What is the pH of a 0.001 M acetic acid solution (Ka = 1.8 x 10^-5)?

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Question: What is the pH of a 0.001 M acetic acid solution (Ka = 1.8 x 10^-5)?

Options:

Correct Answer: 3.87

Solution:

Using the formula for weak acids, pH = 0.5(pKa - logC) = 0.5(4.74 - log(0.001)) = 3.87.

What is the pH of a 0.001 M acetic acid solution (Ka = 1.8 x 10^-5)?

What is the pH of a 0.001 M acetic acid solution (Ka = 1.8 x 10^-5)?

Step 1: Identify the concentration of acetic acid (C) which is given as 0.001 M.
Step 2: Calculate the pKa from the given Ka value. pKa = -log(Ka) = -log(1.8 x 10^-5).
Step 3: Use a calculator to find pKa. pKa ≈ 4.74.
Step 4: Use the formula for weak acids to find pH: pH = 0.5(pKa - logC).
Step 5: Substitute the values into the formula: pH = 0.5(4.74 - log(0.001)).
Step 6: Calculate log(0.001), which is -3.
Step 7: Substitute -3 into the formula: pH = 0.5(4.74 - (-3)).
Step 8: Simplify the equation: pH = 0.5(4.74 + 3) = 0.5(7.74).
Step 9: Calculate the final pH: pH = 3.87.

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