Buffer Solutions Worksheet - Answer Key

 

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  1. What is a buffer solution?

    A buffer solution is one that is able to resist (or minimize) changes in pH. 

     

     

  2. When solving problems for a buffer solution you can bypass the ICE chart and use the Henderson-Hasselbalch equation instead.   What is the Henderson-Hasselbalch equation?

     pH = pKa + log ([base]/[acid])                                 

     

         
  3. Identify the buffer(s)?
    1. HCl and NaClO­4.
    2. HClO and LiClO2
    3. HF and KF
    4. CH3NH2 and CH3NH3Cl

       

       
  4. Determine the pH of the following solutions
    1. 1.00 L solution of 1.00M HNO2 and 1.50M NaNO2. 
      (Ka = 4 x 10-4)

      pH = 3.57
                             
    2. 25.0g of NH3  and 40.0g NH4NO3 in 501.0 mL of water. 
      (Ka = 5.6 x 10-10)

      pH = 9.72

       

       

  5. What is buffer capacity?

    The amount of acid or base a buffer can absorb without having a significant change in pH.

     

     

  6. Consider:

    0.1 M NaF and 0.1M HF
    1.0M NaF and 1.0M HF
    0.01M NaF and 0.01M HF
    1. Which has the highest pH?

      They all have the same pH.
    2. Which has the highest buffer capacity?

      1.0 M NaF and 1.0 M HF
    3. Consider a solution that contains both NH3 and NH4NO3.  If a solution has a pH = 8.5, calculate the ratio of    

      [NH3]
                                                      [NH4+]   

      Ka = 5.6 x 10-10

      0.177

       

       

  7. What volumes of 0.22M CH3COOH and 0.46M NaCH3COO must be mixed to prepare a 1.00L solution buffered at pH = 5.00?  (Ka = 1.76 x 10-5)

    0.457 L NaCH3COO and 0.543 L CH3COOH

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