Acidity $K_{a}$
Basicity $K_{b}$
The Conjugate Seesaw $K_{a}\times K_{b}=K_{w}$

Posts: 55
Joined: Sat Aug 17, 2019 12:15 am

In class, we talked about how the acid is neutral or negatively charged and I was confused as to the whole Ph>Pkka and how the solution would be more Alkaline and is thus more negatively charged. I'd like to know the reasoning behind this.

Joseph Saba
Posts: 154
Joined: Thu Jul 11, 2019 12:16 am

I am also confused about this. In my notes I have that "pH>Pka: the solution is more alkaline and the acid will give off H+ to form A- and is negatively charged." I'm not completely sure what the application of this means though.

Sebastian Lee 1L
Posts: 157
Joined: Fri Aug 09, 2019 12:15 am
Been upvoted: 1 time

What Dr. Lavelle was talking about was how much an acid will dissociate depending on the acidity of the solution it is in. Remember that for Bronsted acids, the acid in solution can dissociate into hydronium ions (H3O+) and the conjugate base (A-). For example, $HF \rightleftharpoons H^{+} + F^{-}$. When we say that the acid is negatively charged in solution, that means that it dissociates into the negative anion and hydronium ions rather than staying bonded together.