Still am having trouble with titration

[westdavi]

Thank you for responding, but I am not sure how to solve this yet. I am sorry. Could you show me a more of the work needed? I teach high school chemistry, and it is beginning to look like the question is beyond the scope of the course, but now I am curious how to solve it.
Anyways, thanks for your help regardless
David Westra
You have two bottles, one filled with 1M HAc (HAc = acetic acid) and one filled with 1M NaOH. You want to make 100ml of a buffer with pH=4.6 by mixing together appropriate amounts of these solutions. How much of each solution do you use?

 

[siddharth]

I edited my reply to make it more detailed in your other post. Hope that helps.

 

[Blueshift5]

Hello David,

I am sorry to hear that you are still having trouble with titration. It can be a difficult concept to grasp, but with practice and guidance, I am sure you will get the hang of it.

In regards to the question you have provided, I understand your concern about it potentially being beyond the scope of your high school chemistry course. However, it is always beneficial to challenge ourselves and learn new things, so I encourage you to try and solve it.

To solve this titration problem, you will need to use the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the pKa of the weak acid and the concentrations of the acid and its conjugate base. In this case, the weak acid is acetic acid (HAc) and its conjugate base is acetate (Ac-).

The first step is to determine the pKa of acetic acid, which is 4.76. Next, using the Henderson-Hasselbalch equation, you can plug in the given pH of 4.6, the pKa of 4.76, and the desired buffer volume of 100ml. This will give you the ratio of [Ac-]:[HAc] needed to achieve a buffer with a pH of 4.6.

Once you have this ratio, you can then calculate the amount of each solution needed to achieve the desired concentrations. Since the solutions are both 1M, you can use the formula C1V1 = C2V2 to determine the volumes of each solution needed.

I hope this explanation has helped and provided you with a starting point to solve the problem. If you need further assistance, please do not hesitate to reach out. Best of luck in your studies!

Sincerely,