Problem: How do you calculate the change in pH when 3.00 mL of 0.100 M   HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq) ?

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We have to calculate the change in pH of a buffer made of NH3(aq) and NH4Cl(aq) when a small amount of HCl is added to the buffer.

The change in pH of the buffer can be calculated through these steps:

  1. Find the initial pH of the buffer using the Henderson-Hasselbalch equation.
  2. Find the changes in concentrations of the buffer components when HCl is added.
  3. Find the new pH of the buffer using the Henderson-Hasselbalch equation.
  4. Calculate the change in pH of the buffer.
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Problem Details

How do you calculate the change in pH when 3.00 mL of 0.100 M   HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq) ?

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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 Buffer concept. You can view video lessons to learn Buffer. Or if you need more Buffer practice, you can also practice Buffer practice problems.