Please see the information Iâve provided in bold, then fill in the blanks below #11 (A-G and the following questions). This is not a long question - I only need a few things answered, and all the information you need is here. I am just struggling with what is the "strong acid" and what numbers to put in for pH. Thanks!
Select 4 250-mL Erlenmeyer Flasks from the pictorial or equipment menu. Keep track of which one is which.
Click on the first flask and add 100 mL of distilled water to it. Click on the second flask and add 100 mL of distilled water to it.
Click on the third flask and add 74.0 mL of 0.1 M acetic acid to it. Also add 1.1 g of sodium acetate to the third flask. Finally add 26.0 mL of distilled water to the third flask. Stir the solution.
Click on the fourth flask and add 74.0 mL of 0.1 M acetic acid to it. Also add 1.1 g of sodium acetate to the fourth flask. Finally add 26.0 mL of distilled water to the fourth flask. Stir the solution.
Right click on each of the flasks and choose pH meter. The pH of each solution should appear in blue below the flask.
Record the pH of each solution on a separate WORD document.
My recordings: pH = 7. 2) pH = 7. 3) pH = 5.0127. 4) pH = 5.0127
Add 5.0 mL of HCl to the first flask. Record the pH on the Report sheet. pH 2.3222
Add 5.0 mL of NaOH to the second flask. Record the pH on the Report sheet. pH 11.6778
Add 5.0 mL of HCl to the third flask. Record the pH on the Report sheet. pH 4.9679
Add 5.0 mL of NaOH to the fourth flask. Record the pH on the Report sheet. pH 5.0590
A. Preparation the buffer solution:
initial pH of buffer solution: ____
B. Titration of a weak acid with a strong base:
initial pH of weak acid: ____
final pH of weak acid: ____
Amount of NaOH added: ____
C. Titration Curve for Weak Acid with a Strong Base
(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)
D. Titration of buffer with a strong base:
pH of buffer solution: ____
Amount of NaOH added: ____
E. Titration Curve for Buffer with a Strong Base
(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)
F. Titration of the buffer with a strong acid:
pH of buffer solution: ____
Amount of HCl added: ____
G. Titration Curve for Buffer with a Strong Acid
(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)
Questions:
What conclusions can you draw from looking at the titration curve of the weak acid with a strong base and comparing it to the titration curve for the buffer with a strong base?
What conclusions can you draw from looking at the titration curve of the buffer with a strong base and comparing it to the titration curve for the buffer with a strong acid?
Please see the information Iâve provided in bold, then fill in the blanks below #11 (A-G and the following questions). This is not a long question - I only need a few things answered, and all the information you need is here. I am just struggling with what is the "strong acid" and what numbers to put in for pH. Thanks!
Select 4 250-mL Erlenmeyer Flasks from the pictorial or equipment menu. Keep track of which one is which.
Click on the first flask and add 100 mL of distilled water to it. Click on the second flask and add 100 mL of distilled water to it.
Click on the third flask and add 74.0 mL of 0.1 M acetic acid to it. Also add 1.1 g of sodium acetate to the third flask. Finally add 26.0 mL of distilled water to the third flask. Stir the solution.
Click on the fourth flask and add 74.0 mL of 0.1 M acetic acid to it. Also add 1.1 g of sodium acetate to the fourth flask. Finally add 26.0 mL of distilled water to the fourth flask. Stir the solution.
Right click on each of the flasks and choose pH meter. The pH of each solution should appear in blue below the flask.
Record the pH of each solution on a separate WORD document.
My recordings: pH = 7. 2) pH = 7. 3) pH = 5.0127. 4) pH = 5.0127
Add 5.0 mL of HCl to the first flask. Record the pH on the Report sheet. pH 2.3222
Add 5.0 mL of NaOH to the second flask. Record the pH on the Report sheet. pH 11.6778
Add 5.0 mL of HCl to the third flask. Record the pH on the Report sheet. pH 4.9679
Add 5.0 mL of NaOH to the fourth flask. Record the pH on the Report sheet. pH 5.0590
A. Preparation the buffer solution:
initial pH of buffer solution: ____
B. Titration of a weak acid with a strong base:
initial pH of weak acid: ____
final pH of weak acid: ____
Amount of NaOH added: ____
C. Titration Curve for Weak Acid with a Strong Base
(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)
D. Titration of buffer with a strong base:
pH of buffer solution: ____
Amount of NaOH added: ____
E. Titration Curve for Buffer with a Strong Base
(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)
F. Titration of the buffer with a strong acid:
pH of buffer solution: ____
Amount of HCl added: ____
G. Titration Curve for Buffer with a Strong Acid
(Paste curve here, or tell me how to get it in Excel or elsewhere - this is something I need help with - not something that I can post)
Questions:
What conclusions can you draw from looking at the titration curve of the weak acid with a strong base and comparing it to the titration curve for the buffer with a strong base?
What conclusions can you draw from looking at the titration curve of the buffer with a strong base and comparing it to the titration curve for the buffer with a strong acid?
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