Problem: The Ka value for acetic acid, CH3COOH(aq), is 1.8 x 10-5. Calculate the pH of a 1.20 M acetic acid solution. Calculate the pH of the resulting solution when 3.50 mL of the 1.20 M acetic acid is diluted to make a 250.0 mL solution.

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The Ka value for acetic acid, CH3COOH(aq), is 1.8 x 10-5. Calculate the pH of a 1.20 M acetic acid solution. 

Calculate the pH of the resulting solution when 3.50 mL of the 1.20 M acetic acid is diluted to make a 250.0 mL solution.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

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Based on our data, we think this problem is relevant for Professor Coleman's class at UCSD.