Questions: What is the pH of an aqueous solution of 0.0654 M sodium hydroxide? pH=

What is the pH of an aqueous solution of 0.0654 M sodium hydroxide? pH=
Transcript text: What is the pH of an aqueous solution of 0.0654 M sodium hydroxide? \[ \mathrm{pH}= \]
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Solution

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Solution Steps

Step 1: Determine the concentration of hydroxide ions

Sodium hydroxide (NaOH) is a strong base and dissociates completely in water. Therefore, the concentration of hydroxide ions (OH\(^-\)) in the solution is equal to the concentration of NaOH.

\[ [\text{OH}^-] = 0.0654 \, \text{M} \]

Step 2: Calculate the pOH of the solution

The pOH of a solution is calculated using the formula:

\[ \text{pOH} = -\log[\text{OH}^-] \]

Substituting the given concentration:

\[ \text{pOH} = -\log(0.0654) \]

Using a calculator:

\[ \text{pOH} \approx 1.1847 \]

Step 3: Calculate the pH of the solution

The pH and pOH are related by the equation:

\[ \text{pH} + \text{pOH} = 14 \]

Solving for pH:

\[ \text{pH} = 14 - \text{pOH} \]

Substituting the calculated pOH:

\[ \text{pH} = 14 - 1.1847 \approx 12.8153 \]

Final Answer

\[ \boxed{\text{pH} \approx 12.82} \]

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