Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Suppose you are asked to prepare a buffer solution for an upcoming experiment using stock solutions of the weak acid and its conjugate base. Use the following information to determine the volumes of weak acid, conjugate base and distilled water you will need to make the buffer solution:
You have 1.0 M stock sodium hydrogencarbonate (NaHCO3) solution, pKa=10.33
You also have 1.0 M stock disodium carbonate (NaCO3) solution
The final buffer solution should have a concentration of 80 mM, a volume of 500 mL, and a pH of 9.60
First, use the HH equation to calculate the ratio of the two stock solutions you will need to mix together to reach the target pH, and report this ratio.
Next, calculate and report the volumes of weak acid, conjugate base and dH2O you will need to prepare the buffer. No sample calculation is necessary.
Hints:
• Calculate the volume of distilled water by considering the HA and A- stock solutions as a single mixture of 1.0 M buffer. This way, it's easier to calculate the volume of water, and the total volume of buffer mixture needed to reach your final volume and buffer concentration.
• Once you have the volume of buffer mixture required, use the ratio of A-/HA determined above to calculate the volume of each stock solution that will make up the total volume of buffer mixture being mixed with the distilled water.
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