[coolusername]

1. 14 mmols of acetic acid and 87 mmols of sodium acetate were dissolved in a final volume
of 1 liter of water. Given our simplifying assumption that we can ignore the ionization of water
having any significant effect and given the pKa of acetic acid is 4.7, what is the pH? What is the
molar concentration of H+? Of OH-?
How should the bottle be labelled?



I used the moles of HA (acetic acid) and A- (sodium acetate) and divided by 1L to get their concentrations. I used the H-H equation to get the pH. However how would I find the molar concentration of H+ and OH-?

Also, would the a bottle containing this solution be labelled?

Are there any circumstances, or any types of buffers you might imagine, for which our
simplifying assumption would not hold true? What are they?

[Borek]

However how would I find the molar concentration of H+ and OH-?

What is pH? What is pOH? How they are related?

Are there any circumstances, or any types of buffers you might imagine, for which our
simplifying assumption would not hold true? What are they?

It matters only for the very diluted solutions.

[Babcock_Hall]

When I label a bottle of buffer, I use the total concentration of both buffering species.  This is something that students often get wrong.