In: Chemistry
The buffer capacity of a solution may be defined as the number of moles of H+ that will change the pH of 1.00 L of the buffer by 1.00 pH units. What is the buffer capacity of a solution which is 0.10 M in acetic acid (Ka = 1.8 × 10-5) and 0.30 M in sodium acetate, in units of mol (H+) per liter? Please show full work. (Answer key says 0.21 mol).
Given Ka, find pKa as pKa = -log (Ka) = -log (1.8*10-5) = 4.74.
Find the pH of the buffer by using the Henderson-Hasslebach equation as
pH = pKa + log [A-]/[HA] (HA denotes acetic acid and A- denotes acetate)
====> pH = 4.74 + log (0.30 M)/(0.10 M)
====> pH = 4.74 + log (3.00) = 4.74 + 0.477 = 5.217 ≈ 5.22.
The pH of the buffer changes by 1.0 unit due to the addition of H+. We know that the addition of H+ lowers the capacity of the pH of the buffer; hence, the new pH is (5.22 – 1.0) = 4.22.
Again, find the ratio of A- and HA using the Henderson-Hasslebach equation as
pH = pKa + log [A-]/[HA]
====> 4.22 = 4.74 + log [A-]/[HA]
====> log [A-]/[HA] = -0.52
====> [A-]/[HA] = antilog (-0.52) = 0.30199 ≈ 0.302
====> [A-] = 0.302*[HA]
We had 1.0 L of 0.10 M acetic acid and 0.30 M sodium acetate; hence, moles HA present in the buffer initially = (1.0 L)*(0.10 M) = 0.10 mole; moles A- present in the buffer initially = (1.0 L)*(0.30 M) = 0.30 mole.
H+ reacts with A- to form to HA as below.
A- + H+ ------> HA
As per the stoichiometric equation,
1 mole H+ = 1 mole A- = 1 mole HA
Let x moles H+ be added to the buffer; therefore, x moles H+ will react with x moles A- to form x moles HA. The number of moles of HA and A- at equilibrium are (0.10 + x) mole and (0.30 – x) mole respectively.
Since the volume of the solution stays same, we have, after the addition of H+,
[HA] = (0.10 + x)mole/(1.0 L) = (0.10 + x) M
[A-] = (0.30 – x)mole/(1.0 L) = (0.30 – x) M
As per the problem,
(0.30 – x) = 0.302*(0.10 + x)
====> 0.30 – x = 0.0302 + 0.302x
====> 0.2698 = 1.302x
====> x = (0.2698)/(1.302) = 0.2072 ≈ 0.21
The number of moles of H+ added is 0.21 mole (ans).