What is the pH of 0.001M NaOH solution?
Correct answer: C. 11
- A. 3
- B. 7
- C. 11
- D. 10
Explanation
To calculate the pH of a 0.001M NaOH solution, first determine its pOH. Since NaOH is a strong base and dissociates completely, the concentration of OH⁻ ions is 0.001M. The pOH is calculated as -log(0.001) = 3. Since pH + pOH = 14 for aqueous solutions, the pH is 14 - 3 = 11. Therefore, the correct answer is Option C: 11. Option A: 3 suggests an acidic solution, Option B: 7 indicates neutrality, and Option D: 10 underestimates the basicity 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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