Problem: A solution is made by adding 50.0 mL of 0.200 M acetic acid (K a = 1.8 X 10 -5) to 50.0 mL of 1.00 X 10-3 M HCl.a. Calculate the pH of the solution.

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FREE Expert Solution

HCl is a strong binary acid. 

  • Strong acids → completely dissociate in water.
  • Acids donate H+ to the base (water in this case).
  • The dissociation of HCl is as follows: 
      HCl(aq) + H2O(l)  H3O+(aq) + ClO4(aq)


CH3COOH is a weak acid. 

  • Weak acids → incomplete dissociation in water.
  • Acids donate H+ to the base (water in this case).
  • The dissociation of CH3COOH is as follows: 
      CH3COOH(aq) + H2O(l)  H3O+(aq) + CHCOO(aq)


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Problem Details

A solution is made by adding 50.0 mL of 0.200 M acetic acid (K a = 1.8 X 10 -5) to 50.0 mL of 1.00 X 10-3 M HCl.

a. Calculate the pH of the 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.

What professor is this problem relevant for?

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

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.