A solution of Acetic acid has a light red color in the presense of the indicator orange IV. When sodium acetate is added to the solution, the color changes to yellow. Explain the reaction which causes the color change.
I have no idea. Does it have to do with the sodium added? I don't understand. Help please!
What is a disadvantage of using pH indicators?
3 answers
Disadvantage of using pH indicators for what? For titrations it is that not all indicators change at the equivalence point pH. If for determining the pH of a solution, it is because most pH indicators have a pH range of about 2 pH units which isn't very close if you want to know the pH closer than 2 pH units.
Joyce, you should have posted your question separately. There is a good chance it will get overlooked by piggy backing on another question.
The answer is that acetic acid/sodium acetate mixtures form a buffered solution. The addition of the acetate changes the pH enough that the indicator changes.
You can calculate the change in pH if you have enough information to plug into the Henderson-Hasselbalch equation which is pH = pKa + log(base/acid).
The answer is that acetic acid/sodium acetate mixtures form a buffered solution. The addition of the acetate changes the pH enough that the indicator changes.
You can calculate the change in pH if you have enough information to plug into the Henderson-Hasselbalch equation which is pH = pKa + log(base/acid).
1 answer