Solution Found!
Solved: To act as an effective buffer, the concentrations
Chapter 16, Problem 91P(choose chapter or problem)
To act as an effective buffer, the concentrations of the acid and the conjugate base should not differ by more than a factor of 10, that is,
\(10 \geq \frac{\text { [conjugate base }]}{[\text { acid }]} \geq 0.1\)
(a) Show that the buffer range, that is, the range of the concentration ratio over which the buffer is effective, is given by \(\mathrm{pH=p}K_\mathrm a \pm 1\).
(b) Calculate the pH range for the following buffer systems: (a) acetate, (b) nitrite, (c) bicarbonate, (d) phosphate.
Questions & Answers
QUESTION:
To act as an effective buffer, the concentrations of the acid and the conjugate base should not differ by more than a factor of 10, that is,
\(10 \geq \frac{\text { [conjugate base }]}{[\text { acid }]} \geq 0.1\)
(a) Show that the buffer range, that is, the range of the concentration ratio over which the buffer is effective, is given by \(\mathrm{pH=p}K_\mathrm a \pm 1\).
(b) Calculate the pH range for the following buffer systems: (a) acetate, (b) nitrite, (c) bicarbonate, (d) phosphate.
ANSWER:
Step 1 of 3
(a)
From the given,
For an effective buffer, the concentration values of the acid and the conjugate base should not differ by more than a factor of 10, this is given by,
