The pH of 0.001M aqueous solution of NaOH is:
Correct answer: C. 11
- A. 6
- B. 13
- C. 11
- D. 12
Explanation
To find the pH of a 0.001M NaOH solution, first recognize that NaOH is a strong base and fully dissociates in water. This means the concentration of OH- ions is 0.001M, or 10-3M. The pOH is calculated as -log(10-3) = 3. Since pH + pOH = 14, the pH is 14 - 3 = 11, confirming that the correct answer is 11. Other options are incorrect because they do not properly apply the relationship between pH and pOH or misinterpret the concentration of the solution.
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About Acids, Bases and Salts
Acid and base behaviour is explained through the Bronsted-Lowry transfer of protons and the Lewis donation or acceptance of electron pairs. The topic includes pH, pOH, ionisation and water equilibrium, plus salt formation and hydrolysis, where a salt solution may become acidic, basic or neutral.
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