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What is the pH of a 0.1 M NaOH solution?
What is the pH of a 0.1 M NaOH solution?
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Q1
What is the pH of a 0.1 M NaOH solution?
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pOH = -log[OH-] = -log(0.1) = 1; pH = 14 - pOH = 14 - 1 = 13
Questions & Step-by-step Solutions
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Q
Q: What is the pH of a 0.1 M NaOH solution?
Solution:
pOH = -log[OH-] = -log(0.1) = 1; pH = 14 - pOH = 14 - 1 = 13
Steps: 7
Show Steps
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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