High School

We appreciate your visit to In a solution of 168 3 mM acetate buffer this is the concentration of all ionization states of the acetate acetic acid combined what is. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!

In a solution of 168.3 mM acetate buffer (this is the concentration of all ionization states of the acetate/acetic acid combined), what is the pH of the solution if the concentration of acetate is 36.6 mM (just the deprotonated state)? The pKa of acetic acid is 4.76. Report your answer to two decimal places.

Answer :

Question: In a solution of 168.3 mM acetate buffer (this is the concentration of all ionization states of the acetate/acetic acid combined), what is the pH of the solution if the concentration of acetate is 36.6 mM (just the deprotonated state)? The pKa of acetic acid is 4.76. Report your answer to two decimal places.

To find the pH of the solution, we can use the Henderson-Hasselbalch equation, which relates the pH of a solution to the concentration of the acid and its conjugate base. The equation is:

pH = pKa + log([A-]/[HA])

Where:
pH is the pH of the solution
pKa is the acid dissociation constant
[A-] is the concentration of the acetate ion (deprotonated state)
[HA] is the concentration of the acetic acid

In this case, the concentration of acetate ([A-]) is given as 36.6 mM, and the pKa of acetic acid is 4.76.

Now let's plug these values into the equation:

pH = 4.76 + log(36.6/([HA]))

Since we know the concentration of acetate ([A-]), we can subtract it from the total concentration of the buffer to find the concentration of acetic acid ([HA]):

[HA] = 168.3 - 36.6 = 131.7 mM

Now we can substitute this value into the equation:

pH = 4.76 + log(36.6/131.7)

Calculating this expression, we get:

pH ≈ 4.76 + log(0.2779)

Using a calculator, we find:

pH ≈ 4.76 + (-0.5562)

pH ≈ 4.20

Therefore, the pH of the solution is approximately 4.20 when the concentration of acetate is 36.6 mM.

Know more about Henderson-Hasselbalch equation here:

https://brainly.com/question/31495136

#SPJ11

Thanks for taking the time to read In a solution of 168 3 mM acetate buffer this is the concentration of all ionization states of the acetate acetic acid combined what is. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!

Rewritten by : Barada