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What is the pH of a 0.1 M NaOH solution?

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Question: What is the pH of a 0.1 M NaOH solution?

Options:

  1. 10
  2. 11
  3. 12
  4. 13

Correct Answer: 12

Solution: 

pOH = -log[OH-] = -log(0.1) = 1; pH = 14 - pOH = 14 - 1 = 13

What is the pH of a 0.1 M NaOH solution?

Practice Questions

Q1
What is the pH of a 0.1 M NaOH solution?
  1. 10
  2. 11
  3. 12
  4. 13

Questions & Step-by-Step Solutions

What is the pH of a 0.1 M NaOH solution?
  • Step 1: Identify the concentration of the NaOH solution, which is 0.1 M. NaOH is a strong base and completely dissociates in water.
  • Step 2: Determine the concentration of hydroxide ions (OH-) in the solution. Since NaOH dissociates completely, [OH-] = 0.1 M.
  • Step 3: Calculate the pOH using the formula pOH = -log[OH-]. Substitute [OH-] with 0.1: pOH = -log(0.1).
  • Step 4: Calculate -log(0.1). This equals 1, so pOH = 1.
  • Step 5: Use the relationship between pH and pOH: pH + pOH = 14.
  • Step 6: Substitute pOH into the equation: pH = 14 - pOH = 14 - 1.
  • Step 7: Calculate pH: pH = 13.
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