What is the pH of a 0.05 M acetic acid solution (Ka = 1.8 x 10^-5)? (2023)

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Question: What is the pH of a 0.05 M acetic acid solution (Ka = 1.8 x 10^-5)? (2023)

Options:

Correct Answer: 4.7

Solution:

Using the formula for weak acids, pH = 0.5(pKa - log[C]) where pKa = -log(1.8 x 10^-5) ≈ 4.74. pH = 0.5(4.74 - log(0.05)) ≈ 4.7.

What is the pH of a 0.05 M acetic acid solution (Ka = 1.8 x 10^-5)? (2023)

What is the pH of a 0.05 M acetic acid solution (Ka = 1.8 x 10^-5)? (2023)

Step 1: Identify the concentration of acetic acid, which is 0.05 M.
Step 2: Find the acid dissociation constant (Ka) for acetic acid, which is 1.8 x 10^-5.
Step 3: Calculate the pKa using the formula pKa = -log(Ka). So, pKa = -log(1.8 x 10^-5).
Step 4: Use a calculator to find pKa, which is approximately 4.74.
Step 5: Use the formula for weak acids to find pH: pH = 0.5(pKa - log[C]). Here, [C] is the concentration of acetic acid, which is 0.05.
Step 6: Calculate log(0.05) using a calculator, which is approximately -1.3.
Step 7: Substitute the values into the pH formula: pH = 0.5(4.74 - (-1.3)).
Step 8: Simplify the equation: pH = 0.5(4.74 + 1.3) = 0.5(6.04).
Step 9: Calculate the final pH: pH ≈ 3.02.

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