Which has greatest buffering capacity

A popular buffer solution consist of carbonate CO3 2- and hydrogen carbonate HCO3- conjugate acid-base pair. Which, if any of the following such buffers has the highest buffer capacity? Of the following solutions, which has the greatest buffering capacity? A Determine whether or not each of the following additions would exceed the capacity of the buffer to neutralize it. There is a. The pH of the buffer is 4. How many moles of NaOH must be added to the buffer solution to increase its pH to 5.

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Log In. What scientific concept do you need to know in order to solve this problem? Our tutors have indicated that to solve this problem you will need to apply the Buffer concept. You can view video lessons to learn Buffer. Or if you need more Buffer practice, you can also practice Buffer practice problems.

Our tutors rated the difficulty of Of the following solutions, which has the greatest buffering Our expert Chemistry tutor, Sabrina took 3 minutes and 38 seconds to solve this problem. You can follow their steps in the video explanation above. If you forgot your password, you can reset it. Join thousands of students and gain free access to 46 hours of Chemistry videos that follow the topics your textbook covers.

Analytical Chemistry Video Lessons. It's always the pK a of the conjugate acid that determines the approximate pH for a buffer system, though this is dependent on the pK b of the conjugate base, obviously. When the desired pH of a buffer solution is near the pK a of the conjugate acid being used i. In this example we will continue to use the hydrofluoric acid buffer. We will discuss the process for preparing a buffer of HF at a pH of 3. This is simply the ratio of the concentrations of conjugate base and conjugate acid we will need in our solution.

How much Sodium Fluoride would we need to add in order to create a buffer at said pH 3. From a table of molar masses, such as a periodic table, we can calculate the molar mass of NaF to be equal to Using this information, we can calculate the amount of F - we need to add.

We could use ICE tables to calculate the concentration of F - from HF dissociation, but, since K a is so small, we can approximate that virtually all of the HF will remain undissociated, so the amount of F - in the solution from HF dissociation will be negligible.

Thus, the [HF] is about 1 M and the [F - ] is close to 0. This will be especially true once we have added more F - , the addition of which will even further suppress the dissociation of HF.

Thus, [F - ] should be about 0.