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What is the pH of a solution that has a hydroxide ion concentration of 1.0 x 10^
What is the pH of a solution that has a hydroxide ion concentration of 1.0 x 10^-3 M?
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Practice Questions
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Q1
What is the pH of a solution that has a hydroxide ion concentration of 1.0 x 10^-3 M?
11
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3
1
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pOH = -log[OH-] = -log(1.0 x 10^-3) = 3. Therefore, pH = 14 - pOH = 14 - 3 = 11.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the pH of a solution that has a hydroxide ion concentration of 1.0 x 10^-3 M?
Solution:
pOH = -log[OH-] = -log(1.0 x 10^-3) = 3. Therefore, pH = 14 - pOH = 14 - 3 = 11.
Steps: 7
Show Steps
Step 1: Identify the hydroxide ion concentration given in the problem, which is 1.0 x 10^-3 M.
Step 2: Use the formula for pOH, which is pOH = -log[OH-].
Step 3: Substitute the hydroxide ion concentration into the formula: pOH = -log(1.0 x 10^-3).
Step 4: Calculate the logarithm: -log(1.0 x 10^-3) equals 3.
Step 5: Now that you have pOH, use the relationship between pH and pOH: pH = 14 - pOH.
Step 6: Substitute the value of pOH into the equation: pH = 14 - 3.
Step 7: Calculate the final pH: 14 - 3 equals 11.
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