Question 19.2: Using Molecular Scenes to Examine Buffers Problem The molecu......
Using Molecular Scenes to Examine Buffers
Problem The molecular scenes below represent equal-volume samples of four HA/A^− buffers (Fig 19.2). (HA is blue and green, and A^− is green; other ions and water are not shown.)
(a) Which buffer has the highest pH?
(b) Which buffer has the greatest capacity?
(c) Should you add a small amount of concentrated strong acid or strong base to convert sample 1 to sample 2 (assuming no volume change)?
Plan The molecular scenes show varying numbers of weak acid molecules (HA) and the conjugate base (A^−). Because the volumes are equal, the scenes represent molarities as well as numbers. (a) As the pH rises, more HA loses its H^+ and becomes A^−, so the [A^−]/[HA] ratio will increase. We examine the scenes to see which has the highest ratio. (b) Buffer capacity depends on buffer-component concentration and ratio. We examine the scenes to see which has a high concentration and a ratio close to 1. (c) Adding strong acid converts some A^− to HA, and adding strong base does the opposite.
Comparing the [A^−]/[HA] ratios in samples 1 and 2 tells which to add.
Solution (a) The [A^−]/[HA] ratios are as follows: For sample 1, [A^−]/[HA] = 3/3 = 1. Similarly, sample 2 = 0.5; sample 3 = 1; sample 4 = 2. Sample 4 has the highest pH because it has the highest [A^−]/[HA] ratio.
(b) Samples 1 and 3 have a [A^−]/[HA] ratio of 1, but sample 3 has the greater capacity because it has a higher concentration.
(c) Sample 2 has a lower [A^−]/[HA] ratio than sample 1, so you would add strong acid to sample 1 to convert some A^− to HA.