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Calculate the pH of a 0.1 M acetic acid solution (Ka = 1.8 x 10^-5).
Calculate the pH of a 0.1 M acetic acid solution (Ka = 1.8 x 10^-5).
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Practice Questions
1 question
Q1
Calculate the pH of a 0.1 M acetic acid solution (Ka = 1.8 x 10^-5).
2.87
3.87
4.87
5.87
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Using the formula for weak acids, pH = 0.5(pKa - log[C]), where pKa = -log(1.8 x 10^-5) ≈ 4.74. Thus, pH = 0.5(4.74 - log(0.1)) = 3.87.
Questions & Step-by-step Solutions
1 item
Q
Q: Calculate the pH of a 0.1 M acetic acid solution (Ka = 1.8 x 10^-5).
Solution:
Using the formula for weak acids, pH = 0.5(pKa - log[C]), where pKa = -log(1.8 x 10^-5) ≈ 4.74. Thus, pH = 0.5(4.74 - log(0.1)) = 3.87.
Steps: 9
Show Steps
Step 1: Identify the concentration of acetic acid, which is 0.1 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. This gives 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 the acid, which is 0.1.
Step 6: Calculate log(0.1). This is equal to -1.
Step 7: Substitute the values into the pH formula: pH = 0.5(4.74 - (-1)).
Step 8: Simplify the equation: pH = 0.5(4.74 + 1) = 0.5(5.74).
Step 9: Calculate the final pH: pH = 2.87.
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