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Chemistry

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Answer

12\textbf{12}

Step-by-step solution

3 steps

  1. Determine the concentration of hydroxide ions.

    Sodium hydroxide (NaOH\text{NaOH}) is a strong base, meaning it dissociates completely in water.
    Therefore, the concentration of hydroxide ions [OH−][\text{OH}^-] is equal to the concentration of the NaOH\text{NaOH} solution.
    Given concentration of NaOH=0.01 M\text{NaOH} = 0.01 \text{ M}.
    So, [OH−]=0.01 M=1×10−2 M[\text{OH}^-] = 0.01 \text{ M} = 1 \times 10^{-2} \text{ M}.

  2. Calculate the pOH of the solution.

    The pOH is calculated using the formula:

    pOH=−log⁡10[OH−]\text{pOH} = -\log_{10}[\text{OH}^-]

    Substitute the concentration of hydroxide ions:

    pOH=−log⁡10(1×10−2)\text{pOH} = -\log_{10}(1 \times 10^{-2}) pOH=−(−2)\text{pOH} = -(-2) pOH=2\text{pOH} = 2

  3. Calculate the pH of the solution.

    The relationship between pH and pOH at 25∘C25^\circ\text{C} is:

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

    Rearrange to solve for pH:

    pH=14−pOH\text{pH} = 14 - \text{pOH}

    Substitute the calculated pOH value:

    pH=14−2\text{pH} = 14 - 2 pH=12\text{pH} = 12

    The final answer is 12\textbf{12}.

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