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What is the pH of a 0.01 M solution of NaOH?
What is the pH of a 0.01 M solution of NaOH?
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1 question
Q1
What is the pH of a 0.01 M solution of NaOH?
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pOH = -log(0.01) = 2; 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 solution of NaOH?
Solution:
pOH = -log(0.01) = 2; pH = 14 - pOH = 14 - 2 = 12.
Steps: 10
Show Steps
Step 1: Understand that NaOH is a strong base and will completely dissociate in water.
Step 2: Recognize that a 0.01 M solution of NaOH means there are 0.01 moles of NaOH in 1 liter of water.
Step 3: Since NaOH dissociates completely, the concentration of OH- ions in the solution is also 0.01 M.
Step 4: Calculate the pOH using the formula pOH = -log[OH-]. Here, [OH-] = 0.01 M.
Step 5: Substitute the value into the formula: pOH = -log(0.01).
Step 6: Calculate -log(0.01), which equals 2.
Step 7: Use the relationship between pH and pOH: pH + pOH = 14.
Step 8: Rearrange the equation to find pH: pH = 14 - pOH.
Step 9: Substitute the value of pOH: pH = 14 - 2.
Step 10: Calculate the final pH: pH = 12.
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