Question:
The pH of a $0.01\text{ M NaOH}$ solution is
The pH of a $0.01\text{ M NaOH}$ solution is
Show Hint
Remember that strong bases like NaOH completely dissociate in water and the concentration of $\text{OH}^-$ ions directly affects the pH calculation.
Updated On: Jun 3, 2026
Show Solution
Verified By Collegedunia
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 (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)
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 (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)
Was this answer helpful?
0
0
Top AP EAPCET Chemistry Questions
- The four quantum numbers of the valence electron of potassium are :
- The volume of $0.02\, M$ acidified permanganate solution required for complete reaction of $60\, mL$ of $0.01\, MI^{-}$ ion solution to form $I_2$ in $mL$ is
- In which of the following the election gain enthalpy of elements is correctly arranged?
- The radii of $ \text{F,}{{\text{F}}^{-}}\text{O} $ and $ {{\text{O}}^{2-}} $ are in the order
- Which of the following has the highest first ionization potential?
View More Questions
Top AP EAPCET Measurement of PH Questions
- 1 L of 0.1 M HCl is added to 1 L of 0.1 M HA (weak acid) solution. To this solution, 16 g of solid NaOH is added. What is the pOH value of resultant solution? (Given molar mass of NaOH is 40 g/mol, $ \log 2 = 0.3, \log 4 = 0.6 $)
- 500 mL of 0.1M HCl is mixed with 500 mL of 0.02M HA (weak acid) solution. To this solution, 2 g of solid NaOH is added. What is the pH of the resultant solution? (Given} \( K_a \) of HA is \( 4 \times 10^{-10} \), molar mass of NaOH is 40 g/mol, log 2 = 0.3, log 4 = 0.6\bf{)
- Which of the following aqueous solutions has highest pH? (Given \(\log 2 = 0.30\), \(\log 3 = 0.48\), \(\log 4 = 0.60\), \(\log 5 = 0.70\))
- When \(30\,\text{mL}\) of \(0.2\,\text{M}\) \(NH_4OH\) is added to \(30\,\text{mL}\) of \(2\,\text{M}\) \(NH_4Cl\) solution. If the pH of the buffer formed is \(8.2\), what is the pKb of \(NH_4OH\)?
- Which of the following is a conjugate acid-base pair?
View More Questions
Top AP EAPCET Questions
- A body is projected from the ground at an angle of $\tan^{-1} \left( \frac{8}{7}\right)$ with the horizontal. The ratio of the maximum height attained by it to its range is
- The four quantum numbers of the valence electron of potassium are :
- A lens forms real and virtual images of an object, when the object is at $u_{1}$ and $u_{2}$ distances respectively. If the size of the virtual image is double that of the real image, then the focal length of the lens is (take, the magnification of the real image as $m$ )
- Two spheres $P$ and $Q$, each of mass $200\, g$ are attached to a string of length one metre as shown in the figure. The string and the spheres are then whirled in a horizontal circle about $O$ at a constant angular speed. The ratio of the tension in the string between $P$ and $Q$ to that of between $P$ and $O$ is $(P$ is at mid-point of the line joining $O$ and $Q$ )
- The volume of $0.02\, M$ acidified permanganate solution required for complete reaction of $60\, mL$ of $0.01\, MI^{-}$ ion solution to form $I_2$ in $mL$ is
View More Questions