Which of the following will increase the pH of an buffer solution?

I. Removing carbonic acid

II. Adding sodium bicarbonate

A buffer using acetic acid (pKa=4.76) is titrated with NaOH. What is the pH at half the equivalence point?

Which of the following combinations cannot be used to produce a buffer solution?

There are many solution systems which can only function as desired when the pH of that solution stays within a narrow range. Maintaining a stable pH in an unstable environment is most often achieved by the use of a buffer system, which is composed of a conjugate acid-base pair. One physiologically important buffer system is the bicarbonate buffer system that resists changes in blood pH.

The acid dissociation constant of carbonic acid

The normal blood pH is tightly regulated between 7.35 and 7.45

When blood pH falls below 7.35 a person is said to have acidosis. Depending upon how far the pH drops, this condition could lead to nervous system impairment, coma, and death.

What is the ratio of bicarbonate ion concentration to carbonic acid concentration at which an individual will be at the threshold of experiencing acidosis

Which of the following solutions has the greatest buffering capacity?

To create a buffer solution, you can use a weak acid and .

Which of the following would best buffer a solution from a pH of 4 to 6?

Which of the following can be used in a buffer solution?

Blood is a physiological buffer. The carbonic acid/bicarbonate system maintains blood’s pH at around 7.35. Carbon dioxide in blood undergoes a complex equilibrium reaction as follows:

Alterations to carbon dioxide levels can change the blood pH.

A patient has abnormally low levels of carbon dioxide in the blood. What can you conclude about this patient?

A researcher is trying to make a buffer solution from a weak acid and its weak conjugate base. The pKa of the acid is 5.9 and the desired pH of the buffer solution is 3.5. Which of the following is the best way to make this buffer solution?