What is the pH of a solution with a hydroxide ion concentration of 0.001 M?

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Question: What is the pH of a solution with a hydroxide ion concentration of 0.001 M?

Options:

Correct Answer: 12

Solution:

pOH = -log[OH-] = -log(0.001) = 3; pH = 14 - pOH = 14 - 3 = 11

What is the pH of a solution with a hydroxide ion concentration of 0.001 M?

What is the pH of a solution with a hydroxide ion concentration of 0.001 M?

Step 1: Identify the concentration of hydroxide ions (OH-) in the solution, which is given as 0.001 M.
Step 2: Use the formula for pOH, which is pOH = -log[OH-].
Step 3: Substitute the value of [OH-] into the formula: pOH = -log(0.001).
Step 4: Calculate the logarithm: -log(0.001) equals 3, so pOH = 3.
Step 5: Use the relationship between pH and pOH, which is pH + pOH = 14.
Step 6: Substitute the value of pOH into the equation: pH = 14 - pOH = 14 - 3.
Step 7: Calculate the final pH: pH = 11.

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