{Na}^+ + \text{OH}^- \]

Since the concentration of NaOH is 0.1 M, the concentration of hydroxide ions \([OH^-]\) produced will also be 0.1 M.

### Step 2: Calculate the pOH
The pOH can be calculated using the formula:
\[ \text{pOH} = -\log[OH^-] \]
Substituting the concentration of hydroxide ions:
\[ \text{pOH} = -\log(0.1) \]
\[ \text{pOH} = -\log(10^{-1}) \]
\[ \text{pOH} = 1 \]

### Step 3: Use the Relationship Between pH and pOH
We know that:
\[ \text{pH} + \text{pOH} = 14 \]
Now, substituting the value of pOH:
\[ \text{pH} + 1 = 14 \]
\[ \text{pH} = 14 - 1 \]
\[ \text{pH} = 13 \]

### Conclusion
The pH value of the 0.1 M NaOH solution is **13**.

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