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What is the pH of a 0.01 M NaOH solution?

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Question: What is the pH of a 0.01 M NaOH solution?

Options:

  1. 12
  2. 2
  3. 10
  4. 1

Correct Answer: 12

Solution: 

For NaOH, which is a strong base, pOH = -log[OH-]. [OH-] = 0.01 M, so pOH = 2. Therefore, pH = 14 - pOH = 14 - 2 = 12.

What is the pH of a 0.01 M NaOH solution?

Practice Questions

Q1
What is the pH of a 0.01 M NaOH solution?
  1. 12
  2. 2
  3. 10
  4. 1

Questions & Step-by-Step Solutions

What is the pH of a 0.01 M NaOH solution?
  • Step 1: Identify that NaOH is a strong base, which means it completely dissociates in water.
  • Step 2: Determine the concentration of hydroxide ions [OH-]. For a 0.01 M NaOH solution, [OH-] = 0.01 M.
  • Step 3: Calculate the pOH using the formula pOH = -log[OH-]. Substitute [OH-] = 0.01 M into the formula.
  • Step 4: Calculate pOH: pOH = -log(0.01) = 2.
  • Step 5: Use the relationship between pH and pOH: pH + pOH = 14.
  • Step 6: Solve for pH: pH = 14 - pOH = 14 - 2 = 12.
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