V. Acids & Bases (pg 9)
AP Chemistry
Buffers
1) Calculate the pH at which the following buffer systems are most effective:
a) HC7H5O2/C7H5O2- (Ka = 6.3 x 10-5)
b) CH3CH2NH2/CH3CH2NH3+ (Kb = 4.3 x 10-4)
2) What is the pH of a buffer prepared by dissolving 0.200 mole of HF and 0.100 mole of
NaF in water to make 1.00 liter of solution? (Ka of HF = 6.8 x 10-4)
3) Calculate the pH of the following buffer solutions:
a) 0.250 M acetic acid and 0.150 M sodium acetate (Ka = 1.8 x 10-5)
b) A solution of 10.0 g each of formic acid (HCHO2) and potassium formate
dissolved in 1.00 L of H2O (Ka of formic acid = 1.8 x 10-4)
c) 0.0345 M ethylamine (C2H5NH2) and 0.0965 M ethyl ammonium chloride. (Kb
= 4.3 x 10-4)
4) An acetate buffer is prepared with 0.250 M acetic acid and 0.100 M sodium acetate. If
0.002 mol of solid NaOH is added to 100 mL of this buffer, calculate the change in pH of
the buffer due to the addition of the NaOH.
5) Using the buffer in question 4, if 0.02 M of HCl is added to this buffer, calculate the
change in pH of the buffer due to the addition of the HCl. (assume that the volume
change is negligible)
6) A formic buffer is prepared with 0.250 M formic acid and 0.150 M sodium formate. If
0.02 M NaOH is added to this buffer, calculate the change in pH of the buffer due to the
addition of NaOH. (Assume that the volume change is negligible)
7) Using the buffer in question 6, if 0.02 M of HCl is added to this buffer, calculate the
change in pH of the buffer due to the addition of the HCl. (assume that the volume
change is negligible)
8) Calculate the pH of a buffer system consisting of 0.23 M CH3CH2NH2 and 0.46 M
CH3CH2NH3+. (Kb = 4.3 x 10-4) a) Calculate the new pH if 0.021 M [OH-] is added to the
system. (Assume that the volume change is negligible)
9)
a) Specify the properties of a buffer solution. Describe the components and the
composition of effective buffer solutions.
b) An employer is interviewing four applicants for a job as a laboratory technician
and asks each how to prepare a buffer solution with a pH close to 9.
Archie A. says he would mix acetic acid and sodium acetate solutions.
Beula B. says she would mix NH4Cl and HCl solutions.
Carla C. says she would mix NH4Cl and NH3 solutions.
Dexter D. says he would mix NH3 and NaOH solutions.
Which of these applicants has given an appropriate procedure? Explain your answer,
referring to your discussion in part a). Explain what is wrong with the erroneous
procedures.
Answers
1)
a) pH = 3.2 – 5.2
b) pH = 9.6 – 11.6
2) pH = 2.87
3) a) pH = 4.52
b) pH = 3.48
c) pH = 10.19
4) ∆pH = 0.11; Buffer pH = 4.35; addition of NaOH pH = 4.46
5) ∆pH = 0.13; buffer pH = 4.35; addition of HCl pH = 4.22
6) ∆pH = 0.09; buffer pH = 3.52; addition of NaOH pH = 3.61
7) ∆pH = 0.09; buffer pH = 3.52; addition of NaOH pH = 3.43
8) Buffer pH = 10.33, a) pH = 10.39
9) a) buffer = weak acid and salt of the conjugate base; also must maintain pH with the
addition or acid or base.
b) Carla C. has a buffer with the pH around 9. She has a weak base and the salt of the
conjugate acid. Although Archie has a buffer, the pH is around 5.