Advanced Equilibria - Lesson 2 - Calculations Involving Buffers by a.mustafasipsak


									                                                              You have seen how buffered solutions
     Calculations Involving                              can be made by adding a conjugate salt to a
            Buffers                                      weak acid or base, and how the pH of the
                                                         buffered solution can be found using the
                                                         ICE method or the Henderson-Hasselbalch
                                                             Calculate the pH of a buffered solution
                                                         containing .700 M methylamine and .500 M
                                                         methylaminium chloride.

Two important characteristics of a
buffer include:                                                 2. Buffering Capacity
             1. pH Range                                 • The buffering capacity of a buffered
• The pH range is the range of pH values                   solution represents the amount of
  over which a buffer system works                         acid or base that can be absorbed by
  effectively.                                             the solution without a significant
• The pH range of an acid or base can be                   change in pH.
  seen as the region of little pH change vs.
  volume of base/acid added on a titration               • A buffer with a large capacity
  curve                                                    contains large concentrations of
• It is best to choose an acid with a pKa                  buffering components.
  close to the desired pH.

    Therefore the capacity of a
                                                          1. Calculate the mass of sodium
buffered solution is determined by the
magnitudes of [HA] and [A-].                                 benzoate that must be added to 1 L
                                                             of 0.40 M benzoic acid (Ka = 6.4 x
    Using the Henderson-Hasselbalch                          10-5) solution to buffer at a pH of
equation, along with these                                   4.5. (Assume no change in total
relationships, we can create a buffer
system at almost any pH.

                  [Base]     pOH = pK b + log
pH = pK a + log
                  [Acid] ,                      [Base]

When Strong Acids or Bases Are                  In the addition of a strong acid or
Added to a Buffer…                                base to a buffered solution, there
 …it is safe to assume that                       are two considerations:
   all of the strong acid or
  base is consumed in the                       1. How does the added acid-base
                   reaction.                       react with the acid-base present in
                                                   the solution (neutralization)
                                                2. How does the neutralization of
                                                   hydronium or hydroxide affect the
                                                   equilibrium of the weak acid-base
                                                   present in the solution?

   Addition of Strong Acid or                                     • Here is a buffered
        Base to a Buffer                                            system in which
                                                                    strong base and
                                                                    strong acid have
               1. Determine how the
                                                                    been added.
                  neutralization reaction
                  affects the amounts of the                      • Let us investigate
                  weak acid and its                                 the results and
                  conjugate base in solution.                       model the
               2. Use the Henderson–                                quantitative
                  Hasselbalch equation to                           procedures needed
                  determine the new pH of                           to derive the
                  the solution.                                     resulting pH’s

Calculating pH Changes in Buffers               Calculating pH Changes in Buffers
  Example Problem:                               Before the reaction, since
   A buffer is made by adding 0.300
   mol HC2H3O2 and 0.300 mol                         mol HC2H3O2 = mol C2H3O2−
   NaC2H3O2 to enough water to
   make 1.00 L of solution. The pH
                                                  pH = pKa = −log (1.8 × 10−5) = 4.74
   of the buffer is 4.74. Calculate the
   pH of this solution after 0.020 mol
   of NaOH is added.

Calculating pH Changes in Buffers                       Calculating pH Changes in Buffers
The 0.020 mol NaOH will react with 0.020                Now use the Henderson–Hasselbalch
mol of the acetic acid:                                 equation to calculate the new pH:
    HC2H3O2(aq) + OH−(aq) → C2H3O2−(aq) + H2O(l)                         (0.320)
                                                         pH = 4.74 + log
                                                                           (0. 200)
                     HC2H3O2     C2H3O2−      OH−
                                                         pH = 4.74 + 0.06       • This problem could be
                                                                                solved using an ICE table,
Before reaction     0.300 mol   0.300 mol   0.020 mol
                                                                                however, it is much simpler
                                                         pH = 4.80              to use the Henderson-
After reaction      0.280 mol   0.320 mol   0.000 mol
                                                                                Hasselbalch equation since
                                                                                it is a buffered solution.

 2. Calculate the change in pH that                      3. Calculate the change in pH that
 occurs when 10.00 mL of 0.500 M                         occurs when 0.10 mol of HCL gas is
 perchloric acid is added to the buffer                  added to 1 L of a buffered solution
 from the example, after the base was                    containing 0.25 M ammonia and 0.40
 added.                                                  M ammonium bromide.


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