You wish to prepare 100 mL of a buffer solution that is 0.025 M in carbonic...
You wish to prepare 100 mL of a buffer solution that is 0.025 M in carbonic acid (H2CO3). The pKa of H2CO3 is 6.351. Calculate the amount of H2CO3, in grams, that you will need to weigh out.
Homework Answers
Since you haven't mentioned pH of buffer solution
We are going to calculate it by H2CO3 concentration.
pH of 0.025 M H2CO3
pKa = -log[Ka] = 6.351
Ka = 4.46 x 10^-7
H2CO3 <==> H+ + HCO3-
let x be the amount of dissociation
Ka = [H+][HCO3-]/[H2CO3]
4.46 x 10^-7 = x^2/0.025
x = [H+] = 1.056 x 10^-4 M
pH = -log[H+] = 3.98 [Substituting this value with a differnt number would change all the further calculation results]
Using Hendersen-Hasselbalck equation,
pH = pKa + log)[base]/[acid])
3.98 = 6.351 + log([HCO3-]/[0.025])
[HCO3-]/[H2CO3] = 0.0042
[H2CO3] = (1/1.0042) x (0.025/0.1) = 0.025 M
[HCO3-] = (0.0042/1.0042) x (0.025/0.1) = 1.046 x 10^-4 M
grams of H2CO3 required = 0.025 x 0.1 x 62.03 = 0.155 g
pl. note. If you have a pH value for buffer, use
Hendersen-Hasselbalck equation directly and follow the procedure
with your calculated value accordingly.
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