Calculate the pH of a 0.01 M of NaOH solution.

Explanation

To calculate the pH of a 0.01 M NaOH solution, follow these steps:

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

### Step 2: Determine the concentration of OH⁻ ions
Since NaOH dissociates completely, the concentration of OH⁻ ions in the solution will be equal to the concentration of NaOH. Therefore:
\[ [\text{OH}^-] = 0.01 \, \text{M} \]

### Step 3: Calculate the pOH
The pOH can be calculated using the formula:
\[ \text{pOH} = -\log[\text{OH}^-] \]
Substituting the concentration of OH⁻:
\[ \text{pOH} = -\log(0.01) \]
\[ \text{pOH} = -(-2) = 2 \]

### Step 4: Use the relationship between pH and pOH
We know that:
\[ \text{pH} + \text{pOH} = 14 \]
Now, substituting the value of pOH:
\[ \text{pH} = 14 - \text{pOH} \]
\[ \text{pH} = 14 - 2 \]
\[ \text{pH} = 12 \]

### Final Answer
The pH of a 0.01 M NaOH solution is **12**.

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