What is the pH of a 0.001 M aqueous solution of Sodium Hydroxide (NaOH) at 25 degrees Celsius?
Answer and explanation
Correct answer: C. 11.0
- Step 1: NaOH dissociates completely: [OH-] = 0.001 M = 10^(-3) M, so pOH = -log(10^(-3)) = 3.0. Step 2. At 25 deg C, pH + pOH = 14 => pH = 14 - 3 = 11.0. Answer: 11.0. Why not the others: 3.0 represents the pOH of the solution; 14.0 is the total pH+pOH sum; 7.0 is the neutral pH of pure water.
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