Question:
The pH of a $0.01\text{ M NaOH}$ solution is}
The pH of a $0.01\text{ M NaOH}$ solution is}
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Remember that strong bases like $\text{NaOH}$ completely dissociate in water and the concentration of $\text{OH}^-$ ions directly affects the pH calculation.
Updated On: May 31, 2026
- 12
- 2
- 10
- 7
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The Correct Option is A
Solution and Explanation
Step 1: Concept
The pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration $[\text{H}^+]$. For strong bases like sodium hydroxide ($\text{NaOH}$), the concentration of $\text{OH}^-$ ions can be used to find the concentration of $\text{H}^+$ ions using the autoionization constant of water, $K_w = [\text{H}^+][\text{OH}^-] = 10^{-14}$ at $25^\circ \text{C}$.
Step 2: Meaning
The given solution is a strong base ($0.01\text{ M NaOH}$), meaning it completely dissociates in water to produce $\text{Na}^+$ and $\text{OH}^-$ ions. The concentration of $\text{OH}^-$ ions will be equal to the concentration of the base, $[\text{OH}^-] = 0.01\text{ M}$.
Step 3: Analysis
To find the pH, we first need to determine the concentration of $\text{H}^+$ ions using the autoionization constant of water: \[[\text{H}^+] = \frac{K_w}{[\text{OH}^-]} = \frac{10^{-14}}{0.01} = 10^{-12}\text{ M}\] Now, we can calculate the pH using the definition of pH: \[\text{pH} = -\log_{10}([\text{H}^+]) = -\log_{10}(10^{-12}) = 12\] This calculation shows that the solution is highly basic and has a pH of 12.
Step 4: Conclusion
The calculated pH for a $0.01\text{ M NaOH}$ solution is 12, which matches option A.
Final Answer: (A)
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