In: Chemistry
A buffer contains 0.17 mol of propionic acid (C2H5COOH) and 0.21 mol of sodium propionate (C2H5COONa) in 1.20 L.
Part A
What is the pH of this buffer?
Part B
What is the pH of the buffer after the addition of 0.02 mol of
NaOH?
Part C
What is the pH of the buffer after the addition of 0.02 mol of
HI?
Given 0.17 mol propionic acid , 0.21 mol sodium propionate in 1.20 L
We recognize the conjugate acid-base pair propionic acid (Ka = 1.3 x 10-5 and pKa = 4.9)
Part A:
[acid] = 0.17 / 1.2 = 0.1417 M
[base] = 0.21/1.2 = 0.175 M
pH of the buffer = 4.9 + log (0.175/0.1417) = 4.9 + 0.092 = 4.992
Part B:
moles acid = 0.17 - 0.02 = 0.15
[acid] = 0.15/1.2 = 0.125 M
moles salt = 0.21 + 0.02 = 0.23
[base] = 0.23/1.2 = 0.1917 M
pH of the buffer = 4.9 + log (0.1917/0.125) = 4.9 + 0.186 = 5.086
Part C:
moles of acid = 0.17 + 0.02 = 0.19
[acid] = 0.19/1.2 = 0.1583
moles of base = 0.21 - 0.02 = 0.19
[base] = 0.19/1.2 = 0.1583
pH of the buffer = 4.9 + log (0.1583/0.1583) = 4.9
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