Problem: Calculate the pH of a solution formed by adding 0.20 moles of NaOH to 1.00 liter of 0.50 M acetic acid. Ka = 1.8 x 10-5 for acetic acid.A. 4.24B. 3.74C. 4.92D. 4.57E. 2.63

FREE Expert Solution

We are being asked to calculate the pH of a solution when 0.20 moles of NaOH is added to 1.00 liter of 0.50 M acetic acid.


We will calculate the pH of the solution using the following steps:

Step 1. Write the chemical equation for the reaction between acetic acid and NaOH.
Step 2. Determine the initial amounts of acetic acid and Ba(OH)2 in moles before the reaction happens.
Step 3. Construct an ICF Chart.
Step 4. Calculate pH.


Step 1. Write the chemical equation for the reaction between acetic acid and Ba(OH)2.

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Problem Details

Calculate the pH of a solution formed by adding 0.20 moles of NaOH to 1.00 liter of 0.50 M acetic acid. Ka = 1.8 x 10-5 for acetic acid.

A. 4.24

B. 3.74

C. 4.92

D. 4.57

E. 2.63

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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 Acid Strong Base Titrations concept. You can view video lessons to learn Weak Acid Strong Base Titrations. Or if you need more Weak Acid Strong Base Titrations practice, you can also practice Weak Acid Strong Base Titrations practice problems.