How do the graphs differ between the titration of buffer with NaOH and the titra
ID: 489951 • Letter: H
Question
How do the graphs differ between the titration of buffer with NaOH and the titration of water with NaOH? Why? How do the graphs differ between the titration of buffer with HCI and the titration of water with HCI? Why? Which solution (HCI or NaOH) required the largest volume to reach equivalence point when titrating the acetate buffer? Why do you think this is the case? How do you hypothesize that these results would differ if a basic buffer was titrated (vs. an acidic one)? Does the buffer action of acetate last over the entire pH range? Why or why not? What evidence do you have of this?Explanation / Answer
Q1.
Titration of buffer will have small pH changes, whereas water will have drastic changes in pH. the pH increases drastically due to OH- ions in water
Q2
Titration of buffer will have small pH changes, whereas water will have drastic changes in pH. the pH decreases drastically due to H+ ions in water
Q3
Impossible to identify... but...
If the amount of acetate > acetic acid.... we require much more Acid than base
If the amount of acetate < acetic acid.... we require much more Base than acid
If the amount of acetate = acetic acid.... we require same Acid as Base
Q4
if we use a basic buffer, pH will be decreasin when adding H and increasing with OH-
Q5.
No, the buffer action only last betwee pH = pKa value
but +/-1 uinits of pH, the buffer will fail
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