Before Class on Tuesday, Feb. 28

After reviewing the quiz we took last class, our new learning targets for Tuesday, Feb. 28 relate to buffers.   You should have picked up a packet of notes for buffers in class. If not they are here:   Buffer Notes .  We will discuss buffers before continuing our discussion of titrations.

After Feb. 28, you will be able to:

  • Describe the common ion effect;
  • Explain how a buffer functions;
  • Calculate the pH of a buffered solution;
  • Calculate the pH of a buffer after the addition of small amounts of a strong acid or a strong base.

Please watch the  4 videos below before Tuesday (12 min, 18 min, 14 min, 12 min.):

Intro to Buffers:

https://www.youtube.com/watch?v=cQZEZB2w3r4

Common Ions and Buffers: (18 min)

https://www.youtube.com/watch?v=RiTzZtQZDdc

Henderson Hasselbach and Buffers: (14 min)

https://www.youtube.com/watch?v=Jk9lRx8w4C0

Using Henderson Hasselbach to calculate pH: (12 min)

https://www.youtube.com/watch?v=qeHRmrxfx1Q

 

 

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2 thoughts on “Before Class on Tuesday, Feb. 28”

  1. In this video I learned about buffers. A buffer uses the common ion effect to ensure that even if an acid or base is added to a solution, its pH will stay the same. This is important in blood. A buffer is created by combining an an acid with its conjugate base. One can calculate the pH of a solution before and after an acid or base is adding using a rice table. A Henderson Hasselbach equation can be used after equilibrium is reached to calculate the pH of a solution. The henderson hasselbach equation states that the pH is equal to pKa plus the log of the weak acid concentration over the weak base concentration. A buffer is stressed when a strong acid is added to it.

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  2. In this video, I learned about buffers and how to calculate the pH based on my knowledge of buffers and acids and bases. I learned the equation in which the pH is equal to the pKa plus the log of the concentration of a weak base divided by the concentration of a weak acid. I also learned that the pH will equals to the pKa is the concentration of weak base is equal to the concentration of the weak acid.

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