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What is the pH of a 0.01 M NaOH solution?
What is the pH of a 0.01 M NaOH solution?
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Practice Questions
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Q1
What is the pH of a 0.01 M NaOH solution?
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For NaOH, which is a strong base, pOH = -log[OH-]. [OH-] = 0.01 M, so pOH = 2. Therefore, pH = 14 - pOH = 14 - 2 = 12.
Questions & Step-by-step Solutions
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Q
Q: What is the pH of a 0.01 M NaOH solution?
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.
Steps: 6
Show Steps
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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